/*! 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 15 Define oxidation and reduction i... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 17: Problem 15

Define oxidation and reduction in terms of both change in oxidation number and electron loss or gain.

Short Answer

Expert verified
Oxidation is a chemical process where a substance loses electrons and experiences an increase in its oxidation number, while reduction is a chemical process where a substance gains electrons and experiences a decrease in its oxidation number. For example, when a carbon atom goes from +2 to +4 oxidation state, it has been oxidized; and when an oxygen atom goes from -1 to -2 oxidation state, it has been reduced. Additionally, oxidation involves electron loss (e.g., sodium atom losing an electron to become Na+), and reduction involves electron gain (e.g., chlorine atom gaining an electron to become Cl-).

Step by step solution

01

Definition of Oxidation

Oxidation is a chemical process in which a substance loses electrons, leading to an increase in its oxidation number.
02

Definition of Reduction

Reduction is a chemical process in which a substance gains electrons, leading to a decrease in its oxidation number.
03

Oxidation in terms of oxidation number

Oxidation occurs when there is an increase in the oxidation number of an atom, ion, or molecule. For example, when a carbon atom goes from an oxidation state of +2 to +4, it has been oxidized.
04

Reduction in terms of oxidation number

Reduction occurs when there is a decrease in the oxidation number of an atom, ion, or molecule. For example, when an oxygen atom goes from an oxidation state of -1 to -2, it has been reduced.
05

Oxidation in terms of electron loss

In oxidation, a substance loses electrons during the chemical process. For example, when a sodium atom loses an electron to become a sodium ion (Na+), it has undergone oxidation.
06

Reduction in terms of electron gain

In reduction, a substance gains electrons during the chemical process. For example, when a chlorine atom gains an electron to become a chloride ion (Cl-), it has undergone reduction.

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

Consider a concentration cell that has both electrodes made of some metal M. Solution \(A\) in one compartment of the cell contains \(1.0 \mathrm{M} \mathrm{M}^{2+}\). Solution \(\mathrm{B}\) in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of \(\mathrm{M}\left(\mathrm{NO}_{3}\right)_{2}\) and 0.0100 mole of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) are dissolved in solution \(\mathrm{B}\) (ignore volume changes), where the reaction $$ \mathbf{M}^{2+}(a q)+\mathbf{S O}_{4}^{2-}(a q) \rightleftharpoons \mathrm{MSO}_{4}(s) $$ occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25 \(^{\circ}\) C. Assume that the process $$ \mathrm{M}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{M} $$ has a standard reduction potential of \(-0.31 \mathrm{V}\) and that no other redox process occurs in the cell. Calculate the value of \(K_{\mathrm{sp}}\) for \(\mathrm{MSO}_{4}(s)\) at \(25^{\circ} \mathrm{C}\)

Consider the following galvanic cell: a. Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow. b. Determine the standard cell potential. c. Which electrode increases in mass as the reaction proceeds, and which electrode decreases in mass?

Gold is produced electrochemically from an aqueous solution of \(\mathrm{Au}(\mathrm{CN})_{2}^{-}\) containing an excess of \(\mathrm{CN}^{-} .\) Gold metal and oxygen gas are produced at the electrodes. What amount (moles) of \(\mathbf{O}_{2}\) will be produced during the production of 1.00 mole of gold?

Balance the following oxidation-reduction reactions that occur in acidic solution using the half-reaction method. a. \(\mathrm{Cu}(s)+\mathrm{NO}_{3}^{-}(a q) \rightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{NO}(g)\) b. \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{Cl}^{-}(a q) \rightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{Cl}_{2}(g)\) c. \(\mathrm{Pb}(s)+\mathrm{PbO}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{PbSO}_{4}(s)\) d. \(\mathrm{Mn}^{2+}(a q)+\mathrm{NaBiO}_{3}(s) \rightarrow \mathrm{Bi}^{3+}(a q)+\mathrm{MnO}_{4}^{-}(a q)\) e. \(\mathrm{H}_{3} \mathrm{AsO}_{4}(a q)+\mathrm{Zn}(s) \rightarrow \mathrm{AsH}_{3}(g)+\mathrm{Zn}^{2+}(a q)\)

What reaction will take place at the cathode and the anode when each of the following is electrolyzed? (Assume standard conditions.) a. \(1.0 M\space \mathrm {KF}\) solution b. \(1.0 M\space \mathrm {CuCl}_{2}\) solution c. \(1.0 M \space \mathrm{MgI}_{2}\) solution
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

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.