1 / 13

Molecular Shape Section 9.4

Molecular Shape Section 9.4. Chemistry. Objectives. Discuss the VSEPR bonding theory Predict the shape of and the bond angles in a molecule Define hybridization. The Shape of Molecules. The shape of molecules determines reaction ability The model we use is the VSEPR model

aysel
Download Presentation

Molecular Shape Section 9.4

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. Molecular ShapeSection 9.4 Chemistry

  2. Objectives • Discuss the VSEPR bonding theory • Predict the shape of and the bond angles in a molecule • Define hybridization

  3. The Shape of Molecules • The shape of molecules determines reaction ability • The model we use is the VSEPR model • Valence Shell Electron Pair Repulsion

  4. VSEPR Model • Minimizes the repulsion of shared and unshared pairs of electrons around the central atom • 7 key shapes you will need to be able to draw and identify

  5. Linear Molecular Shape • Example: BeCl2 • Total Pairs of Electrons: 2 • Shared Pairs of Electrons: 2 • Lone Pairs: 0 • Bond Angle: 180° • Hybrid Orbitals: sp

  6. Trigonal Planar • Example: AlCl3 • Total Pairs of Electrons: 3 • Shared Pairs of Electrons: 3 • Lone Pairs of Electrons: 0 • Bond Angle: 120° • Hybrid Orbitals: sp²

  7. Tetrahedral • Example: CH4 • Total Pairs of Electrons: 4 • Shared Pairs of Electrons: 4 • Lone Pairs of Electrons: 0 • Bond Angle: 109.5° • Hybrid Orbitals: sp³

  8. Trigonal Pyramidal • Example: PH3 • Total Pairs of Electrons: 4 • Shared Pairs of Electrons: 3 • Lone Pairs of Electrons: 1 • Bond Angle: 107.3° • Hybrid Orbitals: sp³

  9. Bent • Example: H2O • Total Pairs of Electrons: 4 • Shared Pairs of Electrons: 2 • Lone Pairs of Electrons: 2 • Bond Angle: 104.5° • Hybrid Orbitals: sp³

  10. Trigonal Bipyramidal • Example: NbBr5 • Total Pairs of Electrons: 5 • Shared Pairs of Electrons: 5 • Lone Pairs of Electrons:0 • Bond Angle: 90°, 120° • Hybrid Orbitals: sp³d

  11. Octahedral • Example: SF6 • Total Pairs of Electrons: 6 • Shared Pairs of Electrons: 6 • Lone Pairs of Electrons: 0 • Bond Angle: 90° • Hybrid Orbitals: sp³d²

  12. Hybridization • Hybridization: A process in which atomic orbitals are mixed to form new, identical hybrid orbitals • Carbon is the most common • The number of hybrid orbitals = the number of total pairs of electrons

  13. Homework • 54-59 on page 262

More Related