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Chapter 17: Problem 25

What is an oxidizing agent? What is a reducing agent?

Short Answer

Expert verified
An oxidizing agent is a substance that gains electrons in a redox reaction, causing another substance to be oxidized. It usually contains oxygen or other electronegative elements, like potassium permanganate (KMnO\(_{4}\)). A reducing agent is a substance that loses electrons in a redox reaction, causing another substance to be reduced. It is often metals or hydrides, such as zinc (Zn), which donates electrons to other species during the reaction.

Step by step solution

01

Define Oxidizing Agent

An oxidizing agent, also known as an oxidant or oxidizer, is a substance that gains electrons in a redox reaction and causes another substance to be oxidized. In other words, an oxidizing agent takes electrons from other species during the reaction. A common characteristic of oxidizing agents is that they usually contain oxygen or other electronegative elements.
02

Example of Oxidizing Agent

An example of an oxidizing agent is potassium permanganate (KMnO\(_{4}\)). In a redox reaction, potassium permanganate gains electrons, and its manganese atom is reduced from its initial oxidation state of +7 to a lower oxidation state.
03

Define Reducing Agent

A reducing agent, also known as a reductant or reducer, is a substance that loses electrons in a redox reaction and causes another substance to be reduced. In other words, a reducing agent gives electrons to other species during the reaction. A common characteristic of reducing agents is that they are usually metals or hydrides.
04

Example of Reducing Agent

An example of a reducing agent is zinc (Zn). In a redox reaction, zinc loses electrons, and its oxidation state increases, meaning it is oxidized. Zinc effectively donates its electrons to another species, causing that species to be reduced.

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Most popular questions from this chapter

Does an oxidizing agent donate or accept electrons? Does a reducing agent donate or accept electrons?

Iodide ion, I\(^{-}\), is one of the most easily oxidized species. Balance each of the following oxidationreduction reactions, which take place in acidic \(50^{-}\) lution, by using the "half-reaction" method. a. \(\mathrm{IO}_{3}^{-}(a q)+\mathrm{I}^{-}(a q) \rightarrow \mathrm{I}_{2}(a q)\) b. \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{I}^{-}(a q) \rightarrow \mathrm{C} \mathrm{r}^{3+}(a q)+\mathrm{I}_{2}(a q)\) c. \(\mathrm{Cu}^{2+}(a q)+\mathrm{I}^{-}(a q) \rightarrow \operatorname{CuI}(s)+\mathrm{I}_{2}(a q)\)

How is an oxidation-reduction reaction set up as a galvanic cell (battery)? How is the transfer of electrons between reducing agent and oxidizing agent made useful?

A solution of chlorine gas in water is used in chemical analysis to test for the presence of \(\mathrm{Br}^{-}\) and \(\mathrm{I}^{-}\) ions in solution. \(\mathrm{Cl}_{2}\) is able to oxidize easily these two ions to the elemental forms \(\mathrm{Br}_{2}\) and \(\mathrm{I}_{2},\) which may then be identified by their colors. Write a balanced oxidation-reduction equation for each of these processes.

Give some examples of how we make good use of oxidation-reduction reactions in everyday life.
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