8 - 1 sublevels and orbitals effective nuclear charge inner (core) electrons act to shield outer...
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8 - 3 Aufbau Principle The Aufbau Principal is used to write the electron configurations of atoms. For any element, the number of electrons in the neutral atom equals the atomic number. Start filling orbitals, from lowest to highest. If two or more orbitals exist at the same energy level, they are degenerate. Do not pair the electrons until you have to.TRANSCRIPT
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Sublevels and OrbitalsSublevels and OrbitalsEffective Nuclear ChargeEffective Nuclear Charge
Inner (core) electrons act to shield outer(valence) electrons from the positive chargeof the nucleus.
Some orbitals penetrate to the nucleus morethan others, therefore s < p < d < f.s < p < d < f.
As a result, there are different energy levelsfor the different sublevels for any givenprincipal quantum number.
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SublevelsSublevelsen
ergy
1s
2s
1s
2s
1s
2s2p 2p
H Li F
2p
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Aufbau PrincipleAufbau Principle
The Aufbau Principal is used to write theelectron configurations of atoms.
For any element, the number of electrons inthe neutral atom equals the atomic
number.
Start filling orbitals, from lowest to highest.
If two or more orbitals exist at the sameenergy level, they are degenerate. Do notpair the electrons until you have to.
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Orbital Filling OrderOrbital Filling Order. s p d f
1 1s2 2s 2p3 3s 3p 3d4 4s 4p 4d 4f5 5s 5p 5d 5f6 6s 6p 6d 6f7 7s 7p 7d 7f
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Hund’s RuleHund’s Rule
When putting electrons into orbitals with thesame energy, place one electron in each orbital before putting two in any one.
In the orbital diagram, each electron musthave opposite spins.
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Applying The Aufbau PrincipalApplying The Aufbau Principal
1s
2s2p
1s
2s2p
1s
2s2p
ener
gy
C O F
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Sublevels on the Periodic Table Sublevels on the Periodic Table
H
Li
Na
Cs
Rb
K
TlHgAuLaBa
Fr
PtIrOsReWTa
He
RnAtPoBiPb
Be
Mg
Sr
Ca
CdAgY PdRhRuTcMoNb
Ra
ZnCu
Hf
Zr
TiSc NiCoFeMnCrV
In XeITeSbSn
Ga KrBrSeAsGe
Al ArClSPSi
B NeFONC
GdCm
TbBk
SmPu
EuAm
NdU
PmNp
CeTh
PrPa
YbNo
AcErFm
TmMd
DyCf
HoEs
f
d
p
LuLr
s
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Using the Periodic Table to apply Using the Periodic Table to apply the Aufbau Principlethe Aufbau Principle
Main Group ElementsAdd electrons to the nsns orbital as you move through s-block.Add electrons to the npnp orbital as you
move through the p-block.
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Using the Periodic Table to apply Using the Periodic Table to apply the Aufbau Principlethe Aufbau Principle
Transition ElementsAdd electrons to the (n-1)d(n-1)d orbital as
you move through d-block.Add electrons to the (n-2)f(n-2)f orbital as
you move through f-block.
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Writing Electron ConfigurationsWriting Electron Configurations
Expanded FormatExpanded Format
O 1s22s22p4 Ti 1s22s22p63s23p64s23d2
Br 1s22s22p63s23p64s23d104p5
Abbreviated FormatAbbreviated Format
O [He]2s22p4 Ti [Ar]4s23d2 Br [Ar]4s23d104p5
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Electron Configurations for IonsElectron Configurations for Ions
Electron configurations can also be writtenfor ions.Start with the ground-state configuration
for the atom.For cations, remove the number of the
outermost electrons equal to the charge.For anions, add the number of outermost
electrons equal to the charge.
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Electron Configurations for AnionsElectron Configurations for Anions
Example: ClExample: Cl- - (chloride)(chloride)
First, write the electron configuration forchlorine:
Cl [Ne]3s23p5
Because the charge is 1-, add one electron.
Cl- [Ne]3s23p6
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Electron Configurations for CationsElectron Configurations for Cations
Example: BaExample: Ba2+2+ (barium) (barium)
First, write the electron configuration forbarium.
Ba [Xe]6s2
Because the charge is 2+, remove twoelectrons.
Ba2+ [Xe]
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Isoelectronic ConfigurationsIsoelectronic ConfigurationsSpecies having the same electronconfigurations.
Each of the following has an electronconfiguration of 1s22s22p6
OO2-2- FF-- NeNe
NaNa++ MgMg2+2+ Al Al3+3+
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Electron Dot DiagramsElectron Dot Diagrams
A simple way to show the valence electronspresent in an atom.
Valence electrons are those electrons foundin the highest numbered principal energylevel (PEL).
Valence electrons are found only in the s and
p sublevels and in most cases are theelectrons responsible for bonding.
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Electron Dot DiagramsElectron Dot Diagrams
The chemical symbol represents the kernel of
the atom.
The kernel of an atom consists of the nucleus
and the core electrons.
Example
X
s px
py
pz
Start with s and proceed cw!
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Electron Dot DiagramsElectron Dot DiagramsExamples
Na [Ne]3s1
Br [Ar]4s23d104p5
Cr [Ar]4s13d5
.
...
. ....
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Heisenberg Uncertainty PrincipleHeisenberg Uncertainty Principle In order to observe an electron, one would need to hit it with photons having a very short wavelength. Short wavelength photons would have a high frequency and a great deal of energy. If one were to hit an electron, it would cause the motion and the speed of the electron to change. Lower energy photons would have a smaller effect but would not give precise data.
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Quantum NumbersQuantum NumbersPrincipal Quantum Number (n)Principal Quantum Number (n)
Tells the size of an orbital and determines its energy. n = 1, 2, 3 …
Angular Momentum (l)Angular Momentum (l) The number of subshells that a principal level contains. It tells the shape of the orbitals. l = 0 to n - 1
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Quantum NumbersQuantum Numbers
Magnetic Quantum Number (mMagnetic Quantum Number (mll))
Describes the orientation of the orbital.
ml = -l to +l (all integers, including zero)
For example, if l = 3, then ml would have values of -3, -2, -1, 0, 1, 2, 3
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Quantum NumbersQuantum Numbers
. n l ml Sublevel Orbitals1 0 0 1s 12 0 0 2s 1
1 -1,0,1 2p 33 0 0 3s 1
1 -1,0,1 3p 32 -2,-1,0,1,2 3d 5
4 0 0 4s 11 -1,0,1 4p 32 -2,-1,0,1,2 4d 53 -3,-2,-
1,0,1,2,34f 7
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The s OrbitalThe s Orbital
The s orbital is a sphere. Every PEL has ones orbital.
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The p OrbitalsThe p Orbitals
There are three p orbitals: px, py and pz
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Electron SpinElectron Spin
Pauli added one additional quantum numberthat would allow only two electrons to be inan orbital.Spin quantum number (mSpin quantum number (mss))..
It can have values of +1/2 and -1/2Pauli Exclusion PrinciplePauli Exclusion Principle
Pauli also proposed that no two electrons in an atom can have the same set of four quantum numbers.
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WavesWavesWavelengthWavelength (l) (l)
The distance measured from crest to crest or from trough to trough (m, cm, nm).
AmplitudeAmplitude
The vertical distance from the node to the height of a wave (m, cm, nm).
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FrequencyFrequency (f) (f)
The number of cycles or complete vibrations that pass a point each
second (s-1, vib/s).
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Electromagnetic RadiationElectromagnetic Radiation
A form of energy consisting of perpendicularelectrical and magnetic fields that change, atthe same time and in phase with time.
The SI unit of frequency (f) is the hertz (Hz) 1 Hz = 1 s1 Hz = 1 s-1 -1 = 1/s= 1/s
Wavelength and frequency are related c = f λc = f λ c = 3.00 x10c = 3.00 x1088 m/s m/s
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Energy ProblemsEnergy ProblemsCalculate the frequency of a quantum of
light, aphoton, with a wavelength of 6.00 x 10-7 m.
λ = 6.00 × 10-7 m c = 3.00 × 108 m/s
C = f × λ f = =
C λ
=5.00 × 1014 /s3.00 × 108 m/s 6.00 × 10-7 m
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Energy ProblemsEnergy ProblemsCalculate the energy of a photon, with awavelength of 6.00 x 10-7 m.
λ = 6.00 × 10-7 m c = 3.00 × 108 m/sh = 6.63 × 10-34 J•s
E = h × f c = f × λ f = c/λ
E = h × c/λ
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E = h × c/λ
E = 6.63 × 10-34 J•s × 3.00 × 108 m/s 6.0 × 10-7 m
E = 3.3 × 10-19 J