10.50. What hybrid orbitals would be expected for the central atom in each of the following molecules or ions? a. PCl3 b. SiCl4 c. BeF2 d. SO2 10.52. a. Nitrogen trifluoride, NF3, is a relatively unreactive, colorless gas. How would you describe the bonding in the NF3 molecule in terms of valence bond theory? Use hybrid orbitals. b. Silicon tetrafluoride, SiF4 ‍, is a colorless gas formed when hydrofluoric acid attacks silica (SiO2)‍ or glass. Describe the bonding in the ‍ SiF4 molecule, using valence bond theory. 10.57. Describe the electronic structure of each of the following, using molecular orbital theory. Calculate the bond order of each and decide whether it should be stable. For each, state whether the substance is diamagnetic or paramagnetic. a. Be2 b. He2+ c. N2- 10.58. Use molecular orbital theory to describe the bonding in the following. For each one, find the bond order and decide whether it is stable. Is the substance diamagnetic or paramagnetic? a. C2+ b. Be2+ c. Ne2