/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 140 Ozone \(\left(\mathrm{O}_{3}\rig... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

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路). 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路) 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路). 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.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Ozone structure
Ozone \(\left(\mathrm{O}_{3}\right)\) is a fascinating molecule with three oxygen atoms. It's not arranged in a straight line, but rather in a bent shape. This is because of its unique resonance structure. Resonance involves the sharing of electrons between different configurations, allowing the molecule to stabilize itself.

The central oxygen atom forms a double bond with one of the outer oxygen atoms and a single bond with the other, while also holding a lone pair of electrons. All this gives ozone its distinct bent appearance with a bond angle around 116.8 degrees. The structure is key to its properties, especially its role as an oxidizing agent.
Bond dissociation energy
Bond dissociation energy is the energy required to break a bond in a molecule. For ozone, the splitting of the oxygen-oxygen single bond requires about 37 kcal/mol.

This energy is relatively low, meaning the bond is weak and can be easily broken. When this bond breaks, it forms free radicals, which are highly reactive species.
  • Weak bonds break easily, releasing energy.
  • Low energy requirements lead to the formation of radicals.
Understanding this allows us to see why ozone is ready to participate in chemical reactions by creating these potent radicals.
Formation of oxygen radicals
When ozone breaks down, it doesn't just vanish; it transforms. This transformation is known as homolytic cleavage. During this process, ozone splits into an oxygen molecule \(\left(\mathrm{O}_{2}\right)\) and an oxygen radical \(\left(\mathrm{O}\cdot\right)\).

Oxygen radicals are incredibly reactive due to their unpaired electron, which seeks another atom or molecule to pair with. This makes them eager participants in chemical reactions, including oxidation. Here's what happens:
  • The breaking of the ozone bond releases a radical.
  • This radical carries an unpaired electron.
  • The unpaired electron drives chemical reactivity.
These attributes are why oxygen radicals are central to ozone's role as a robust oxidizing agent.
Oxidation reactions
Ozone is renowned for its ability to oxidize substances鈥攁 process crucial to many chemical and environmental processes.

When ozone breaks into an oxygen molecule and a radical, the oxygen radical's high reactivity comes into play. This radical seeks other substances to react with, initiating oxidation.
  • Ozone decomposes into reactive radicals.
  • These radicals interact with other substances.
  • They transfer oxygen, causing oxidation.
As a strong oxidizing agent, ozone can transform chemicals by adding oxygen to them or removing electrons. This property makes it powerful but also hazardous if not controlled.

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

The blood alcohol level of a person can be detected by reacting a sample of blood plasma with dichromate ion, \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}\), which takes part in an electron-transfer reaction with ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\), in the blood: \(2 \mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}+16 \mathrm{H}^{+} \rightarrow\) \(4 \mathrm{Cr}^{3+}+2 \mathrm{CO}_{2}+11 \mathrm{H}_{2} \mathrm{O}\) Assign an oxidation state to each atom in this reaction and indicate the oxidizing agent and the reducing agent.

Metal strips are immersed in aqueous solutions of various salts. In which combinations do you expect a spontaneous redox reaction: (a) Silver strip in \(\operatorname{CuBr}_{2}(a q)\) (b) Copper strip in \(\mathrm{ZnSO}_{4}(a q)\) (c) Zinc strip in \(\operatorname{AgNO}_{3}(a q)\) (d) Gold strip in \(\mathrm{FeCl}_{2}(a q)\) (e) Copper strip in \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

A student claims that in his battery, the electrons flow from the positive to the negative electrode. In fact, this is not true for any battery. Explain why electrons would never flow in this direction and how the direction of electron flow tells you that the cathode is where reduction occurs.

A battery was produced using copper metal in a solution of Cu \(^{2+}\) ions connected to rhodium metal in a solution of \(\mathrm{Rh}^{3+}\) ions. Copper is the anode and rhodium is the cathode. Is rhodium higher or lower than copper in the EMF series?

A piece of magnesium can be attached to the iron hull of a boat to prevent it from rusting. (a) Why is the magnesium called a sacrificial metal? (b) How does the Mg keep the iron hull from rusting? (c) Which can be thought of as the positive cathode, the \(\mathrm{Mg}\) or the steel hull? Explain. (d) Putting a block of \(\mathrm{Mg}\) on a steel boat hull does not create a battery. Why not?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

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.