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Molecular Shape Section 9.4

Explore VSEPR theory, predict molecule shapes & bond angles, define hybridization, identify key molecular shapes including Linear, Trigonal Planar, Tetrahedral, and more. Complete homework exercises from page 262.

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Molecular Shape Section 9.4

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  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

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