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Chapter 9: Problem 41

Of the four general types of solids, which one(s) (a) are generally low-boiling? (b) are ductile and malleable? (c) are generally soluble in nonpolar solvents?

Short Answer

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Provide examples for each property. Answer: (a) Molecular solids typically exhibit low boiling points due to the weak intermolecular forces between their molecules, such as in sugar, ice, and dry ice (solid CO2). (b) Metallic solids, such as gold, silver, and copper, are ductile and malleable due to their metallic bonds and the "sea" of delocalized electrons surrounding the metal atoms. (c) Nonpolar molecular solids, like iodine (I2) and fullerenes (e.g., C60), are soluble in nonpolar solvents (e.g., hexane or benzene) because their weak London dispersion forces get disrupted by other nonpolar molecules.

Step by step solution

01

(a) Low-Boiling Solids:

Low-boiling solids are those that transition from the solid phase to the gaseous phase at relatively low temperatures. In the context of the four general types of solids, molecular solids typically exhibit low boiling points. Molecular solids consist of weak intermolecular forces (like van der Waals forces and hydrogen bonds) between their molecules, which require less energy to break. Examples of molecular solids include sugar, ice, and dry ice (solid CO2).
02

(b) Ductile and Malleable Solids:

Ductile and malleable solids are those that can be stretched or deformed without breaking or cracking. In the context of the four general types of solids, metallic solids are ductile and malleable. Metallic bonds consist of metal atoms surrounded by a "sea" of delocalized electrons that contribute to their ability to hold their structure even when significant stress is applied. Examples of ductile and malleable solids include gold, silver, and copper.
03

(c) Soluble in Nonpolar Solvents:

Solids that are soluble in nonpolar solvents generally have a similar nature as nonpolar solvents; that is, they exhibit low polarity or no polarity at all. Within the four types of solids, molecular solids (with nonpolar molecules) demonstrate solubility in nonpolar solvents. Furthermore, nonpolar molecular solids are held together by weak London dispersion forces, which get disrupted by other nonpolar molecules. Examples of nonpolar molecular solids include iodine (I2) and fullerenes (like C60), which are soluble in nonpolar solvents like hexane or benzene.

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Most popular questions from this chapter

Consider a sealed flask with a movable piston that contains \(5.25 \mathrm{~L}\) of \(\mathrm{O}_{2}\) saturated with water vapor at \(25^{\circ} \mathrm{C}\). The piston is depressed at constant temperature so that the gas is compressed to a volume of \(2.00 \mathrm{~L}\). (Use the table in Appendix 1 for the vapor pressure of water at various temperatures.) (a) What is the vapor pressure of water in the compressed gas mixture? (b) How many grams of water condense when the gas mixture is compressed?

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?

Explain in terms of forces between structural units why (a) \(\mathrm{Br}_{2}\) has a lower melting point than \(\mathrm{NaBr}\). (b) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) has a higher boiling point than butane, \(\mathrm{C}_{4} \mathrm{H}_{10}\). (c) \(\mathrm{H}_{2} \mathrm{O}\) has a higher boiling point than \(\mathrm{H}_{2} \mathrm{Te}\). (d) Acetic acid \(\mathrm{CH}_{3}-\mathrm{C}-\mathrm{OH}\) has a lower boiling point

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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