Unit 3: Intermolecular Forces and Properties

Which substance would have the highest boiling point?

A liquid has a high surface tension, high viscosity, and a boiling point much higher than predicted by molar mass alone. Which intermolecular force best accounts for these observations?

Which intermolecular force is primarily responsible for the high boiling point of water?

Which substance would be expected to have the highest boiling point?

At 25°C and 1 atm, which of the following best explains why the vapor pressure of ethanol (C₂H₅OH) is lower than that of dimethyl ether (CH₃OCH₃), despite having the same molar mass?

A substance has a very high melting point, conducts electricity when dissolved in water but not as a solid, and is brittle. The substance is most likely

Which of the following molecules can form hydrogen bonds with other molecules of the same kind?

A solution is made by dissolving NaCl in water. Which type of intermolecular force is most important in the dissolution process?

The surface tension of water is higher than that of most other liquids. This is primarily due to

Diamond and graphite are both forms of carbon. Diamond is extremely hard and does not conduct electricity, while graphite is soft and conducts electricity. The best explanation for these differences is

London dispersion forces are present in:

A substance with strong intermolecular forces will have:

Water's high boiling point compared to similar-sized molecules is due to:

Chromatography separates mixtures based on differences in:

The vapor pressure of a liquid increases with temperature because:

Solubility generally increases with temperature for:

Colligative properties depend on:

At the boiling point, the vapor pressure of a liquid equals:

Which of the following best explains why HF has the highest boiling point despite having the lowest molar mass?

Which substance is expected to have the highest boiling point?

Based on the data, which statement about these two liquids is correct?

Which dye has the strongest attraction to the stationary phase (paper)?

Which of the following best explains the trend in boiling points among these isomers?

Why is hexane insoluble in water while ethanol is miscible?

Which correctly ranks these liquids by increasing strength of intermolecular forces?

Which property most directly explains why glycerol has the highest viscosity?

At room temperature, HF (MM = 20 g/mol) is a liquid while HCl (MM = 36.5 g/mol) is a gas, despite HCl having a greater molar mass. Which of the following best explains this observation?

A sample of an ideal gas at 2.0 atm and 300 K occupies a volume of 5.0 L. If the temperature is increased to 600 K while the pressure remains constant, what is the new volume?

Ethanol (C₂H₅OH, MW = 46) has a boiling point of 78°C, while dimethyl ether (CH₃OCH₃, MW = 46) has a boiling point of −24°C. Both have the same molecular formula. The large difference in boiling points is best explained by