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Chapter 4: Problem 46

Can oxidation occur without accompanying reduction? Explain.

Short Answer

Expert verified
In short, oxidation cannot occur without an accompanying reduction. This is because oxidation and reduction reactions are intrinsically linked through the conservation of charge and the transfer of electrons in a redox process. In a redox reaction, the electrons lost by one species during oxidation must be gained by another species during reduction to maintain the conservation of charge.

Step by step solution

01

Understanding Oxidation and Reduction

Oxidation and reduction are chemical reactions that involve the transfer of electrons between atoms or molecules. In an oxidation reaction, an atom or molecule loses one or more electrons, whereas in a reduction reaction, an atom or molecule gains one or more electrons.
02

Redox Reactions

Oxidation and reduction reactions often occur together, forming a "couple," with the oxidized molecule providing the electrons needed for the reduced molecule to gain its electrons. These paired reactions are known as redox reactions (short for reduction-oxidation reactions).
03

Why Oxidation and Reduction are Coupled

In a redox reaction, the substance undergoing oxidation loses electrons to the substance undergoing reduction. For every electron that is lost by one species, there must be another species that gains that electron. Therefore, an oxidation reaction and a reduction reaction must always be paired in any redox process.
04

Example of a Redox Reaction

Let's consider the following example: 2H鈧�(g) + O鈧�(g) 鈫� 2H鈧侽(l) In this reaction, hydrogen gas (H鈧�) and oxygen gas (O鈧�) combine to form water (H鈧侽). Hydrogen undergoes oxidation, losing electrons to form H鈦� ions, while oxygen undergoes reduction, gaining electrons to form O虏鈦� ions: Oxidation: H鈧� 鈫� 2H鈦� + 2e鈦� Reduction: O鈧� + 4e鈦� 鈫� 2O虏鈦� The electrons released by the oxidation of hydrogen are the same electrons gained by the reduction of oxygen. This is an example of a redox reaction, where the oxidation of one species is accompanied by the reduction of another species.
05

Can Oxidation Occur Without Reduction?

As we've seen, the principles of oxidation and reduction are founded on the transfer of electrons between species. Oxidation requires a species to lose electrons, which must be subsequently gained by another species for the reaction to be balanced. Therefore, oxidation cannot occur without an accompanying reduction, as the electrons that are lost during the oxidation process need to be gained by another species to maintain the conservation of charge. In conclusion, oxidation reactions cannot occur without accompanying reduction reactions, as they are intrinsically linked through the conservation of charge and the transfer of electrons in a redox process.

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Most popular questions from this chapter

Which of the following solutions has the largest concentration of solvated protons: (a) \(0.2 \mathrm{MLiOH}\), (b) \(0.2 \mathrm{M} \mathrm{HI}\), (c) \(1.0 \mathrm{M}\) methyl alcohol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) ? Explain.

The average concentration of bromide ion in seawater is \(65 \mathrm{mg}\) of bromide ion per \(\mathrm{kg}\) of seawater. What is the molarity of the bromide ion if the density of the seawater is \(1.025 \mathrm{~g} / \mathrm{mL}\) ?

(a) Use the following reactions to prepare an activity series for the halogens: $$ \begin{aligned} \mathrm{Br}_{2}(a q)+2 \mathrm{NaI}(a q) & \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q) \\ \mathrm{Cl}_{2}(a q)+2 \mathrm{NaBr}(a q) & \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(a q) \end{aligned} $$ (b) Relate the positions of the halogens in the periodic table with their locations in this activity series. (c) Predict whether a reaction occurs when the following reagents are mixed: \(\mathrm{Cl}_{2}(a q)\) and \(\mathrm{KI}(a q) ; \mathrm{Br}_{2}(a q)\) and \(\mathrm{LiCl}(a q)\).

Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid; (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.

Acetone, \(\mathrm{CH}_{3} \mathrm{COCH}_{3}\), is a nonelectrolyte; hypochlorous acid, \(\mathrm{HClO}\), is a weak electrolyte; and ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl}\), is a strong electrolyte. (a) What are the solute particles present in aqueous solutions of each compound? (b) If \(0.1 \mathrm{~mol}\) of each compound is dissolved in solution, which one contains \(0.2 \mathrm{~mol}\) of solute particles, which contains \(0.1 \mathrm{~mol}\) of solute particles, and which contains somewhere between \(0.1\) and \(0.2 \mathrm{~mol}\) of solute particles?
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