1. The problem statement, all variables and given/known data 2Ag2S(s) + O2(g) = Ag2O(s) + S(s) Which is being oxidized? 2. Relevant equations N/a 3. The attempt at a solution Reactants: Ag2S is neutral, with Ag having +1 charge and S having 2- charge. O2 is neutral Products: Ag2O is neutral, with Ag having a 1+ charge and O having -2 charge. S is neutral. So: Reactants and products have the same net charge? But, S when from 2- to 0 charge. Therefore, it was oxidized (gained two electrons). Oxygen went form 0 to 2-. So, it was reduced. Ag stayed the same. 1+ to 1+. But, I read that Ag is actually being oxidized. I'm not really sure what's happening.