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In the reaction Zn + CuSOтВД тЖТ ZnSOтВД + Cu, which substance is oxidized?
Zn
CuSO4
ZnSO4
Cu
Zn
In the given displacement reaction, zinc (Zn)loses two electrons to form zinc ions (Zn2+),thereby increasing its oxidation state from 0 to +2. Since oxidation is defined as the loss of electrons or an increase in oxidation state, zinc is the substance that gets oxidized.
In the given displacement reaction, zinc (Zn)loses two electrons to form zinc ions (Zn2+),thereby increasing its oxidation state from 0 to +2. Since oxidation is defined as the loss of electrons or an increase in oxidation state, zinc is the substance that gets oxidized.
Think of zinc as a generous donor giving away two items (electrons) to become more positive, while copper accepts them. The one giving away the items undergoes oxidation.
OIL RIG: Oxidation Is Loss, Reduction Is Gain (of electrons).
Zn\rightarrow Zn2++2eтБ╗ тАФ Oxidation half-reaction
Cu2++2eтБ╗ \rightarrow CuтАФReduction half-reaction
This is a classic redox (reduction-oxidation) reaction, specifically a single displacement reaction. Zinc is a more reactive metal than copper and displaces copper ions (Cu2+)from the copper sulfate solution. The oxidation half-reaction is Zn\rightarrow Zn2++2eтБ╗, making zinc the reducing agent.
Oxidation is characterized by the loss of electrons and an increase in oxidation state.
A more reactive metal displaces a less reactive metal from its salt solution.
The substance oxidized always acts as the reducing agent in the reaction.
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Option B (CuSOтВД) contains copper in the +2 oxidation state, which gets reduced to metallic copper, making it the oxidizing agent.
Option D (Cu) is the final reduced product of the reaction.
A is correct тАФ Zinc (Zn)undergoes oxidation by losing electrons and increasing its oxidation state from 0 to +2.
Always refer to the metal reactivity series for displacement reactions to instantly identify the more reactive metal, which will always be the one that undergoes oxidation.
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