7-Electon Configurations

# 7-Electon Configurations - 5.111 Lecture Summary #7...

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5.111 Lecture Summary #7 September 23, 2009 Reading for today: Sections 1.10-1.11 Reading for Lecture 8: Sections 1.12-1.13 HYDROGEN ATOM WAVEFUNCTIONS P ORBITALS, Electron Configurations p orbitals have θ,φ dependence – they are not spherically symmetric Probability density maps: Z Y X 2 2p z Ψ Z Y X 2 2p x Ψ Z Y X 2 2p y Ψ HIGHEST PROB Along z axis Along x axis Along y axis POSITIVE ψ where z is positive where x is positive where y is positive NODAL PLANE xy plane θ = 90° yz plane φ = 90° xz plane φ = 0° 2p z orbital ⎛⎞ ψ= θ ⎜⎟ π ⎝⎠ 3/2 1/2 r2a o 210 oo 11 r 3 ec o s aa 4 26 p orbitals have nodal planes (planes that have no electron density) because of angular nodes in wavefunction. Angular nodes: values of θ and φ at which ψ = 0. In general: an orbital has n – 1 total nodes A angular nodes n – 1 – A radial nodes

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5.111 Lecture Summary #7 September 23, 2009 For 2p: n – 1 = 1 total node A = 1 angular node n – 1 – A = 0 radial node RADIAL PROBABILITY DISTRIBUTIONS r 5a 0 10a 0 15a 0 20a 0 n = 3, A = 2 3d 3 2 1 0
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## This note was uploaded on 02/08/2010 for the course CHEM 143 taught by Professor Mike during the Spring '10 term at École Normale Supérieure.

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7-Electon Configurations - 5.111 Lecture Summary #7...

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