In the following redox reaction, which species has lost electrons (i.e., has been oxidized)?Zn(s) + Cu^{2+}(aq) ightarrow Zn^{2+}(aq) + Cu(s)

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

Answer: (A)

Verified step by step guidance

1. Identify the oxidation states of each species before and after the reaction. For Zn(s), the oxidation state is 0 because it is in elemental form. For Cu^{2+}(aq), the oxidation state is +2 as indicated by the charge.
2. Determine the oxidation states of the products. Zn^{2+}(aq) has an oxidation state of +2, and Cu(s) has an oxidation state of 0 because it is elemental copper.
3. Compare the oxidation states of each element from reactants to products. Zinc changes from 0 to +2, indicating it loses electrons. Copper changes from +2 to 0, indicating it gains electrons.
4. Recall that oxidation is the loss of electrons, and reduction is the gain of electrons. Since zinc's oxidation state increases, it has lost electrons and is oxidized.
5. Conclude that Zn(s) is the species that has been oxidized in this redox reaction.