Question #14. Relative Boiling Points. For each of the pair of substances in the table below, identify the most important type of "intermolecular" force for each substance in the pair, and then tell which substance in the pair would have the higher boiling point. Most Important Forces for Most Important Forces for Substance with Pair of Substances First Substance Second Substance Higher Boiling Point O2 and N2 [ Select ] V [ Select ] [ Select ] London dispersion forces Hydrogen bonding Dipole-dipole forces lon-dipole forces SİH4 and GeH4 [ Select ] [ Select ] lon-ion forces HF and HI [ Select ] [ Select ]

Question #14. Relative Boiling Points. For each of the pair of substances in the table below, identify the most important type of "intermolecular" force for each substance in the pair, and then tell which substance in the pair would have the higher boiling point. Most Important Forces for Most Important Forces for Substance with Pair of Substances First Substance Second Substance Higher Boiling Point O2 and N2 [ Select ] V [ Select ] [ Select ] London dispersion forces Hydrogen bonding Dipole-dipole forces lon-dipole forces SİH4 and GeH4 [ Select ] [ Select ] lon-ion forces HF and HI [ Select ] [ Select ]

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter15: Gases,liquids, And Solids

Section: Chapter Questions

Problem 99E

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Similar questions

Identify two common observations indicating some liquids have sufficient vapor pressures to noticeably evaporate?
What feature characterizes the dynamic equilibrium between a liquid and its vapor in a closed container?
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.
8.45 Describe how interactions between molecules affect the vapor pressure of a liquid.
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.
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.