14.2 Hybridization (Chemistry)
Reason for Hybridization
Atom can form stronger covalent bonds with greater overlap, due to different energies, shapes, orientation
Evidence of Hybridization
Carbon has one 's' orbital and 3 'p' orbitals (slightly higher energy) but all bonds are equal (e.g. in CH4) suggesting hybridization for equal energy for all orbitals
Lone Pairs and Hybridization
Lone pairs are also involved in hybridization, e.g. NH₃ has sp³ hybridization with 3 bonding and 1 lone pair
Hybridization
Mixing of atomic orbitals to form new hybrid atomic orbitals of intermediate energy
sp Hybridization
One 's' and one 'p' orbital hybridize into two 'sp' and two unhybridized 'p' orbitals
sp³ Hybridization
One 's' and three 'p' orbital hybridize into four 'sp' orbitals
sp² Hybridization
One 's' and three 'p' orbital hybridize into three 'sp²' and one unhybridized 'p' orbital
sp³ Geometry
Orbitals orientate at 109.5°, tetrahedral molecular geometry, overlap of each hybrid orbital forms 4σ bonds, e.g. CH₄
sp² Geometry
Orbitals orientate at 120°, trigonal planar molecular geometry, overlap of each hybrid orbital forms 3σ bonds, e.g. C₂H₄
sp Geometry
Orbitals orientate at 180°, linear molecular geometry, overlap of each hybrid orbital forms 2σ bonds, e.g. C₂H₂