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+?