Chapter Questions
Starting with $\mathrm{N}_2$, describe completely the commercial synthesis of nitric acid.
Explain why numerous nitrogen compounds are explosive.
Explain why the $\mathrm{NF}_5$ molecule does not exist (although $\mathrm{NF}_4{ }^{+} \mathrm{F}^{-}$is known), whereas $\mathrm{PF}_5$ exists as a molecule.
Draw structures for the following species:(a) Diimine(b) Hydrazine(c) Hyponitrous acid(d) The cyanamide ion(e) Hydroxylamine
Write the series of balanced equations for the preparation of hydrazine.
Explain why $\mathrm{NH}_3$ is more polar than $\mathrm{NCl}_3$.
Complete and balance the following.(a) $\mathrm{NH}_4 \mathrm{NO}_2 \stackrel{\text { heat }}{\longrightarrow}$(b) $\mathrm{Mg}+\mathrm{N}_2 \mathrm{O} \rightarrow$(c) $\mathrm{Zn}+\mathrm{HNO}_3($ dil $) \rightarrow$(d) $\mathrm{N}_2 \mathrm{O}_3+\mathrm{NaOH} \rightarrow$(e) $\mathrm{NO}_2+\mathrm{H}_2 \mathrm{O} \rightarrow$
When a burning strip of magnesium is thrust into a bottle containing $\mathrm{N}_2 \mathrm{O}$, it continues to burn. Write the equation for the reaction, and explain how it lends support for the structure of $\mathrm{N}_2 \mathrm{O}$ being what it is known to be.
Both hyponitrous acid and nitroamide (also known as nitramide) have the formula $\mathrm{H}_2 \mathrm{~N}_2 \mathrm{O}_2$. Draw the structures for these molecules, and explain any difference in acidbase properties.
Draw the structure for nitrosyl chloride. After you have drawn the correct structure, draw structures showing how the atoms would not be arranged and explain why they would not be arranged in that order. What symmetry elements does the nitrosyl chloride possess?
Some metals do not react extensively with nitric acid. What is the reason for this behavior?
There is only a slight difference in the $\mathrm{N}-\mathrm{O}$ bond lengths in the $\mathrm{FNO}, \mathrm{CINO}$, and $\mathrm{BrNO}$ molecules. Predict which would have the shortest $\mathrm{N}-\mathrm{O}$ bond length. Which would have the longest $\mathrm{N}-\mathrm{O}$ bond length? Explain your predictions.
Complete the following equations for reactions that take place in liquid ammonia.(a) $\mathrm{Li}_3 \mathrm{~N}+\mathrm{NH}_4 \mathrm{Cl} \rightarrow$(b) $\mathrm{CaNH}+\mathrm{NH}_3 \rightarrow$(c) $\mathrm{NaH}+\mathrm{NH}_3 \rightarrow$(d) $\mathrm{KNH}_2+\mathrm{NH}_4 \mathrm{~F} \rightarrow$(e) $\mathrm{AgCl}+\mathrm{NaNO}_3 \rightarrow$
(a) Write the equation for the autoionization of liquid $\mathrm{N}_2 \mathrm{O}_4$.(b) Write the formula for a substance that would be an acid in liquid $\mathrm{N}_2 \mathrm{O}_4$.(c) Write the formula for a substance what would be a base in liquid $\mathrm{N}_2 \mathrm{O}_4$.(d) Write the neutralization reaction for the acid in (b) with the base in (c).
The base constants for hydrazine are $K_{\mathrm{b} 1}=8.5 \times 10^{-7}$ and $K_{\mathrm{b} 2}=8.9 \times 10^{-16}$. Explain this large difference between the $K_{\mathrm{b}}$ values.
The bond angles in $\mathrm{FNO}, \mathrm{CINO}$, and $\mathrm{BrNO}$ are $110^{\circ}, 113^{\circ}$, and $117^{\circ}$, respectively. Explain this trend.
The molecule $\mathrm{N}_4 \mathrm{O}$ is nitrosyl azide. Draw the structure of this molecule and describe the bonding.
In most compounds that contain $\mathrm{N}=\mathrm{O}$ bonds, the length of the bond is approximately $120 \mathrm{pm}$. Explain why the bond length in $\mathrm{NO}^{+}$and gaseous $\mathrm{NO}$ differ from that value.
Complete and balance the following.(a) $\mathrm{CaCN}_2+\mathrm{H}_2 \mathrm{O} \rightarrow$(b) $\mathrm{NH}_4 \mathrm{NO}_3 \stackrel{\text { heat }}{\longrightarrow}$(c) $\mathrm{NBr}_3+\mathrm{H}_2 \mathrm{O} \rightarrow$(d) $\mathrm{SeF}_4+\mathrm{N}_2 \mathrm{~F}_4 \rightarrow$(c) $\mathrm{PF}_5+\mathrm{N}_2 \mathrm{~F}_2 \rightarrow$
Account for the fact that the $\mathrm{N}-\mathrm{N}$ bond length in $\mathrm{N}_2 \mathrm{O}_3$ is $186 \mathrm{pm}$ although that in $\mathrm{N}_2 \mathrm{H}_4$ is $145 \mathrm{pm}$.