Consider the following half-reactions: Half-reaction E° (V) I2 (s) + 2e - 2I - (aq) 0.535V 2H + (aq) + 2e - H2 (g) 0.000V Zn2 + (aq) + 2e - Zn (s) - 0.763V (1) The weakest oxidizing agent is: Zn2 + (aq) enter formula (2) The strongest reducing agent is: Zn (s) (3) The strongest oxidizing agent is: I2 (s) (4) The weakest reducing agent is: I - (aq) (5) Will I - (aq) reduce Zn2 + (aq) to Zn (s) ? (6) Which species can be reduced by H2 (g) ? If none, leave box blank.

The weakest oxidizing agent is Zn^2 + (aq)

The strongest reducing agent is Zn (s)

The strongest oxidizing agent is I2 (s)

The weakest reducing agent is I^ - (aq)

I^ - cannot reduce Zn^2 + to Zn (s)

I2 (s) can be reduced by hydrogen gas

Explanation:

In looking at oxidizing and reducing agents, our primary guide is the reduction potentials of each specie. The more negative the reduction potential of a specie, the better its function as a reducing agent. Zn has a very negative reduction potential hence it a very good reducing agent. Similarly, iodine has a very positive reduction potential hence it is a good oxidizing agent.

Only a specie having a more negative reduction potential than zinc can reduce it in aqueous solution. Similarly, the reaction potential of hydrogen is less than that of iodine hence hydrogen gas can reduce iodine.