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Chapter 4: Problem 45

Define oxidation and reduction in terms of (a) electron transfer and (b) oxidation numbers.

Short Answer

Expert verified
(a) In terms of electron transfer, oxidation is the loss of electrons by a species, while reduction is the gain of electrons by a species. (b) In terms of oxidation numbers, oxidation involves an increase in the oxidation number of a species, whereas reduction involves a decrease in the oxidation number of a species.

Step by step solution

01

Define oxidation in terms of electron transfer

Oxidation is a chemical process that occurs when an atom, ion, or molecule loses one or more electrons. In this process, the oxidizing agent gains electrons, and the oxidation state of the species undergoing oxidation increases.
02

Define reduction in terms of electron transfer

Reduction is a chemical process in which an atom, ion, or molecule gains one or more electrons. In this process, the reducing agent loses electrons, and the oxidation state of the species undergoing reduction decreases.
03

Define oxidation numbers

Oxidation numbers (or oxidation states) are used to keep track of the electrons in an atom, ion, or molecule during a redox reaction. It is a hypothetical charge assigned to an atom, considering that all its bonds are either completely ionic or completely covalent. The sum of oxidation numbers of all atoms in a neutral molecule is equal to zero, while in a polyatomic ion, it is equal to the charge of the ion.
04

Define oxidation in terms of oxidation numbers

An oxidation process involves an increase in the oxidation number of the species undergoing oxidation. The oxidizing agent gains electrons and thereby is reduced – its oxidation number decreases.
05

Define reduction in terms of oxidation numbers

A reduction process involves a decrease in the oxidation number of the species undergoing reduction. The reducing agent loses electrons and thereby is oxidized – its oxidation number increases.

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Most popular questions from this chapter

Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a) could you distinguish any of the three magnesium substances from the other two? If so how? (c) If excess \(\mathrm{HCl}(a q)\) is added, would the clear solutions left behind after the reaction is complete contain the same or different ions in each case?

(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 \(\mathrm{KI}(a q) ; \operatorname{Br}_{2}(a q)\) and \(\operatorname{LiCl}(a q)\)

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