Lecture 10 notes (exam 2 review)

Azimuthal quantum number l l 0 to n 1 defines the

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Unformatted text preview: l (ml = –l to +l ) • Defines the orientation of the orbital. Azimuthal quantum number, l (l = 0 to n −1) • Defines the shape of an orbital. • Orbitals with equal l (and equal n) are in the same subshell. Example List all sets of quantum numbers for an n = 3 e-. • Code letters identify l l = 0, or 1, or 2 if n = 3 and l = 2 (3d), ml is ‐2, ‐1, 0, 1 or 2. if n = 3 and l = 1 (3p), ml is ‐1, 0, or 1. if n = 3 and l = 0 (3s), ml must be 0. l Code 0 s 1 p 2 d 3 f 4 g 5 h ... ... Every (n, l, ml) set has a different shape and/or orientation. 1 2/6/2009 Electron Spin Quantum Numbers Experiments showed a 4th quantum no. was needed spin quantum number, ms • +½ or −½ only. Electron Shell (n) 1 2 View an e‐ as a spinning sphere. Spinning charges act as magnets. 3 4 • Pauli: every e- in an atom must have a unique set of (n, l, ml, ms). Maximum of 2e- per orbital (opposite spins). Pauli exclusion principle. s Orbitals 5 Subshell type s s p s p d s p d f s p d f g* Number of Orbitals Available (= 2l + 1) Number of Electrons Possible in Subshell 1 1 3 1 3 5 1 3 5 7 1 3 5 7 9 Maximum Ele...
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