1 / 14

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

bkoch
Télécharger la présentation

II. Molecular Geometry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related