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Chapter 4: Problem 151

Is the following reaction a redox reaction? Explain. \(3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{O}_{3}(g)\)

Short Answer

Expert verified
No, the given reaction is not a redox reaction because there is no change in the oxidation states of the elements involved. No loss or gain of electrons has occurred.

Step by step solution

01

Understand the reaction

Firstly, identify the reactant and product of the reaction given. Here, the reaction shows \(3 \mathrm{O}_{2}(g)\) as the reactant converting into \(2 \mathrm{O}_{3}(g)\) as the product.
02

Determine oxidation states

Oxygen in its elemental state \(\mathrm{O}_{2}(g)\) has an oxidation state of 0. In the ozone molecule \(\mathrm{O}_{3}(g)\), oxygen is also in its elemental state and thus maintains the oxidation state of 0.
03

Identify changes in oxidation states

The oxidation states of oxygen in both reactant and product is 0, which means there is no change in oxidation state. This indicates that no electrons were transferred.
04

Conclude from findings

Since there are no changes in the oxidation states of any atoms in the reaction, it can be concluded that this is not a redox reaction as no reduction or oxidation occurred.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidation States
Understanding oxidation states is crucial in identifying redox reactions. The oxidation state, or oxidation number, represents the degree of oxidation of an atom within a compound. It indicates the number of electrons an atom gains, loses, or shares in a chemical bonding. For instance, in the reaction involving oxygen:
  • Oxygen, as a diatomic molecule (\(\text{O}_2(g)\)), has an oxidation state of 0. This is because it is in its elemental form.
  • Similarly, ozone (\(\text{O}_3(g)\)) is also composed of oxygen atoms in their elemental state, maintaining an oxidation state of 0.
Identifying changes in oxidation states helps determine electron transfer, thereby classifying whether a reaction is a redox process. When the oxidation state remains unchanged, as seen with oxygen in both reactants and products, no redox reaction takes place.
Electron Transfer
Electron transfer is a pivotal concept in redox reactions. It refers to the movement of electrons from one atom to another during a chemical reaction. Redox reactions involve two interconnected processes:
  • Oxidation: The loss of electrons by an atom or a molecule.
  • Reduction: The gain of electrons by an atom or a molecule.
For a redox reaction to occur, there must be a change in oxidation state, signifying that some atoms have gained electrons while others have lost them. In the given example of converting \(\text{O}_2(g)\) to \(\text{O}_3(g)\), since the oxidation states do not change, there is no electron transfer taking place. Thus, it can be concluded that the reaction is not a redox reaction.
Chemical Reactions
Chemical reactions are processes where reactants convert into products, involving changes in the arrangement of atoms. They can be classified into various types such as:
  • Combination reactions
  • Decomposition reactions
  • Single replacement reactions
  • Double replacement reactions
  • Redox (oxidation-reduction) reactions
In the specific reaction of oxygen molecules forming ozone, the process is a conversion with no electron transfer, hence not a redox reaction.
Chemical reactions involve breaking old bonds and forming new ones, altering the energy dynamics of the atoms involved. However, without electron transfer, the reaction represents a straightforward chemical transformation rather than a redox change. Thus, understanding the nature of electron interactions can reveal the true character of a chemical process.

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Most popular questions from this chapter

Chemical tests of four metals \(\mathrm{A}, \mathrm{B}, \mathrm{C},\) and \(\mathrm{D}\) show the following results. (a) Only \(\mathrm{B}\) and \(\mathrm{C}\) react with \(0.5 \mathrm{M} \mathrm{HCl}\) to give \(\mathrm{H}_{2}\) gas. (b) When \(\mathrm{B}\) is added to a solution containing the ions of the other metals, metallic \(\mathrm{A}, \mathrm{C},\) and \(\mathrm{D}\) are formed. (c) A reacts with \(6 M \mathrm{HNO}_{3}\) but \(\mathrm{D}\) does not. Arrange the metals in the increasing order as reducing agents. Suggest four metals that fit these descriptions.

Distilled water must be used in the gravimetric analysis of chlorides. Why?

On the basis of oxidation number considerations, one of the following oxides would not react with molecular oxygen: \(\mathrm{NO}, \mathrm{N}_{2} \mathrm{O}, \mathrm{SO}_{2}, \mathrm{SO}_{3}, \mathrm{P}_{4} \mathrm{O}_{6}\) Which one is it? Why?

Phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) is an important industrial chemical used in fertilizers, in detergents, and in the food industry. It is produced by two different methods. In the electric furnace method, elemental phosphorus \(\left(\mathrm{P}_{4}\right)\) is burned in air to form \(\mathrm{P}_{4} \mathrm{O}_{10},\) which is then reacted with water to give \(\mathrm{H}_{3} \mathrm{PO}_{4} .\) In the wet process, the mineral phosphate rock fluorapatite \(\left[\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{~F}\right]\) is reacted with sulfuric acid to give \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (and \(\mathrm{HF}\) and \(\mathrm{CaSO}_{4}\) ). Write equations for these processes and classify each step as precipitation, acid-base, or redox reaction.

Ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) with a standard \(\mathrm{NaOH}\) solution. In one experiment a \(0.2041-\mathrm{g}\) sample of industrially prepared \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) required \(24.42 \mathrm{~mL}\) of \(0.1023 \mathrm{M} \mathrm{NaOH}\) for neutralization. (a) Write a net ionic equation for the reaction. (b) What is the percent purity of the sample?
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