Chapter 11 Journal

Chapter 11 Journal - Forms a region of high electron...

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Chapter 9 A valence bond theory and hybridization 1) Space overlapped has maximum capacity of two electrons with opposite with spins 2) The greater the orbital overlap, the stronger the bond. Hybridization 1) sp 2) sp 2
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3) sp 3 CH 4
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4) sp 3 d 5) sp 3 d 2
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Types of covalent bond 1) End-to end overlap Sigma ( σ ) bonding: highest electron density along the bond axis 2) Side-to side overlap Pi ( π ) bonding: occupy two regions (lobes of bond) One π bond has two electrons. 3) Double bond: consists of one σ bond and one π bond 4) Triple bond: consists of one σ bond and two π bond 5) σ bond allows free rotation; π bond restricts rotation C 2 H 4
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C 2 H 2 Molecular orbital (MO)
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1) MO bond order = 1/2 [ (no. of e - in bonding MO) – (no. of e - in antibonding Mo) ] a Bonding MO: adding the wave function together.
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Unformatted text preview: Forms a region of high electron density between the nuclei b Antibonding MO: subtracting the wave functions from each other A region of high zero electron density (a node) between the nuclei Homonuclear of Period 2 Elements The energy order for MOs in 2p orbital is: 2p < 2p < 2p < 2p For B, C, N, large orbitals with small repulsions: 2p, 2s mix. Then: 2p < 2p < 2p < 2p Heteronuclear Diatomic Molecules Put the atom with higher polarity lower in the diagram, the atom with lower polarity higher in the diagram. And fill in all the bonding and nobonding MOs in order of energy. Example:...
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This note was uploaded on 12/03/2011 for the course ECON 0200 taught by Professor Staff during the Fall '08 term at Pittsburgh.

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Chapter 11 Journal - Forms a region of high electron...

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