2Cu2+ + 2S2- --> 2Cu+ + 2S- --> 2Cu+ + (S2)2-In this process the one missing d-electron ("hole") of the d9 configuration is transferred to the sulfur. Sometimes that leads to sulfur pair formation sometimes not.
The result is that Cu is essentially monovalent in all these compounds. What lies near the Fermi level is a valence band predominantly S 2p character
Most of them are metallic because if the pairformation is incomplete the remaining holes in the valence band lead to metallic conductivity. E.g. in CuS only two thirds of the sulfurs occur as pairs (disulfide ions).
CuS2 is a special case. It has the pyrite structure. In this structure all sulfurs occur as pairs (disulfide ions). However because Cu is essentially Cu+, the disulfide ions are essentially (S-S)-1 rather than (S-S)-2. In other words there is an extra hole on the disulfide ion. As it is delocalized, this pyrite is metallic. By contrast the mineral pyrite FeS2 consists of Fe2+ ions and (S-S)-2 ions and is a semiconductor.