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Molecular Molecular ShapeShape
Section 9.4Section 9.4
ChemistryChemistry
ObjectivesObjectives• Discuss the VSEPR bonding theory• Predict the shape of and the bond
angles in a molecule• Define hybridization
The Shape of MoleculesThe Shape of Molecules• The shape of molecules determines
reaction ability• The model we use is the VSEPR
model– Valence Shell Electron Pair Repulsion
VSEPR ModelVSEPR 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 ShapeLinear Molecular Shape
• Example: BeCl2• Total Pairs of Electrons: 2• Shared Pairs of Electrons: 2• Lone Pairs: 0• Bond Angle: 180°• Hybrid Orbitals: sp
Trigonal PlanarTrigonal Planar
• Example: AlCl3• Total Pairs of Electrons: 3• Shared Pairs of Electrons: 3• Lone Pairs of Electrons: 0• Bond Angle: 120°• Hybrid Orbitals: sp²
TetrahedralTetrahedral
• 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 PyramidalTrigonal 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
BentBent
• 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 BipyramidalTrigonal 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
OctahedralOctahedral
• Example: SF6
• Total Pairs of Electrons: 6• Shared Pairs of Electrons: 6• Lone Pairs of Electrons: 0• Bond Angle: 90°• Hybrid Orbitals: sp³d²
HybridizationHybridization• 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
HomeworkHomework• 54-59 on page 262