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Chapter 9: Problem 30

Which of the following would show hydrogen bonding? (a) \(\mathrm{CH}_{3} \mathrm{~F}\) (b) \(\mathrm{HO}-\mathrm{OH}\) (c) \(\mathrm{NH}_{3}\) (d) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{O}-\mathrm{CH}_{3}\)

Short Answer

Expert verified
(a) \(\mathrm{CH}_{3} \mathrm{F}\) (b) \(\mathrm{HO}-\mathrm{OH}\) (c) \(\mathrm{NH}_{3}\) (d) \(\mathrm{H}_{3} \mathrm{C}-\mathrm{O}-\mathrm{CH}_{3}\) Answer: (b) \(\mathrm{HO}-\mathrm{OH}\) and (c) \(\mathrm{NH}_{3}\)

Step by step solution

01

Analyze Molecule (a) - \(\mathrm{CH}_{3} \mathrm{F}\)

The first molecule features a covalent bond between carbon and fluorine, with three hydrogen atoms bonded to the carbon. However, none of the hydrogen atoms are attached to a highly electronegative atom such as nitrogen, oxygen, or fluorine. Therefore, hydrogen bonding cannot occur in this molecule.
02

Analyze Molecule (b) - \(\mathrm{HO}-\mathrm{OH}\)

The second molecule is water, with an oxygen atom sharing covalent bonds with two hydrogen atoms. Oxygen is a highly electronegative atom, and hydrogen bonding can occur between water molecules. The hydrogens covalently bonded to oxygen will also be attracted to the oxygen atoms of other nearby water molecules, creating hydrogen bonds. So, this molecule can show hydrogen bonding.
03

Analyze Molecule (c) - \(\mathrm{NH}_{3}\)

In this molecule, a nitrogen atom shares covalent bonds with three hydrogen atoms. Nitrogen is also a highly electronegative atom, resulting in hydrogen bonding between different ammonia molecules. The hydrogens covalently bonded to nitrogen will be attracted to the nitrogen atoms of other nearby ammonia molecules, establishing hydrogen bonds. Therefore, this molecule can also show hydrogen bonding.
04

Analyze Molecule (d) - \(\mathrm{H}_{3} \mathrm{C}-\mathrm{O}-\mathrm{CH}_{3}\)

This molecule has an oxygen atom sharing covalent bonds with two carbon atoms. The two \(\mathrm{H}_{3} \mathrm{C}\) groups on either side of the oxygen cannot form hydrogen bonds because they are bonded to carbon, not a highly electronegative atom. Consequently, this molecule cannot show hydrogen bonding as there are no suitable hydrogen donors or acceptors within the molecule.
05

Conclusion

Based on the analysis of the four molecules, the ones that can show hydrogen bonding are: (b) \(\mathrm{HO}-\mathrm{OH}\) (c) \(\mathrm{NH}_{3}\)

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Most popular questions from this chapter

Methyl alcohol can be used as a fuel instead of, or combined with, gasoline. A sample of methyl alcohol, \(\mathrm{CH}_{3} \mathrm{OH}\), in a flask of constant volume exerts a pressure of \(254 \mathrm{~mm} \mathrm{Hg}\) at \(57^{\circ} \mathrm{C}\). The flask is slowly cooled. (a) Assuming no condensation, use the ideal gas law to calculate the pressure of the vapor at \(35^{\circ} \mathrm{C}\); at \(45^{\circ} \mathrm{C}\). (b) Compare your answers in (a) with the equilibrium vapor pressures of methyl alcohol: \(203 \mathrm{~mm} \mathrm{Hg}\) at \(35^{\circ} \mathrm{C} ; 325 \mathrm{~mm} \mathrm{Hg}\) at \(45^{\circ} \mathrm{C}\). (c) On the basis of your answers to (a) and (b), predict the pressure exerted by the methyl alcohol in the flask at \(35^{\circ} \mathrm{C} ;\) at \(45^{\circ} \mathrm{C}\). (d) What physical states of methyl alcohol are present in the flask at \(35^{\circ} \mathrm{C} ?\) At \(45^{\circ} \mathrm{C} ?\)

Iodine has a triple point at \(114^{\circ} \mathrm{C}, 90 \mathrm{~mm} \mathrm{Hg}\). Its critical temperature is \(535^{\circ} \mathrm{C}\). The density of the solid is \(4.93 \mathrm{~g} / \mathrm{cm}^{3}\), and that of the liquid is \(4.00 \mathrm{~g} / \mathrm{cm}^{3}\). Sketch the phase diagram for iodine and use it to fill in the blanks using either "liquid" or "solid." (a) Iodine vapor at \(80 \mathrm{~mm} \mathrm{Hg}\) condenses to the when cooled sufficiently. (b) Iodine vapor at \(125^{\circ} \mathrm{C}\) condenses to the pressure is applied. (c) Iodine vapor at \(700 \mathrm{~mm} \mathrm{Hg}\) condenses to the when cooled above the triple point temperature.

Of the four general types of solids, which one(s) (a) are generally insoluble in water? (b) have very high melting points? (c) conduct electricity as solids?

Naphthalene, \(\mathrm{C}_{10} \mathrm{H}_{8}\), is the substance present in some moth balls. Its vapor pressure at \(25^{\circ} \mathrm{C}\) is \(0.300 \mathrm{~mm} \mathrm{Hg}\). (a) How many milligrams of naphthalene will sublime into an evacuated 1.000-L flask? (b) If \(0.700 \mathrm{mg}\) of naphthalene is used, what will the final pressure be? What physical state(s) of naphthalene is (are) in the flask? (c) If \(4.00 \mathrm{mg}\) of naphthalene is used, what will the final pressure be? What physical state(s) of naphthalene is (are) in the flask?

Classify each of the following solids as metallic, network covalent, ionic, or molecular. (a) It melts below \(100^{\circ} \mathrm{C}\) and is insoluble in water. (b) It conducts electricity only when melted. (c) It is insoluble in water and conducts electricity.
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