Chapter 20

Write the Lewis structure of \(\mathrm{P}_{4}\).

What is meant by the fixation of nitrogen with hydrogen?

Write the Lewis structures of \(\mathrm{NO}_{2}\) and \(\mathrm{N}_{2} \mathrm{O}_{3}\). What is the hybridization of the nitrogen atoms in each compound?

Write the Lewis structures of \(\mathrm{N}_{2} \mathrm{O}\) and \(\mathrm{N}_{2} \mathrm{O}_{4} .\) What is the hybridization of the nitrogen atoms in each?

Write an equation for each of the following reactions. (a) reaction between magnesium and nitrogen (b) preparation of \(\mathrm{P}_{4} \mathrm{O}_{10}\) (c) reaction of nitrogen dioxide with water

Write an equation for each of the following reactions. (a) preparation of dinitrogen oxide (b) reaction of hydrazine with oxygen (c) reaction between \(\mathrm{P}_{4} \mathrm{O}_{10}\) and water

Write two reactions that show how NO gas can catalytically decompose large amounts of ozone, \(\mathrm{O}_{3}\).

\text { How is nitric acid prepared by the Ostwald process? }

The largest use of nitric acid is in the production of ammonium nitrate. Write the equation for this process.

Describe two allotropic forms of sulfur.

Identify the three main types of reactions that sulfuric acid undergoes.

Draw the Lewis structures and assign the shapes of \(\mathrm{XeF}_{2}\) and \(\mathrm{XeO}_{3}\). Is either of these compounds polar?

Draw the Lewis structures and assign the shapes of \(\mathrm{XeF}_{4}\) and \(\mathrm{XeO}_{4}\). Is either of these compounds polar?

Write the equation for the oxidation of ammonia to nitrogen monoxide (the first step in the Ostwald process). What mass of ammonia is needed to produce \(25 \mathrm{~kg}\) nitrogen monoxide?

Write the equation for the preparation of ammonium nitrate from \(\mathrm{NH}_{3}\). What mass of ammonia is needed to produce \(5.22 \mathrm{~kg}\) ammonium nitrate?

Compare the boiling points of \(\mathrm{NH}_{3}\) and \(\mathrm{PH}_{3}\), and explain the difference.

Given that the \(\mathrm{H}-\mathrm{P}-\mathrm{H}\) angles in phosphine are about 90 degrees, what orbitals on the phosphorus are used to make the \(\mathrm{H}-\mathrm{P}\) bonds?

Oxygen can be prepared in the laboratory by heating \(\mathrm{KClO}_{3}\) in the presence of \(\mathrm{MnO}_{2}\). Write the equation; then determine the mass of \(\mathrm{KClO}_{3}\) needed to produce \(0.50 \mathrm{~L}\) \(\mathrm{O}_{2}\) gas at \(27{ }^{\circ} \mathrm{C}\) and 755 torr pressure.

Write the equation for the roasting of lead sulfide. What volume of \(\mathrm{SO}_{2}\) gas measured at standard temperature and pressure is produced from the roasting of \(1.0 \times 10^{2} \mathrm{~g}\) lead sulfide?

As outlined in this chapter, hydrazine is used to remove oxygen from water used in boilers of electrical generating plants. If the water contains \(2.0 \times 10^{-8} \mathrm{~g} \mathrm{O}_{2}\) per gram of water, what mass of hydrazine is needed to remove the oxygen in 10 tons of water?

What is the most important crystal force that holds each of the following substances together? (a) \(\mathrm{Pb}\) (b) \(\mathrm{SiO}_{2}\) (c) \(\mathrm{P}_{4}\) (d) buckyballs

Write the Lewis structure and use valence shell electronpair repulsion theory to predict the shape of \(\mathrm{XeF}_{4} \mathrm{O}_{2}\).

Draw all possible resonance forms of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{HNO}_{3}\). Explain why resonance forms that do not show formal charges can be written for \(\mathrm{H}_{2} \mathrm{SO}_{4}\) but not \(\mathrm{HNO}_{3}\).

Write the Lewis structure and molecular orbital diagram for NO. What bond order and number of unpaired electrons does each predict for \(\mathrm{NO}\) ?