1 / 24

Molecular Geometry (p. 232 – 236)

Ch. 8 – Molecular Structure. Molecular Geometry (p. 232 – 236). A. VSEPR Theory. V alence S hell E lectron P air R epulsion T heory Electron pairs orient themselves in order to minimize repulsive forces. Lone pairs repel more strongly than bonding pairs!!!. A. VSEPR Theory.

Melvin
Télécharger la présentation

Molecular Geometry (p. 232 – 236)

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. Ch. 8 – Molecular Structure Molecular Geometry(p. 232 – 236)

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

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

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

  5. Know the 13 common shapes & their bond angles! B. Determining Molecular Shape • Draw the Lewis Diagram • Tally up e- pairs on central atom (bonds + lone pairs) • double/triple bonds = ONE pair • Shape is determined by the # of bonding pairs and lone pairs

  6. BeH2 C. Common Molecular Shapes 2 total 2 bond 0 lone → Electronic Geometry = linear Hybridization = sp LINEAR 180°

  7. BF3 C. Common Molecular Shapes → Electronic Geometry = trigonal planar Hybridization = sp2 3 total 3 bond 0 lone TRIGONAL PLANAR 120°

  8. NO21- C. Common Molecular Shapes → Electronic Geometry = trigonal planar Hybridization = sp2 3 total 2 bond 1 lone BENT <120°

  9. CH4 C. Common Molecular Shapes → Electronic Geometry = tetrahedral Hybridization = sp3 4 total 4 bond 0 lone TETRAHEDRAL 109.5°

  10. NCl3 C. Common Molecular Shapes → Electronic Geometry = tetrahedral Hybridization = sp3 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° <109.5°

  11. H2O C. Common Molecular Shapes → Electronic Geometry = tetrahedral Hybridization = sp3 4 total 2 bond 2 lone BENT 104.5° <109.5°

  12. PI5 C. Common Molecular Shapes → Electronic Geometry = trigonal bipyramidal Hybridization = dsp3 5 total 5 bond 0 lone TRIGONAL BIPYRAMIDAL 120°/90°

  13. KrF4 C. Common Molecular Shapes → Electronic Geometry = trigonal bipyramidal Hybridization = dsp3 5 total 4 bond 1 lone SEESAW <120°/<90°

  14. ClF3 C. Common Molecular Shapes → Electronic Geometry = trigonal bipyramidal Hybridization = dsp3 5 total 3 bond 2 lone T-SHAPE <90°

  15. I31- C. Common Molecular Shapes → Electronic Geometry = trigonal bipyramidal Hybridization = dsp3 5 total 3 bond 2 lone LINEAR 180°

  16. SH6 C. Common Molecular Shapes → Electronic Geometry = octahedral Hybridization = d2sp3 6 total 6 bond 0 lone OCTAHEDRAL 90°

  17. IF5 C. Common Molecular Shapes → Electronic Geometry = octahedral Hybridization = d2sp3 6 total 5 bond 1 lone SQUARE PYRAMIDAL <90°

  18. SF4 C. Common Molecular Shapes → Electronic Geometry = octahedral Hybridization = d2sp3 6 total 4 bond 2 lone SQUARE PLANAR 90°

  19. O O Se O D. Examples • SeO3 3 total 3 bond 0 lone E.G. = TRIGONAL PLANAR M.G. = TRIGONAL PLANAR 120°

  20. H As H H D. Examples • AsH3 4 total 3 bond 1 lone E.G. = TETRAHEDRAL M.G. = TRIGONAL PYRAMIDAL 107° (<109.5°)

  21. E. Hybridization • Provides information about molecular bonding and molecular shape • Several atomic orbitals mix to form same total of equivalent hybrid orbitals

  22. E. Hybridization • Carbon is common example (orbital diagram) • One of 2s electrons is promoted to 2p • 4 identical orbitals form sp3 hybridization

  23. Remember the subscript is the orbital, not e- configuration! E. Hybridization • Other types of hybridization • Be – 2 ve- forms sp • Al – 3 ve- forms sp2 • Si – 4 ve- forms sp3 • Kr – 8 ve- forms dsp3 • S – 6 ve- forms d2sp3 exceptions

  24. F. Hybridization Example • Compare shapes and hybrid orbitals: PF3 PF5

More Related