1. IV. Electron Configuration (p. 105 - 116, 128 - 139)
Ch. 5 - Electrons in Atoms
IV. Electron Configuration (p , )
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2. A. General Rules Pauli Exclusion Principle
Each orbital can hold TWO electrons with opposite spins.
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3. A. General Rules Aufbau Principle
Electrons fill the lowest energy orbitals first.
“Lazy Tenant Rule”
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4. A. General Rules WRONG RIGHT Hund’s Rule
Within a sublevel, place one e- per orbital before pairing them.
“Empty Bus Seat Rule”
WRONG
RIGHT
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5. 1s2 2s2 2p4 O B. Notation 1s 2s 2p 8e- Orbital Diagram
Electron Configuration
1s2 2s2 2p4
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6. S 16e- 1s2 2s2 2p6 3s2 3p4 S 16e- [Ne] 3s2 3p4 B. Notation
Longhand Configuration
S 16e-
1s2
2s2
2p6
3s2
3p4
Core Electrons
Valence Electrons
Shorthand Configuration (Noble-gas notation)
S 16e- [Ne] 3s2 3p4
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7. C. Periodic Patterns s p d (n-1) f (n-2) 1 2 3 4 5 6 7 6 7
© 1998 by Harcourt Brace & Company
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8. 1s1 C. Periodic Patterns 1st column of s-block 1st Period s-block
Example - Hydrogen
1s1
1st column of s-block
1st Period
s-block
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9. C. Periodic Patterns p s d (n-1) f (n-2) Shorthand Configuration
Core e-: Go up one row and over to the Noble Gas.
Valence e-: On the next row, fill in the # of e- in each sublevel. s
d (n-1)
f (n-2) p
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10. [Ar] 4s2 3d10 4p2 C. Periodic Patterns Example - Germanium
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11. D. Stability Full energy level Full sublevel (s, p, d, f)
Half-full sublevel
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12. D. Stability Electron Configuration Exceptions Copper
EXPECT: [Ar] 4s2 3d9
ACTUALLY: [Ar] 4s1 3d10
Copper gains stability with a full d-sublevel.
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13. D. Stability Electron Configuration Exceptions Chromium
EXPECT: [Ar] 4s2 3d4
ACTUALLY: [Ar] 4s1 3d5
Chromium gains stability with a half-full d-sublevel.
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14. D. Stability 1+ 2+ 3+ NA 3- 2- 1- Ion Formation
Atoms gain or lose electrons to become more stable.
Isoelectronic with the Noble Gases. 1+ 2+ 3+ NA 3- 2- 1-
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15. O2- 10e- [He] 2s2 2p6 D. Stability Ion Electron Configuration
Write the e- config for the closest Noble Gas
EX: Oxygen ion  O2-  Ne
O e [He] 2s2 2p6
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16. Electron Dot Structure
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17. Electron Dot Structure
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18. B. Quantum Mechanics Orbital (“electron cloud”)
Region in space where there is 90% probability of finding an e-
Orbital
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19. C. Quantum Numbers Four Quantum Numbers:
Specify the “address” of each electron in an atom
UPPER LEVEL
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20. C. Quantum Numbers 1. Principal Quantum Number ( n ) Energy level
Size of the orbital
n2 = # of orbitals in the energy level
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21. C. Quantum Numbers f d s p 2. Angular Momentum Quantum # ( l )
Energy sublevel
Shape of the orbital f d s p
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22. C. Quantum Numbers 3. Magnetic Quantum Number ( ml )
Orientation of orbital
Specifies the exact orbital within each sublevel
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23. C. Quantum Numbers px py pz
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24. C. Quantum Numbers 2s 2px 2py 2pz
Orbitals combine to form a spherical shape. 2s
2pz
2py
2px
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25. C. Quantum Numbers 4. Spin Quantum Number ( ms )
Electron spin  +½ or -½
An orbital can hold 2 electrons that spin in opposite directions.
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26. C. Quantum Numbers Pauli Exclusion Principle
No two electrons in an atom can have the same 4 quantum numbers.
Each e- has a unique “address”:
1. Principal # 
2. Ang. Mom. # 
3. Magnetic # 
4. Spin # 
energy level
sublevel (s,p,d,f)
orbital
electron
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27. Bohr Models
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28. Bohr Models
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29. Bohr Models
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30. Classwork
#24 on page 160
#29 on page 162 (don’t draw the orbital diagrams)
#85 on 167
#87 on page 168
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31. Classwork ELECTRON DOT CONFIGURATION Page 162 do #33
Page 168 do #90, 92, and 93
Page 979 do #5, 6, 7, 8, 9 (b, c, d) for Chapter 5
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