Lecture 18 - Chemical bond

Lecture 18 - Chemical bond - Radial Electron Distribution...

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Radial Electron Distribution in H-atom Radial Wavefunction r e α 2 r e Probability Density 2 2 2 ) ( 4 ) ( r R r dr r R π = =
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Multi-Electron Atoms Electron repulsion 12 0 2 4 r e πε Effective nuclear charge: Z eff = Z - σ Electron Shielding = 1s 2 = 1s 2 2s 1 2 2 0 2 4 2 1 8 n h e m Z E e n ε = ) ( ) ( ) , ( 2 1 1 1 2 1 r r r r s s He φ Ψ ) ( ) ( ) ( ) , , ( 3 2 2 1 1 1 3 2 1 r r r r r r s s s Li Ψ He He He E H ψψ = ˆ
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The Chemical Bond (Chapter 12) Valence Bond Theory Molecular Orbital Theory Hw: 2, 4, 6, 8, 9, 10, 12, 14, 16, 18, 20, 22, 24, 26, 28, 36, 38, 40, 42, 46, 47, 48, 50
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H H .. - Covalent bond formed by equal sharing of electrons between atoms. - Each atom (except H) surrounded by 8 valence electrons: octet rule . - Octet rule applies to 2 nd row elements C, N, O, and F (but NOT B). - Formal Charge = valence electrons vs bonding/unpaired electrons. - Lewis structures do not explain geometry or shape of molecule. - Lewis structures fail to give quantitative bond strength and length. Sulfate Ion Lewis Electron Dot Structures O H H C H H H H C O - O S + O - O O - O S B Cl Cl Cl ..
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This note was uploaded on 04/06/2011 for the course CHEM 107B taught by Professor Jamesames during the Winter '09 term at UC Davis.

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Lecture 18 - Chemical bond - Radial Electron Distribution...

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