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Electron Configuration
Electrons in Atoms
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Energy levels, sublevels and orbitals
Energy level(cloud or shell)
Sublevels Orbitals Number of electrons
1 s 1 s orbital 2
2 s, p 1 s orbital
3 p orbitals
8
3 s, p, d 1 s orbital
3 p orbitals
5 d orbitals
18
4, 5, 6, 7 s, p, d, f 1 s orbital
3 p orbitals
5 d orbitals
7 f orbitals
32
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s orbitals
1s 2s 3s
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Three p Orbitals
px pz py
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A. General Rules
Pauli Exclusion Principle
Each orbital can hold TWO electrons
with opposite spins.
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A. General Rules
Aufbau Principle
Electrons fill the lowest energy orbitals first.
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RIGHTWRONG
A. General Rules
Hund’s Rule
Within a sublevel, place one e- per orbital before pairing them.
“Empty Bus Seat Rule”
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O
8e-
Orbital Diagram
Electron Configuration
1s2 2s2 2p4
B. Notation
1s 2s 2p
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Shorthand Configuration
S 16e-
Valence Electrons
Core Electrons
S 16e- [Ne] 3s2 3p4
1s2 2s2 2p6 3s2 3p4
B. Notation
Longhand Configuration
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© 1998 by Harcourt Brace & Company
sp
d (n-1)
f (n-2)
1234567
67
C. Periodic Patterns
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C. Periodic Patterns
Period # (Row) indicates the highest energy level (subtract
for d & f)
Group # (column) Indicates the total # of valence e-
Column within sublevel block # of e- in sublevel
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s-block
1st Period
1s11st column of s-block
C. Periodic Patterns
Example - Hydrogen
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1
2
3
4
5
6
7
C. Periodic Patterns
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.
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[Ar] 4s2 3d10 4p2
C. Periodic Patterns
Example - Germanium
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Full energy level
1
2
3
4 5
6
7
Full sublevel (s, p, d, f)Half-full sublevel
D. Stability
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Electron Configuration Exceptions
Copper
EXPECT: [Ar] 4s2 3d9
ACTUALLY: [Ar] 4s1 3d10
Copper gains stability with a full d-sublevel.
D. Stability
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Electron Configuration Exceptions
Chromium
EXPECT: [Ar] 4s2 3d4
ACTUALLY: [Ar] 4s1 3d5
Chromium gains stability with a half-full d-sublevel.
D. Stability
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D. Stability
Ion Formation Atoms gain or lose electrons to become
more stable. Isoelectronic with Noble Gases.
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D. Stability
Ion Electron Configuration
Find the Noble Gas with the same number of electrons and write its symbol in brackets
EX: Oxygen ion O2- = 10 electrons
= [ Ne ]
Ex: Potassium ion K+ = 18 electrons
= [Ar]
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Photoelectric Effect
The emission of electrons from a metal when light shines on the metal only occurs if the photons in the
light have a certain minimum frequency (energy)
Different metals require different minimum frequencies
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Line Emission Spectrum
The lowest energy state of an atom is called the ground state
A state in which an atom has a higher potential energy than the ground state is called an excited state
When an excited atom returns to the ground state, it gives off energy, usually in the form of light
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Line Emission Spectrum
When this light is shined through a prism, it is separated into a series of specific frequencies of light
The bands of light are known as the line emission spectrum for the element
Line emission spectrum for hydrogen