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Chapter 2: Problem 1

How does ozone differ from oxygen in its chemical formula? In its properties?

Short Answer

Expert verified
Oxygen is \(O_2\), and is essential for respiration; ozone is \(O_3\), blocking UV rays but can be a pollutant.

Step by step solution

01

Understand Chemical Formulas

The chemical formula tells us the number and type of atoms in a molecule. Oxygen, in its common form, exists as a diatomic molecule with the chemical formula \(O_2\), meaning it consists of two oxygen atoms. Ozone, on the other hand, has the chemical formula \(O_3\), indicating that it consists of three oxygen atoms.
02

Analyze Physical Properties

Oxygen is a colorless, odorless gas at room temperature, essential for animal and plant respiration. It supports combustion and is highly reactive with many elements. Ozone, however, is a pale blue gas with a distinct sharp smell at the same conditions and serves as a protective layer in the Earth's stratosphere, absorbing harmful ultraviolet radiation. Ozone is also less stable than molecular oxygen and can be a powerful oxidizing agent.
03

Consider Environmental Roles

While molecular oxygen is crucial for life, providing the air we breathe, ozone has a more complex role. In the stratosphere, it forms the ozone layer which is critical for blocking harmful UV radiation. However, at the ground level, ozone can be a pollutant contributing to smog and respiratory problems in living organisms.

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Key Concepts

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

Chemical Formula
The concept of a chemical formula is fundamental in chemistry as it shows the composition and quantity of atoms within a molecule.
When examining oxygen, its most common form called dioxygen is represented by the chemical formula \(O_2\). This indicates that a molecule of oxygen consists of two oxygen atoms bonded together.
Ozone, however, differs by having the chemical formula \(O_3\). In this case, the molecule is composed of three oxygen atoms.
These differing formulas imply distinct characteristics and roles for each form of oxygen.
Physical Properties
Understanding the physical properties of substances like oxygen and ozone is crucial in determining their behavior and applications.
Oxygen is a colorless and odorless gas under standard conditions such as room temperature. It is essential to life as it is used in respiration by many living organisms. Oxygen is also known for supporting combustion, which makes it reactive with a wide array of elements.
On the other hand, ozone presents itself as a pale blue gas with a sharp, distinctive smell. Ozone's higher reactivity compared to oxygen makes it a powerful oxidizing agent, but it is also less stable, which means it can decompose and change the chemical makeup more easily.
These distinct physical properties highlight their unique applications and impacts in the environment.
Environmental Roles
Oxygen and ozone have different, yet crucial roles in the environment.
Molecular oxygen (\(O_2\)) is indispensable for life on Earth as it provides the oxygen necessary for the process of respiration in both animals and plants.
In contrast, ozone (\(O_3\)) plays a more specialized role in the Earth's stratosphere by forming the protective ozone layer. This layer absorbs and scatters the sun's ultraviolet radiation, preventing it from reaching the surface in harmful amounts.
While ozone is beneficial high in the atmosphere, it can pose significant problems at ground level. It can act as a pollutant contributing to smog, leading to respiratory issues and other health problems for living organisms.
Understanding these roles emphasizes the importance of balance and sustainability in environmental health.

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Most popular questions from this chapter

Assuming that the octet rule applies, draw the Lewis structure for each of these molecules. a. \(\mathrm{CCl}_{4}\) (carbon tetrachloride, a substance formerly used as a cleaning agent) b. \(\mathrm{H}_{2} \mathrm{O}_{2}\) (hydrogen peroxide, a mild disinfectant; the atoms are bonded in this order: \(\mathrm{H}-\mathrm{O}-\mathrm{O}-\mathrm{H})\) c. \(\mathrm{H}_{2} \mathrm{~S}\) (hydrogen sulfide, a gas with the unpleasant odor of rotten eggs) d. \(\mathrm{N}_{2}\) (nitrogen gas, the major component of the atmosphere) e. HCN (hydrogen cyanide, a molecule found in space and a poisonous gas) f. \(\mathrm{N}_{2} \mathrm{O}\) (nitrous oxide, "laughing gas"; the atoms are bonded \(\mathrm{N}-\mathrm{N}-\mathrm{O}\) ) g. \(\mathrm{CS}_{2}\) (carbon disulfide, used to kill rodents; the atoms are bonded \(S-C-S\) )

The text states that the odor of ozone can be detected in concentrations as low as \(10 \mathrm{ppb}\). Would you be able to smell ozone in either of these air samples? a. \(0.118 \mathrm{ppm}\) of ozone, a concentration reached in an urban area b. \(25 \mathrm{ppm}\) of ozone, a concentration measured in the stratosphere

Give the name and symbol for the element with this number of protons. a. 2 b. 19 c. 29

Consider the Lewis structures for \(\mathrm{SO}_{2}\). How do they compare with the Lewis structures for ozone?

Resonance structures can be used to explain the bonding in charged groups of atoms as well as in neutral molecules, such as ozone. The nitrate ion, \(\mathrm{NO}_{3}{ }^{-}\), has one additional electron plus the outer electrons contributed by nitrogen and oxygen atoms. That extra electron gives the ion its charge. Draw the resonance structures, verifying that each obeys the octet rule.
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