electronic structure

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9 Terms

1
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principal (n)

shell number

2
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azimuthal (l)

subshell (type of orbital)

s = 0

p =1

d = 2

f = 3

3
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magnetic (ml)

specific orbital (orientation in space)

4
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spin (ms)

up or down

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Aufbau principle

electrons fill the lowest energy orbitals first

6
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Hunds Rule

degenerate orbitals each get an electron before pairing

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Pauli exclusion principle

no 2 electrons in an atom have the same 4 quantum numbers

8
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paramagnetic

attraction to a magnetic field, occurs due to presence of unpaired electrons

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diamagnetic

very slight repulsion to magnetic field, occurs when all electrons are paired