/*! 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 57 Ozone is desirable in the upper ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 19: Problem 57

Ozone is desirable in the upper atmosphere but undesirable in the lower atmosphere. A dictionary states that ozone has the scent of a spring thunderstorm. How can these seemingly conflicting statements be reconciled in terms of the chemical properties of ozone?

Short Answer

Expert verified
Ozone (O3) is a powerful oxidizing agent and plays different roles in the atmosphere. In the upper atmosphere (stratosphere), ozone is crucial for protecting life on Earth from harmful UV radiation by acting as a shield. In the lower atmosphere (troposphere), it acts as a pollutant, reacting with other substances to form harmful compounds, causing respiratory and eye irritation, and is a major component of smog. The distinct scent of ozone, often associated with a spring thunderstorm, is the result of ozone's strong oxidizing properties reacting with other molecules in the atmosphere. Thus, these seemingly conflicting statements can be reconciled when considering ozone's chemical properties and its varying roles in the atmosphere.

Step by step solution

01

Understanding ozone's chemical properties

Ozone (O3) is a gas composed of three oxygen atoms, which makes it less stable than the more common diatomic oxygen molecule (O2). Ozone is a powerful oxidizing agent, meaning it can easily react with other substances, and in large concentrations, ozone can be harmful to living organisms.
02

Ozone's role in the upper atmosphere

In the upper atmosphere (specifically, the stratosphere), ozone plays a crucial role in protecting life on Earth from harmful ultraviolet (UV) radiation. Ozone absorbs the high-energy UV radiation from the sun, effectively acting as a shield and preventing most of it from reaching Earth's surface. This process is essential for maintaining a stable and life-supporting environment on our planet.
03

Ozone's role in the lower atmosphere

In the lower atmosphere (troposphere), ozone acts as a pollutant. This is because ozone formed close to the ground can react with various other substances, leading to the formation of harmful compounds. These compounds can cause respiratory and eye irritation and exacerbate existing health problems, particularly in susceptible individuals such as those with asthma or other respiratory issues. Ozone in the lower atmosphere is harmful to humans, animals, and plants, and is a major component of smog.
04

The scent of ozone

Ozone has a distinct scent that is often described as similar to that of a spring thunderstorm. This scent is the product of ozone's strong oxidizing properties. The electrical discharges from thunderstorms (lightning) can cause the formation of ozone, which then reacts with other molecules in the atmosphere, producing the distinct scent.
05

Reconciling the seemingly conflicting statements

Based on our understanding of ozone's chemical properties, we can reconcile the statements mentioned in the exercise. While ozone is an essential component of the upper atmosphere that protects life on Earth from harmful ultraviolet radiation, it is also a harmful pollutant in the lower atmosphere due to its reactivity and negative effects on human health and the environment. The distinct scent of ozone after a spring thunderstorm is a result of the chemical reactions occurring due to ozone's strong oxidizing properties.

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!

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

Discuss the importance of the \(\mathrm{C}-\mathrm{C}\) and \(\mathrm{Si}-\mathrm{Si}\) bond strengths and of \(\pi\) bonding to the properties of carbon and silicon.

While selenic acid has the formula \(\mathrm{H}_{2} \mathrm{SeO}_{4}\) and thus is directly related to sulfuric acid, telluric acid is best visualized as \(\mathrm{H}_{6} \mathrm{TeO}_{6}\) or \(\mathrm{Te}(\mathrm{OH})_{6}\) a. What is the oxidation state of tellurium in \(\operatorname{Te}(\mathrm{OH})_{6} ?\) b. Despite its structural differences with sulfuric and selenic acid, telluric acid is a diprotic acid with \(\mathrm{p} K_{\mathrm{a}_{1}}=7.68\) and \(\mathrm{p} K_{\mathrm{a}_{2}}=11.29 .\) Telluric acid can be prepared by hydrolysis of tellurium hexafluoride according to the equation $$\operatorname{TeF}_{6}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\operatorname{Te}(\mathrm{OH})_{6}(a q)+6 \mathrm{HF}(a q)$$ Tellurium hexafluoride can be prepared by the reaction of elemental tellurium with fluorine gas:$$\operatorname{Te}(s)+3 \mathrm{F}_{2}(g) \longrightarrow \operatorname{Te} \mathrm{F}_{6}(g)$$.If a cubic block of tellurium (density \(=6.240 \mathrm{g} / \mathrm{cm}^{3}\) ) measuring \(0.545 \mathrm{cm}\) on edge is allowed to react with 2.34 L fluorine gas at 1.06 atm and \(25^{\circ} \mathrm{C}\), what is the \(\mathrm{pH}\) of a solution of \(\mathrm{Te}(\mathrm{OH})_{6}\) formed by dissolving the isolated \(\operatorname{Te} \mathrm{F}_{6}(g)\) in \(115 \mathrm{mL}\) solution? Assume \(100 \%\) yield in all reactions.

For each of the following, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybridization of the central atom. a. \(\mathrm{KrF}_{2}\) c. \(\mathrm{XeO}_{2} \mathrm{F}_{2}\) b. \(\mathrm{KrF}_{4}\) d. \(\mathrm{XeO}_{2} \mathrm{F}_{4}\)

Use bond energies to estimate the maximum wavelength of light that will cause the reaction $$\mathrm{O}_{3} \stackrel{h v}{\longrightarrow} \mathrm{O}_{2}+\mathrm{O}$$

Nitrous oxide \(\left(\mathrm{N}_{2} \mathrm{O}\right)\) can be produced by thermal decomposition of ammonium nitrate:$$\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \stackrel{\text { heat}}{\rightarrow} \mathrm{N}_{2} \mathrm{O}(g)+2 \mathrm{H}_{2} \mathrm{O}(l).$$ What volume of \(\mathrm{N}_{2} \mathrm{O}(g)\) collected over water at a total pressure of \(94.0 \mathrm{kPa}\) and \(22^{\circ} \mathrm{C}\) can be produced from thermal decomposition of \(8.68 \mathrm{g} \mathrm{NH}_{4} \mathrm{NO}_{3} ?\) The vapor pressure of water at \(22^{\circ} \mathrm{C}\) is 21 torr.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Organic Chemistry

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.