Which of the following half-reactions correctly represents an oxidation process?

• A. Fe^{2+} ightarrow Fe^{3+} + e^{-}
• B. Cu^{2+} + 2e^{-} ightarrow Cu
• C. Cl_{2} + 2e^{-} ightarrow 2Cl^{-}
• D. Ag^{+} + e^{-} ightarrow Ag

Answer: (A)

Verified step by step guidance

1. Recall that oxidation is the loss of electrons, while reduction is the gain of electrons. In a half-reaction, oxidation will show electrons as products, and reduction will show electrons as reactants.
2. Examine each half-reaction to identify whether electrons are on the product side (indicating oxidation) or on the reactant side (indicating reduction).
3. For the half-reaction \(Fe^{2+} \rightarrow Fe^{3+} + e^{-}\), electrons are produced, so this represents oxidation.
4. For the half-reactions \(Cu^{2+} + 2e^{-} \rightarrow Cu\), \(Cl_{2} + 2e^{-} \rightarrow 2Cl^{-}\), and \(Ag^{+} + e^{-} \rightarrow Ag\), electrons are consumed, indicating reduction processes.
5. Therefore, the half-reaction that correctly represents an oxidation process is the one where the species loses electrons, which is \(Fe^{2+} \rightarrow Fe^{3+} + e^{-}\).