which is capable of oxidizing Cu (s) to Cu+2 (aq) when added to Cu (s) in solution?
A. Al+3 (aq)
B. Ag+ (aq)
C. Ni (s)
D. I- (aq)
E. Au+3 (aq)
Answer: B
I chose D. at first because of the negative charge wanting to take H's but that is wrong because negative charge means it already has extra electrons so I would need to pick something very positive. So my second answer choice after I figured out the mistake I made was choice Al+3 over Au+3 but i am not sure exactly why.
I do know oxidizing agent is something that will become reduced, but how do you figure this one out? Do I need to memorize reduction potentials?
Any ideas, can someone guide me through this please?
I wanted to add, I think I know why it is Ag+ because it is 4d10 electron configuration so taking 2 from Cu it will fill its shell to 4d105s2 so the s2 is complete. I think this is the special trend with this element where the d orbital will fill to 10 and the s will be 1 instead of 4d9s2 Cr and Mo do something similar instead of 3d4s2 its 3d5s1 the exception is Cr, Mo, Cu, Ag and Au