Answer:
Zinc is reduced.
The oxidation number of chlorine does not change.
Aluminum is oxidized.
Explanation:
<em>2AI(s) + 3ZnCI₂(g) → 3Zn(s) + 2AICI₃(aq). </em>
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- For the elements in the reactants side:
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.
<em>and can not check: Zinc is the reducing agent. </em>
<em />
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.
<em>and can not check: Aluminum atoms transfer electrons to chlorine atoms. </em>
<em />
<em>Zinc is reduced.</em>
<em>The oxidation number of chlorine does not change.</em>
<em>Aluminum is oxidized. </em>
