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 Valence Shell Electron Pair Repulsion
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
Linear Molecular Shape Example: BeCl2 Total Pairs of Electrons: 2 Shared Pairs of Electrons: 2 Lone Pairs: 0 Bond Angle: 180° Hybrid Orbitals: sp
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
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
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
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
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
Octahedral Example: SF6 Total Pairs of Electrons: 6 Shared Pairs of Electrons: 6 Lone Pairs of Electrons: 0 Bond Angle: 90° Hybrid Orbitals: sp³d²
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
Homework 54-59 on page 262