CHM 2353 Lecture Notes - Lecture 2: Paramagnetism, Isoelectronicity, Valence Electron
Document Summary
Principal quantum number: n: orbital size, as n increases, energy and size of orbital increases. If n = 1, l = 0; if n = 2, l = 0, 1: orbital shape, from 0 to n-1, value of l designated by letter s, p, d, f. Magnetic quantum number: ml: orbital orientation, all integers from -l to +l. Spin number: ms: + or (up or down spin) Quantum numbers and emission: emission of e = release of e, thus transition from higher to lower energy. This means that n must decrease (decrease in n = decrease in e) Pauli exclusion principle: no 2 e- in same atom can have same set of 4 quantum #s, electrons in the same orbital must have opposing spins, each orbital can contain no more than 2 e- One e- w/ ms = + , one e- w/ ms = - .