Chapter 10, Problem 10.102QP

Solid sulfur normally consists of crystals of S₈ molecules, but when heated strongly, the solid vaporizes to give S₂ molecules (among other molecular species). Describe the bonding in S₂ in molecular orbital terms, assuming the orbitals are analogous to those of the preceding period. What would you expect to happen to the sulfur sulfur bond length if two electrons were added to give the S₂²⁻ ion? What would you expect to happen to the bond length if, instead, two electrons were taken away to give S₂²⁺?