Chapter 9 Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals - Study Questions - Page 369a: 8

See the answer below.

a) Two double bonds, no lone pairs: linear geometry, $sp$ hybridization. b) One double and one single bonds, one lone pair: bent geometry, $sp^2$ hybridization. c) One double and two single bonds, no lone pairs: trigonal planar geometry, $sp^2$ hybridization. d) Four single bonds, no lone pairs: tetrahedral geometry, $sp^3$ hybridization.