In the redox reaction: Zn(s) + Cu^{2+}(aq) → Zn^{2+}(aq) + Cu(s), which compound is oxidized?

• A. Zn^{2+}(aq)
• B. Zn(s)
• C. Cu^{2+}(aq)
• D. Cu(s)

Answer: (B)

Verified step by step guidance

1. Identify the species that undergoes oxidation and reduction by examining the changes in oxidation states of the elements involved in the reaction.
2. Write down the oxidation states of each element before and after the reaction: Zn(s) starts with an oxidation state of 0, and Zn^{2+}(aq) has an oxidation state of +2; Cu^{2+}(aq) starts with +2, and Cu(s) ends with 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 Zn goes from 0 to +2, it loses two electrons and is oxidized. Cu goes from +2 to 0, gaining two electrons and is reduced.
5. Conclude that Zn(s) is the compound that is oxidized in this redox reaction.