Final answer:
The reaction provided signifies a voltaic (or galvanic) cell where zinc reacts at the anode, making option 3) voltaic; zinc the correct answer.
Step-by-step explanation:
The given reaction is characteristic of a voltaic (or galvanic) cell, which operates based on a spontaneous redox reaction. In the described scenario between metallic zinc and cupric ions, zinc is the metal that will react at the anode. The reaction Zn(s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu(s), shows zinc being oxidized to Zn²⁺ ions while copper ions are reduced to copper metal. Thus, in this voltaic cell, the zinc electrode serves as the anode and undergoes oxidation.
As the reaction progresses, the mass of the zinc anode will decrease due to its dissolution into solution, while the copper cathode gains mass as the Cu²⁺ ions in solution are reduced and deposited onto the copper electrode. Since we know this cell is a voltaic cell and zinc is the metal at the anode, the correct answer for the student's question would be option 3) voltaic; zinc.