Chp6 - Chapter 6 Molecular Structure and Bonding VSEPR and...

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Chapter 6 Molecular Structure and Bonding VSEPR and Molecular Geometry Valence Bond Theory σ and π Bonding Hybridization MO Theory for Delocalization Structure and Bonding From Lewis Structures
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VSEPR V alence S hell E lectron P air R epulsion “Regions” or “groups” of negative charge around an atom will adopt a position to minimize the repulsions between them Allows for the transition from a 2-D (Lewis) to a 3-D structure (molecular shape/geometry)
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Electron Region Defined as a lone pair (LP) or a bonding pair (BP) Single, double, or triple bonds are all considered to be ONE region Atoms which obey the octet rule can have 2, 3, or 4 electron groups Hydrogen has 1 electron group
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Electron Geometry Molecule Shape Bond < AX 2 Linear 180 o AX 2 E Bent 120 o AX 3 Trigonal planar 120 o AX 2 E 2 Bent 109 o AX 3 E Pyramidal 109 o AX 4 Tetrahedral 109 o
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Molecular Shapes Relative strengths of interactions: LP-LP > LP-BP > BP-BP CO 2 , 180o, linear SO 3 , 120o, trigonal planar SO 2 , ~120o, bent H 2 O, ~109o, bent NH 3 , ~109o, pyramidal CH 4 , 109o, tetrahedral
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Determining Shape Draw Lewis structure Count electron regions – LP and bonds Determine electron geometry from # of e - groups Determine molecular shape by considering ATOMS ONLY
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Electron Geometry Molecular Shape linear trigonal planar tetrahedral
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Expanded Octet Can apply to atoms with more than an octet of VE Atoms after 2 nd period 5 groups; trigonal bipyramidal (tbp) – LP in equatorial 6 groups; octahedral – multiple LP on same axis (180 o apart)
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This note was uploaded on 10/30/2009 for the course CH Ch101 taught by Professor Bigham during the Fall '08 term at N.C. State.

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Chp6 - Chapter 6 Molecular Structure and Bonding VSEPR and...

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