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Chapter 20: Problem 13

(a) What is meant by the term oxidation? (b) On which side of an oxidation half-reaction do the electrons appear? (c) What is meant by the term oxidant? (d) What is meant by the term oxidizing agent?

Short Answer

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(a) Oxidation is a chemical process where a substance loses electrons, resulting in an increase in oxidation state. (b) In an oxidation half-reaction, electrons appear on the right side (product side) of the equation since they are lost by the substance being oxidized. (c) An oxidant, or oxidizing agent, is a substance capable of oxidizing other substances by causing them to lose electrons while itself getting reduced. (d) An oxidizing agent is a substance that causes the oxidation of other substances by accepting or taking their electrons, undergoing reduction in the process.

Step by step solution

01

(a) Definition of Oxidation

Oxidation is a chemical process in which a substance loses electrons. In other words, the oxidation state of an element within a compound increases. This process usually involves a transfer of electrons from one atom (being oxidized) to another atom (being reduced). Oxidation is one half of a redox (reduction-oxidation) reaction.
02

(b) Position of Electrons in an Oxidation Half-Reaction

In an oxidation half-reaction, electrons are lost by the substance being oxidized. These electrons appear on the right side (product side) of the half-reaction equation. This is because the atom or compound losing electrons is transformed into a new species, and the released electrons are now considered as separate entities (products).
03

(c) Definition of Oxidant

An oxidant, also known as an oxidizing agent, is a substance that has the ability to oxidize other substances, i.e., cause them to lose electrons. An oxidant gains electrons during this reaction and thus, undergoes reduction itself. It is responsible for removing electrons from another substance while simultaneously getting reduced.
04

(d) Definition of Oxidizing Agent

The term oxidizing agent refers to the same concept as an oxidant. An oxidizing agent is a substance that has the ability to oxidize other substances by accepting or taking their electrons. In other words, it causes the oxidation of other substances while itself getting reduced in the process. Some common examples of oxidizing agents include oxygen, hydrogen peroxide, and halogens such as chlorine and bromine.

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Most popular questions from this chapter

In a galvanic cell the cathode is an \(\mathrm{Ag}^{+}(1.00 \mathrm{M}) / \mathrm{Ag}(s)\) half-cell. The anode is a standard hydrogen electrode immersed in a buffer solution containing 0.10\(M\) benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) and 0.050 \(\mathrm{M}\) sodium benzoate \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-} \mathrm{Na}^{+}\right) .\) The measured cell voltage is 1.030 \(\mathrm{V}\) . What is the \(\mathrm{p} K_{\mathrm{a}}\) of benzoic acid?

(a) Which electrode of a voltaic cell, the cathode or the anode, corresponds to the higher potential energy for the electrons? (b) What are the units for electrical potential? How does this unit relate to energy expressed in joules?

Indicate whether the following balanced equations involve oxidation-reduction. If they do, identify the elements that undergo changes in oxidation number. $$ \begin{array}{l}{\text { (a) } 2 \mathrm{AgNO}_{3}(a q)+\mathrm{CoCl}_{2}(a q) \longrightarrow 2 \mathrm{AgCl}(s)+} \\\ {\quad\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(a q)} \\ {\text { (b) } 2 \mathrm{PbO}_{2}(s) \longrightarrow 2 \mathrm{PbO}(s)+\mathrm{O}_{2}(g)} \\\ {\text { (c) } 2 \mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaBr}(s) \rightarrow \mathrm{Br}_{2}(l)+\mathrm{SO}_{2}(g)+} \\ {\quad \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)}\end{array} $$

A mixture of copper and gold metals that is subjected to electrorefining contains tellurium as an impurity. The standard reduction potential between tellurium and its lowest common oxidation state, \(\mathrm{Te}^{4+},\) is $$ \mathrm{Te}^{4+}(a q)+4 \mathrm{e}^{-} \longrightarrow \mathrm{Te}(s) \quad E_{\mathrm{red}}^{\circ}=0.57 \mathrm{V} $$ Given this information, describe the probable fate of tellurium impurities during electrorefining. Do the impurities fall to the bottom of the refining bath, unchanged, as copper is oxidized, or do they go into solution as ions? If they go into solution, do they plate out on the cathode?

A voltaic cell utilizes the following reaction: $$ \mathrm{Al}(s)+3 \mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Al}^{3+}(a q)+3 \mathrm{Ag}(s) $$ What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode half-cell, diluting the solution. (b) The size of the aluminum electrode is increased. (c) A solution of AgNO \(_{3}\) is added to the cathode half-cell, increasing the quantity of Ag' but not changing its concentration. (d) HCl is added to the AgNO\(_{3}\) solution precipitating some of the Ag' as AgCl.
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