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Chapter 2: Problem 72

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: (a) N2O: Dinitrogen monoxide (nitrous oxide) (b) NO: Nitrogen monoxide (nitric oxide) (c) NO2: Nitrogen dioxide (d) N2O5: Dinitrogen pentoxide (e) N2O4: Dinitrogen tetroxide

Step by step solution

01

Determine the oxidation states of nitrogen in each compound

For each compound, we can find the oxidation state of nitrogen by considering the oxidation state of oxygen (-2) and using the formula for the oxidation state in each compound: (a) N2O: the oxidation state must be +1 because 2x(+1) + 1x(-2) = 0 (b) NO: the oxidation state must be +2 because 1x(+2) + 1x(-2) = 0 (c) NO2: the oxidation state must be +4 because 1x(+4) + 2x(-2) = 0 (d) N2O5: the oxidation state must be +5 because 2x(+5) + 5x(-2) = 0 (e) N2O4: the oxidation state must be +4 because 2x(+4) + 4x(-2) = 0
02

Name each compound using common naming conventions for nitrogen oxides

Now that we know the oxidation states of nitrogen in each compound, we can name them: (a) N2O: Dinitrogen monoxide (also known as nitrous oxide or "laughing gas") (b) NO: Nitrogen monoxide (also known as nitric oxide) (c) NO2: Nitrogen dioxide (d) N2O5: Dinitrogen pentoxide (e) N2O4: Dinitrogen tetroxide

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Most popular questions from this chapter

Summarize the evidence used by J. J. Thomson to argue that cathode rays consist of negatively charged particles.

For each of the following elements, write its chemical symbol, locate it in the periodic table, give its atomic number, and indicate whether it is a metal, metalloid, or nonmetal: (a) chromium, (b) helium, (c) phosphorus, (d) zinc, (e) magnesium, (f) bromine, (g) arsenic.

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: $$ \begin{array}{ccc} \hline \text { Compound } & \text { Mass of lodine (g) } & \text { Mass of Fluorine (g) } \\ \hline 1 & 4.75 & 3.56 \\ 2 & 7.64 & 3.43 \\ 3 & 9.41 & 9.86 \\ \hline \end{array} $$ (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 names and charges of the cation and anion in each of the following compounds: (a) \(\mathrm{CaO},\) (b) \(\mathrm{Na}_{2} \mathrm{SO}_{4},\) (c) \(\mathrm{KClO}_{4}\), (d) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\), (e) \(\mathrm{Cr}(\mathrm{OH})_{3}\)

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