lone-pair - becomes “trigonal pyramidal” • AX 3 E •...

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VSEPR: Lone Pairs VSEPR: Lone Pairs
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Lone pairs Lone pairs Thus far we have considered (built) only structures where there are no free electrons around the central atom These electrons that are not involved in bonds are called “lone pairs” Essentially, they have the same influence on molecular structure as electron pairs in bonds The result is some weird shapes and or Vs. or H C H H H H C H H H H N H H H N H H
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Variations on Tetrahedral Molecule Variations on Tetrahedral Molecule The tetrahedral molecule is AX 4 Lone pairs can be indicated with AX Y E Z , where Z is the number of lone pairs By replacing 1 bond with a lone pair the tetrahedral shape
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Unformatted text preview: becomes “trigonal pyramidal” • AX 3 E • By replacing two bonds with lone pairs we get a “bent” (non-linear) shape (AX 2 E 2 ) (Fig. 7.7, pg. Variations on Trigonal Bipyramidal Variations on Trigonal Bipyramidal • AX 5 is trigonal bipyramidal • AX 4 E is unsymmetrical tetrahedron • AX 3 E 2 is T-shaped • AX 2 E 3 is linear See Fig. 7.8 on pg. 251 Variations on Octahedral Shape Variations on Octahedral Shape • AX 6 is octahedral • AX 5 E is square pyramidal • AX 4 E 2 is square planar See Fig. 7.9 on pg. 252 For more lessons, visit www.chalkbored.com...
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This note was uploaded on 04/12/2011 for the course CHEM 1010 taught by Professor Marshall during the Spring '11 term at North Texas.

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lone-pair - becomes “trigonal pyramidal” • AX 3 E •...

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