Complete the Lewis structures of the following molecules. Predict the molecular structure, polarity, bond angles, and hybrid orbitals used by the atoms marked by asterisks for each molecule. a. \(\mathrm{BH}_{3}\) a. \(\mathrm{BH}_{3}\) b. \(\mathrm{N}_{2} \mathrm{F}_{2}\) c. \(\mathrm{C}_{4} \mathrm{H}_{6}\)

a. BH₃: Lewis structure is B surrounded by three H atoms in a trigonal planar geometry. The molecule is nonpolar with bond angles of 120° and uses sp² hybrid orbitals for B. b. N₂F₂: Lewis structure has two N atoms connected by a double bond and each N atom bonded to an F atom. The molecule is nonpolar with bond angles of 180° and uses sp² hybrid orbitals for N atoms. c. C₄H₆: Lewis structure forms a cyclic triangle with three C atoms and one triple bond between the first and third C atom. The molecule is nonpolar with bond angles of approximately 60° in the cyclic part. The carbon atoms in the cycle use sp² hybrid orbitals, while the carbon atom with the triple bond uses sp hybrid orbitals.