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II. Molecular Geometry

II. Molecular Geometry. – Molecular Structure. A. VSEPR Theory. V alence Shell Electron Pair Repulsion Theory Electron pairs orient themselves in order to minimize repulsive forces. A. VSEPR Theory. Types of e - Pairs Bonding pairs - form bonds Lone pairs - nonbonding e -.

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II. Molecular Geometry

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  1. II. Molecular Geometry – Molecular Structure

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

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

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

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

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

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

  8. C. Common Molecular Shapes 3 total 2 bond 1 lone SO2 BENT <120°

  9. 4 total 4 bond 0 lone C. Common Molecular Shapes CH4 TETRAHEDRAL 109.5°

  10. 4 total 3 bond 1 lone C. Common Molecular Shapes NH3 TRIGONAL PYRAMIDAL 107°

  11. 4 total 2 bond 2 lone C. Common Molecular Shapes H2O BENT 104.5°

  12. 5 total 5 bond 0 lone C. Common Molecular Shapes PCl5 TRIGONAL BIPYRAMIDAL 120°/90°

  13. 6 total 6 bond 0 lone C. Common Molecular Shapes SF6 OCTAHEDRAL 90°

  14. PF3 D. Examples F P F F 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107°

  15. CO2 D. Examples OCO 2 total 2 bond 0 lone LINEAR 180°

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