Howdy. I'm looking at a mercury battery reaction which goes like so: HgO(l) + Zn(s) --> ZnO(s) + Hg(l) I need to figure out the oxidation half reaction. What I can tell so far is that Zn is oxidized, since on the reactant side it has a charge of zero, and on the product side, Zn has an individual charge of 2+ in the ZnO compound. It must be losing electrons. I believe the oxidation half reaction should have Zn on the reactant side and ZnO and some electrons (two?) on the product side, but I can't figure out how to work in the oxygen for the reactant side. Sorry, I'm totally new at this. And I kinda suck at it besides. Any help is appreciated. Thanks in advance!