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Chapter 9: Problem 36

What are the strongest attractive forces that must be overcome to (a) boil silicon hydride \(\mathrm{SiH}_{4} ?\) (b) vaporize calcium chloride? (c) dissolve \(\mathrm{Cl}_{2}\) in carbon tetrachloride, \(\mathrm{CCl}_{4} ?\) (d) melt iodine?

Short Answer

Expert verified
Answer: (a) In boiling SiH4, the van der Waals forces between the SiH4 molecules must be overcome. (b) To vaporize CaCl2, the ionic bonds between the calcium cations and chloride anions need to be broken. (c) In dissolving Cl2 in CCl4, the van der Waals forces between Cl2 and CCl4 molecules must be overcome. (d) To melt I2, the van der Waals forces between the I2 molecules need to be overcome.

Step by step solution

01

(a) Boiling Silicon Hydride (SiH4)

Silicon hydride has covalent bonds between silicon and hydrogen atoms. To boil SiH4, we need to overcome the van der Waals forces between the SiH4 molecules, as these are the main intermolecular forces. The stronger the van der Waals forces, the more energy is needed to overcome them.
02

(b) Vaporizing Calcium Chloride (CaCl2)

Calcium chloride is an ionic compound, comprised of calcium cations (Ca2+) and chloride anions (Cl-). In order to vaporize CaCl2, the ionic bonds between these ions must be broken. Ionic forces are stronger than covalent and van der Waals forces, so a significant amount of energy is required to vaporize CaCl2.
03

(c) Dissolving Chlorine (Cl2) in Carbon Tetrachloride (CCl4)

Chlorine is a diatomic molecule composed of two covalently bonded chlorine atoms, while carbon tetrachloride is made up of a carbon atom bonded to four chlorine atoms. The intermolecular forces between Cl2 and CCl4 are the weak van der Waals forces. To dissolve Cl2 in CCl4, these van der Waals forces must be overcome.
04

(d) Melting Iodine (I2)

Iodine is a diatomic molecule formed by two covalently bonded iodine atoms. In solid iodine, the main intermolecular forces are van der Waals forces between the I2 molecules. To melt iodine, these van der Waals forces must be overcome, allowing the I2 molecules to move more freely in the liquid state.

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Most popular questions from this chapter

The normal boiling point for methyl hydrazine \(\left(\mathrm{CH}_{3} \mathrm{~N}_{2} \mathrm{H}_{3}\right)\) is \(87^{\circ} \mathrm{C}\). It has a vapor pressure of \(37.0 \mathrm{~mm} \mathrm{Hg}\) at \(20^{\circ} \mathrm{C}\). What is the concentration (in \(\mathrm{g} / \mathrm{L}\) ) of methyl hydrazine if it saturates the air at \(25^{\circ} \mathrm{C}\) ?

What are the strongest attractive forces that must be overcome to (a) boil silicon hydride \(\mathrm{SiH}_{4} ?\) (b) vaporize calcium chloride? (c) dissolve \(\mathrm{Cl}_{2}\) in carbon tetrachloride, \(\mathrm{CCl}_{4} ?\) (d) melt iodine?

The density of liquid mercury at \(20^{\circ} \mathrm{C}\) is \(13.6 \mathrm{~g} / \mathrm{cm}^{3}\), its vapor pressure is \(1.2 \times 10^{-3} \mathrm{~mm} \mathrm{Hg}\). (a) What volume (in \(\mathrm{cm}^{3}\) ) is occupied by one mole of \(\mathrm{Hg}(l)\) at \(20^{\circ} \mathrm{C}\) ? (b) What volume (in \(\mathrm{cm}^{3}\) ) is occupied by one mole of \(\mathrm{Hg}(\mathrm{g})\) at \(20^{\circ} \mathrm{C}\) and the equilibrium vapor pressure? (c) The atomic radius of \(\mathrm{Hg}\) is \(0.155 \mathrm{~nm}\). Calculate the volume (in \(\mathrm{cm}^{3}\) ) of one mole of \(\mathrm{Hg}\) atoms \(\left(V=4 \pi r^{3} / 3\right)\). (d) From your answers to (a), (b), and (c), calculate the percentage of the total volume occupied by the atoms in \(\mathrm{Hg}(l)\) and \(\mathrm{Hg}(g)\) at \(20^{\circ} \mathrm{C}\) and \(1.2 \times 10^{-3} \mathrm{~mm} \mathrm{Hg}\)

In which of the following processes is it necessary to break covalent bonds as opposed to simply overcoming intermolecular forces? (a) melting mothballs made of naphthalene (b) dissolving HBr gas in water to form hydrobromic acid (c) vaporizing ethyl alcohol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) (d) changing ozone, \(\mathrm{O}_{3}\), to oxygen gas, \(\mathrm{O}_{2}\)

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 \(45^{\circ} \mathrm{C} ?\)
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