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Notes – Unit 2 Section B /
Chapter 5Earth’s Mineral
Resources / Electron structure
Earth’s composition
1) Atmosphere: Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide
Earth’s composition
1) Atmosphere: Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide
2) Hydrosphere: Liquid portion composed of water and dissolved minerals and salts.
Earth’s composition
1) Atmosphere: Gaseous part of earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide
2) Hydrosphere: Liquid portion composed of water and dissolved minerals and salts.
Earth’s composition1) Atmosphere: Gaseous part of
earth. Provides nitrogen, oxygen, neon, argon, water vapor, and carbon dioxide
2) Hydrosphere: Liquid portion composed of water and dissolved minerals and salts.
3) Lithosphere: solid part of earth. Greatest variety of chemical resources. Includes petroleum and metal-bearing ores.
Earth’s composition
3) Lithosphere: solid part of earth. Greatest variety of chemical resources. Includes petroleum and metal-bearing ores.
Earth’s composition
3) Lithosphere: solid part of earth. Greatest variety of chemical resources. Includes petroleum and metal-bearing ores.
Ore – Naturally occurring rock or mineral that can be mined
Earth’s composition
3) Lithosphere: Includes petroleum and metal-bearing ores.
Ore – Naturally occurring rock or mineral that can be mined.
Minerals -
Earth’s composition
3) Lithosphere: Includes petroleum and metal-bearing ores.
Ore – Naturally occurring rock or mineral that can be mined.
Minerals – Naturally occurring solid compounds containing elements or groups of elements
Earth’s composition
3) Lithosphere: Includes petroleum and metal-bearing ores.
Ore – Naturally occurring rock or mineral that can be mined.
Minerals – Naturally occurring solid compounds containing elements or groups of elements
Granite – Rock (Ore)
Quartz - mineral
Metals, Nonmetals and reactivity
• Metals are not generally found in their pure state.
• They react and combine with other elements to form ionic and covalent compounds.
• Their reactivity depends on their chemical families and properties
Types of Atomic particles
• Atoms - The building blocks of matter.
• Particles –Electrons (-) e-
Protons (+) p+
Neutrons (no charge) no• Nucleus Protons and neutrons
Atomic Particles
• Sodium =Atomic Mass =
Mass
# = - #(rounded) mass =
p+ =e- =no =
• Chlorine =Atomic Mass =
Mass
# = - #(rounded) mass =
p+ =e- =no =
Atomic Particles
• Sodium = Na Atomic Mass = 22.99
Mass 23
# = 11 - # 11(rounded) mass = 23
p+ = 11e- = 11no = 12
• Chlorine =Atomic Mass =
Mass
# = - #(rounded) mass =
p+ =e- =no =
Atomic Particles
• Sodium = Na Atomic Mass = 22.99
Mass 23
# = 11 - # 11(rounded) mass = 23
p+ = 11+e- = 11-no = 120
• Chlorine = ClAtomic Mass = 35 .453
Mass 35
# = 17 - # 17(rounded) mass = 35
p+ = 17+e- = 17-no = 180
Electrons
Electrons – Negatively charged particles orbiting the nucleusPeriods – Show the number of electron shells or orbitals. Horizontal columns.Families – Vertical columns. Show the number of outside electrons.
Electrons
Electrons – Negatively charged particles orbiting the nucleusPeriods – Show the number of electron shells or orbitals. Horizontal columns.Families – Vertical columns. Show the number of outside electrons.
1
23 4 5 6 7
8
1
2
3
4
5
6
7
Valence electrons
Periods
Electrons
Valence Electrons – The electrons found in the outside energy levelThe number of valence electrons determines many properties of that elementThe number of valence electrons make up families
Valence electrons
Electrons
Valence Electrons – The electrons found in the outside energy levelThe number of valence electrons determines many properties of that elementThe number of valence electrons make up families
Valence electrons
Honors ChemChapter 5
Electrons in Atoms
Atomic models• Dalton – 1st Atom – no internal
structures
• Thomson – Plum pudding, electrons in sphere of positive
• Rutherford - small dense positive nucleus with electrons around nucleus
• Bohr – electrons in circular orbitals with fixed distances from nucleus. Lowest energy inside highest energy furthest from nucleus
Atomic models
• Schrodinger – mathematical equation for location. Electron cloud model
• Quantum Mechanical model – modern description from Schrodinger’s mathematical equations
Atomic models
• Schrodinger – mathematical equation for location. Electron cloud model
• Quantum Mechanical model – modern description from Schrodinger’s mathematical equations
Electron configuration
• Quantum – the amount of energy required to move an electron from its present energy level to the next higher one
• Energy levels – region in space around nucleus where an electron is likely moving
Electron configuration• Quantum – the amount of
energy required to move an electron from its present energy level to the next higher one
• Energy levels – region in space around nucleus where an electron is likely moving
• Energy levels are labeled by principle quantum numbers (n).
• n = 1,2,3,4, etc
Electron configuration
Electron configuration• Quantum – the amount of
energy required to move an electron from its present energy level to the next higher one
• Energy levels – region in space around nucleus where an electron is likely moving
• Energy levels are labeled by principle quantum numbers (n).
• n = 1,2,3,4, etc• The higher the energy level
occupied by an electron, the more energetic it is
Electron configuration
• Energy levels are labeled by principle quantum numbers (n).
• n = 1,2,3,4, etc• The quantum # equals the
number of sublevels for each principle energy level
• The formula 2n2 equals the maximum number of electrons allowed in a principle energy level
• Shell n 2n2
• K 1 2(1)2=• L 2 2(2)2=• M 3 2(3)2=• N 4 2(4)2=
Energy levels
• Energy levels are labeled by principle quantum numbers (n).
• n = 1,2,3,4, etc• The quantum # equals the
number of sublevels for each principle energy level
• The formula 2n2 equals the maximum number of electrons allowed in a principle energy level
• Shell n 2n2
• K 1 2(1)2=• L 2 2(2)2=• M 3 2(3)2=• N 4 2(4)2=
Electrons
• Electrons are found in orbitals or shells
• The electrons with the highest energy are on the outside shell.
• The electrons with the lowest energy are on the inside
Electrons
• Each shell can only hold a certain amount of electrons
• The electrons with the highest energy are on the outside shell.
• The electrons with the lowest energy are on the inside
# of electrons in orbitals
ShellK
LMN
n 2n2
1234
# of electrons in orbitals
ShellK
LMN
n 2n2
1 2234
# of electrons in orbitals
ShellK
LMN
n 2n2
1 22 834
# of electrons in orbitals
ShellK
LMN
n 2n2
1 22 83 184
# of electrons in orbitals
ShellK
LMN
n 2n2
1 22 83 184 32
# of electrons in orbitals
ShellK
LMN
n 2n2
1 22 83 18 (8)4 32 (8)
Electron shells
• Electrons fill from the inside out
• The first shell has 2, the second shell has 8, the third shell has 18(8)
• Octet rule – The maximum number of electrons in the outside shell is 8. The exception is shell # 1 with 2.
Electron shells
• The atomic number of an element tells the number of protons and electrons
• Electrons are drawn in shells in pairs from inside out.
• The outside are valence electrons
Valence electrons
1
23 4 5 6 7
8
Electron shells
• The atomic number of an element tells the number of protons and electrons
• Electrons are drawn in shells in pairs from inside out.
• The outside are valence electrons
N
Atomic # = 7 1st = 2Period = 2 2nd = 8
3rd = 8
Electron shells
• The atomic number of an element tells the number of protons and electrons
• Electrons are drawn in shells in pairs from inside out.
• The outside are valence electrons
S
Atomic # = 16 1st = 2Period = 3 2nd = 8
3rd = 8
1
23 4 5 6 7
8
Electron dot diagram
• Shows each element with its valence electrons only
• Outside electrons are placed in pairs
• Dots show outside electrons
S
Electron dot diagram
• Shows each element with its valence electrons only
• Outside electrons are placed in pairs
• Dots show outside electrons
• Elements will lose or gain e- to become stable and reach the octet (8 or 0)
Electron dot diagram• Shows each element with its valence
electrons only• Outside electrons are placed in pairs• Dots show outside electrons
• Elements will lose or gain e- to become stable and reach the octet (8 or 0)
Elements that lose e- become positive , those that gain e-
become negative
Li =
C =
O =
1
23 4 5 6 7
8
Electron dot diagram• Shows each element with its valence
electrons only• Outside electrons are placed in pairs• Dots show outside electrons• Elements will lose or gain e- to become
stable and reach the octet (8 or 0)
Elements that lose e- become positive charged , those that
gain e- become negative charged
• Dots are placed R-L-T-B and then repeat pattern in pairs
Al =
N =
Cl =
Ar =
Electron dot diagram• Shows each element with its valence
electrons only• Outside electrons are placed in pairs• Dots show outside electrons• Elements will lose or gain e- to become
stable and reach the octet (8 or 0)
Elements that lose e- become positive charged , those that
gain e- become negative charged
• Dots are placed R-L-T-B and then repeat pattern in pairs
Al = lose/gain _____ charge = ___
N = lose/gain _____ charge = ___
Cl = lose/gain _____ charge = ___
Ar = lose/gain _____ charge = ___
Electron dot diagram
• Shows each element with its valence electrons only
• Outside electrons are placed in pairs
• Dots show outside electrons
S
Electrons and Periodic Table
• Valence electrons in atoms show reactivity
• Atoms will lose or gain electrons to reach the octet (8) rule level.
• Inert (Noble) Gases have 8 valence electrons (2 for He) and are stable
Electrons and Periodic Table
• Inert (Noble) Gases have 8 valence electrons (2 for He) and are stable
• Nonmetals –Groups 5a to 7a will gain electrons to become stable
• Metals – Groups 1a to 3a will lose electrons to become stable
Electrons and Periodic Table
• Inert (Noble) Gases have 8 valence electrons (2 for He) and are stable
• Nonmetals –Groups 5a to 7a will gain electrons to become stable
• Metals – Groups 1a to 3a will lose electrons to become stable
Orbitals
• Atomic orbitals – regions around the nucleus within which the electrons have the highest probability of being found
• Orbitals are sublevels which correspond to different shapes.
• s are spherical, p are dumbell shaped, etc
• Sublevel orbitals can contain differing numbers of orbitals.
• s = 1 orbital• p = 3 orbitals• d = 5 orbitals• f = 7 orbitals
Electron Arrangements in Atoms
Electron configuration – The ways in which electrons are arranged around the nuclei of atoms3 Rules:•1) Aufbau principle – electrons enter orbitals of the lowest energy first•2) Pauli exclusion principle
Electron Arrangements in Atoms
Electron configuration – The ways in which electrons are arranged around the nuclei of atoms3 Rules:•1) Aufbau principle – electrons enter orbitals of the lowest energy first•2) Pauli exclusion principle
Electron Arrangements in Atoms3 Rules:•2) Pauli exclusion principle – atomic orbitals can hold no more than two electrons•3) Hund’s rule – When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins.
Calculating Electron Configurations
• The shorthand method for writing electron configurations of an atom involves writing the energy level and symbol for every sublevel occupied by an electron and indicating the number of electrons in each sublevel with a subscript
Calculating Electron Configurations
• The shorthand method for writing electron configurations of an atom involves writing the energy level and symbol for every sublevel occupied by an electron and indicating the number of electrons in each sublevel with a subscript.
Calculating Electron Configurations• The shorthand method for
writing electron configurations of an atom involves writing the energy level and symbol for every sublevel occupied by an electron and indicating the number of electrons in each sublevel with a subscript.
• Nitrogen – Atomic # 7• Shorthand = 1s22s22p3
• Write the electron configuration for Phosphorus,
• atomic # 15
Calculating Electron Configurations
Write the electron configuration for Phosphorus, atomic # 1515 e-
Calculating Electron Configurations
Write the electron configuration for Phosphorus, atomic # 1515 e-
Calculating Electron ConfigurationsConfiguration = 1s22s22p63s23p3 = 15 electrons
• Write the electron configuration for Carbon, Argon, and Nickel
Calculating Electron Configurations
• Write the electron configuration for Carbon (6), Argon (18), and Nickel(28)
Calculating Electron Configurations
Write the electron configuration for Carbon, atomic # 66e-
Calculating Electron Configurations
Write the electron configuration for Argon, atomic # 1818e-
Calculating Electron Configurations
Write the electron configuration for Nickel, atomic # 2828e-
Calculating Electron Configurations
Physics and the Quantum Mechanical Model
• Quantum mechanical model grew out of the study of Light
• Light consists of waves and particles
• Wave principles:• Amplitude = wave
height• Wavelength ( ) =
distance between crests
Physics and the Quantum Mechanical Model
• Quantum mechanical model grew out of the study of Light
• Light consists of waves and particles
• Wave principles:• Amplitude = wave
height• Wavelength ( ) =
distance between crests
Physics and the Quantum Mechanical Model
• Wave principles:• Amplitude = wave height• Wavelength ( ) = distance
between crests• Frequency ( ) = wave
cycles past a given point per unit time– Cycles/second = hertz (Hz) s-1
• Speed of light constant
Physics and the Quantum Mechanical Model
• Wave principles:• Amplitude = wave height• Wavelength ( ) = distance
between crests
• Frequency ( ) = wave cycles past a given point per unit time– Cycles/second =
hertz (Hz) s-1
• Speed of light constant
Physics and the Quantum Mechanical Model
• Frequency ( ) = wave cycles past a given point per unit time– Cycles/second = hertz
(Hz) s-1
• Speed of light constant
Physics and the Quantum Mechanical Model
• Speed of light constant
C = 2.988 x 108 meters/second• (186,000 miles/second)
Physics and the Quantum Mechanical Model
• Speed of light constant
C = 2.988 x 108 meters/second• (186,000 miles/second)• Wavelength and frequency are
inversely proportional
– High = Low– Low = High
• All electromagnetic waves travel at same speed = 3.0 x 108 m/s
Physics and the Quantum Mechanical Model
• Wavelength and frequency are inversely proportional
– High = Low– Low = High
• All electromagnetic waves travel at same speed = 3.0 x 108 m/s
• Light = Quanta of energy calledPhotons
• Atomic Spectra – When atoms absorb energy, electrons move into higher energy levels. These electrons than lose energy by emitting light.
High
High Low
Low
Physics and the Quantum Mechanical Model
• Wavelength and frequency are inversely proportional
– High = Low– Low = High
• All electromagnetic waves travel at same speed = 3.0 x 108 m/s
• Light = Quanta of energy calledPhotons
• Atomic Spectra – When atoms absorb energy, electrons move into higher energy levels. These electrons than lose energy by emitting light.
Physics and the Quantum Mechanical Model
• Wavelength and frequency are inversely proportional
– High = Low– Low = High
• All electromagnetic waves travel at same speed = 3.0 x 108 m/s
• Light = Quanta of energy calledPhotons
• Atomic Spectra – When atoms absorb energy, electrons move into higher energy levels. These electrons than lose energy by emitting light.
Physics and the Quantum Mechanical Model
• Wavelength and frequency are inversely proportional
– High = Low– Low = High
• All electromagnetic waves travel at same speed = 3.0 x 108 m/s
• Light = Quanta of energy calledPhotons
• Atomic Spectra – When atoms absorb energy, electrons move into higher energy levels. These electrons than lose energy by emitting light.
Physics and the Quantum Mechanical Model
• Wavelength and frequency are inversely proportional
– High = Low– Low = High
• All electromagnetic waves travel at same speed = 3.0 x 108 m/s
• Light = Quanta of energy calledPhotons
• Atomic Spectra – When atoms absorb energy, electrons move into higher energy levels. These electrons than lose energy by emitting light.
Chemical Bonds – Chemical forces which hold atoms together and form complete
electrons shellsIon – is an atom or group of
atoms that have an electric charge.Atoms become charged when they lose or gain electrons to become stableAtoms which lose electrons become positive (+) Atoms which gain electrons become negative (-)
Chemical Bonds – Chemical forces which hold atoms together and form complete
electrons shells• Ionic Bond – Positive (+) and
negative (-) ions attract – formed by the transfer of valence electrons.Na 11p+ 11p+
11e- 10e- = +1 Na
Cl 17p+ 17p+17e- 18e- = -1 Cl
Na +1 + Cl-1 = NaCl o