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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

When balancing equations in Chapter \(5,\) we did not mention that reactions must be charge balanced as well as mass balanced. What do charge balanced and mass balanced mean? How are redox equations charge balanced?

When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?

Sketch the galvanic cells based on the following half-reactions. Show the direction of electron flow, show the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation, and determine \(\mathscr{C}^{\circ}\) for the galvanic cells. Assume that all concentrations are \(1.0 M\) and that all partial pressures are 1.0 atm. a. \(\mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_{2} \mathrm{O} \quad \mathscr{E}^{\circ}=1.78 \mathrm{V}\) \(\mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}_{2} \quad \quad \mathscr{E}^{\circ}=0.68 \mathrm{V}\) b. \(\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn} \quad \mathscr{E}^{\circ}=-1.18 \mathrm{V}\) \(\mathrm{Fe}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe} \quad \mathscr{E}^{\circ}=-0.036 \mathrm{V}\)

Consider the following half-reactions: \(\begin{aligned} \mathrm{Pt}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pt} & & & \mathscr{E}^{\circ}=1.188 \mathrm{V} \\ \mathrm{PtCl}_{4}^{2-}+2 \mathrm{e}^{-} \longrightarrow & \mathrm{Pt}+4 \mathrm{Cl}^{-} & & \mathscr{E}^{\circ}=0.755 \mathrm{V} \\ \mathrm{NO}_{3}^{-}+4 \mathrm{H}^{+}+3 \mathrm{e}^{-} & \longrightarrow \mathrm{NO}+2 \mathrm{H}_{2} \mathrm{O} & & \mathscr{E}^{\circ}=0.96 \mathrm{V} \end{aligned}\) Explain why platinum metal will dissolve in aqua regia (a mixture of hydrochloric and nitric acids) but not in either concentrated nitric or concentrated hydrochloric acid individually.

Consider a galvanic cell based on the following half-reactions: $$\begin{array}{ll} & \mathscr{E}^{\circ}(\mathrm{V}) \\ \mathrm{La}^{3+}+3 \mathrm{e}^{-} \longrightarrow \mathrm{La} & -2.37 \\ \mathrm{Fe}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Fe} & -0.44 \\ \hline \end{array}$$ a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at \(25^{\circ} \mathrm{C}\) with \(\left[\mathrm{Fe}^{2+}\right]=2.00 \times 10^{-4} \mathrm{M}\) and \(\left[\mathrm{La}^{3+}\right]=3.00 \times 10^{-3} \mathrm{M},\) what is the expected cell potential?
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