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Chapter 7: Problem 41

What is an oxidation-reduction reaction? What is transferred during such a reaction?

Short Answer

Expert verified
An oxidation-reduction reaction, or redox reaction, is a chemical reaction involving the transfer of electrons between two species. It consists of two half-reactions: oxidation, where a substance loses electrons and acts as a reducing agent, and reduction, where a substance gains electrons and acts as an oxidizing agent. During a redox reaction, electrons are transferred from the species being oxidized (reducing agent) to the species being reduced (oxidizing agent). For example, in the reaction \(2Na + Cl_2 \rightarrow 2NaCl\), sodium loses electrons and is oxidized, while chlorine gains electrons and is reduced, resulting in the formation of sodium chloride.

Step by step solution

01

Definition of Oxidation-Reduction Reaction

An oxidation-reduction reaction, commonly known as a redox reaction, is a chemical reaction that involves the transfer of electrons between two species. It consists of two half-reactions: oxidation and reduction.
02

Oxidation

Oxidation is the process where a substance loses one or more electrons. This results in an increase in the oxidation state of the substance. The substance that loses electrons is called the reducing agent. Example: In the reaction \(2Na + Cl_2 \rightarrow 2NaCl\), sodium (Na) loses one electron to form sodium ion (Na+). This means that sodium is oxidized and acts as a reducing agent.
03

Reduction

Reduction is the process where a substance gains one or more electrons. This results in a decrease in the oxidation state of the substance. The substance that gains electrons is called the oxidizing agent. Example: In the reaction \(2Na + Cl_2 \rightarrow 2NaCl\), chlorine (Cl2) gains one electron to form chloride ion (Cl-). This means that chlorine is reduced and acts as an oxidizing agent.
04

Electron transfer during Oxidation-Reduction Reaction

During a redox reaction, electrons are transferred from the species being oxidized (reducing agent) to the species being reduced (oxidizing agent). Example: In the reaction \(2Na + Cl_2 \rightarrow 2NaCl\), one electron from each sodium atom is transferred to a chlorine atom. As a result, two sodium ions (Na+) and two chloride ions (Cl-) are formed, combining to form sodium chloride (NaCl).

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Most popular questions from this chapter

Complete and balance each of the following equations that describe combustion reactions. Complete and balance each of the following equations that describe combustion reactions. a. \(\mathrm{C}_{4} \mathrm{H}_{10}(l)+\mathrm{O}_{2}(g) \rightarrow\) b. \(C_{4} \mathrm{H}_{10} \mathrm{O}(l)+\mathrm{O}_{2}(g) \rightarrow\) c. \(C_{4} H_{10} O_{2}(l)+O_{2}(g) \rightarrow\)

Balance each of the following equations that describe precipitation reactions. a. \(\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{CaCl}_{2}(a q) \rightarrow \mathrm{CaSO}_{4}(s)+\mathrm{NaCl}(a q)\) b. \(\operatorname{Co}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{S}(a q) \rightarrow\) \(\cos (s)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) c. \(\mathrm{KOH}(a q)+\mathrm{NiCl}_{2}(a q) \rightarrow \mathrm{Ni}(\mathrm{OH})_{2}(s)+\mathrm{KCl}(a q)\)

Two "driving forces" for reactions discussed in this section are the formation of water in an acid-base reaction and the formation of a gaseous product. Write balanced chemical equations showing two examples of each type.

Classify the reactions represented by the following unbalanced equations by as many methods as possible. Balance the equations. a. \(\mathrm{I}_{4} \mathrm{O}_{9}(s) \rightarrow \mathrm{I}_{2} \mathrm{O}_{6}(s)+\mathrm{I}_{2}(s)+\mathrm{O}_{2}(g)\) b. \(\mathrm{Mg}(s)+\mathrm{AgNO}_{3}(a q) \rightarrow \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Ag}(s)\) c. \(\operatorname{SiCl}_{4}(l)+\operatorname{Mg}(s) \rightarrow \operatorname{MgCl}_{2}(s)+\operatorname{Si}(s)\) d. \(\mathrm{CuCl}_{2}(a q)+\mathrm{AgNO}_{3}(a q) \rightarrow\) \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{AgCl}(s)\) e. \(\mathrm{Al}(s)+\mathrm{Br}_{2}(l) \rightarrow \mathrm{AlBr}_{3}(s)\)

Classify the reactions represented by the following unbalanced equations by as many methods as possible. Balance the equations. a. \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{HCl}(a q)+\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \rightarrow\) \(\mathrm{AgCl}(s)+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) c. \(\mathrm{HCl}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{H}_{2} \mathrm{O}_{2}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) e. \(\mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)
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