chem notes 12-3 - -possible s overlaps- + = oval sigma...

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December 3, 2007 Dr. Stevens Gen. Chem. 1 Molecular Orbital Theory: (MO Theory) -useful for diatomics -tells diamagnetic or paramagnetic -tells order of bonds -strength and sigma v. pi -wave character assumed for e- in orbitals -constructive interference -bigger single wave created by two smaller waves in sync -bond in formation -destructive interference -straight line created by two smaller waves opposite of each other -no e- region -anti-bond -bonding orbital lower energy than lone e- greater stability than lone e- -covalent bond -anti-bonding orbital higher energy than lone e- less stability than lone e-
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Unformatted text preview: -possible s overlaps- + = oval sigma bond- + = sigma anti-bond-when MO form:-# of total orbital conserved-atomic (s,p) molecular (sigma, pi)-E is conserved-H2 2 H each one 1 s to start-bond order: of total # bonding e- minus total # of anti-bonding e--H2 = (2) (0) = 1 => H-H (sigma)-possible p overlaps- + = side-to-side pi bond- + = bend away like chromatids pi anti-bond- + = head-to-head sigma bond- + = candy-wrapper sigma bond-C2- (4) (0) = 2-2 pi bonds...
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This note was uploaded on 04/23/2008 for the course CH 151 taught by Professor Stevens during the Fall '08 term at Whitworth University.

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