Half-cell potential??? According to an online chemistry website ( www.chem1.com) If the half-cell potential for Zn/Zn+ electrode is defined as the potential difference between a piece of metallic zinc and the solution when the reaction Zn2+ + 2e- -> Zn (s) takes place. That is E cell = V metal - V solution What does this means? Is the metal referring to the electrode and the solution referring to the Zn2+??? If it is so, then why do half cells with higher potential difference undergo reduction more readily than half cells with lower potential difference? I mean the potential difference is supposed to be associated with positive charges, right? So if one thing has higher potential, then positive charges would want to move to another thing with fewer amount of positive charges. That, in reality, means that the e- would flow from Ag+ to Ag. Which is not the usual case??? Could anyone help me with this? I understand that in the activity series, we're comparing the performance of each species to those of Hydrogen, so the higher the potential, the better electron acceptor it will be. But what about this potential thingy?? Thanks!