CH 1010 Chapter 3 Part 2

ml

ml

= (2l -1)

n=1

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

s-level

spherical orbital 1 shell 1 sub orbital

n=2

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

p-level

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

n=3

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

d-level

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

n=4

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

f-level

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

degenerate

orbitals in the same sub shell are _______

different

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

n

principle quantum number

l

Angular Momentum Quantum Number

ml

Magnetic Quantum Number

smaller

As n increases, the energy differences between shells becomes _______

overlap

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

Ms

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

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)

aufbau principle

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

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)

transition metals

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