Describe the redox reaction. check all that apply 2ai(s) + 3znci2(g) → 3zn(s) + 2aici3(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.

Zinc is reduced.

The oxidation number of chlorine does not change.

Aluminum is oxidized.

Explanation:

2AI(s) + 3ZnCI₂(g) → 3Zn(s) + 2AICI₃(aq).

Al has (0) oxidation state and converted to (+3) oxidation state in the products (AlCl₃), which means Al is oxidized and it is the reducing agent.

So, we can check that: Aluminum is oxidized.

Zn has the oxidation state (+2) in the reactants side (ZnCl₂) and converted to (0) in the products side (Zn), which means that Zn is reduced and it is the oxidizing agent.

So, we can check that: Zinc is reduced.

and can not check: Zinc is the reducing agent.  

The oxidation state of Cl does not change, it is the same in both sides (-1).

So, we can check: The oxidation number of chlorine does not change.

and can not check: Aluminum atoms transfer electrons to chlorine atoms.

Zinc is reduced.

The oxidation number of chlorine does not change.

Aluminum is oxidized.

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