CH 1010 Chapter 3 Part 2

= (2l -1)

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

spherical orbital 1 shell 1 sub orbital

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

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

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

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

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

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

orbitals in the same sub shell are _______

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

principle quantum number

Angular Momentum Quantum Number

Magnetic Quantum Number

As n increases, the energy differences between shells becomes _______

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

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

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)

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

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)

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