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II. Molecular Geometry

II. Molecular Geometry. Ch. 9– Molecular Structure. A. VSEPR Theory. V alence Shell Electron Pair Repulsion Theory Electron pairs orient themselves in order to minimize repulsive forces. Lone pairs repel more strongly than bonding pairs!!!. A. VSEPR Theory. Types of e - Pairs

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II. Molecular Geometry

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  1. II. Molecular Geometry Ch. 9– Molecular Structure C. Johannesson

  2. A. VSEPR Theory • Valence Shell Electron Pair Repulsion Theory • Electron pairs orient themselves in order to minimize repulsive forces. C. Johannesson

  3. Lone pairs repel more strongly than bonding pairs!!! A. VSEPR Theory • Types of e- Pairs • Bonding pairs - form bonds • Lone pairs - nonbonding e- C. Johannesson

  4. Bond Angle A. VSEPR Theory • Lone pairs reduce the bond angle between atoms. C. Johannesson

  5. Know the 8 common shapes & their bond angles! B. Determining Molecular Shape • Draw the Lewis Diagram. • Tally up e- pairs on central atom. • double/triple bonds = ONE bond pair • Shape is determined by the # of bonding pairs and lone pairs. C. Johannesson

  6. BeH2 C. Common Molecular Shapes 2 total 2 bond 0 lone LINEAR 180° C. Johannesson

  7. BF3 C. Common Molecular Shapes 3 total 3 bond 0 lone TRIGONAL PLANAR 120° C. Johannesson

  8. CH4 C. Common Molecular Shapes 4 total 4 bond 0 lone TETRAHEDRAL 109.5° C. Johannesson

  9. NH3 C. Common Molecular Shapes 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° C. Johannesson

  10. H2O C. Common Molecular Shapes 4 total 2 bond 2 lone BENT 104.5° C. Johannesson

  11. PCl5 C. Common Molecular Shapes 5 total 5 bond 0 lone TRIGONAL BIPYRAMIDAL 120°/90° C. Johannesson

  12. SF6 C. Common Molecular Shapes 6 total 6 bond 0 lone OCTAHEDRAL 90° C. Johannesson

  13. F P F F D. Examples • PF3 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° C. Johannesson

  14. OCO D. Examples • CO2 2 total 2 bond 0 lone LINEAR 180° C. Johannesson

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