In cell notation, which of the following correctly represents a galvanic cell where zinc metal is oxidized and copper(II) ion is reduced?

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

Answer: (D)

Verified step by step guidance

1. Recall that in cell notation for galvanic cells, the anode (where oxidation occurs) is written on the left, and the cathode (where reduction occurs) is written on the right.
2. Identify the species undergoing oxidation and reduction: Zinc metal (Zn) is oxidized to Zn^{2+} ions, and copper(II) ions (Cu^{2+}) are reduced to copper metal (Cu).
3. Write the anode half-cell on the left side: since Zn is oxidized, write Zn(s) | Zn^{2+}(aq).
4. Write the cathode half-cell on the right side: since Cu^{2+} is reduced, write Cu^{2+}(aq) | Cu(s).
5. Separate the two half-cells with a double vertical line '||' to represent the salt bridge or membrane separating the two solutions, resulting in the cell notation: \(Zn(s) | Zn^{2+}(aq) || Cu^{2+}(aq) | Cu(s)\).