describe the redox reaction. check all that apply. 2al(s) + 3zncl₂(g) → 3zn(s) + 2alcl₃(aq) aluminum atoms…

describe the redox reaction. check all that apply. 2al(s) + 3zncl₂(g) → 3zn(s) + 2alcl₃(aq) 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. done

describe the redox reaction. check all that apply. 2al(s) + 3zncl₂(g) → 3zn(s) + 2alcl₃(aq) 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. done

Answer

Brief Explanations:

  1. In the reaction (2Al(s)+3ZnCl_{2}(g)\rightarrow3Zn(s) + 2AlCl_{3}(aq)), aluminum ((Al)) goes from an oxidation - state of 0 to +3 in (AlCl_{3}), so aluminum is oxidized. Oxidation is the loss of electrons.
  2. Zinc ((Zn)) goes from an oxidation - state of +2 in (ZnCl_{2}) to 0 in (Zn), so zinc is reduced. Reduction is the gain of electrons.
  3. The reducing agent is the substance that causes reduction by losing electrons. Here, aluminum is the reducing agent as it donates electrons.
  4. Chlorine ((Cl)) has an oxidation - state of -1 in both (ZnCl_{2}) and (AlCl_{3}), so its oxidation number does not change. Also, aluminum atoms transfer electrons to zinc ions, not chlorine atoms.

Answer:

B. Zinc is reduced. D. The oxidation number of chlorine does not change. E. Aluminum is oxidized.