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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.

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Most popular questions from this chapter

Calculate \(\mathscr{E}^{\circ}\) for the following half-reaction: $$ \mathrm{AgI}(s)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)+\mathrm{I}^{-}(a q) $$ (Hint: Reference the \(K_{\mathrm{sp}}\) value for AgI and the standard reduction potential for \(\mathrm{Ag}^{+} .\) )

An experimental fuel cell has been designed that uses carbon monoxide as fuel. The overall reaction is $$ 2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g) $$ The two half-cell reactions are $$ \begin{array}{c} \mathrm{CO}+\mathrm{O}^{2-} \longrightarrow \mathrm{CO}_{2}+2 \mathrm{e}^{-} \\\ \mathrm{O}_{2}+4 \mathrm{e}^{-} \longrightarrow 2 \mathrm{O}^{2-} \end{array} $$ The two half-reactions are carried out in separate compartments connected with a solid mixture of \(\mathrm{CeO}_{2}\) and \(\mathrm{Gd}_{2} \mathrm{O}_{3}\). \(\mathrm{Ox}\) ide ions can move through this solid at high temperatures (about \(800^{\circ} \mathrm{C}\) ). \(\Delta G\) for the overall reaction at \(800^{\circ} \mathrm{C}\) under certain concentration conditions is -380 kJ. Calculate the cell potential for this fuel cell at the same temperature and concentration conditions.

The compound with the formula TII \(_{3}\) is a black solid. Given the following standard reduction potentials, $$ \begin{aligned} \mathrm{T}^{3+}+2 \mathrm{e}^{-} \longrightarrow & \mathrm{Tl}^{+} & & \mathscr{E}^{\circ}=1.25 \mathrm{V} \\ \mathrm{I}_{3}^{-}+2 \mathrm{e}^{-} & \longrightarrow 3 \mathrm{I}^{-} & & \mathscr{E}^{\circ}=0.55 \mathrm{V} \end{aligned} $$ would you formulate this compound as thallium(III) iodide or thallium(I) triiodide?

The free energy change for a reaction, \(\Delta G,\) is an extensive property. What is an extensive property? Surprisingly, one can calculate \(\Delta G\) from the cell potential, \(\mathscr{E},\) for the reaction. This is surprising because \(\mathscr{E}\) is an intensive property. How can the extensive property \(\Delta G\) be calculated from the intensive property \(\mathscr{E} ?\)

An electrochemical cell consists of a nickel metal electrode immersed in a solution with \(\left[\mathrm{Ni}^{2+}\right]=1.0 \mathrm{M}\) separated by a porous disk from an aluminum metal electrode. a. What is the potential of this cell at \(25^{\circ} \mathrm{C}\) if the aluminum electrode is placed in a solution in which \(\left[\mathrm{Al}^{3+}\right]=7.2 \times\) \(10^{-3} M ?\) b. When the aluminum electrode is placed in a certain solution in which \(\left[\mathrm{Al}^{3+}\right]\) is unknown, the measured cell potential at \(25^{\circ} \mathrm{C}\) is \(1.62 \mathrm{V}\). Calculate \(\left[\mathrm{Al}^{3+}\right]\) in the unknown solution. (Assume Al is oxidized.)
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