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Chemistry 8.3

Chemistry 8.3. 8.3. 8.3. VSEPR Theory. VSEPR Theory: The Valence-Shell Electron-Repulsion Theory states that molecular shapes adjust in order for valence-electron pairs to stay as far apart as possible. 8.3. VSEPR Theory.

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Chemistry 8.3

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  1. Chemistry 8.3 8.3

  2. 8.3 VSEPR Theory • VSEPR Theory: The Valence-Shell Electron-Repulsion Theory states that molecular shapes adjust in order for valence-electron pairs to stay as far apart as possible.

  3. 8.3 VSEPR Theory • Nine Possible Molecular Shapes: (You will be tested over the first five!)

  4. 8.3 VSEPR Theory • Example: Methane Tetrahedral Angle

  5. 8.3 VSEPR Theory • Example: Ammonia has one unshared electron Pair. Pyramidal

  6. VSEPR Theory • Example: Water (H2O) has 2 unshared pairs. Bent

  7. VSEPR Theory • Example: Carbon Dioxide – Carbon has no unshared pairs. Linear (180̊)

  8. VSEPR Theory • Example: 3 bonding pairs and 0 unshared pairs. Trigonal Planar

  9. 8.3 Section Quiz. • 8.3.

  10. 8.3 Section Quiz. • 1. A molecular orbital belongs to a • specific atom. • molecule as a whole. • specific pair of atoms. • central atom.

  11. 8.3 Section Quiz. • 2. VSEPR theory enables prediction of 3-dimensional molecular shape because the valence electron pairs • are attracted to each other. • form molecules with only four possible shapes. • stay as far apart as possible. • always form tetrahedral shapes.

  12. 8.3 Section Quiz. • 3. Orbital hybridization provides information about • both molecular bonding and molecular shape. • both molecular bonding and bond energy. • neither molecular bonding nor molecular shape. • neither molecular bonding nor bond energy.

  13. END OF SHOW

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