Oxidizing Agent, TPR G-Chem

Hi everyone,

I thought I understood oxidation, reduction, oxidation agents and reduction agents (I've been searching for explanations in reddit, bless) but this question threw me for a loop.

On page 468, example 10-9 asks "of the following, which is the strongest oxidizing agent?"

A. Al3+

B. Ag+

C. Au3+

D Cu2+

Why is the answer C and not A? I thought you had to go into the table and look up the half reactions and then reverse the charge on the volts because it is asking for the oxidizing agent?

For reference the table is:

Reactions Volts

Li+ +e- --> Li = -3.05V

Mg2+ +2e- --> Mg = -2.36V

A13+ +3e- --> Al = -1.67V

Zn2+ +2e- --> Zn = -0.76V

Fe2+ +2e- --> Fe = -0.44V

Pb2+ + 2e- --> Pb = -0.13V

2H+ +2e- --> H2 = 0.00V

Cu2+ +2e- --> Cu = 0.34V

Ag+ +e- --> Ag = 0.80V

Pd2+ +2e- --> Pd = 0.99V

Pt2+ + 2e- --> Pt = 1.20V

Au3+ +3e- --> Au = 1.50V

F2 +2e- --> 2FE- = 2.87V

Thanks so much!

edit; formatting, grammar and because I wrote the answer wrong lol.