Standard electrode potential values can be used to judge the reducing ability of a metal. When I was introduced to this topic a simple picture was painted: you put a metal into a solution of its ions. An equilibrium is set up. You do so for another metal. If you now hook up the two electrodes and measure the voltage, you can tell which one is 'more negative' hence more electron donating.
My question is that suppose we have two metals, A and B. A produces +1 ions. B produces +2 ions.
A ---> A(+1) + e
B ---> B(2+) + 2e
Suppose these two processes have the same tendency ( it is just as energetically feasible for both to form their respective ions) So in a half-cell of B and its ions, plate B should be more negatively charged compared to plate A in its own half cell. Charge should flow from B to A in the external circuit. The electrode potentials will be different when measured practically. I think this is all true and fine. Now, we can use electrode potentials to tell us about the relative ability of a metal to lose or gain electrons. But in this case, the difference isn't due to a tendency difference: only the number of electrons is different.
How does this line up with the oft-taught idea that we can use reduction potentials to judge the ability to gain or lose?
I am aware I've asked a similar question, but apparently, I did not realize my wording was off and then it was too late to edit it all out