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Chapter 9: Problem 37

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

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a) Boil silicon hydride SiH4 b) Vaporize calcium chloride c) Dissolve Cl2 in carbon tetrachloride CCl4 d) Melt iodine

Step by step solution

01

a) Boil silicon hydride SiH4

To boil silicon hydride (SiH4), the strongest attractive forces to overcome are the van der Waals forces (or London dispersion forces) between SiH4 molecules since SiH4 is a nonpolar covalent compound. The stronger these forces, the higher the boiling point it will have.
02

b) Vaporize calcium chloride

To vaporize calcium chloride (CaCl2), the strongest attractive forces to overcome are the ionic bonds between the positively charged calcium ions (Ca2+) and negatively charged chloride ions (Cl-) in the crystal lattice, as CaCl2 is an ionic compound. The strength of the ionic bond depends on the charges and sizes of the ions involved; the higher the charge and smaller the size, the stronger the bond.
03

c) Dissolve Cl2 in carbon tetrachloride CCl4

To dissolve Cl2 (chlorine) in carbon tetrachloride (CCl4), the attractive forces to overcome are London dispersion forces present between the nonpolar chlorine molecules and nonpolar CCl4 molecules. Cl2 and CCl4 have similar polarities, which makes it easier for Cl2 to dissolve in CCl4. However, these van der Waals forces between molecules must still be overcome for the dissolving process to occur.
04

d) Melt iodine

To melt iodine (I2), the strongest attractive forces to overcome are the London dispersion forces between iodine molecules in the solid-state. Iodine is a nonpolar covalent compound with a relatively high molecular weight, which results in stronger van der Waals forces and, thus, a higher melting point compared to other Group 17 elements (except for astatine).

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Most popular questions from this chapter

What are the strongest attractive forces that must be overcome to (a) melt ice? (b) sublime bromine? (c) boil chloroform (CHCl \(_{3}\) )? (d) vaporize benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) ?

Benzene, a known carcinogen, was once widely used as a solvent. \(\mathrm{A}\) sample of benzene vapor in a flask of constant volume exerts a pressure of \(325 \mathrm{~mm} \mathrm{Hg}\) at \(80^{\circ} \mathrm{C}\). The flask is slowly cooled. (a) Assuming no condensation, use the ideal gas law to calculate the pressure of the vapor at \(50^{\circ} \mathrm{C} ;\) at \(60^{\circ} \mathrm{C}\). (b) Compare your answers in (a) to the equilibrium vapor pressures of benzene: \(269 \mathrm{~mm} \mathrm{Hg}\) at \(50^{\circ} \mathrm{C}, 389 \mathrm{~mm} \mathrm{Hg}\) at \(60^{\circ} \mathrm{C}\). (c) On the basis of your answers to (a) and (b), predict the pressure exerted by the benzene at \(50^{\circ} \mathrm{C} ;\) at \(60^{\circ} \mathrm{C}\).

Arrange the following in order of increasing boiling point. (a) Ar (b) He (c) Ne (d) Xe

In which of the following processes is it necessary to break covalent bonds as opposed to simply overcoming intermolecular forces? (a) subliming dry ice (b) vaporizing chloroform \(\left(\mathrm{CHCl}_{3}\right)\) (c) decomposing water into \(\mathrm{H}_{2}\) and \(\mathrm{O}_{2}\) (d) changing chlorine molecules into chlorine atoms

\(p\) -Dichlorobenzene, \(\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}\), can be one of the ingredients in mothballs. Its vapor pressure at \(20^{\circ} \mathrm{C}\) is \(0.40 \mathrm{~mm} \mathrm{Hg}\). (a) How many milligrams of \(\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}\) will sublime into an evacuated 750-mL flask at \(20^{\circ} \mathrm{C}\) ? (b) If \(5.0 \mathrm{mg}\) of \(p\) -dichlorobenzene were put into an evacuated 750 -mL flask, how many milligrams would remain in the solid phase? (c) What is the final pressure in an evacuated 500 -mL flask at \(20^{\circ} \mathrm{C}\) that contains \(2.00 \mathrm{mg}\) of \(p\) -dichlorobenzene? Will there be any solid in the flask?
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