The document compares the shapes of molecules with and without non-bonding electron pairs. It lists common molecules and their number of electron pairs, shapes both with and without non-bonding pairs, and the hybridization of the central atom. Key information included is that methane has 4 electron pairs in a tetrahedral shape from sp3 hybridization, ammonia has 4 pairs in a tetrahedral shape with non-bonding pairs and a trigonal pyramidal shape without from sp3 hybridization, and sulfur hexafluoride has 6 pairs in an octahedral shape from d2sp3 hybridization.

1. Shape with non- Shape without non-
Molecule bonding electron pair bonding electron pairs "Live" Molecules
(if any)
BeH2
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BF3
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CH4
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NH3
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H2S
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PF5
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BrF3
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2. TeCl4
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SF6
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XeF4
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XeF2
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Answers: (Click the arrow to go back to the top of the "live" examples)
Molecule # of electron pairs Shapes with, and without non- Hybridization
bonding e pair of central atom
BeH2 2 linear, linear sp
BF3 3 trigonal planar, trigonal planar sp2
CH4 4 tetrahedral, tetrahedral sp3
NH3 4 tetrahedral, trigonal pyramidal sp3
H2S 4 tetrahedral, bent sp3
PF5 5 trigonal bipyramidal, trigonal dsp3
bipyramidal

3. BrF3 5 trigonal bipyramidal, T- dsp3
shaped
TeCl4 5 trigonal bipyramidal, Seesaw dsp3
SF6 6 octahedral, octehedral d2sp3
XeF4 6 octahedral, square planar d2sp3
XeF2 5 trigonal bipyramidal, linear dsp3