Multiple Choice
In redox reactions, why is the term 'reduction' used to describe the gain of electrons by a species?
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6. Chemical Quantities & Aqueous Reactions
Redox Reactions
Multiple Choice
Which of the following equations describes a reduction process?
A
Fe^{3+} + e^- ightarrow Fe^{2+}
B
Zn ightarrow Zn^{2+} + 2e^-
C
Cu^{2+} ightarrow Cu + 2e^-
D
Cl_2 ightarrow 2Cl^- + 2e^-
Verified step by step guidance1
Understand that a reduction process involves the gain of electrons by a species, which decreases its oxidation state.
Examine each equation to identify whether electrons are on the reactant side (indicating gain of electrons) or on the product side (indicating loss of electrons).
For the equation \(Fe^{3+} + e^- \rightarrow Fe^{2+}\), note that an electron is added to \(Fe^{3+}\), reducing its charge from +3 to +2, which is a reduction.
For the equation \(Zn \rightarrow Zn^{2+} + 2e^-\), electrons are produced on the product side, indicating loss of electrons, which is oxidation, not reduction.
Similarly, for \(Cu^{2+} \rightarrow Cu + 2e^-\) and \(Cl_2 \rightarrow 2Cl^- + 2e^-\), electrons are on the product side, indicating oxidation processes.
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