Question

Describe the redox reaction. Check all that apply.

Upper A l (s) plus 3 upper Z n upper C l subscript 2 (g) right arrow 3 upper Z n (s) plus 2 upper A l upper C l subscript 3 (a q).


Aluminum atoms transfer electrons to chlorine atoms.

Zinc is reduced.

Zinc is the reducing agent.

The oxidation number of chlorine does not change.

Aluminum is oxidized.

Answer 1

First correct the balanced equation (for electron bookkeeping):
2 Al(s) + 3 ZnCl2 → 3 Zn(s) + 2 AlCl3

Now evaluate each statement:

- "Aluminum atoms transfer electrons to chlorine atoms." — False. Aluminum loses electrons (is oxidized) and those electrons reduce Zn2+ to Zn0, not chlorine. Chloride stays Cl−.

- "Zinc is reduced." — True. Zn goes from +2 in ZnCl2 to 0 in Zn(s).

- "Zinc is the reducing agent." — False. A reducing agent is oxidized; zinc is reduced here, so zinc is the oxidizing agent.

- "The oxidation number of chlorine does not change." — True. Cl is −1 in both ZnCl2 and AlCl3.

- "Aluminum is oxidized." — True. Al goes from 0 to +3 (loses electrons).