Chapter 10. Solids and Liquids
End-of-Chapter Material
Additional Exercises
- All other things being equal, rank the intermolecular forces in order of increasing strength.
- Which subatomic particles (protons, neutrons, electrons) are most responsible for intermolecular forces? Explain your answer.
- Can a molecule experience more than one intermolecular force at the same time? Why or why not?
- Of the properties boiling point, structure of the solid phase, and molar mass, which are influenced by hydrogen bonding? Explain your answer.
- How many grams of solid water can be melted with 1.55 kJ of energy?
- How many grams of Hg can be vapourized using 29,330 J of energy?
- Another way to minimize freezer burn is to wrap food tightly before freezing. Why would this minimize freezer burn?
- The ΔHsub of naphthalene (C10H8) is 72.6 kJ/mol. What energy is needed to sublime 100.0 g of C10H8?
- Which do you think would have a higher surface tension — liquid neon or liquid krypton? Explain your answer.
- Under what condition would a liquid not show either capillary rise or capillary depression?
Answers
- dispersion forces < dipole-dipole interactions < hydrogen bonding < ionic bonding
- Yes, but one intermolecular force usually dominates.
- 4.64 g
- Water in the vapour phase has no space to evaporate into.
- Liquid krypton, because it would have stronger dispersion forces.
