Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 18: Problem 23

Do the reactions involved in ozone depletion involve changes in oxidation state of the O atoms? Explain.

Short Answer

Expert verified
In the reactions involved in ozone depletion, the oxidation state of the O atoms does not change. In the formation of ozone from molecular oxygen and the destruction of ozone by chlorine radicals, the oxidation state of O atoms remains the same throughout the reactions.

Step by step solution

01

Identify the main reactions involved in ozone depletion

The main reactions involved in ozone depletion are: 1. Formation of ozone (O3) from molecular oxygen (O2) by ultraviolet (UV) radiation: \[ O_2 + UV \rightarrow 2 O \] \[ O + O_2 \rightarrow O_3 \] 2. Destruction of ozone (O3) by chlorine (Cl) radicals: \[ Cl + O_3 \rightarrow ClO + O_2 \] \[ ClO + O \rightarrow Cl + O_2 \]
02

Determine the oxidation state of O atoms in each reaction

To determine the oxidation state change, we first identify the oxidation state of each element in the reactants and products: 1. Formation of ozone (O3) from molecular oxygen (O2) by ultraviolet (UV) radiation: - O2: Each O atom has an oxidation state of 0, as it's in its elemental form. - O3: Each O atom has an average oxidation state of 0, as they are in different oxidation states but have equal contributions (one O atom is +2, and two O atoms are -1). 2. Destruction of ozone (O3) by chlorine (Cl) radicals: - Cl: The oxidation state is 0, as it's in its elemental form. - ClO: The Cl atom has an oxidation state of +1, and the O atom has an oxidation state of -1.
03

Determine if there's a change in the oxidation state of O atoms

1. Formation of ozone (O3) from molecular oxygen (O2) by ultraviolet (UV) radiation: - In this reaction, the oxidation state of O atoms remains 0 in both O2 and O3. Therefore, there is no change in the oxidation state of the O atoms in this reaction. 2. Destruction of ozone (O3) by chlorine (Cl) radicals: - In the reaction between Cl and O3, there's no change in the oxidation state of the O atoms (-1 in ClO and O3). - In the reaction between ClO and O, again, there's no change in the oxidation state of the O atoms (-1 in ClO and O).
04

Conclusion

In conclusion, the reactions involved in ozone depletion do not involve changes in the oxidation state of the O atoms. Both in the formation of ozone from molecular oxygen and in the destruction of ozone by chlorine radicals, the oxidation state of the O atoms remains the same.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Nitrogen oxides like \(\mathrm{NO}_{2}\) and \(\mathrm{NO}\) are a significant source of acid rain. For each of these molecules write an equation that shows how an acid is formed from the reaction with water.

Why is rainwater naturally acidic, even in the absence of polluting gases such as \(\mathrm{SO}_{2} ?\)

The Earth's oceans have a salinity of \(35 .\) What is the concentration of dissolved salts in seawater when expressed in ppm? What percentage of salts must be removed from sea-water before it can be considered freshwater (dissolved salts \(<500\) ppm \() ?[\operatorname{Section} 18.3]\)

An important reaction in the formation of photochemical smog is the photodissociation of \(\mathrm{NO}_{2} :\) $$\mathrm{NO}_{2}+h \nu \longrightarrow \mathrm{NO}(g)+\mathrm{O}(g)$$ The maximum wavelength of light that can cause this reaction is 420 \(\mathrm{nm}\) . (a) In what part of the electromagnetic spectrum is light with this wavelength found? (b) What is the maximum strength of a bond, in kJ/mol, that can be broken by absorption of a photon of \(420-\mathrm{nm}\) light? (c) Write out the photodissociation reaction showing Lewis-dot structures.

The average concentration of carbon monoxide in air in an Ohio city in 2006 was 3.5 ppm. Calculate the number of CO molecules in 1.0 L of this air at a pressure of 759 torr and a temperature of \(22^{\circ} \mathrm{C}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free