See the answer below.
Work Step by Step
a) $F.\ Charge= NVE-LPE-BE/2$ In both cases: $6-4-4/2=0$ b) Angle 1: 109°, bent geometry from the tetrahedral archetype (2 ligands, 2 lone pairs) Angle 2: 109°, tetrahedral geometry (4 ligands, no lone pairs) Angle 2: 120°, trigonal planar geometry (3 ligands, no lone pairs) c) The two C=C bonds because bond length decreases with bond order. d) Both C-O bonds because they have the biggest difference in electronegativity. e) The molecule is polar because it has asymetrical polar bonds. f) To maintain the tetrahedral shape with the lone electron pairs, the oxygen must be above the carbons' plane.