Lecture 13

Lecture 13 - Chemistry 11500 Lecture 13, the first 1/2...

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1 Chemistry 11500 Lecture 13, the first 1/2 Reading: Sec 9.7, pp. 397-205, VESPR Theory
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2 How do chemists think about molecular shape?
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3 VSEPR V alence S hell E lectron P air R epulsion predicts the shapes of molecules Principle: Valence shell electron units around a central atom will arrange themselves so that they are as far from each other as possible. ( minimizing their repulsions )
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4 Two electron units: Linear Examples: CS 2 , HCN, BeF 2
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5 The two molecular shapes of the trigonal planar electron- group arrangement. Class Shape Examples: SO 3 , BF 3 , NO 3 - , CO 3 2- Examples: SO 2 , O 3 , PbCl 2 , SnBr 2 Bond angle <120 o
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6 The three molecular shapes of the tetrahedral electron- group arrangement. Examples: CH 4 , SiCl 4 , SO 4 2- , ClO 4 - NH 3 PF 3 ClO 3 H 3 O + H 2 O OF 2 SCl 2 Ideal bond angle 109.5 o Bond angle < 109.5 o Bond angle < 109.5 o
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7 Perspective
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The four molecular shapes of the trigonal bipyramidal electron-group arrangement. SF
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This note was uploaded on 10/24/2011 for the course CHEM 116 taught by Professor Stevenson during the Spring '08 term at Purdue.

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Lecture 13 - Chemistry 11500 Lecture 13, the first 1/2...

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