# Oxidation Half Reaction Chemistry

I was always confused as to how electrons where donated from the anode in a galvanic cell. But after doing research, I found that there are four fundamental ways as to where electrons in anodic transformations can come from:

1) Surface metal atoms

2) Solvent molecules

3) Electrolyte anions

4)Base ligands

My question is how do I know from these four options, which is providing the electron?

As an example, consider the reaction, what is the oxidation number of sulfur in this particular molecule, $S_2O_3$. According to these rules, which are in order of priority, the oxidation number of oxygen is $-2$, unless it is bonded with hydrogen or fluorine, which in this case, it is not. Given that we have three oxygen atoms in this molecule, the total oxidation of oxygen is $-6$, which must be offset by two sulfur atoms so the total oxidation number is $0$. Obviously, the oxidation number of a single sulfur must then be $+3$, so that the molecule is neutral.