In the reaction cu(s) + ag^+(aq) → cu^+(aq) + ag(s), which metal is being oxidized?

• A. Both copper and silver
• B. Neither copper nor silver
• C. Copper (Cu)
• D. Silver (Ag)

Answer: (C)

Verified step by step guidance

1. Identify the oxidation states of the elements before and after the reaction. Copper (Cu) starts as a solid metal with an oxidation state of 0, and silver ion (Ag^+) starts with an oxidation state of +1 in aqueous solution.
2. Look at the products: copper ion (Cu^+) is in aqueous solution with an oxidation state of +1, and silver (Ag) is a solid metal with an oxidation state of 0.
3. Determine which element loses electrons (oxidation) and which gains electrons (reduction). Oxidation involves an increase in oxidation state, while reduction involves a decrease.
4. Since copper goes from 0 to +1, it loses one electron and is oxidized. Silver goes from +1 to 0, gaining one electron and is reduced.
5. Conclude that copper is the metal being oxidized in this reaction because its oxidation state increases.