quantum-II-handout - Quantum Mechanics: Quantum Numbers...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Quantum Mechanics: the sequel Quantum Numbers • Read on pg. 200 from “The theory of quantum…” (about third paragraph) to “The Magnetic Quantum Number, m l ” on pg. 201. Do PE 3 m l : the magnetic quantum number • Recall: we are looking at the first three of four quantum numbers: n, l , m l , m s • The magnetic quantum number is m l , it further divides subshells into “orbitals” • Recall that even though you can visualize these divisions as spherical regions around the nucleus, they really refer to different waveforms •m l ranges from - l to + l , in intervals of one • when l = 1, the values of m l are -1, 0, 1 m l : the magnetic quantum number Read the remainder of 201. • What is m l when l = 3 (f)? When l = 0 (s)? • PE 4: How many orbitals are in a g subshell? More practice with quantum #s • Complete the chart on the study sheet • Look at the last two columns of the chart. • A maximum of two electrons can fit in each
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.
Ask a homework question - tutors are online