The figure shows a galvanic cell.As the cell works, which electrode l…

The correct answer is Option (2) → Zinc, because zinc atoms are oxidised and pass into the solution as Zn²⁺ ions

The arrow in the figure shows electrons flowing from the zinc rod to the copper rod in the external circuit. Electrons leave the electrode at which oxidation occurs, so zinc atoms are oxidised and pass into the solution as Zn²⁺ ions, and the zinc electrode loses mass. At the copper electrode, Cu²⁺ ions take up these electrons and are deposited as copper.

    Zinc electrode: \( \ce{Zn(s) -> Zn^2+ + 2e^-} \)

    Copper electrode: \( \ce{Cu^2+ + 2e^- -> Cu(s)} \)

Why the other options are incorrect

Option (1) Copper, because Cu²⁺ ions from the solution are deposited on it — Incorrect. Deposition of Cu²⁺ ions adds mass to the copper electrode; it does not remove it.

Option (3) Copper, because copper atoms are oxidised and pass into the solution as Cu²⁺ ions — Incorrect. Electrons flow towards copper, so reduction, not oxidation, occurs on the copper electrode, and it gains mass.

Option (4) Zinc, because Zn²⁺ ions from the solution are deposited on it — Incorrect. Zn²⁺ ions are formed at the zinc electrode; they are not deposited on it.

NCERT (2026-27 edition):
2.2 Galvanic Cells – “…This reaction is a combination of two half reactions whose addition gives the overall cell reaction:”

    (i) Cu²⁺ + 2e^– → Cu(s)    (reduction half reaction)    (2.2)

    (ii) Zn(s) → Zn²⁺ + 2e^–    (oxidation half reaction)    (2.3)

“These reactions occur in two different portions of the Daniell cell. The reduction half reaction occurs on the copper electrode while the oxidation half reaction occurs on the zinc electrode.”

Fig. 2.1: Daniell cell having electrodes of zinc and copper dipping in the solutions of their respective salts.