Problem

Consider the general oxidation of a species A in solution: A→ A+ + e-. The term oxidation...

Consider the general oxidation of a species A in solution: A→ A+ + e-. The term oxidation potential is sometimes used to describe the ease with which species A is oxidized—the easier a species is to oxidize, the greater its oxidation potential.

(a) What is the relationship between the standard oxidation potential of A and the standard reduction potential of A+? (b) Which of the metals listed in Table has the highest standard oxidation potential? Which has the lowest?

Table Activity Series of Metals in Aqueous Solution

Metal	Oxidation Reaction
Lithium	Li(s) → Li+(aq)+ e-
Potassium	K(s) → K+(aq)+ e-
Barium	Ba(s) → Ba2+(aq)+ 2e-
Calcium	Ca(s) → Ca2+(aq)+ 2e-
Sodium	Na(s) → Na+(aq)+ e-
Magnesium	Mg(s) → Mg2+(aq)+ 2e-
Aluminum	Al(s) → Al3+(aq)+ 3e-
Manganese	Mn(s) → Mn2+(aq)+ 2e-
Zinc	Zn(s) → Zn2+(aq)+ 2e-
Chromium	Cr(s) → Cr3+(aq)+ 3e-
Iron	Fe(s) → Fe2+(aq)+ 2e-
Cobalt	Co(s) → Co2+(aq)+ 2e-
Nickel	Ni(s) → Ni2+(aq)+ 2e-
Tin	Sn(s) → Sn2+(aq)+ 2e-
Lead	Pb(s) → Pb2+(aq)+ 2e-
Hydrogen	H2(g) → 2 H+(aq) + 2e-
Copper	Cu(s) → Cu2+(aq)+ 2e-
Silver	Ag(s) → Ag+(aq)+ e-
Mercury	Hg(l) → Hg2+(aq)+ 2e-
Platinum	Pt(s) → Pt2+(aq)+ 2e-
Gold	Au(s) → Au3+(aq)+ 3e-

(c) For a series of substances, the trend in oxidation potential is often related to the trend in the first ionization energy. Explain why this relationship makes sense.