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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

Which electrode in a galvanic cell is the anode? Which is the cathode?

In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation numbers. a. \(\mathrm{Zn}(s)+2 \mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2}(g)\) b. \(\mathrm{H}_{2}(g)+\operatorname{CuSO}_{4}(a q) \rightarrow \operatorname{Cu}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q)\) c. \(\mathrm{N}_{2}(g)+3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{NBr}_{3}(g)\) d. \(2 \mathrm{KBr}(a q)+\mathrm{Cl}_{2}(g) \rightarrow 2 \mathrm{KCl}(a q)+\mathrm{Br}_{2}(l)\)

Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{MnO}_{2}\) b. \(\mathrm{BaCrO}_{4}\) C. \(\mathrm{H}_{2} \mathrm{SO}_{3}\) d. \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

An oxidizing agent causes the (oxidation/reduction) of another species, and the oxidizing agent itself is (oxidized/reduced).

Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{Na}_{2} \mathrm{CrO}_{4}\) b. \(\mathrm{Na}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) c. \(\mathrm{Cr} \mathrm{Cl}_{3}\) d. \(\mathrm{Cr}_{2} \mathrm{O}_{3}\)
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