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Electrons in Electrons in AtomsAtoms
Chap. 5Chap. 5Chap. 5Chap. 5
I.I. Light (electromagnetic Light (electromagnetic radiation)radiation)
I.I. Light (electromagnetic Light (electromagnetic radiation)radiation)A. Two componentsA. Two components
I.I. Light (electromagnetic Light (electromagnetic radiation)radiation)A. Two componentsA. Two components
1.1. Electrical waveElectrical wave
I.I. Light (electromagnetic Light (electromagnetic radiation)radiation)A. Two componentsA. Two components
1.1. Electrical waveElectrical wave2.2. Magnetic waveMagnetic wave
I.I. Light (electromagnetic Light (electromagnetic radiation)radiation)A. Two componentsA. Two components
B. Two naturesB. Two natures
I.I. Light (electromagnetic Light (electromagnetic radiation)radiation)A. Two componentsA. Two components
B. Two naturesB. Two natures1.1. ParticleParticle
I.I. Light (electromagnetic Light (electromagnetic radiation)radiation)A. Two componentsA. Two components
B. Two naturesB. Two natures1.1. ParticleParticle2.2. WaveWave
I.I. LightLightC.C. Characteristics of a Characteristics of a
Light WaveLight Wave
1.1. wavelengthwavelength
I.I. LightLightC.C. Characteristics of a Characteristics of a
Light WaveLight Wave
1.1. wavelengthwavelength
The distance between successive wave crestsThe distance between successive wave crests
I.I. LightLightC.C. Characteristics of a Characteristics of a
Light WaveLight Wave
1.1. wavelengthwavelength2.2. frequencyfrequency
The time it takes a wave to pass a given pointThe time it takes a wave to pass a given point
I.I. LightLightC.C. Characteristics of a Characteristics of a
Light WaveLight Wave
1.1. wavelengthwavelength2.2. frequencyfrequency3.3. amplitudeamplitude
The height of a waveThe height of a wave
I.I. LightLightC.C. Characteristics of a Characteristics of a
Light WaveLight Wave
1.1. wavelengthwavelength2.2. frequencyfrequency3.3. amplitudeamplitude4.4. speedspeed
I.I. LightLightC.C. Characteristics of a Characteristics of a
Light WaveLight Wave
C.C. Characteristics of a Characteristics of a Light WaveLight Wave
D.D. The Wave EquationThe Wave Equation
I.I. LightLight
C.C. Characteristics of a Characteristics of a Light WaveLight Wave
D.D. The Wave EquationThe Wave Equation1.1. inverse relation of inverse relation of
wavelength and frequencywavelength and frequency
I.I. LightLight
C.C. Characteristics of a Characteristics of a Light WaveLight Wave
D.D. The Wave EquationThe Wave Equation1.1. inverse relation of inverse relation of
wavelength and frequencywavelength and frequency
2.2. check the unitscheck the units
I.I. LightLight
The Wave EquationThe Wave Equation
c = λ x υ
Self Check – Ex. 1Self Check – Ex. 1
A light wave has a A light wave has a frequency of 2.6 frequency of 2.6 xx 10 101414 Hz. Hz. What is the wavelength?What is the wavelength?
Self Check – Ex. 2Self Check – Ex. 2
What is the frequency of What is the frequency of light with a wavelength of light with a wavelength of 0.0000072 m?0.0000072 m?
C.C. Characteristics of a Characteristics of a Light WaveLight Wave
D.D. The Wave EquationThe Wave Equation
E.E. Planck’s EquationPlanck’s Equation
I.I. LightLight
Planck’s EquationPlanck’s Equation
EE = = hh xx υυ
hh = 6.63 = 6.63 xx 10 10-34-34 J·s J·s
Self Check – Ex. 3Self Check – Ex. 3
A light photon has 4.2 A light photon has 4.2 xx 10 10-19 -19 J J of energy. What is the of energy. What is the frequency of this light?frequency of this light?
Self Check – Ex. 4Self Check – Ex. 4
How much energy does a How much energy does a photon of orange light have photon of orange light have ((λλ = 630 nm)? = 630 nm)?
101099 nm = 1 m nm = 1 m
C.C. Characteristics of a Characteristics of a Light WaveLight Wave
D.D. The Wave EquationThe Wave Equation
E.E. Planck’s EquationPlanck’s Equation
F.F. The Electromagnetic The Electromagnetic SpectrumSpectrum
I.I. LightLight
Electromagnetic SpectrumElectromagnetic SpectrumLong waves
Short waves
Electromagnetic SpectrumElectromagnetic Spectrum
Radio waves
Long waves
Short waves
Electromagnetic SpectrumElectromagnetic Spectrum
Radio waves
Micro-waves
Long waves
Short waves
Electromagnetic SpectrumElectromagnetic Spectrum
Radio waves
Micro-waves
Long waves
Short waves
Infra-red
Electromagnetic SpectrumElectromagnetic Spectrum
Radio waves
Micro-waves
Long waves
Short waves
Infra-red
Visible
Electromagnetic SpectrumElectromagnetic Spectrum
Radio waves
Micro-waves
Long waves
Short waves
Infra-red
Visible
Ultra-violet
Electromagnetic SpectrumElectromagnetic Spectrum
Radio waves
Micro-waves
Long waves
Short waves
Infra-red
Visible
Ultra-violet
X-rays
Electromagnetic SpectrumElectromagnetic Spectrum
Radio waves
Micro-waves
Long waves
Short waves
Infra-red
Visible
Ultra-violet
X-rays
Gamma rays
II.II. Emission SpectraEmission Spectra
A.A. DefinitionDefinitionII.II. Emission SpectraEmission Spectra
Emission Spectrum:Emission Spectrum:
The various types of light given off when an atom is excited
The various types of light given off when an atom is excited
A.A. DefinitionDefinition
B.B. ExamplesExamples
II.II. Emission SpectraEmission Spectra
400 nm 500 nm 600 nm 700 nm
Hydrogen’s SpectrumHydrogen’s Spectrum
Note – only a few colors are present
400 nm 500 nm 600 nm 700 nm
Mercury’s SpectrumMercury’s Spectrum
400 nm 500 nm 600 nm 700 nm
Neon’s SpectrumNeon’s Spectrum
A.A. DefinitionDefinition
B.B. ExamplesExamples
C.C. Explanation – Bohr’s Explanation – Bohr’s ModelModel
II.II. Emission SpectraEmission Spectra
e-
Bohr’s Model of an AtomBohr’s Model of an Atom
Electrons orbit the nucleus (like planets orbiting the sun)
Bohr’s Model of an AtomBohr’s Model of an Atom
e-
Electrons must be in a specific orbit (never between orbits)
Bohr’s Model of an AtomBohr’s Model of an Atom
e-
n=1
n=2n=3
Electron wants to be in the lowest unoccupied level
Bohr’s Model of an AtomBohr’s Model of an Atom
e-
The energy of the electrons depends on the distance from the nucleus
Bohr’s Model of an AtomBohr’s Model of an Atom
e-low energy
high energy
Light is emitted when electrons fall to lower energy levels
Bohr’s Model of an AtomBohr’s Model of an Atom
e-
Only certain sized falls are permitted.
Bohr’s Model of an AtomBohr’s Model of an Atom
e-
410 nm
434 nm
486 nm 656 nm
Hydrogen’s SpectrumHydrogen’s SpectrumWhat is the energy for each line produced?
Color Wavelength Frequency Energy
Red 6.56x10-7 m
Green 4.86x10-7 m
Blue 4.34x10-7 m
Purple 4.10x10-7 m
410 nm
434 nm
486 nm 656 nm
Hydrogen’s SpectrumHydrogen’s SpectrumWhat is the energy for each line produced?
Color Wavelength Frequency Energy
Red 6.56x10-7 m 4.57x1014 Hz
Green 4.86x10-7 m 6.17x1014 Hz
Blue 4.34x10-7 m 6.91x1014 Hz
Purple 4.10x10-7 m 7.32x1014 Hz
410 nm
434 nm
486 nm 656 nm
Hydrogen’s SpectrumHydrogen’s SpectrumWhat is the energy for each line produced?
Color Wavelength Frequency Energy
Red 6.56x10-7 m 4.57x1014 Hz 3.03x10-19 J
Green 4.86x10-7 m 6.17x1014 Hz 4.09x10-19 J
Blue 4.34x10-7 m 6.91x1014 Hz 4.58x10-19 J
Purple 4.10x10-7 m 7.32x1014 Hz 4.85x10-19 J
III. A new modelIII. A new model
III. A new modelIII. A new model
Electrons’ location cannot be accurately determined
A. Quantum MechanicsA. Quantum Mechanics
1. Orbitals1. Orbitals
III. A new modelIII. A new modelA. Quantum MechanicsA. Quantum Mechanics
OrbitalOrbital
A region of space around the nucleus where an electron is likely to be found.
A region of space around the nucleus where an electron is likely to be found.
Types of Orbitals
1.1. s orbitals orbital
1.1. s orbitals orbital
2.2. p orbitalsp orbitals
Types of Orbitals
1.1. s orbitals orbital
2.2. p orbitalsp orbitals
3.3. d orbitalsd orbitals
Types of Orbitals
1.1. s orbitals orbital
2.2. p orbitalsp orbitals
3.3. d orbitalsd orbitals
4.4. f orbitalsf orbitals
Types of Orbitals
1.1. OrbitalsOrbitals
2.2. SublevelsSublevels
III. A new modelIII. A new modelA. Quantum MechanicsA. Quantum Mechanics
Sub-levelSub-level
A group of orbitals that have the same shape and energy.A group of orbitals that have the same shape and energy.
III. A new modelIII. A new modelA. Quantum MechanicsA. Quantum Mechanics
1.1. OrbitalsOrbitals
2.2. SublevelsSublevelsa.a. A few examplesA few examples
1.1. OrbitalsOrbitals
2.2. SublevelsSublevels
III. A new modelIII. A new modelA. Quantum MechanicsA. Quantum Mechanics
a.a. A few examplesA few examples
b.b. Their electron capacityTheir electron capacity
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds ______ electrons electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds _2__2_ electrons electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds _2__2_ electrons electrons
3.3. A ‘p’ sublevel is made of A ‘p’ sublevel is made of THREETHREE orbitals, so it holds orbitals, so it holds ______ electrons electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds _2__2_ electrons electrons
3.3. A ‘p’ sublevel is made of A ‘p’ sublevel is made of THREETHREE orbitals, so it holds orbitals, so it holds _6__6_ electrons electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds _2__2_ electrons electrons
3.3. A ‘p’ sublevel is made of A ‘p’ sublevel is made of THREETHREE orbitals, so it holds orbitals, so it holds _6__6_ electrons electrons
4.4. A ‘d’ sublevel is made of A ‘d’ sublevel is made of FIVEFIVE orbitals, so it holds orbitals, so it holds ________ electrons electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds _2__2_ electrons electrons
3.3. A ‘p’ sublevel is made of A ‘p’ sublevel is made of THREETHREE orbitals, so it holds orbitals, so it holds _6__6_ electrons electrons
4.4. A ‘d’ sublevel is made of A ‘d’ sublevel is made of FIVEFIVE orbitals, so it holds orbitals, so it holds _10__10_ electrons electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds _2__2_ electrons electrons
3.3. A ‘p’ sublevel is made of A ‘p’ sublevel is made of THREETHREE orbitals, so it holds orbitals, so it holds _6__6_ electrons electrons
4.4. A ‘d’ sublevel is made of A ‘d’ sublevel is made of FIVEFIVE orbitals, so it holds orbitals, so it holds _10__10_ electrons electrons
5.5. An ‘f’ sublevel is made of An ‘f’ sublevel is made of SEVENSEVEN orbitals, so it holds orbitals, so it holds ________ electrons electrons
Sublevels Capacity1.1. Each Each orbitalorbital can hold 2 electrons can hold 2 electrons
2.2. An ‘s’ sublevel is made of An ‘s’ sublevel is made of ONEONE orbital, so it holds orbital, so it holds _2__2_ electrons electrons
3.3. A ‘p’ sublevel is made of A ‘p’ sublevel is made of THREETHREE orbitals, so it holds orbitals, so it holds _6__6_ electrons electrons
4.4. A ‘d’ sublevel is made of A ‘d’ sublevel is made of FIVEFIVE orbitals, so it holds orbitals, so it holds _10__10_ electrons electrons
5.5. An ‘f’ sublevel is made of An ‘f’ sublevel is made of SEVENSEVEN orbitals, so it holds orbitals, so it holds _14__14_ electrons electrons
1.1. OrbitalsOrbitals
2.2. SublevelsSublevels
III. A new modelIII. A new modelA. Quantum MechanicsA. Quantum Mechanics
a.a. A few examplesA few examples
b.b. Their electron capacityTheir electron capacity
c.c. The ordered listThe ordered list
III. A new modelIII. A new modelB. Arrangement of electronsB. Arrangement of electrons
1.1. Aufbau principleAufbau principle
III. A new modelIII. A new modelB. Arrangement of electronsB. Arrangement of electrons
Electrons fill the lowest energy level first.Electrons fill the lowest energy level first.
1.1. Aufbau principleAufbau principle
2.2. Pauli Exclusion PrinciplePauli Exclusion Principle
III. A new modelIII. A new modelB. Arrangement of electronsB. Arrangement of electrons
Two electrons per orbital with opposite spinTwo electrons per orbital with opposite spin
1.1. Aufbau principleAufbau principle
2.2. Pauli Exclusion PrinciplePauli Exclusion Principle
3.3. Hund’s RuleHund’s Rule
III. A new modelIII. A new modelB. Arrangement of electronsB. Arrangement of electrons
Half fill all orbitals in a sublevel before completely filling themHalf fill all orbitals in a sublevel before completely filling them
1.1. Aufbau principleAufbau principle
2.2. Pauli Exclusion PrinciplePauli Exclusion Principle
3.3. Hund’s RuleHund’s Rule
4.4. A pictorial representationA pictorial representation
III. A new modelIII. A new modelB. Arrangement of electronsB. Arrangement of electrons
‘The Aufbau Hotel’‘The Aufbau Hotel’
IV. Orbital DiagramsIV. Orbital Diagrams
A representation of the electrons in an atomA representation of the electrons in an atom
A.A. Boxes represent . . .Boxes represent . . .
IV. Orbital DiagramsIV. Orbital Diagrams
A.A. Boxes represent . . .Boxes represent . . .
IV. Orbital DiagramsIV. Orbital Diagrams
1.1. An ‘An ‘ff’ sublevel should have ’ sublevel should have 77 boxesboxes
A.A. Boxes represent . . .Boxes represent . . .
IV. Orbital DiagramsIV. Orbital Diagrams
1.1. An ‘An ‘ff’ sublevel should have ’ sublevel should have 77 boxesboxes
2.2. ‘‘dd’ = 5 boxes’ = 5 boxes
A.A. Boxes represent . . .Boxes represent . . .
IV. Orbital DiagramsIV. Orbital Diagrams
1.1. An ‘An ‘ff’ sublevel should have ’ sublevel should have 77 boxesboxes
2.2. ‘‘dd’ = 5 boxes’ = 5 boxes
3.3. ‘‘pp’ = 3 boxes’ = 3 boxes
A.A. Boxes represent . . .Boxes represent . . .
IV. Orbital DiagramsIV. Orbital Diagrams
1.1. An ‘An ‘ff’ sublevel should have ’ sublevel should have 77 boxesboxes
2.2. ‘‘dd’ = 5 boxes’ = 5 boxes
3.3. ‘‘pp’ = 3 boxes’ = 3 boxes
4.4. ‘‘ss’ = 1 box ’ = 1 box
A.A. Boxes represent . . .Boxes represent . . .
B.B. Arrows represent . . .Arrows represent . . .
IV. Orbital DiagramsIV. Orbital Diagrams
A.A. Boxes represent . . .Boxes represent . . .
B.B. Arrows represent . . .Arrows represent . . .
C.C. These boxes are filled in a These boxes are filled in a specific orderspecific order
IV. Orbital DiagramsIV. Orbital Diagrams
See Aufbau, Pauli Exclusion, and Hund aboveSee Aufbau, Pauli Exclusion, and Hund above
Self Check – Ex. 5Self Check – Ex. 5
Write the orbital diagrams Write the orbital diagrams for:for:
FluorineFluorineVanadiumVanadiumGermaniumGermanium
V. Electron ConfigurationV. Electron Configuration
A shorthand notation of electron positions in an atomA shorthand notation of electron positions in an atom
V. Electron ConfigurationV. Electron ConfigurationA.A. Number represents Number represents
energy levelenergy level
V. Electron ConfigurationV. Electron ConfigurationA.A. Number represents Number represents
energy levelenergy level
B.B. Letter shows the type of Letter shows the type of sublevelsublevel
V. Electron ConfigurationV. Electron ConfigurationA.A. Number represents Number represents
energy levelenergy level
B.B. Letter shows the type of Letter shows the type of sublevelsublevel
C.C. Electrons are counted and Electrons are counted and written as an exponentwritten as an exponent
V. Electron ConfigurationV. Electron ConfigurationD.D. The ordered listThe ordered list
V. Electron ConfigurationV. Electron ConfigurationD.D. The ordered listThe ordered list
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d107p6
Self Check – Ex. 6Self Check – Ex. 6
Write the electron Write the electron configurations for:configurations for:
MagnesiumMagnesiumSulfurSulfurSilverSilver
VI. Electron Config. using VI. Electron Config. using P.T.P.T.
VI. Electron Config. using VI. Electron Config. using P.T.P.T.A.A. The The ss-block-block
VI. Electron Config. using VI. Electron Config. using P.T.P.T.A.A. The The ss-block-block
B.B. The The pp-block-block
VI. Electron Config. using VI. Electron Config. using P.T.P.T.A.A. The The ss-block-block
B.B. The The pp-block-block
C.C. The The dd-block-block
VI. Electron Config. using VI. Electron Config. using P.T.P.T.A.A. The The ss-block-block
B.B. The The pp-block-block
C.C. The The dd-block-block
D.D. The The ff-block-block
VI. Electron Config. using VI. Electron Config. using P.T.P.T.A.A. The The ss-block-block
B.B. The The pp-block-block
C.C. The The dd-block-block
D.D. The The ff-block-block
E.E. The order of sublevels The order of sublevels ((made easy!made easy!))
Self Check – Ex. 7Self Check – Ex. 7
Use your P.T. to write Use your P.T. to write electron configurations for:electron configurations for:
PotassiumPotassiumArsenicArsenicRhodiumRhodium
VII. Electron Config. using VII. Electron Config. using abbreviationsabbreviations
VII. Electron Config. using VII. Electron Config. using abbreviationsabbreviationsA.A. Abbreviate the Abbreviate the previousprevious
noble gas in bracketsnoble gas in brackets
VII. Electron Config. using VII. Electron Config. using abbreviationsabbreviationsA.A. Abbreviate the Abbreviate the previousprevious
noble gas in bracketsnoble gas in brackets
B.B. Write configuration of Write configuration of remaining electronsremaining electrons
Self Check – Ex. 8Self Check – Ex. 8
Write the abbreviated Write the abbreviated electron configurations for:electron configurations for:
IridiumIridiumTerbiumTerbiumRadonRadon
VII. Exceptions to AufbauVII. Exceptions to Aufbau
VII. Exceptions to AufbauVII. Exceptions to AufbauA.A. CopperCopper
1s22s22p63s23p64s13d9
VII. Exceptions to AufbauVII. Exceptions to AufbauA.A. CopperCopper
B.B. ChromiumChromium
1s22s22p63s23p64s13d5
VII. Exceptions to AufbauVII. Exceptions to AufbauA.A. CopperCopper
B.B. ChromiumChromium
C.C. There are othersThere are others
IX. Lewis Dot DiagramsIX. Lewis Dot Diagrams
A diagram that uses dots to represent valence electrons
A.A. Valence electronValence electron
IX. Lewis Dot DiagramsIX. Lewis Dot Diagrams
A.A. Valence electronValence electron
IX. Lewis Dot DiagramsIX. Lewis Dot Diagrams
1.1. The outermost electrons (the The outermost electrons (the ones that bond)ones that bond)
A.A. Valence electronValence electron
IX. Lewis Dot DiagramsIX. Lewis Dot Diagrams
1.1. The outermost electrons (the The outermost electrons (the ones that bond)ones that bond)
2.2. Determined by adding the Determined by adding the highest energy highest energy ss and and pp electronselectrons
Self Check – Ex. 9Self Check – Ex. 9
How many valence electrons How many valence electrons do the following have?do the following have?
NitrogenNitrogenArsenicArsenicChlorineChlorine
A.A. Valence electronValence electron
B.B. We write these for We write these for representative elementsrepresentative elements
IX. Lewis Dot DiagramsIX. Lewis Dot Diagrams
Representative elements are found in the ‘s’ and ‘p’ blocks
Self Check – Ex. 5Self Check – Ex. 5
Write Lewis structures for:Write Lewis structures for:
StrontiumStrontiumIodineIodine
1s22s22p63s23p64s23d104p65s24d105p3
The End