Given the following standard reduction potentials:A^{2+} + 2e^- → A(s)E^ext{°} = -0.50ext{ V}B^{+} + e^- → B(s)E^ext{°} = +0.20ext{ V}Which species is the stronger oxidizing agent under standard conditions?

• A. A^{2+}
• B. B(s)
• C. B^{+}
• D. A(s)

Answer: (C)

Verified step by step guidance

1. Recall that the strength of an oxidizing agent is related to its tendency to gain electrons, which corresponds to the standard reduction potential (E^{\circ}). The species with the higher (more positive) standard reduction potential is the stronger oxidizing agent.
2. Identify the given half-reactions and their standard reduction potentials: \(A^{2+} + 2e^- \rightarrow A(s) \quad E^{\circ} = -0.50\ \text{V}\) \(B^{+} + e^- \rightarrow B(s) \quad E^{\circ} = +0.20\ \text{V}\)
3. Compare the standard reduction potentials: since \(+0.20\ \text{V} > -0.50\ \text{V}\), the species \(B^{+}\) has a higher tendency to be reduced (gain electrons) than \(A^{2+}\).
4. Because the oxidizing agent is the species that gets reduced, the stronger oxidizing agent under standard conditions is the one with the higher reduction potential, which is \(B^{+}\).
5. Therefore, among the options given, \(B^{+}\) is the stronger oxidizing agent.