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**Molecular Shape Section 9.4**

Chemistry

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**Objectives Discuss the VSEPR bonding theory**

Predict the shape of and the bond angles in a molecule Define hybridization

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

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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

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**Linear Molecular Shape**

Example: BeCl2 Total Pairs of Electrons: 2 Shared Pairs of Electrons: 2 Lone Pairs: 0 Bond Angle: 180° Hybrid Orbitals: sp

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**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

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**Tetrahedral Example: CH4 Total Pairs of Electrons: 4**

Shared Pairs of Electrons: 4 Lone Pairs of Electrons: 0 Bond Angle: ° Hybrid Orbitals: sp³

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**Trigonal Pyramidal Example: PH3 Total Pairs of Electrons: 4**

Shared Pairs of Electrons: 3 Lone Pairs of Electrons: 1 Bond Angle: ° Hybrid Orbitals: sp³

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**Bent Example: H2O Total Pairs of Electrons: 4**

Shared Pairs of Electrons: 2 Lone Pairs of Electrons: 2 Bond Angle: ° Hybrid Orbitals: sp³

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**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

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**Octahedral Example: SF6 Total Pairs of Electrons: 6**

Shared Pairs of Electrons: 6 Lone Pairs of Electrons: 0 Bond Angle: 90° Hybrid Orbitals: sp³d²

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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

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Homework 54-59 on page 262

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