Lect13 - This isn't right This isn't even wrong Wolfgang...

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“This isn't right. This isn't even wrong.” - Wolfgang Pauli “It was absolutely marvelous working for Pauli. You could ask him anything. There was no worry that he would think a particular question was stupid, since he thought all questions were stupid.” - Victor Frederick Weisskopf
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Building Atoms and Molecules + e r + e ψ even ψ odd d Plane of hydrogen atoms Review session Sunday Extra office hours (TBA) Th, Fr
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Overview Overview z Atomic Configurations z Building atoms with the Pauli exclusion principle z Transitions induced by electric fields: selection rules z Molecular Wavefunctions: origins of covalent bonds z Example: H + H H 2
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Filling the atomic Filling the atomic orbitals orbitals according to the according to the Pauli Principle Pauli Principle 2 2 n Z n eV 6 . 13 E = is valid only for one electron in the Coulomb potential of Z protons. The energy levels shift as more electrons are added, due to electron-electron interactions. Nevertheless, this hydrogenic diagram helps us keep track of where the added electrons go. Energy n 4 3 2 1 l = 0 1 2 3 4 s p d f g Example: Na Z = 11 1s 2 2s 2 2p 6 3s 1 l label #orbitals (2 l +1) 0 s 1 1 p 3 2 d 5 3 f 7 Z = atomic number = number of protons
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Act 1: Pauli Exclusion Principle Act 1: Pauli Exclusion Principle 1. Which of the following states (n, l ,m l ,ms) is/are NOT allowed? (a). (2, 1, 1, -1/2) (b). (4, 0, 0, 1/2) (c). (3, 2, 3, -1/2) (d). (5, 2, 2, 1/2) (e). (4, 4, 2, -1/2) 2. Which of the following atomic electron configurations violates the Pauli Exclusion Principle? (a). 1s 2 , 2s 2 , 2p 6 , 3d 10 (b). 1s 2 , 2s 2 , 2p 6 , 3d 4 (c). 1s 2 , 2s 2 , 2p 8 , 3d 8 (d). 1s 1 , 2s 2 , 2p 6 , 3d 5 (e). 1s 2 , 2s 2 , 2p 3 , 3d 11
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Act 1: Pauli Exclusion Principle Act 1: Pauli Exclusion Principle 1. Which of the following states (n, l ,m l ,ms) is/are NOT allowed? (a). (2, 1, 1, -1/2) (b). (4, 0, 0, 1/2) (c). (3, 2, 3, -1/2) (d). (5, 2, 2, 1/2) (e). (4, 4, 2, -1/2) m A = - l , -( l -1), … ( l -1), l n > l 2. Which of the following atomic electron configurations violates the Pauli Exclusion Principle? (a). 1s 2 , 2s 2 , 2p 6 , 3d 10 (b). 1s 2 , 2s 2 , 2p 6 , 3d 4 (c). 1s 2 , 2s 2 , 2p 8 , 3d 8 (d). 1s 1 , 2s 2 , 2p 6 , 3d 5 (e). 1s 2 , 2s 2 , 2p 3 , 3d 11
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Act 1: Pauli Exclusion Principle Act 1: Pauli Exclusion Principle 1. Which of the following states (n, l ,m l ,ms) is/are NOT allowed? (a). (2, 1, 1, -1/2) (b). (4, 0, 0, 1/2) (c). (3, 2, 3, -1/2) (d). (5, 2, 2, 1/2) (e). (4, 4, 2, -1/2) m A = - l , -( l -1), … ( l -1), l n > l 2. Which of the following atomic electron configurations violates the Pauli Exclusion Principle? 2(2 l +1) = 6 allowed electrons 2(2 l +1) = 10 allowed electrons (a). 1s 2 , 2s 2 , 2p 6 , 3d 10 (b). 1s 2 , 2s 2 , 2p 6 , 3d 4 (c). 1s 2 , 2s 2 , 2p 8 , 3d 8 (d). 1s 1 , 2s 2 , 2p 6 , 3d 5 (e). 1s 2 , 2s 2 , 2p 3 , 3d 11
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FYI: Handy pocket guide for filling Atomic FYI: Handy pocket guide for filling Atomic Orbitals Orbitals -- -- example: Bromine example: Bromine Due to electron-electron interactions, the hydrogen levels fail to give us the correct filling order as we go higher in the periodic table.
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This note was uploaded on 09/15/2008 for the course PHYS 214 taught by Professor Debevec during the Spring '07 term at University of Illinois at Urbana–Champaign.

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Lect13 - This isn't right This isn't even wrong Wolfgang...

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