Exam 3 Notecard

Exam 3 Notecard - Bond Angles: Linear 180 Trigonal Planar...

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Unformatted text preview: Bond Angles: Linear 180 Trigonal Planar 120 Tetrahedral 109.5 Ammonia 107.5 (1 lone pair) Water 104.5 (2 lone pairs) Trigonal-Bipyramidal 120 & 90 Octahedral 90 Multiple Covalent Bonds: C, N, O, S = x3 or x2 to self and others C = N, O, S N = O, S S = O\ Formal Charge: FC = Group # - (LPE - .5 BE) Bond Order: # of e pairs / # of bonds (Bonding Antibonding) / 2 If above 0, then molecule exists Molecular Polarity Covalent if EN = 0 Polar if EN = 0 1.5 Ionic if EN = 1.5 + Molecular Orbital Theory Robert Mullihan Valence e are delocalized Valence Bond Theory Linus Pauling Valence e are localized between atoms (or LP) .5 filled atomic orbitals overlap to form bonds sp = linear sp 2 = trigonal-planar sp 3 = tetrahedral sp 3 d = trigonal bipyramidal sp 3 d 2 = octahedral Conversions & Values: 1 bar = 1 x 10 5 Pa = 1 x 10 2 kPa = .9872 atm 1 atm = 760 mm Hg = 760 torr 1 Pa = 1 newton/meter 2 .082057 L*atm / mol * K 82.057 m L*atm / mol * K82....
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This note was uploaded on 04/29/2008 for the course CHEM 103 taught by Professor Wendt during the Fall '07 term at Wisconsin.

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