/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 28 Does an oxidizing agent increase... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 17: Problem 28

Does an oxidizing agent increase or decrease its own oxidation state when it acts on another atom? Does a reducing agent increase or decrease its own oxidation state when it acts on another substance?

Short Answer

Expert verified
When an oxidizing agent acts on another atom, its oxidation state decreases as it accepts electrons and undergoes reduction. On the other hand, when a reducing agent acts on another substance, its oxidation state increases as it donates electrons and undergoes oxidation.

Step by step solution

01

Understanding Oxidizing and Reducing Agents

Oxidizing agents and reducing agents play essential roles in redox reactions. In such reactions, one substance loses electrons (getting oxidized), while the other gains electrons (getting reduced). An oxidizing agent is a substance that has the ability to accept electrons from another substance, causing it to be reduced. The oxidizing agent itself, in the process, gets oxidized. A reducing agent is a substance that has the ability to donate electrons to another substance, causing it to be oxidized. The reducing agent, in the process, gets reduced.
02

Oxidation State of an Oxidizing Agent

When an oxidizing agent acts on another atom, it accepts electrons from the other atom. Since the process of accepting electrons is called reduction, the oxidizing agent gets reduced. When a substance undergoes reduction, its oxidation state decreases. Therefore, an oxidizing agent decreases its own oxidation state when it acts on another atom.
03

Oxidation State of a Reducing Agent

When a reducing agent acts on another substance, it donates electrons to that substance. Since the process of losing electrons is called oxidation, the reducing agent gets oxidized. When a substance undergoes oxidation, its oxidation state increases. Therefore, a reducing agent increases its own oxidation state when it acts on another substance. In conclusion: - An oxidizing agent decreases its own oxidation state when it acts on another atom. - A reducing agent increases its own oxidation state when it acts on another substance.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

For each of the following oxidation-reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a. \(3 \mathrm{Zn}(s)+\mathrm{N}_{2}(g) \rightarrow \mathrm{Zn}_{3} \mathrm{N}_{2}(s)\) b. \(\operatorname{Co}(s)+S(s) \rightarrow \cos (s)\) c. \(4 \mathrm{K}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{K}_{2} \mathrm{O}(s)\) d. \(4 \mathrm{Ag}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Ag}_{2} \mathrm{O}(s)\)

In what two respects must oxidation-reduction reactions be balanced?

Balance each of the following half-reactions. a. \(\mathrm{Al} \rightarrow \mathrm{Al}^{3+}\) b. \(\mathrm{I}^{-} \rightarrow \mathrm{I}_{2}\) c. \(\mathrm{C o}^{3+} \rightarrow \mathrm{C o}^{2+}\) d. \(\mathrm{P}^{3-} \rightarrow \mathrm{P}_{4}\)

Why is fluorine always assigned an oxidation state of \(-1 ?\) What oxidation number is \(u\) sually assigned to the other halogen elements when they occur in compounds? In an interhalogen compound involving fluorine (such as ClF), which atom has a negative oxidation state?

Balance each of the following oxidation-reduction reactions, which take place in acidic solution, by using the "half-reaction" method. a. \(\mathrm{Mg}(s)+\mathrm{Hg}^{2+}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Hg}_{2}^{2+}(a q)\) b. \(\mathrm{NO}_{3}^{-}(a q)+\mathrm{Br}^{-}(a q) \rightarrow \mathrm{NO}(g)+\mathrm{Br}_{2}(l)\) c. \(\mathrm{Ni}(s)+\mathrm{NO}_{3}^{-}(a q) \rightarrow \mathrm{Ni}^{2+}(a q)+\mathrm{NO}_{2}(g)\) d. \(\mathrm{ClO}_{4}^{-}(a q)+\mathrm{Cl}^{-}(a q) \rightarrow \mathrm{ClO}_{3}^{-}(a q)+\mathrm{Cl}_{2}(g)\)
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.