Post on 27-Jun-2015
Chapter 4 Electrons in Atoms
This chapter is about electrons in the atom- a tricky
subject at best- and the evolution of the atomic model
This chapter covers much material some of it very
difficult and abstract It is essential that you bring your
book to class and do all assigned homework
Chapter 4 Arrangement of Electrons in Atoms
bull Atomic Models
- already discussed atomic structure ndash what was it
- inadequate ndash describes only a few properties of atoms
- need a model that is focused on arrangement of ____ the basis of chemistry
Rutherford Model of the AtomThe Rutherford Model (aka the Planetary Model) was an
improvement over the previous models but it was still incomplete It did not include the distribution of the negatively
charged electrons in the atom
We know that negative and positive particles (that is e- and p+)
attract each other so the big question became
Why donrsquot the electrons crash into the nucleus
If + and ndash charges attract why donrsquot e- collapse into the nucleus
In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in
concentric circles around the nucleus (patterned after the movement of planets around the sun)
The Planetary Model
Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus
analogous to the rungs of a ladder More on this later
The Planetary Model of the Atom
But first letrsquos talk about
The Properties of LightBefore 1900 scientists thought light behaved solely as a wave
What idiots It was soon discovered that light also has particle
characteristics But letrsquos first review the wavelike properties
The Electromagnetic Spectrum
The electromagnetic spectrum shows all the types of
electromagnetic radiation- a form of energy that exhibits wavelike
behavior as it travels through space
All forms of electromagnetic radiation move at a constant speed
of 300 x 108 ms through a vacuum This is about 186000 miless
Also known as the speed of light
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Chapter 4 Arrangement of Electrons in Atoms
bull Atomic Models
- already discussed atomic structure ndash what was it
- inadequate ndash describes only a few properties of atoms
- need a model that is focused on arrangement of ____ the basis of chemistry
Rutherford Model of the AtomThe Rutherford Model (aka the Planetary Model) was an
improvement over the previous models but it was still incomplete It did not include the distribution of the negatively
charged electrons in the atom
We know that negative and positive particles (that is e- and p+)
attract each other so the big question became
Why donrsquot the electrons crash into the nucleus
If + and ndash charges attract why donrsquot e- collapse into the nucleus
In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in
concentric circles around the nucleus (patterned after the movement of planets around the sun)
The Planetary Model
Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus
analogous to the rungs of a ladder More on this later
The Planetary Model of the Atom
But first letrsquos talk about
The Properties of LightBefore 1900 scientists thought light behaved solely as a wave
What idiots It was soon discovered that light also has particle
characteristics But letrsquos first review the wavelike properties
The Electromagnetic Spectrum
The electromagnetic spectrum shows all the types of
electromagnetic radiation- a form of energy that exhibits wavelike
behavior as it travels through space
All forms of electromagnetic radiation move at a constant speed
of 300 x 108 ms through a vacuum This is about 186000 miless
Also known as the speed of light
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Rutherford Model of the AtomThe Rutherford Model (aka the Planetary Model) was an
improvement over the previous models but it was still incomplete It did not include the distribution of the negatively
charged electrons in the atom
We know that negative and positive particles (that is e- and p+)
attract each other so the big question became
Why donrsquot the electrons crash into the nucleus
If + and ndash charges attract why donrsquot e- collapse into the nucleus
In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in
concentric circles around the nucleus (patterned after the movement of planets around the sun)
The Planetary Model
Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus
analogous to the rungs of a ladder More on this later
The Planetary Model of the Atom
But first letrsquos talk about
The Properties of LightBefore 1900 scientists thought light behaved solely as a wave
What idiots It was soon discovered that light also has particle
characteristics But letrsquos first review the wavelike properties
The Electromagnetic Spectrum
The electromagnetic spectrum shows all the types of
electromagnetic radiation- a form of energy that exhibits wavelike
behavior as it travels through space
All forms of electromagnetic radiation move at a constant speed
of 300 x 108 ms through a vacuum This is about 186000 miless
Also known as the speed of light
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
If + and ndash charges attract why donrsquot e- collapse into the nucleus
In 1913 a student of Rutherfordrsquos created a new model for the atom he proposed the e-rsquos were arranged in
concentric circles around the nucleus (patterned after the movement of planets around the sun)
The Planetary Model
Along with this he stated that the e-rsquos have fixed energy that allows them to avoid falling into the nucleus
analogous to the rungs of a ladder More on this later
The Planetary Model of the Atom
But first letrsquos talk about
The Properties of LightBefore 1900 scientists thought light behaved solely as a wave
What idiots It was soon discovered that light also has particle
characteristics But letrsquos first review the wavelike properties
The Electromagnetic Spectrum
The electromagnetic spectrum shows all the types of
electromagnetic radiation- a form of energy that exhibits wavelike
behavior as it travels through space
All forms of electromagnetic radiation move at a constant speed
of 300 x 108 ms through a vacuum This is about 186000 miless
Also known as the speed of light
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Planetary Model of the Atom
But first letrsquos talk about
The Properties of LightBefore 1900 scientists thought light behaved solely as a wave
What idiots It was soon discovered that light also has particle
characteristics But letrsquos first review the wavelike properties
The Electromagnetic Spectrum
The electromagnetic spectrum shows all the types of
electromagnetic radiation- a form of energy that exhibits wavelike
behavior as it travels through space
All forms of electromagnetic radiation move at a constant speed
of 300 x 108 ms through a vacuum This is about 186000 miless
Also known as the speed of light
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
But first letrsquos talk about
The Properties of LightBefore 1900 scientists thought light behaved solely as a wave
What idiots It was soon discovered that light also has particle
characteristics But letrsquos first review the wavelike properties
The Electromagnetic Spectrum
The electromagnetic spectrum shows all the types of
electromagnetic radiation- a form of energy that exhibits wavelike
behavior as it travels through space
All forms of electromagnetic radiation move at a constant speed
of 300 x 108 ms through a vacuum This is about 186000 miless
Also known as the speed of light
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The electromagnetic spectrum shows all the types of
electromagnetic radiation- a form of energy that exhibits wavelike
behavior as it travels through space
All forms of electromagnetic radiation move at a constant speed
of 300 x 108 ms through a vacuum This is about 186000 miless
Also known as the speed of light
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Letrsquos talk about waves and wave motion for a minute
Frequency and wavelength are mathematically related This relationship is
c = λv
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
c = λvIn the equation c is the speed of light (in ms) λ is the wavelength of
the electromagnetic wave (in m) and v is the frequency of the electromagnetic wave (in s-1 or Hz)
Important λ and v are inversely proportional so as the wavelength of light increases the frequency decreases and vice versa
Practice Problems
1 Determine the frequency of light whose wavelength is 4257 x 10-5 m
2 Determine the wavelength (λ) of a photon whose frequency is 355 x 1017 s-1
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Electromagnetic Spectrum
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Photoelectric Effect
The photoelectric effect is a phenomenon that refers to
the emission of electrons from a metal when light shines
on the metal
Yoursquore most likely thinking who cares
Well herersquos the thing- for any given metal no electrons were
emitted if the lightrsquos frequency were below a certain minimum
Metal
Light
Electrons
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Photoelectric Effect (contrsquod)
So obviously light was known to be a form of energy capable of
knocking electrons loose from metal But (important)
the wave theory of light predicted that any frequency of light could
supply enough energy to eject an electron so the fact that there had
to be a minimum frequency for a given metal made no sense
Something about the assumption of light behavior was wrong
Metal
Light
Electrons
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Particle Description of Light
The German physicist Max Planck came up with the idea that light
is emitted in small packets called quanta
A quantum of energy is the minimum quantity of energy that
can be gained or lost by an atom
Here is the relationship between quantum and frequency of radiation
E = hvWhere E is the energy (J) v is the frequency (s-1) and h is the
physical constant called Planckrsquos Constant h = 6626 x 10-34 Js
Srsquoup
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Particle Description of Light
In 1905 Einstein took this idea further by stating that light can
act as both a wave and a stream of particles Each particle of light
carries a quantum of energy and is called a photon
A photon is a particle of electromagnetic radiation having zero
mass and carrying a quantum of energy
Ephoton = hvEinstein was able to explain the photoelectric effect this way
Different metals bind their electrons differently so v changes
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Hydrogen-Atom Line-Emission Spectrum
When an electric current is passed through a gas sample at low
pressure the potential energy of the gas changes
The ground state of an electron the energy level it normally occupies is the state of lowest energy for that electron
There is also a maximum energy that each electroncan have and still be part of its atom Beyond that energy the electron is no longer bound to the nucleus of the atom and it is considered to be ionized
When an electron temporarily occupies an energy state greater than its ground state it is in an excited state An electron can become excited if it is given extra energy such as if it absorbs a photon or packet of light or collides with a nearby atom or particle
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Hydrogen-Atom Line-Emission Spectrum
So what does this mean
Well when scientists passed an electric current through a vacuum
tube with a pure gas in it (like H or O) each atom would go through
the steps listed above they would gain energy and then reemit it
in the form of a photon or light This light was then passed through
a prism and the wavelengths (colors) in that element could be seen
Electrons do not stay in excited states for very long ndash they soon return to their ground states emitting a photon with the same energy as the one that was absorbed
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Hydrogen-Atom Line-Emission Spectrum
So letrsquos use the example of helium A tube of helium has a current of electricity
pass through it and the absorbed energy is then released in the form of light thus
the tube glows That light is then passed through a prism which separates all the
colors (wavelengths) in that light Helium has a particular emission-spectra or set
of lines at specific color spectra
Every element has a signature color spectra
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Hydrogen-Atom Line-Emission Spectrum
But why are there only some colors appearing and
not all of them
Because the electrons in these atoms have specific
fixed energy levels and only give off certain colors
when jumping from level to level Whenever an
excited helium atom falls to its ground state or to a
lower-energy excited state it emits a photon of
radiation The energy of this photon (Ephoton = hv) is
equal to the difference in energy between the atomrsquos initial state and
itrsquos final state Because different atoms have different energy levels
different atoms give off different frequencies (colors) of light
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Bohr Model of the Hydrogen Atom
Niels Bohr scientist extraordinaire solved the puzzle of why different atoms give off different color spectra He linked the
atomrsquos electrons to photon (color spectra) emission According to his new model electrons can only circle the nucleus in allowed
paths or orbits Notice this
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Bohr Model of the Hydrogen Atom (contrsquod)When energy is added to an atom the electrons move up energy level(s)
Conversely when energy is given off by an atom (in the form of a photon)
the electrons move down one or more energy levels
The principal quantum number is
denoted with the letter n and it
indicates the main energy level
occupied by the electron As n
increases the electronrsquos energy and
itrsquos average distance from the nucleus
increases
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Plotting the Electron ldquoOrbitrdquoIt would be inaccurate to say that the electrons orbit the nucleus in
the same way the planets orbit the sun ie in a fixed and set path The Heisenberg Uncertainty Principle states that you can know the position and velocity of an electrons at any given point but
never both at the same time So if you were to plot the position of an electron many many times you would begin to build a picture
of where it occupies space 90 of the time This is called an orbital
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Plotting the Electron ldquoOrbitrdquoOrbital the probable location of an electron around the nucleus
As n increases the number of different types of orbitals increases as well At n = 1 there is one type of orbital at n = 2 there are two types of orbitals and so on The number of orbitals at any given energy level is equal to the principal quantum number (n) These
are known as sublevels
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Types of Orbitals1 s-orbitals s-orbitals are spherical in shape representing a hollow
ball where you can find the electron 95 of the time They are
labeled 1-s 2-s and so on to denote how close they are to the
nucleus
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Types of Orbitals (contrsquod)2 p-orbitals At the 1st energy level the only orbital available to the
electrons is the s-orbital But at the 2nd energy level- after the 2-s
orbital- there is the 2-p orbital The p-orbitals are dumbbell shaped
to represent where the electron can be found 95 of the time
Notice that near the nucleus the area where they are usually found
is very narrow
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Types of Orbitals (contrsquod)2 p-orbitals (contrsquod) unlike s-orbitals p-orbitals point in a particular
direction At any one energy level it is possible to have three
absolutely equivalent p orbitals pointing mutually at right angles to
each other These are arbitrarily given the symbols px py and pz
This is simply for convenience - what you might think of as the x
y or z direction changes constantly as the atom tumbles in space
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Types of Orbitals (contrsquod)3 d-orbitals after the s and p orbitals there is another set of orbitals
which becomes available for electrons to inhabit at higher energy
levels At the third level there is a set of five d orbitals (with more
complex shapes names) as well as the 3s and 3p orbitals (3px 3py
3pz) At the third level there are a total of nine orbitals altogether
3dxy 3dxz 3dyz
3dx2
-y2 3dz
2
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
N
ldquoRungs of a ladderrdquo
Energy of e- increases as you travel further away from the nucleus
e- can jump from energy levels when they gainlose energy
Quantum = amount of energy reqrsquod to move an e- from its present energy level to the next highest ldquoquantum leaprdquo
Unlike a ladder levels are not evenly spaced closer further away thus easier to move bt or leave
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
The Quantum Mechanical Model (QMM)
bull This is the most modern description of e- in an atom it is purely mathematical and describes the _____ and _____ of an e-
bull All previous models differed bc they were _______
bull This model doesnrsquot define an exact path of an e- rather the QMM does what
ldquoChancerdquo
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull QMM = probability of finding an e- within a certain volume surrounding the nucleus represented by an electron cloud
The gt probability of finding an e- is within these areas surrounding the nucleus (represent where the e- is 90 of the time)
N
The ldquofatterrdquo the area of the e- cloud the greater the chance of finding an e- and vice versa
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Atomic Orbitals
bull Designate energy levels that e- are in by using principal quantum numbers (n)
bull n is ordered from lowest highest energy level (1234hellip) thus the higher the principal quantum the further the e- is from the nucleus
bull ie) an e- in the 3rd principal energy level has more ___ and is further from the ___ than an e- in the 2nd principal energy level
n =1
n = 2
n = 3
n = 4
uarr en
erg
y uarr
dis
tan
ce fr
om
nucl
eus
darr s
pac
ing
N
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull Within each energy level
there are sublevels the of sublevels equals the principal energy level (n)
bull The sublevels are also arranged from lowest to highest energy
bull These sublevels have orbitals within them each orbital can hold a max of 2 e-
Principal energy level (n)
of sublevels in that level
n = 1 1 sublevel
n = 2 2 sublevels
n = 3 3 sublevels
Sublevels (lowest highest energy)
of orbitals within each sublevel
1st = s 1 orbital
2nd = p 3 orbitals
3rd = d 5 orbitals
4th = f 7 orbitals
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Do Now
1 Discuss points you have learned about the PT
a What does it tell us
b How can we use it to talk about an element and its characteristics
c How and why do we use the Aufbau Diagram
Homework
1 Finish electron configuration sheet QUIZ
2 Bring all lab materials tomorrowhellip
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Basicallyhellip
Principal energy level (n) Energy sublevels Orbitals in sublevels
n = 1 2 3 4hellip s p d f ghellip s =1 p = 3 d = 5 f = 7
(2 e- 6 e- 10 e- 14 e-)
QMM describes an e- position within an e- probability cloud e- donrsquot travel in fixed circular paths therefore we cannot call them orbits Rather we call them atomic orbitals (s p d f ghellip) SHAPES OF ATOMIC ORBITALS DICTATE PROBABILITY
s orbital
p orbital (x 3)d orbital (perpendicular orbital coming at you x 5)
Fig 134 5 in book
Low to High
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Another representation of the atomic orbitalshellip
Cloudsrdquobubblesrdquo indicate where yoursquoll find e- most of the time
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull Notice w p and d orbitals the regions close to the nucleus where probability of finding an e- is very narrow = node
bull Again the and types of atomic orbitals depends on what
bull Example lowest principle energy level is n = 1 it has 1 atomic orbital called 1s
Does the probability of finding an e- vary with direction in 1s Does the same hold true for p and d orbitals
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull The 2nd energy level (n = 2) has 2 sublevels s and p
N PP
P
P
P
Coming you
Going away from you
3) Spaces represent what
P
S2) How many total orbitals are there What are the max of e- that can be held in n= 2
1) P orbitals stick out further therefore they have gt ____
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull The 3rd principal energy level (n = 3) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull The 4th principal energy level (n = 4) has how many orbitals Can you name them What is the max of e- this energy level can hold
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull As mentioned the principal quantum always
equals the of sublevels in that energy levelbull The max of e- that can occupy a principal
energy level is given by the formulahellip
2n2
What is the max of e- in the 6th principal energy level Sublevels
Still confused Review p 366 for max e- per energy level
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Homework
bull Electron configuration worksheet (work on wkst)
bull Have homework out to go overhellipbull Do Now1 What is the Aufbau Diagram How do
you create it What does it tell about filling orbitals (use book to help you out)
2 What is the total of e- in n = 9 n = 53 What does the quantum tell you
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Electron Configurations
bull Natural phenomena to work towards stability ndash lowest possible energy
WHY
High energy systems are very unstable
Atom works to attain the most stable e- configuration possible
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull There are 3 rules that help you to determine this
1 Aufbau Principle
2 Pauli Exclusion Principle
3 Hundrsquos Rule
1 s 2 s 2 p
Long form vs Short form
Electron ConfigurationsAufbau Diagrams
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
1) Aufbau principle Electrons enter orbitals of lowest energy first The various sublevels of a principle energy level are always of equal energy Furthermore within a principle energy level the s sublevel is always the lowest-energy sublevel Each box represents an atomic orbital
Aufbau Diagram
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
2) Pauli exclusion principle An atomic orbital may describe at most two electrons For example either one or two electrons may occupy an s orbital or p orbital A vertical arrow represents an electron and its direction of spin (uarr or darr) An orbital containing paired electrons is written as uarrdarr
3) Hundrsquos Rule When electrons occupy orbitals of equal energy one electron enters each orbital until all the orbitals contain one electron with parallel spins For example three electrons would occupy three orbitals of equal energy as follows uarr uarr uarr Second electrons then add to each orbital so their spins are paired with the first electrons
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Some practice
____
5s ___ ___ ___
4p
___ ___ ___
4d
___ ___
Element
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Electron Configuration
This is the order which electrons will fill their energy levels
You MUST learn this
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Electron Configuration (contrsquod)
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Noble Gas ConfigurationsA much easier way to write electron configurations abbreviates all the orbital notation This is an acceptable way to write electron configurations on quizzes or
tests
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Show the electron configuration of the following elements
1) Fe 1s22s22p63s23p64s23d6
2) Ga 1s22s22p63s23p64s23d104p1
3) Ar 1s22s22p63s23p6
4) Sr 1s22s22p63s23p64s23d104p65s2
5) Mg 1s22s22p63s2
6) Ru 1s22s22p63s23p64s23d104p65s24d6
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Homework
bull Have worksheets out to quickly review questions (131 and 2)
bull Complete 133 12 4 6 (on loose-leaf neatly showing equations used all work and cancellations in a vertical fashion) will go over next session use p 375 example to help
bull Do Now1 Starting form n = 1 (to n = 4) list the order that
electrons would fill sublevelshellip2 Quickly list and discuss all three rules for e-
configuration discussed previouslyhellip
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Take Quiz ndash 7 minutes
Do Now1 What is the difference between an atom and its
ion2 What is a node3 Why is it unnatural for systemsatoms to be at
high energy How do atoms fix this problem
Homework ndash Complete chapter 13 worksheet (1st page front and back on the worksheet)
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Physics and the QMM
bull QMM developed through study of light
bull Through its study found light was energy that contained _____ and moved by ____
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
bull According to the ldquowave modelrdquo light consists of electromagnetic waves
bull Includeshellip
All waves travel in a vacuum at
30 x 10^10 cms (or 30 x 10^8
ms) =
Irsquom smarter
than he is Howrsquod he measure
that
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Anatomy of a Wavelength
origin
amplitude
Λ = ldquolambdardquo
Frequency (ν) = ldquonurdquo
= of wave cycles that that pass through a point in a given time
= Hertz (Hz) or s^-1
Wavelength and frequency are inversely related Which leads us tohellip
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Take 3 minutes only for quiz ndash hand in when finished
Do Now1 Give the basic anatomy of a wavelength2 What do we broad term describes all forms of light
Which portion makes up the smallest portion of this ldquospectrumrdquo
3 How are wavelength and frequency related Do they relate to anything else
4 Have essays and homework questions readyHomework1 Massive quiz on Monday (in lab) on all ch 132 Remember to bring notebooks to class3 Tuesday ndash Print out a PT and after reading chapter 14
create a ldquomaprdquo of how to interpret the periodic trends
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
ν ldquotimesrdquo λ = speed of light
bull Every time
bull Light bends through prisms to create thehellip
Electromagnetic Spectrum = relative size
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Every element bends light in a specific wayhellip
Open book and complete sample 132 and practice problem 11
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379
Another idea that came about through the study of lighthellip
bull The color change associated with the heatingcooling of an object occurs through the +- of energy units = ldquobricks of a wallrdquo
bull Large energy change = emissionabs of high frequency radiation and vice versahellip thus frequency and Planckrsquos constant areE (ldquoradiant energyrdquo)= frequency x Planckrsquos
constant bull E = bull Problem 13 on page 379