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.

Answer 2

Step 1: Understand the concept of oxidizing capacity.
The oxidizing capacity of a species depends on its ability to gain electrons and undergo reduction. The stronger the oxidizing agent, the higher its standard reduction potential (\( E^\circ \)).

Step 2: Recall the relationship between \( E^\circ \) value and oxidizing strength.
A species with a higher (more positive) standard reduction potential has a greater tendency to gain electrons, and hence acts as a stronger oxidizing agent.

Step 3: Analyze the given data.
Among the given p-block ions, we are comparing their standard reduction potential (\( E^\circ \)) values. The species with the highest \( E^\circ \) value will be the one with the strongest oxidizing power.

Given data (from the options):
\[ E^\circ_{\text{Pb}^{4+}/\text{Pb}^{2+}} = +1.67\, \text{V} \] This is a highly positive potential, indicating that Pb⁴⁺ has a very strong tendency to gain electrons and get reduced to Pb²⁺, thereby making it a very strong oxidizing agent.

Step 4: Conclusion.
Since \( E^\circ_{\text{Pb}^{4+}/\text{Pb}^{2+}} = +1.67 \, \text{V} \) is the highest among the given values, it corresponds to the species with the strongest oxidizing capacity.

Final Answer:
\[ \boxed{E^\circ_{\text{Pb}^{4+}/\text{Pb}^{2+}} = +1.67 \, \text{V}} \]