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In the chemical reaction Zn + CuSO4 → ZnSO4 + Cu, which substance is being oxidized?
Zn
CuSO4
ZnSO4
Cu
Zn
Zinc (Zn) is oxidized because its oxidation state increases from 0 in elemental form to +2 in zinc sulfate, corresponding to the loss of electrons. Oxidation is fundamentally defined as the loss of electrons or an increase in oxidation number.
Zinc (Zn) is oxidized because its oxidation state increases from 0 in elemental form to +2 in zinc sulfate, corresponding to the loss of electrons. Oxidation is fundamentally defined as the loss of electrons or an increase in oxidation number.
Oxidation is like an electron donor parting with cash (electrons), resulting in a deficit of negative charge and a higher positive state.
OIL RIG (Oxidation Is Loss, Reduction Is Gain)
Zn→Zn2++2e− — Oxidation half-reaction
Cu2++2e−→Cu — Reduction half-reaction
Zinc atoms transfer two valence electrons to copper(II) ions (Cu2+) in solution, forming Zn2+ ions that dissolve as ZnSO4. The oxidation half-reaction is given by Zn→Zn2++2e−.
Oxidation number of Zn changes from 0 to +2.
Copper(II) is reduced from +2 to 0.
This is a single-displacement redox reaction driven by the electrochemical series.
Galvanic cell operations
Metal displacement and extraction processes
Zn acts as the reducing agent while CuSO4 acts as the oxidizing agent.
Option B (CuSO4) is the oxidizing agent, not the substance oxidized.
Option C (ZnSO4) is the reaction product.
Option D (Cu) is the reduced product.
A is correct — Zinc (Zn) is oxidized as it loses 2 electrons and its oxidation state increases from 0 to +2.
In metal displacement reactions, the more reactive metal higher in the electrochemical series undergoes oxidation and displaces the less reactive metal ion.
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