[Chris11]

Hello! I am preparing a project for chemistry class and got a little confused.

I know that sulfur's got 3 possible oxidation numbers, II-, IV+ and VI+.
If we look at the electron configuration of sulfur, the ox. nr. II- can be explained very easily (two electrons remain to achieve the stabilised ox. nr. 0)

But I can't explain the excited states! S* equals ox. nr. IV+ and S** equals ox. nr. VI+? Why?! I understand how excitation works, but the "how many electrons remain to ox. nr. 0" method doesn't work here anymore! Also, why is the ox. number + all of a sudden? Does this have to do something with the d orbital?

Thank you in advance!