Silver plating on copper occurs when copper is oxidized and acts as the reducing agent. Which statement correctly describes the plating process?

• A. Copper is reduced and is the oxidizing agent
• B. Copper is reduced and is the reducing agent
• C. Copper is oxidized and is the oxidizing agent
• D. Copper is oxidized and is the reducing agent

Answer: (D)

In this silver plating scenario, copper metal donates electrons to silver ions, so copper is oxidized and acts as the reducing agent. In redox terms, the reducing agent is the species that loses electrons, and it becomes oxidized. Here, copper loses electrons to form Cu2+ in solution, while Ag+ gains those electrons and is reduced to metallic silver that deposits on the copper surface. That’s why the statement describing copper as being oxidized and functioning as the reducing agent is correct. If copper were reduced, it would gain electrons instead, which would not drive the deposition of silver. If copper were the oxidizing agent, it would be accepting electrons and being reduced, which also doesn’t match the observed plating process.