6L7 7th Ed

[Summer de Vera 2C]

Hi! Why is it that for a), Ag is the one being reduced while Br is used for the oxidation reaction? Isn't it being oxidized because it's going from AgBr(s) --> <-- Ag+(aq) + Br-?

[LorenzoDuvergne3I]

Hi,
I'm having issues with this problem as well. I think it has to do with the fact that if you add an electron to AgBr, Br is the one more likely to receive it since it's a halogen and thus more electronegative. If you flip that reaction, you have an oxidation reaction where Ag loses an electron. I suppose that you have to also reduce Ag to make it a redox reaction?? I'm really not sure..