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Chapter 2: Problem 78

The oxides of nitrogen are very important components in urban air pollution. Name each of the following compounds: (a) \(\mathrm{N}_{2} \mathrm{O}\) \(,(\mathbf{b}) \mathrm{NO}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (e) \(\mathrm{N}_{2} \mathrm{O}_{4}\)

Short Answer

Expert verified
The names of the given nitrogen oxide compounds are as follows: (a) \(N_{2}O\) is called dinitrogen monoxide. (b) \(NO\) is called nitrogen oxide. (c) \(NO_{2}\) is called nitrogen dioxide. (d) \(N_{2}O_{5}\) is called dinitrogen pentoxide. (e) \(N_{2}O_{4}\) is called dinitrogen tetroxide.

Step by step solution

01

(a) Naming N2O

This compound has two nitrogen (N) atoms and one oxygen (O) atom. In order to name this compound, we use the prefix "di-" for two nitrogen atoms and the prefix "mono-" for one oxygen atom. Therefore, the name for this compound is "dinitrogen monoxide".
02

(b) Naming NO

This compound has one nitrogen (N) atom and one oxygen (O) atom. As there's only one of each element, we don't need to use prefixes. We can simply combine the names of the elements, and the name for this compound is "nitrogen oxide".
03

(c) Naming NO2

This compound has one nitrogen (N) atom and two oxygen (O) atoms. We use the prefix "di-" for two oxygen atoms. So, the name for this compound is "nitrogen dioxide".
04

(d) Naming N2O5

In this compound, there are two nitrogen (N) atoms and five oxygen (O) atoms. We use the prefix "di-" for two nitrogen atoms and "penta-" for five oxygen atoms. Thus, the name for this compound is "dinitrogen pentoxide".
05

(e) Naming N2O4

This compound consists of two nitrogen (N) atoms and four oxygen (O) atoms. We use the prefix "di-" for two nitrogen atoms and "tetra-" for four oxygen atoms. The name for this compound is "dinitrogen tetroxide".

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Key Concepts

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

Understanding Nitrogen Oxides
Nitrogen oxides are a group of gases that contain nitrogen and oxygen in varying quantities. These gases are crucial players in urban air pollution. Nitrogen oxides can exist in different forms, depending on the number of nitrogen and oxygen atoms they contain. Here are a few common forms:
  • Dinitrogen monoxide ( N_2O): Contains two nitrogen atoms and one oxygen atom.
  • Nitrogen oxide ( NO): Made up of one nitrogen atom and one oxygen atom.
  • Nitrogen dioxide ( NO_2): Comprises one nitrogen atom and two oxygen atoms.
  • Dinitrogen pentoxide ( N_2O_5): Consists of two nitrogen atoms and five oxygen atoms.
  • Dinitrogen tetroxide ( N_2O_4): Made up of two nitrogen atoms and four oxygen atoms.
These various compounds contribute to different environmental issues, such as acid rain and smog. Learning their names is crucial for understanding their respective roles in environmental chemistry.
Chemical Nomenclature
Chemical nomenclature is the systematic method of naming chemical compounds. It helps scientists accurately describe the composition and structure of compounds. This system uses names that are informative and standardized, reducing confusion. Here are some basics of naming chemical compounds:
  • Prefixes are used to indicate the number of atoms. "Mono-" is for one, "di-" for two, "tri-" for three, and so forth.
  • The element closest to the left on the periodic table is usually named first.
  • The second element typically ends with "-ide." This suffix suggests that the element is acting as a negatively charged ion.
In the case of nitrogen oxides:
  • N_2O is called dinitrogen monoxide. "Di-" signifies two nitrogen atoms, and "mono-" indicates one oxygen atom.
  • NO is nitrogen oxide, needing no prefix due to having one of each atom.
  • NO_2 is nitrogen dioxide. The "di-" prefix shows there are two oxygen atoms.
Having a clear understanding of chemical nomenclature helps in communicating chemical compositions and reactions effectively.
Air Pollution Chemistry
Air pollution chemistry focuses on the chemical processes taking place in the atmosphere that are caused by pollutants, such as nitrogen oxides. These compounds, when released into the atmosphere, can undergo several reactions leading to significant environmental impacts:
  • Nitrogen oxides are major contributors to smog formation. Once in the atmosphere, they can react with volatile organic compounds in sunlight to produce photochemical smog.
  • They are also involved in the formation of acid rain. When nitrogen oxides react with water vapor in the air, they can form nitric acid, which then precipitates as acid rain.
  • The presence of nitrogen dioxide ( NO_2) can compromise air quality, leading to respiratory problems in humans.
Understanding these chemical processes is key to addressing air quality issues, crafting regulations to limit emissions, and developing technologies to reduce pollutants.

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Most popular questions from this chapter

Locate each of the following elements in the periodic table; give its name and atomic number, and indicate whether it is a metal, metalloid, or nonmetal: (a) \(\mathrm{Hg},(\mathbf{b}) \mathrm{At},(\mathbf{c}) \mathrm{Mo},\) (d) \(\mathrm{W},(\mathbf{e}) \mathrm{Sn},(\mathbf{f}) \mathrm{V},(\mathbf{g}) \mathrm{K}\).

There are two different isotopes of bromine atoms. Under normal conditions, elemental bromine consists of \(\mathrm{Br}_{2}\) molecules, and the mass of a \(\mathrm{Br}_{2}\) molecule is the sum of the masses of the two atoms in the molecule. The mass spectrum of \(\mathrm{Br}_{2}\) consists of three peaks: $$ \begin{array}{lc} \hline \text { Mass (u) } & \text { Relative Size } \\ \hline 157.836 & 0.2569 \\ 159.834 & 0.4999 \\ 161.832 & 0.2431 \\ \hline \end{array} $$ (a) What is the origin of each peak (of what isotopes does each consist)? (b) What is the mass of each isotope? (c) Determine the average molecular mass of a \(\mathrm{Br}_{2}\) molecule. (d) Determine the average atomic mass of a bromine atom. (e) Calculate the abundances of the two isotopes.

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: $$ \begin{array}{lcc} \hline \text { Compound } & \text { Mass of Iodine (g) } & \text { Mass of Fluorine (g) } \\ \hline 1 & 4.75 & 3.56 \\ 2 & 7.64 & 3.43 \\ 3 & 9.41 & 9.86 \\ \hline \end{array} $$ (a) Calculate the mass of fluorine per gram of iodine in each compound. (b) How do the numbers in part (a) support the atomic theory?

Give the chemical names of each of the following familiar compounds: (a) \(\mathrm{NaCl}\) (table salt), (b) \(\mathrm{NaHCO}_{3}\) (baking soda), (c) NaOCl (in many bleaches),(d) \(\mathrm{NaOH}\) (caustic soda), (e) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}\) (smelling salts), (f) \(\mathrm{CaSO}_{4}\) (plaster of Paris).

Sodium reacts with oxygen in air to form two compounds: sodium oxide and sodium peroxide. In forming sodium oxide, \(23.0 \mathrm{~g}\) of sodium combines with \(8.0 \mathrm{~g}\) of hydrogen. In forming sodium peroxide, \(23.0 \mathrm{~g}\) of sodium combines with \(16.0 \mathrm{~g}\) of oxygen. (a) What are the mass ratios of oxygen in the two compounds? (b) What fundamental law does this experiment demonstrate?
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