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1. Which one of the following decreases as the strength of the attractive intermolecular forces increases?
[A] The normal boiling temperature.
[B] The vapor pressure of a liquid.
[C] The sublimation temperature of a solid.
[D] The extent of deviations from the ideal gas law.
[E] The heat of vaporization.
2. Order the intermolecular forces (dipole-dipole, London Dispersion, ionic, and hydrogen-bonding) from weakest to strongest.
[A] Dipole-dipole, London Dispersion, ionic, and hydrogen-bonding
[B] Dipole-dipole, ionic, London Dispersion, and hydrogen-bonding
[C] Hydrogen-bonding, dipole-dipole, London Dispersion, and ionic
[D] London Dispersion, dipole-dipole, hydrogen-bonding, ionic
[E] London Dispersion, ionic, dipole-dipole, and hydrogen-bonding
3. Hydrogen bonds account for which of the following observation?
[A] Air is more dense than hydrogen gas.
[B] Hydrogen naturally exists as a diatomic molecule.
[C] Water molecules are bent or â€œV-shaped.â€
[D] For its molar mass, water has a high boiling point.
[E] Hydrogen is easily combustible with oxygen.
4. Which of the following would you expect to have the highest boiling point?
[E] All of these have the same boiling point.
Increasing attractive intermolecular forces causes molecules in the liquid to bond more strongly to each other. Thus it is more difficult for the molecules to escape into the gas phase and......
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