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Solids, Liquids, and Intermolecular Forces: Review Questions for AP Chemistry (page 2)

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By — McGraw-Hill Professional
Updated on Feb 2, 2011

Answers and Explanations

  1. B—This answer describes a metallic solid.
  2. C—This answer describes an ionic solid.
  3. A—This answer describes a covalent network solid.
  4. D—This answers describes a solid consisting of discrete polar molecules.
  5. D—Each of the carbon atoms is covalently bonded to four other carbon atoms.
  6. E—Sulfur dioxide molecules are polar.
  7. A—Hydrogen bonding occurs when hydrogen is directly bonded to F, O, and in this case N.
  8. A— This is the definition of the critical point.
  9. B—The gas–liquid line always has a positive slope. B negates C. The triple point is below the freezing point. The triple point may be above or below 1 atm.
  10. A—Argon is a noble gas; none of the bonding choices are options.
  11. B—Diamond is a covalent network solid with a large number of strong covalent bonds between the carbon atoms.
  12. B—The bottom of the liquid region on the phase diagram is the triple point.
  13. D—The size of the container is irrelevant. Sealing the container will cause an increase in pressure that will increase the boiling point. A decrease in pressure will lower the boiling point.
  14. E—The compound with the higher surface tension is the one with the stronger intermolecular force. The hydrogen bonding in 1-butanol is stronger than the dipole–dipole attractions in diethyl ether.
  15. A—The sequence for these similar molecules is nonpolar, then one hydrogen bond, then two hydrogen bonds.
  16. A—This change is condensation, so the energy is the heat of condensation.
  17. C—The only applicable factor listed is the charge difference. The chloride ion is larger than the fluoride ion. The ion ratio is not important.
  18. E—The point must be on the line separating the solid from the liquid phase.
  19. D—The solid begins to melt at A, and finishes melting at B.

 

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