Chemistry_1031_day39_050109_actual

Chemistry_1031_day39_050109_actual - General Chemistry I...

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General Chemistry I CHE-1031 Dr. Jonathan M. Smith Friday, May 1, 2009
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Bonding => molecular geometry Valence shell electron pair repulsion (VSEPR) continued… Hydridization of atomic orbitals sp3 : tetrahedral arrangement of electron pairs sp2 : trigonal Keep working along… Read Chapter 10 Mastering Chemistry problems Final Exam practice
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Tro, Chemistry: A Molecular Approach 3
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Tro, Chemistry: A Molecular Approach 4 Because the bonds are not identical, the observed angles are slightly different from ideal.
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Tro, Chemistry: A Molecular Approach 5 when there are 4 electron groups around the central atom, they will occupy positions in the shape of a tetrahedron around the central atom this results in the molecule taking a tetrahedral geometry the bond angle is 109.5°
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Tro, Chemistry: A Molecular Approach 6
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Tro, Chemistry: A Molecular Approach 7
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lone pair groups “occupy more space” on the central atom because their electron density is exclusively on the central atom rather than shared like bonding electron groups relative sizes of repulsive force interactions is: Lone Pair – Lone Pair > Lone Pair – Bonding Pair > Bonding Pair – Bonding Pair this effects the bond angles, making them smaller than expected Tro, Chemistry: A Molecular Approach 8
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Tro, Chemistry: A Molecular Approach 9 The bonding electrons are shared by two atoms, so some of the negative charge is removed from the central atom. The nonbonding electrons are localized on the central atom, so area of negative charge takes more space.
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Tro, Chemistry: A Molecular Approach 10 when there are 3 electron groups around the central atom, and 1 of them is a lone pair, the resulting shape of the molecule is called a trigonal planar - bent shape the bond angle is < 120°
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This note was uploaded on 05/09/2010 for the course CHEM 1031 taught by Professor Thomas during the Spring '06 term at Temple.

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Chemistry_1031_day39_050109_actual - General Chemistry I...

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