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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

Expert verified
Answer: The strongest attractive forces to be overcome in each process are (a) London dispersion forces in boiling silicon hydride, (b) ionic bonds in vaporizing calcium chloride, (c) London dispersion forces in dissolving chlorine gas in carbon tetrachloride, and (d) London dispersion forces in melting iodine.

Step by step solution

01

(a) Boiling Silicon Hydride (SiH4)

In order to boil silicon hydride, \(\mathrm{SiH}_{4}\), the strongest intermolecular forces that need to be overcome are the molecule-molecule interactions called London dispersion forces. These forces arise from temporary fluctuations in electron density that create temporary dipoles, and they are present in all molecules, regardless of polarity.
02

(b) Vaporizing Calcium Chloride (CaCl2)

To vaporize calcium chloride (CaCl2), the strongest attractive forces to be overcome are the ionic bonds between calcium (Ca2+) and chloride (Cl-) ions. Calcium chloride is an ionic compound, which means it is made up of positively and negatively charged ions that are attracted to one another by electrostatic forces.
03

(c) Dissolving Cl2 in Carbon Tetrachloride (CCl4)

In order to dissolve \(\mathrm{Cl}_{2}\) in carbon tetrachloride (\(\mathrm{CCl}_{4}\)), the strongest intermolecular forces that need to be overcome are the London dispersion forces. Both \(\mathrm{Cl}_{2}\) and \(\mathrm{CCl}_{4}\) are nonpolar molecules, so the main type of intermolecular force between them is London dispersion forces.
04

(d) Melting Iodine (I2)

To melt iodine (I2), the strongest forces that need to be overcome are also London dispersion forces. Iodine is a diatomic molecule and is nonpolar, which means that the primary intermolecular forces between iodine molecules are due to London dispersion forces. These forces must be overcome in order to change the iodine from a solid to a liquid state.

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Most popular questions from this chapter

In the blanks provided, answer the questions below, using LT (for is less than), GT (for is greater than), \(\mathrm{EQ}\) (for is equal to), or MI (for more information required). (a) The boiling point of \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(\mathrm{MM}=60.0 \mathrm{~g} / \mathrm{mol})\) _______ the boiling point of \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{C}=\mathrm{O} \quad(\mathrm{MM}=\) \(58.0 \mathrm{~g} / \mathrm{mol})\) (b) The vapor pressure of \(X\) is \(250 \mathrm{~mm} \mathrm{Hg}\) at \(57^{\circ} \mathrm{C}\). Given a sealed flask ________ at \(57^{\circ} \mathrm{C}\) that contains only gas, the pressure in the flask \(245 \mathrm{~mm} \mathrm{Hg}\). (c) The melting-point curve for \(Y\) tilts to the right of a straight line. The density of \(Y(l)\) _______ the density of \(\mathrm{Y}(s)\) (d) The normal boiling point of \(A\) is \(85^{\circ} \mathrm{C},\) while the normal boiling point of \(\mathrm{B}\) is \(45^{\circ} \mathrm{C}\). The vapor pressure of A at \(85^{\circ} \mathrm{C}\) ______ the vapor pressure of \(\mathrm{B}\) at \(45^{\circ} \mathrm{C}\). (e) The triple point of \(\mathrm{A}\) is \(25 \mathrm{~mm} \mathrm{Hg}\) and \(5^{\circ} \mathrm{C}\). The melting point of \(\mathrm{A}\) _______ \(5^{\circ} \mathrm{C}\).

1\. 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 \(45^{\circ} \mathrm{C} ?\)

Explain in terms of forces between structural units why (a) HI has a higher boiling point than HBr. (b) \(\mathrm{GeH}_{4}\) has a higher boiling point than \(\mathrm{SiH}_{4}\). (c) \(\mathrm{H}_{2} \mathrm{O}_{2}\) has a higher melting point than \(\mathrm{C}_{3} \mathrm{H}_{8}\). (d) \(\mathrm{NaCl}\) has a higher boiling point than \(\mathrm{CH}_{3} \mathrm{OH}\).

A pure substance A has a liquid vapor pressure of 6 atm at \(550^{\circ} \mathrm{C}\). Its triple point is at \(5 \mathrm{~atm}, 350^{\circ} \mathrm{C}\). The solid phase is denser than the liquid phase. (a) Sketch the phase diagram for compound \(A\). (b) From the phase diagram, estimate the temperature at which the compound boils when 6.3 atm of pressure are applied. (c) What changes occur when, at a constant pressure of 4 atm, the temperature drops from \(400^{\circ} \mathrm{C}\) to \(100^{\circ} \mathrm{C} ?\)

Dichloromethane, \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\), is widely used as a "degreaser" and paint stripper. Its vapor pressure is \(381.0 \mathrm{~mm} \mathrm{Hg}\) at \(21.9^{\circ} \mathrm{C}\) and \(465.8 \mathrm{~mm} \mathrm{Hg}\) at \(26.9^{\circ} \mathrm{C}\). Estimate (a) its heat of vaporization \(\left(\Delta H_{\text {vap }}\right)\). (b) its normal boiling point.
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