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Chapter 22: Problem 86

Explain why \(\mathrm{SO}_{2}\) can be used as a reducing agent but \(\mathrm{SO}_{3}\) cannot.

Short Answer

Expert verified
SO鈧� can be used as a reducing agent because it can donate electrons and be oxidized to SO鈧�, where sulfur has its highest oxidation state of +6. In contrast, SO鈧� cannot act as a reducing agent since sulfur is already in its highest oxidation state and cannot be further oxidized or donate electrons.

Step by step solution

01

Understand Reducing Agents

A reducing agent is a substance that can reduce other substances, which means it can donate electrons to other substances during a chemical reaction. Reducing agents themselves are oxidized in the process, meaning they lose electrons. To determine if a molecule can act as a reducing agent, we should examine its ability to donate electrons and its willingness to be oxidized.
02

Examine Oxidation States and Stability of SO鈧�

In SO鈧�, the sulfur atom has an oxidation state of +4. SO鈧� is able to be oxidized further to SO鈧�, in which sulfur has the oxidation state of +6, the highest possible oxidation state for sulfur. In this process, SO鈧� donates electrons to other molecules, reducing them and becoming more oxidized itself: SO鈧� + 陆 O鈧� 鈫� SO鈧� Thus, SO鈧� can act as a reducing agent, as it can donate electrons and be oxidized.
03

Examine Oxidation States and Stability of SO鈧�

In SO鈧�, the sulfur atom has the oxidation state of +6. This is the highest possible oxidation state for sulfur, meaning SO鈧� cannot be oxidized further. Since it cannot be further oxidized, SO鈧� has no electrons to donate and cannot act as a reducing agent.
04

Compare SO鈧� and SO鈧�

Comparing the oxidation states and stability of SO鈧� and SO鈧�, it is clear that SO鈧� can act as a reducing agent because it is capable of donating electrons while being oxidized to SO鈧�. In contrast, SO鈧� is already in its highest oxidation state and cannot be further oxidized, making it unable to act as a reducing agent. Overall: SO鈧� can be used as a reducing agent due to its ability to donate electrons and be oxidized to SO鈧�, while SO鈧� cannot be used as a reducing agent because it is already in its highest oxidation state and cannot be further oxidized.

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Most popular questions from this chapter

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) chlorate ion, (b) hydroiodic acid, (c) iodine trichloride, (d) sodium hypochlorite, (e) perchloric acid, (f) xenon tetrafluoride.

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