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The Electron Configuration
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• Write the electron configuration for a variety of atoms and ions
• Relate the electron configuration of an element to its valence electron(s) and its position on the periodic table.
Additional KEY TermsShorthand notation
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NUCLEUS
1s
2s 2p
3s
3p 3d
4s 4p 4d 4f
Quantum Level
Shapes Total Orbitals
1 s 1s = 1
2 s,p 1s+3p = 4
3 s,p,d 1s+3p+5d = 9
4 s,p,d,f 1s+3p+5d+7f = 16
n n types n2
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1. Pauli Exclusion Principle• Electrons are constantly spinning which creates
a magnetic field• Two electrons can occupy the same orbital only
if they have opposite spins
Each orbital (m) of a shape can hold two spinning electrons (s)
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n = 1
1s2
n = 22s22p6 n = 33s2 3p6 3d10
OLD way
NEW way
2e- 8e- 18e-
8e-
8e-
2e-
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Quantum Level
Shapes Total orbitals e- capacity
1 s 1 = 1 2
2 s,p 1+3 = 4 8
3 s,p,d 1+3+5 = 9 18
4 s,p,d,f 1+3+5+7 = 16 32
n n types n2 2n2
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2. Aufbau Principle
Unexcited electrons fill the lowest, most stable, energy orbital available – ground state.
Notice: as you get further from the nucleus the energy
differences are similar enough to mess-up the
“order”
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3. Hund ruleElectrons must enter empty orbitals of equal energy first before joining occupied orbitals.
The “get your own room” principle – no one wants a bunkmate
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Electron Configuration
Orbital Box Diagrams
1s 2s 2p 3s 3p 3d4s
These are the two ways of representing electron location – we will focus on Electron Configuration
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Periodic Table shows orbital filling for the electron configuration of elements.
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Draw orbital box and electron config for carbon.
C: 1s2 2s2 2p2
1s 2s 2p
Draw orbital box and electron config for Mg.
Mg: 1s2 2s2 2p6 3s2
1s 2s 2p 3s
First ask yourself “how many total electrons,” then
put them in their correct orbitals
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Draw electron config for germanium.
Ge – atomic number 32
Ge: 4s2 3d10 4p2
• Shorthand notation using noble gas “kernels.”
Ge: [Ar] 4s2 3d10 4p2
1s2 2s2 2p6 3s2 3p6
[Ar]
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12345
Write the shorthand configurations for Mn and Ag.
Mn: [Ar] 4s2 3d5 Ag: [Kr] 5s2 4d9
Find the last filled Noble Gas to use as the kernel
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• Valence configuration includes the electrons in the outer-most or highest quantum level (n).
F = 9 electrons
1s2 2s2 2p5 Valence configuration - 2s2 2p5
Ge = 32 electrons
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
Valence configuration - 4s2 4p2
It’s not just the last ones, but the total electrons in the outer
quantum level
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F-1 = 9 electrons + 1 gained
The ION configuration is 1s2 2s2 2p6
Fe+2 = 26 electrons – 2 lost
The ION configuration is 1s2 2s2 2p6 3s2 3p6 3d6
Valence electrons are removed from the highest quantum level
1s2 2s2 2p5
1s2 2s2 2p6 3s2 3p6 4s2 3d6
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Some exceptions to the rule:
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• Half-filled and completely filled orbitals have extra stability
• Atoms will “promote” electrons to improve overall stability
Electron Promotion
Look for configurations ending in “p2” ,“p5” OR “d4” ,“d9” - one electron from being half or
complete filled…”
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Cr: [Ar] 4s2 3d4 Cu: [Ar] 4s2 3d9
Actual configurations:Cr: [Ar] 4s1 3d5 Cu: [Ar] 4s1 3d10
4s 3d 4s 3d
Electron promotion accounts for multiple ionization states (Fe+2, Fe+3…)
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CAN YOU / HAVE YOU?
• Write the electron configuration or orbital box diagrams for a variety of atoms and ions
• Relate the electron configuration of an element to its valence electron(s) and its position on the periodic table.
Additional KEY TermsShorthand notation