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Understanding VSEPR Theory in Molecular Geometry

Valence Shell Electron Pair Repulsion (VSEPR) theory explains how electrons arrange around an atom to minimize repulsions. Used to determine molecular shapes beyond Lewis dot structures. Learn about CO2, BF3, CH4, PF5, and SF6 molecular geometries.

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Understanding VSEPR Theory in Molecular Geometry

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  1. Valence Shell Electron Pair Repulsion (VSEPR) Theory Valence shell electrons will arrange themselves about a central atom so that replusions among them are as small as possible Used to determine the Molecular Geometry (Shape) of a molecule (Lewis Dot structures only give us the order of bonding) Count the # of regions of high electron density: a region of high e- density is a bond (single, double or triple) or a lone pair.

  2. CO2 • Lewis Dot Structure • O=C=O • only tells us the bonding and not the Geometry • VSEPR • # of high e- density regions around the central atom • 2 bonds and 0 lone pairs • Linear O=C=O OCO  180o • Therefore, the Molecular Geometry (Shape) is linear

  3. BF3 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 3 bonds and 0 lone pairs Trigonal Planar FBF  120o  the Molecular Geometry (Shape) is Trigonal Planar

  4. H H C H H CH4 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 4 bonds and 0 lone pairs Tetrahedral HCH  109.5o  the Molecular Geometry (Shape) is Tetrahedral

  5. F F F P F F PF5 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 5 bonds and 0 lone pairs Trigonal Bipyramidal FPF 90.0o & 120.0o & 180.0o  the Molecular Geometry (Shape) is Trigonal Bipyramidal

  6. F F SF6 Lewis Dot Structure VSEPR # of high e- density regions around the central atom 6 bonds and 0 lone pairs Octahedral FSF 90.0o & 180.0o  the Molecular Geometry (Shape) is Octahedral S F F F F

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