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Understanding VSEPR Theory: A Guide to Molecular Shapes and Structures

Dive into VSEPR Theory to learn how electron pairs orient to minimize repulsive forces, affecting molecular shapes. Explore common shapes like linear, trigonal planar, tetrahedral, trigonal pyramidal, and more, with examples like BeH2, BF3, NH3, and PCl5. Discover how lone pairs influence bond angles and shapes in molecules. With this comprehensive guide, grasp the relationship between bonding and lone electron pairs in determining molecular geometry.

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Understanding VSEPR Theory: A Guide to Molecular Shapes and Structures

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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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