lone-pair - becomes trigonal pyramidal AX 3 E By replacing...

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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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lone-pair - becomes trigonal pyramidal AX 3 E By replacing...

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