Which of the following statements is correct for the galvanic cell?

The half-cell in which oxidation takes place is called anode and has a negative potential with respect to the solution.

The correct answer is Option (1) → The half-cell in which oxidation takes place is called anode and has a negative potential with respect to the solution.

Core Concept

In a galvanic cell:

Oxidation occurs at anode

Reduction occurs at cathode

Anode develops negative potential

Cathode develops positive potential

This happens due to electron flow generated by spontaneous redox reaction.

Explanation of Option 1

This statement is correct.

At anode, oxidation occurs: $Zn → Zn^{2+} + 2e^-$

Electrons are produced at anode, making it electron-rich. Because of excess electrons, anode becomes negatively charged relative to the solution. Hence, oxidation at anode and negative potential is the correct relationship.

Explanation of Option 2

This statement is incorrect.

Although it correctly states that oxidation occurs at anode, it wrongly assigns positive potential to the anode. In galvanic cells, anode always becomes negative because electrons are released there. Positive potential is associated with cathode, not anode. Therefore, this option is wrong due to incorrect electrode polarity.

Explanation of Option 3

This statement is incorrect.

Reduction does occur at cathode: $Cu^{2+}+2e^-→Cu$

But cathode becomes electron-deficient since electrons are consumed. Hence, cathode develops positive potential relative to the solution. The option incorrectly states that cathode has negative potential. Thus, the polarity mentioned here is wrong.

Explanation of Option 4

This statement is incorrect.

Reduction occurs at cathode, not anode. This option wrongly assigns reduction to anode. Although it mentions negative potential correctly for anode, the reaction type assigned is incorrect. Therefore, this statement is conceptually incorrect.