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Which half-reaction correctly represents oxidation? A Fe() →Fe +2 (aq) + 2e- B Fe +2 2² (aq) → Fe + 2e- с Fe(s) + 2e → Fe +2 D Fe +2 + 2e → (aq) (aq) Fe(s)

Which half-reaction correctly represents oxidation? A Fe() →Fe +2 (aq) + 2e- B Fe +2 2² (aq) → Fe + 2e- с Fe(s) + 2e → Fe +2 D Fe +2 + 2e → (aq) (aq) Fe(s)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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--- **Question:** Which half-reaction correctly represents oxidation? **Options:** - **A.** \( Fe_{(s)} \rightarrow Fe^{+2}_{(aq)} + 2e^- \) - **B.** \( Fe^{+2}_{(aq)} \rightarrow Fe_{(s)} + 2e^- \) - **C.** \( Fe_{(s)} + 2e^- \rightarrow Fe^{+2}_{(aq)} \) - **D.** \( Fe^{+2}_{(aq)} + 2e^- \rightarrow Fe_{(s)} \) **Correct Answer:** Option **A.** \( Fe_{(s)} \rightarrow Fe^{+2}_{(aq)} + 2e^- \) **Explanation:** Oxidation is defined as the loss of electrons. In a redox reaction, the species that loses electrons gets oxidized. The correct half-reaction for oxidation among the given options is one that shows a species losing electrons. - In option **A**, solid iron (\(Fe_{(s)}\)) loses two electrons (2e^-) to form iron ions in an aqueous solution (\(Fe^{+2}_{(aq)}\)). This denotes oxidation. The other options reflect different reactions but do not correspond to the definition of oxidation, as they do not show a species losing electrons correctly. ---
Transcribed Image Text:--- **Question:** Which half-reaction correctly represents oxidation? **Options:** - **A.** \( Fe_{(s)} \rightarrow Fe^{+2}_{(aq)} + 2e^- \) - **B.** \( Fe^{+2}_{(aq)} \rightarrow Fe_{(s)} + 2e^- \) - **C.** \( Fe_{(s)} + 2e^- \rightarrow Fe^{+2}_{(aq)} \) - **D.** \( Fe^{+2}_{(aq)} + 2e^- \rightarrow Fe_{(s)} \) **Correct Answer:** Option **A.** \( Fe_{(s)} \rightarrow Fe^{+2}_{(aq)} + 2e^- \) **Explanation:** Oxidation is defined as the loss of electrons. In a redox reaction, the species that loses electrons gets oxidized. The correct half-reaction for oxidation among the given options is one that shows a species losing electrons. - In option **A**, solid iron (\(Fe_{(s)}\)) loses two electrons (2e^-) to form iron ions in an aqueous solution (\(Fe^{+2}_{(aq)}\)). This denotes oxidation. The other options reflect different reactions but do not correspond to the definition of oxidation, as they do not show a species losing electrons correctly. ---
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