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Hint

1

ml

= (2l -1)

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2

n=1

l=0, s-level, ml =0, 1 shell

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3

s-level

spherical orbital 1 shell 1 sub orbital

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4

n=2

l=1, p-level, ml = -1, 0, 1; sub shells: 1, 3, with 4 shells

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5

p-level

second lowest energy level, 4 shells, 1/3 sub shell

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6

n=3

l=2, d-level, ml = -2, -1, 0, 1, 2. Sub shells: 1, 3, 5, with 9 shells

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7

d-level

third lowest energy level, 9 shells, 1/3/5 sub shell

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8

n=4

l=3, ml= -3,-2,-1, 0, 1, 2, 3. Subshells 1, 3, 5, 7 with 16 shells

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9

f-level

fourth lowest energy level, 16 shells, 1/3/5/7 sub shell

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10

degenerate

orbitals in the same sub shell are _______

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11

different

For a given shell, the subshells are NOT degenerate, the subshells have ____ energies

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12

n

principle quantum number

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13

l

Angular Momentum Quantum Number

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14

ml

Magnetic Quantum Number

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15

smaller

As n increases, the energy differences between shells becomes _______

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16

overlap

There is an ________ or penetration of the n=4 and higher shells

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17

Ms

the fourth quantum number (spin), independent of ml, l, and n. Either equal to -1/2 or +1/2.

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18

pauli exclusion principle

no two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers (ml, n or l). Electrons that occupy the same orbital have thee identical quantum numbers (ex. 2, 1, 3)

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19

aufbau principle

Lowest energy orbitals fill up first, then higher energy orbitals. (Do not pair first!)

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20

Anomalous electron configurations

Result from the unusual stability of half-filled and full-filled sub shells. These occur where the sub shell energy differences are small. (ex. 4s v. 3d) (only in transition metals)

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21

transition metals

when subtracting electrons, take from the s-level before the d, only in the ____ ______

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