Chapter 3 – Atoms and the Periodic Table
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Transcript of Chapter 3 – Atoms and the Periodic Table
Chapter 3 – Atoms and the Periodic Table
3.1 Atomic Structure
AtomsDerived from the Greek word meaning “unable to divide”.
They are the building blocks of molecules.
Every element is made of tiny, unique particles that cannot be subdivided.
Atoms of the same element are exactly the same.
Atoms of different elements can join to form molecules.
Atoms are made of protons, neutrons,
and electrons.
NucleusThe center of an atom; made up of
protons and neutrons.
ProtonA positively charged subatomic particle in
the nucleus of the atom
NeutronA neutral subatomic
particle in the nucleus of an atom.
Electron A tiny negatively charged subatomic
particle moving around outside of an
atom.
Atoms have no overall charge.
Even though atoms have charged protons and electrons. They have an equal number of each. So, they cancel each other out.
Bohr’s ModelIn 1913, Neils Bohr suggested that electrons moves about a set path about the nucleus.
The path defines the electron’s energy level.
Energy LevelAny of the possible
energies of an electron may have
in an atom.
Modern theory states that electrons behave
more like waves.In 1925, Bohr proposed a
new model, that the electrons do not follow a set path.
Although we cannot know how the electron travels around the nucleus we can know where it spends the
majority of its time (thus, we can know position but not trajectory).
The “probability” of finding an electron around a nucleus can be calculated.Relative probability is indicated by a
series of dots, indicating the “electron cloud”.
Electrons are found in
orbitals within energy levels.
OrbitalA region in an atom where there is a high probability of finding electrons.
Electrons may occupy four
different orbitals.
s - orbital- Simplest orbital.- Can only have one orientation in space, because its shaped like a sphere.
- Its shape enables it to surround the nucleus.
- 90% electron probability/cloud for 1s orbital (notice higher probability toward the center)
- It can hold a maximum of 2 electrons.
p - orbital-it is a dumbbell-shaped and can be oriented in 3 different ways in space. (3-Dimensions)
d - orbital-a more complex orbital.
-There are a possible of 5 orientations.
-All orbitals are very different in shape, each can contain a maximum 2 electrons.
-Can contains a total of 10 electrons in all.
Four of the d orbital’s resemble two dumbbells in a clover shape. The last d orbital resembles a p orbital with a donut wrapped around the middle.
f - orbital-a more complex orbital.
-There are a possible of 7 orbitals.
-All orbitals are very different in shape, each can contain a maximum 2 electrons.
-Can contains a total of 14 electrons in all.
Electrons usually occupy the lowest
energy levels available.
And within each energy level,
electrons occupy orbitals with the lowest energy.
An s orbital has the lowest energy.
A p orbital has slightly more energy, followed by a d orbital.
An f orbital has the greatest energy.
Every atom has one or more
valence electron.
Valence ElectronAn electron in the outermost energy level of an atom.
3.2 A Guided Tour of the
Periodic Table.
Periodic LawProperties of elements tend
to change in a regular pattern when elements are arranged in order of increasing atomic number, or number of protons in their atoms.
PeriodA horizontal row
elements in the periodic table.
As you move across a row the # of protons
increases by 1. As does the # of electrons.
Elements in the same group have similar properties.
Group(family) – a vertical column of elements in the periodic table
Elements in the same group have
the same # of valence
electrons.
These elements are not exactly alike,
they have a different # of protons and
electrons.
Some atoms form ions
Some atoms may under go
ionization.
IonizationThe process of adding electrons to or removing electrons from an atom or groups of atoms.
These are valence electrons.
IonsAn atom or a group of atoms that has lost or gained 1 or more electrons and therefore has a net charge.
CationAn ion with a positive charge
Example: Lithium atomLithium is so reactive, it reacts with air. It has 1 electron in the outer level of the s orbital. This one electron makes very reactive.
Removing this electron forms a positive ion (Li+)
Li+ is less reactive, because now its outer energy level is full.
AnionAn ion with a
negative charge.
Example: Fluorine atom
Fluorine is also very reactive; however it gains an electron to become less reactive.
It has 7 valence electrons and needs only 1 to complete its outer energy level.
Therefore, easily gaining 1 electron & becoming a negative ion (F-).
Atomic Structure of Atoms
All atoms have different structure and different properties; therefore, different structure.
Atomic Number (Z)
The number of protons in the
nucleus of an atom.
Examples:Helium (He) has 2 protonsZ = 2
Cesium (Cs) has 55 protonsZ = 55
Mass Number (A)Mass number equals the # of protons and neutrons in the nucleus in the atom.
Ex: Fluorine (F) has 9 protons and 10 neutrons, A = 19 for fluorine.
Although atoms of the same element always
have the same Atomic number, they can have a different
mass numbers.
IsotopesAny atoms have the same # of protons, but a different # of
neutrons.
Ex: Hydrogen has 3 isotopes.
1. Protium – has 1 proton in its nucleus. (A = 1) Most common form
2. Deuterium – has 1 proton and 1 neutron in its nucleus, call heavy hydrogen. (A = 2)
3. Tritium – has 1 proton and 2 neutrons in its nucleus. (A = 3)
Atomic numbers (Z) and mass numbers (A) maybe included with the chemical symbol.
XAZ
U23592
Atomic Number
Mass Number
Calculating the # of neutrons in an atom.
If you know the Atomic number and the Mass number, all you have to do is subtract.
# of Neutrons =
mass # – atomic #
(# of Neutrons = A – Z )
Ex: For our Uranium - 235
# of Neutrons = A – Z# of Neutrons = 235 – 92
# of Neutrons = 143
The mass of an atom.
The mass of a single atom is very small. A single Fluorine atom is one trillionth of one billionth of a gram.
Because it is very hard to work with atomic
mass are expressed in atomic mass units
(amu).
atomic mass unit (amu)
A quantity equal to 1/12 of the mass of a Carbon-12 atom.
average atomic mass
The weighted average of the masses of all naturally occurring isotopes of an element.
EX: If we look back at Hydrogen.
There are 3 isotopes. The average atomic mass 1.00794 amu. This means there are more isotopes of Hydrogen-1, than Hydrogen-2 or Hydrogen-3.
3.3 Families of Elements
Elements are either classified as Metals
or Nonmetals.
MetalsThe elements that are good conductors for heat and electricity.
Most elements are metals.
Usually solids and shiny.
NonmetalsThe elements that
are usually poor conductors of heat
and electricity.
Nonmetals, except Hydrogen, are found on the right side of the periodic table.
Can be solids, liquids, or gases.
Solids are dull and brittle.
There are some nonmetals that can
conduct under certain
circumstances.
SemiconductorsThe intermediate conductors of heat and electricity.
Sometimes called metalloids.
Metals can be classified even further into 4
different groups.
Alkali MetalsHighly reactive metallic elements located in Group 1 of the periodic table.
•Has 1 valence electron.
•Can be easily removed to form a +1 ion.
•Highly reactive.
Look on your Periodic table.
Lithium SodiumPotassium RubidiumCesium Francium
Since they are so reactive, these elements are not found in nature. They combine with other elements to form
compounds.
Alkaline Earth Metals
The reactive metallic elements located in
Group 2 of the Periodic Table.
•They have 2 valence electrons.
•They are less reactive than alkali metals.
•May form an ion of a +2 charge if both valence electrons are removed.
Look at the Periodic Table
•Beryllium Magnesium
•Calcium Strontium
•Barium Radium
They are combine with other elements to form compounds.
Ex: Calcium Compounds – shells of sea life, coral reefs, limestone, or marble.
Magnesium Compounds – speeds up the
processes of the human body.
Transition MetalsThe metallic
elements located in groups 3 – 12 of the
periodic table.
•Much less reactive than Alkali or Alkaline Metals.
•Can lose electrons to form + ions.
•Some metals can lose up to 4 electrons.
All Metals are good heat and electrical
conductors.
They can be stretched and shaped without breaking.
Mercury is the only metal that is a liquid at room temperature.
Technetium and Promethium are
synthetic elements.
•Man made elements that are radioactive.
•Technetium is used to help diagnose cancer and other medical problems.
•Promethium is used in ‘glow in the dark’ paint.
•Elements with atomic # greater than 92 are man made as well.
Nonmetals•Found on the right side of the periodic table.
•Some elements in groups13-16 and all in groups 17 & 18.
•May gain electrons to form – ions
•Carbon combines with other elements to form millions of carbon containing compounds.
•Carbon compounds are found in both living and nonliving things.
Nonmetals and there compounds are plentiful on
Earth.
HalogensThe highly reactive elements located in Group 17 of the periodic table.
•The valence shell is almost full; therefore, these elements easily accept an electron.
•Creating a (-) ion, anion.
•Fluorine•Chlorine•Bromine•Iodine•Astatine
Noble Gases•The unreactive gases located in Group 18 of the Periodic Table.
•These elements exist only as single atoms, instead of molecules.
•All gases are inert, non-reactive.
•Outer level is full of electrons.
•They don’t form with other elemental atoms to form atoms.
Helium Neon
Argon Krypton
Xenon Radon
Semiconductors•Elements classified as nonmetals, each one has some properties of metals.
•Known as ‘metalloids’
•They are able to conduct heat & electricity.
•Silicon most familiar, used for computers and other electronic devices.
•Boron Silicon•Germanium•Arsenic•Antimony•Tellurium
3.4 Using Moles to
Count Atoms.
Counting Things•One of the first things we do as child.
•When we count large #’s of small things, we use counting units.
The mole is useful for counting small
particles.
MoleThe SI base unit that describes the amount
of a substance.
A mole is a collection of a very large
number of particles.
602,213,670,000,000,000,000,000
Avogadro’s Constant
•The # of particles in 1 mol; equals 6.022 x 1023 /mol.
Molar MassThe mass in
grams of 1 mol of a substance.
Ex: 1 mole of Titanium-22 atoms has a molar mass of
47.87 g
•Think of it as 47.87 grams per mole of Titanium.
•47.87 g/mol
Molar mass of an element in grams
is the same as average atomic mass in amu.
Find the molar mass for the following elements:1.Gold2.Einsteinium3.Gallium4.Cesium
Find the molar mass for the following elements:1.Gold 196.97 g2.Einsteinium 252.08 g3.Gallium 69.72 g4.Cesium 132.91 g
Conversion FactorsA ratio equal to one
that expresses the same quantity in
two ways.
Can be anything:1 ream of = 500 sheets paper of paper
1 inch = 2.54 cm10 km = 6.2 miles
Converting Amount (mol) to
Mass (g)
•1st establish the amount of matter in moles from the problem.
•2nd look up the element of the period table and find its molar mass in g for conversion factor
Conversion factor will be:
Atomic mass(g)=1 mole or
1 mole=Atomic mass(g)
Set up for factor label method.
Given info
Set up for factor label method.
Given atomic mass of info element
Set up for factor label method.
Given atomic mass of info element
1mole of element
Ex: How many grams in 23 moles of Silver?
23 mol of Ag
Conversion Factor 1 mol of Ag
= 107.8682 g of Ag
Ex: How many grams in 23 moles of Silver?
23 mol 107.8682 g of Ag of Ag
Ex: How many grams in 23 moles of Silver?
23 mol 107.8682 g of Ag of Ag
1 mol of Ag
2480.96 g of Ag- Multiply #’s above the horizontal line
- Units of moles of Ag will cancel leaving just grams of Ag.
Ex: How many grams in 2.8 moles of Radon?
2.8 mol of Rn
Conversion Factor 1 mol of Rn
= 222.0176 g of Rn
Ex: How many grams in 2.8 moles of Radon?
2.8 mol 222.0176 g of Rn of Rn
Ex: How many grams in 2.8 moles of Radon?
2.8 mol 222.0176 g of Rn of Rn
1 mol of Rn
621.64928 g of Rn
Converting Mass (g) to Amount (mol) Set up is the same
except we switch/flip the conversion factor
ratio.
Ex: Convert 729 g of Th to moles.
729 g of Th
Conversion Factor1 mol of Th
=232.0381 g of Th
Ex: Convert 729 g of Th to moles.
729 g 1 mol of Th of Th
Ex: Convert 729 g of Th to moles.
729 g 1 mol of Th of Th
232.0381 g of Th
3.142 mol of Th
Ex: Convert 50 g of Sr to moles.
50 g of Sr
Conversion Factor1 mole of Sr
= 87.62 g of Sr
Ex: Convert 50 g of Sr to moles.
50 g 1 mol of Sr of Sr
Ex: Convert 50 g of Sr to moles.
50 g 1 mol of Sr of Sr
87.62 g of Sr
0.571 mol of Sr