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Chapter 10: Problem 140

Ozone \(\left(\mathrm{O}_{3}\right)\) is a strong oxidizing agent. Explain why this is so.

Short Answer

Expert verified
Ozone (\(\mathrm{O}_{3}\)) is a strong oxidizing agent due to its molecular structure and low bond dissociation energy. The structure of ozone comprises three oxygen atoms and can also be represented as a resonance hybrid of two main Lewis structures, leading to a bent molecular geometry with 116.8-degree angles. Furthermore, the bond dissociation energy of the oxygen-oxygen single bond in ozone is relatively low, about 37 kcal/mol, allowing ozone to break down easily into an oxygen molecule and a highly reactive oxygen radical (O·). This radical has an unpaired electron, making it highly reactive, and thus participating in various oxidation reactions. As a result, ozone can effectively oxidize a wide range of substances due to its tendency to generate potent oxygen radicals.

Step by step solution

01

Understand the ozone molecule structure

Ozone (O3) is a triatomic molecule consisting of three oxygen atoms. The structure of ozone can be represented as a resonance hybrid of two main Lewis structures with a central oxygen atom doubly bonded to one of the noncentral oxygen atoms and singly bonded to the other noncentral oxygen atom. A lone electron pair is present on the central oxygen atom. This structure results in an overall molecular geometry of approximately bent, with bond angles of approximately 116.8 degrees.
02

Determine bond dissociation energy

Bond dissociation energy is the energy needed to break a bond to form free radicals. The bond dissociation energy of the oxygen-oxygen single bond in ozone is relatively low, approximately 37 kcal/mol. A lower bond dissociation energy indicates that the bond is weaker and can be more easily broken, creating oxygen radicals.
03

Understand the formation of oxygen radicals

When ozone undergoes homolytic cleavage, an oxygen molecule (O2) and a highly reactive oxygen radical (O·) are formed. The oxygen radical has an unpaired electron that makes it very reactive and can readily undergo various chemical reactions, including oxidation reactions.
04

Explain the oxidizing ability of ozone

Ozone is a strong oxidizing agent because it can easily break down into an oxygen molecule (O2) and a highly reactive oxygen radical (O·). The oxygen radical is then able to participate in various oxidation reactions due to its high reactivity resulting from the unpaired electron. Consequently, ozone can oxidize various substances by transferring the oxygen radical to the target substance during the oxidation process, making it a potent oxidizing agent.

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Most popular questions from this chapter

Assign an oxidation number to each atom and identify the oxidizing agent and reducing agent: \(3 \mathrm{Na}_{2} \mathrm{SO}_{3}+2 \mathrm{KMnO}_{4}+\mathrm{H}_{2} \mathrm{O} \rightarrow\) \(3 \mathrm{Na}_{2} \mathrm{SO}_{4}+2 \mathrm{MnO}_{2}+2 \mathrm{KOH}\)

You are trapped on a desert island with plenty of water (both fresh and salt), a drinking glass, some wire, a radio, and no batteries. You do have a tin cup, a tube of toothpaste containing stannous fluoride \(\left(\mathrm{Sn} \mathrm{F}_{2}\right.\), a source of \(\mathrm{Sn}^{2+}\) ions), a silver pendant, and undeveloped black-andwhite film (such film has silver bromide, \(\mathrm{AgBr}\), in it, a source of \(\mathrm{Ag}^{+}\) ions). (a) How would you use the above materials to construct a battery? Show how with a diagram, including an arrow over the wire to show which way the electrons flow. (You can make a salt bridge by soaking a sock in salt water and then dipping one end of the sock in one cell and the other end in the other cell.) (b) Which metal would be eaten away? Explain. (c) Which is the oxidizing agent? (d) Which is the reducing agent?

Identify the oxidizing and reducing agents in the reaction \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} \rightarrow \mathrm{N}_{2}+\mathrm{Cr}_{2} \mathrm{O}_{3}+4 \mathrm{H}_{2} \mathrm{O}\)

Use the shortcut rules to assign an oxidation state to each atom: (a) \(\mathrm{NaPO}_{3}\) (b) \(\mathrm{B}(\mathrm{OH})_{3}\) (c) \(\mathrm{V}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{K}_{2} \mathrm{TiF}_{6}\)

A battery consists of a strip of titanium metal in a solution of \(\mathrm{Ti}^{2+}\) ions connected to a strip of zinc metal in a solution of \(\mathrm{Zn}^{2+}\) ions. Over time, the concentration of \(\mathrm{Zn}^{2+}\) ions decreases and the concentration of \(\mathrm{Ti}^{2+}\) ions increases. (a) Which metal is the anode? (b) Which metal is the cathode? (c) Where must titanium be on the EMF scale relative to zinc? (d) Write an equation that describes the spontaneous electron-transfer reaction occurring in this battery.
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