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Published byCrystal Cook Modified over 4 years ago

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Molecular Geometry

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2-D and 3-D Lewis Structures explain the two dimensional structure of molecules In order to model the actual structure of a molecule we need a model that is three dimensional

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VSEPR Valence Shell Electron Pair Repulsion Basically, the paired electrons in the covalent bonds of a molecule exert a repulsive force on each other. Given the number of bonded pairs, and the number of lone pairs, we can predict the 3-D shape of a molecule

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Linear Form: AX or AX 2 One or Two Bonded Pairs Zero Lone Pairs Bond Angle = 180° Hybridization: sp

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Trigonal Planar Form: AX 3 Three Bonded Pairs Zero Lone Pairs Bond Angle = 120° Hybridization: sp 2

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Tetrahedral Form: AX 4 Four Bonded Pairs Zero Lone Pairs Bond Angle = 109.5° Hybridization: sp 3

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Trigonal Pyramidal Form: AX 3 E Three Bonded Pairs One Lone Pair Bond Angle = 107° Hybridization: sp 3

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Bent Form: AX 2 E 2 Two Bonded Pairs Two Lone Pairs Bond Angle = 104.5° Hybridization: sp 3

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