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Chapter 18: Problem 21

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, there are changes in the oxidation state of the O atoms, specifically in the chlorine-catalyzed ozone destruction reactions. In these reactions, the oxidation state of the O atoms changes from 0 to -2, and then back to 0. However, there is no change in the oxidation state of O atoms in the ozone formation and decomposition reactions.

Step by step solution

01

Identify the reactions involved in ozone depletion

The main reactions involved in ozone depletion are the ozone formation and decomposition reactions and chlorine-catalyzed ozone destruction reactions. Ozone formation and decomposition reactions: 1. \( O_2 + O \xrightarrow{Sunlight} O_3 \) 2. \( O_3 + O \xrightarrow{Sunlight} 2O_2 \) Chlorine-catalyzed ozone destruction reactions: 1. \( Cl + O_3 \rightarrow ClO + O_2 \) 2. \( ClO + O \rightarrow Cl + O_2 \)
02

Examine the oxidation states of O atoms

To determine if there are any changes in the oxidation state of the O atoms, let's examine the oxidation states of oxygen in each reaction. Oxidation states: 1. In diatomic oxygen (\( O_2 \)), the oxidation state of an O atom is 0. 2. In ozone (\( O_3 \)), the oxidation state of each O atom in the molecule is 0. 3. In a single O atom, the oxidation state is 0. 4. In the chlorate ion (\( ClO^- \)), the oxidation state of O is -2. Reviewing the reactions: Ozone formations and decomposition reactions: 1. \( O_2 + O \xrightarrow{Sunlight} O_3 \) 0 + 0 鈫� 0 2. \( O_3 + O \xrightarrow{Sunlight} 2O_2 \) 0 + 0 鈫� 0 + 0 Chlorine-catalyzed ozone destruction reactions: 1. \( Cl + O_3 \rightarrow ClO + O_2 \) 0 鈫� -2 + 0 2. \( ClO + O \rightarrow Cl + O_2 \) -2 + 0 鈫� 0 + 0
03

Determine if changes in oxidation state occur

Based on our examination of the oxidation states, we can see that for the ozone formation and decomposition reactions, there is no change in the oxidation state of the O atoms. However, in the chlorine-catalyzed ozone destruction reactions, there is a change in the oxidation state of the O atoms from 0 to -2 and back to 0. Therefore, ozone depletion does involve changes in the oxidation state of the O atoms, particularly in the chlorine-catalyzed ozone destruction reactions.

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Most popular questions from this chapter

Ferrous sulfate \(\left(\mathrm{FeSO}_{4}\right)\) is often used as a coagulant in water purification. The iron(II) salt is dissolved in the water to be purified, then oxidized to the iron(III) state by dissolved oxygen, at which time gelatinous \(\mathrm{Fe}(\mathrm{OH})_{3}\) forms, assuming the \(\mathrm{pH}\) is above approximately \(6 .\) Write balanced chemical equations for the oxidation of \(\mathrm{Fe}^{2+}\) to \(\mathrm{Fe}^{3+}\) by dissolved oxygen and for the formation of \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\) by reaction of \(\mathrm{Fe}^{3+}(a q)\) with \(\mathrm{HCO}_{3}^{-}(a q)\).

The concentration of \(\mathrm{H}_{2} \mathrm{O}\) in the stratosphere is about \(5 \mathrm{ppm}\). It undergoes photodissociation according to: $$ \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{H}(g)+\mathrm{OH}(g) $$ (a) Write out the Lewis-dot structures for both products and reactant. (b) Using Table \(8.4,\) calculate the wavelength required to cause this dissociation. (c) The hydroxyl radicals, OH, can react with ozone, giving the following reactions: $$ \begin{array}{l} \mathrm{OH}(g)+\mathrm{O}_{3}(g) \longrightarrow \mathrm{HO}_{2}(g)+\mathrm{O}_{2}(g) \\ \mathrm{HO}_{2}(g)+\mathrm{O}(g) \longrightarrow \mathrm{OH}(g)+\mathrm{O}_{2}(g) \end{array} $$ What overall reaction results from these two elementary reactions? What is the catalyst in the overall reaction? Explain.

The organic anion is found in most detergents. Assume that the anion undergoes aerobic decomposition in the following manner: $$ \begin{array}{r} 2 \mathrm{C}_{18} \mathrm{H}_{29} \mathrm{SO}_{3}^{-}(a q)+51 \mathrm{O}_{2}(a q) \longrightarrow \\ 36 \mathrm{CO}_{2}(a q)+28 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{H}^{+}(a q)+2 \mathrm{SO}_{4}^{2-}(a q) \end{array} $$ What is the total mass of \(\mathrm{O}_{2}\) required to biodegrade \(10.0 \mathrm{~g}\) of this substance?

The estimated average concentration of \(\mathrm{NO}_{2}\) in air in the United States in 2006 was 0.016 ppm. (a) Calculate the partial pressure of the \(\mathrm{NO}_{2}\) in a sample of this air when the atmospheric pressure is 755 torr \((99.1 \mathrm{kPa})\). (b) How many molecules of \(\mathrm{NO}_{2}\) are present under these conditions at \(20{ }^{\circ} \mathrm{C}\) in a room that measures \(15 \times 14 \times 8 \mathrm{ft}\) ?

One of the principles of green chemistry is that it is better to use as few steps as possible in making new chemicals. How does this principle relate to energy efficiency?
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