Question

The standard reduction potential values of some of the p-block ions are given below. Predict the one with the strongest oxidizing capacity.

• A. \( E^\circ_{\text{I}^- / \text{I}_2} = +1.26 \, \text{V} \)
• B. \( E^\circ_{\text{Al}^{3+} / \text{Al}} = -1.66 \, \text{V} \)
• C. \( E^\circ_{\text{Pb}^{4+} / \text{Pb}^{2+}} = +1.67 \, \text{V} \)
• D. \( E^\circ_{\text{Sn}^{4+} / \text{Sn}^{2+}} = +1.15 \, \text{V} \)

Hint:

The higher the reduction potential, the stronger the oxidizing agent, as it more readily gains electrons.

Answer 1

The Correct Option is C

In order to determine which of the given chemical species has the strongest oxidizing capacity, we need to examine their standard reduction potential values. The species with the highest standard reduction potential will have the strongest oxidizing capacity, as a higher reduction potential indicates a greater tendency to gain electrons and thereby oxidize other substances.

Here are the given standard reduction potentials:
 

• \(E^\circ_{\text{I}^- / \text{I}_2} = +1.26 \, \text{V}\)
• \(E^\circ_{\text{Al}^{3+} / \text{Al}} = -1.66 \, \text{V}\)
• \(E^\circ_{\text{Pb}^{4+} / \text{Pb}^{2+}} = +1.67 \, \text{V}\)
• \(E^\circ_{\text{Sn}^{4+} / \text{Sn}^{2+}} = +1.15 \, \text{V}\)

 

Comparing these values, \(E^\circ_{\text{Pb}^{4+} / \text{Pb}^{2+}} = +1.67 \, \text{V}\) is the highest. Therefore, the ion \( \text{Pb}^{4+} \) has the strongest oxidizing capacity because it more readily accepts electrons to be reduced.