a) For each of the following substances, identify the most important type of "intermolecular" attractions. Then rank the four substances 1-4 in order of strength of those attractions, with 1 being the substance with the weakest attractions and 4 being the substance with the strongest attractions. Explain your reasoning in the next question.

a) For each of the following substances, identify the most important type of "intermolecular" attractions. Then rank the four substances 1-4 in order of strength of those attractions, with 1 being the substance with the weakest attractions and 4 being the substance with the strongest attractions. Explain your reasoning in the next question.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.84PAE

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What are intermolecular forces? How do they differ from intramolecular forces? What are dipole-dipole forces? How do typical dipole-dipole forces differ from hydrogen bonding interactions? In what ways are they similar? What are London dispersion forces? How do typical London dispersion forces differ from dipole-dipole forces? In what ways are they similar? Describe the relationship between molecular size and strength of London dispersion forces. Place the major types of intermolecular forces in order of increasing strength. Is there some overlap? That is, can the strongest London dispersion forces be greater than some dipole-dipole forces? Give an example of such an instance.
Classify each of the following statements as true or false. a Intermolecular attractions are stronger in liquids than in gases. b Substances with weak intermolecular attractions generally have low vapor pressures. c Liquids with high molar heats of vaporization usually are more viscous than liquids with low molar heats of vaporization. d A substance with a relatively high surface tension usually has a very low boiling point. e All other things being equal, hydrogen bonds are weaker than induced dipole or dipole forces. f Induced dipole forces become very strong between large molecules. g Other things being equal, nonpolar molecules have stronger intermolecular attractions than polar molecules. h The essential feature of a dynamic equilibrium is that the rates of opposing changes are equal. i Equilibrium vapor pressure depends on the concentration of a vapor above its own liquid. j The heat of vaporization is equal to the heat of fusion, but with opposite sign. k The boiling point of a liquid is a fixed property of the liquid. l If you break shatter an amorphous solid, it will break in straight lines, but if you break a crystalline solid, it will break in curved lines. m Ionic crystals are seldom soluble in water. n Molecular crystals are nearly always soluble in water. o The numerical value of heat of vaporization is always larger than the numerical value of heat of condensation. p The units of heat of fusion are kJ/gC. q The temperature of water drops while it is freezing. r Specific heat is conerned with a change in temperature.
Which of the following substances can be liquefied by applying pressure at 25C? For those that cannot, describe the conditions under which they can be liquefied. Substance Critical Temperature Critical Pressure Sulfur dioxide, SO2 158C 78 atm Acetylene, C2H2 36C 62 atm Methane. CH4 82C 46 atm Carbon monoxide, CO 140C 35 atm
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?
Methane (CH4) cannot be liquefied at room temperature, no matter how high the pressure. Propane (C3H8), another simple hydrocarbon, has a critical pressure of 42 atm and a critical temperature of 96.7 C. Can this compound be liquefied at room temperature?
8.51 Suppose that three unknown pure substances are liquids at room temperature. You determine that the boiling point of substance A is 53°C, that of substance B is 117°C, and that of substance C is 77°C. Based on this information, rank the three substances in order of their vapor pressures at room temperature.
8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
Diethyl ether (CH3CH2OCH2CH3) was one of the first chemicals used as an anesthetic. At 34.6C, diethyl ether has a vapor pressure of 760. torr, and at 17.9C, it has a vapor pressure of 400. torr. What is the H of vaporization for diethyl ether?
The vapor pressure of I2(s) at 30C is 0.466 mm Hg. (a) How many milligrams of iodine will sublime into an evacuated 750.0-mL flask? (b) If 3.00 mg of I2 are used, what will the final pressure in the flask be? (c) If 7.85 mg of I2 are used, what will the final pressure in the flask be?

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