In the reaction 2Al(s) + 3Br2(g) → 2AlBr3(s), which element is oxidized and which is reduced?

• A. Both Al and Br2 are reduced.
• B. Both Al and Br2 are oxidized.
• C. Al is reduced; Br2 is oxidized.
• D. Al is oxidized; Br2 is reduced.

Answer: (D)

Verified step by step guidance

1. Identify the oxidation states of each element in the reactants and products. For aluminum (Al) in its elemental form, the oxidation state is 0. For bromine (Br2) as a diatomic molecule, the oxidation state is also 0.
2. Determine the oxidation states of the elements in the product, aluminum bromide (AlBr3). Aluminum typically has an oxidation state of +3 in compounds, and bromine typically has an oxidation state of -1.
3. Compare the oxidation states of aluminum from reactants to products. Aluminum goes from 0 to +3, which means it loses electrons and is oxidized.
4. Compare the oxidation states of bromine from reactants to products. Bromine goes from 0 to -1, which means it gains electrons and is reduced.
5. Conclude that aluminum is oxidized and bromine is reduced in the reaction, matching the correct answer: Al is oxidized; Br2 is reduced.