AP CHEMISTRY: CHAPTER 10
Liquids and Solids
This is a key chapter in the text. The correlation of structure and properties is central to all chemistry and
illustrates the way chemists solve problems. It brings together what you have learned in the previous
chapters about the nature of bonding and geometry which can be used to predict the nature and relative
strengths of interparticle forces. This is the key to the physical and chemical properties of materials.
Ionic solids, molecular substances, macromolecules, and metals will be studied. The concepts of hydrogen
bonding and dispersion forces are particularly important.
CA State Standards: 2.d,h
Concepts:
1. What is equal about equilibrium?
2. In the definition of vapor pressure, one condition is critical, and sets this particular sort of equilibrium
apart from the others. What is that condition?
3. What is the effect of volume on vapor pressure?
4. To what, exactly, does heat of vaporization refer? What are the factors which affect this quantity?
5. Suppose 200mL of water is in a 400mL sealed flask, and that the flask is connected by a closed
stopcock (of negligible volume) to an identical flask. The second flask has been completely evacuated
(P=0mmHg). The first flask has come to equilibrium at a vapor pressure of 700mmHg. Describe
exactly what will happen once the stopcock is opened. What will the new pressure be?
6. Describe the effect of a change in temperature on vapor pressure. Mathematically, how does vapor
pressure vary with temperature?
7. Write the Clausius-Claperon Equation and clearly define each term. Give examples of 3 ways you
might use the C-C equation.
8. What are the conditions necessary for boiling to occur?
9. Why is it necessary to define normal boiling point?
10. How are critical temperature and critical pressure related?
11. How can you determine from a phase diagram if sublimation will occur?
12. If the solid phase of a substance is denser than the liquid phase, will the solid/liquid boundary line
have a positive or negative slope? Explain why this must be true.
13. Compare the relative magnitudes of the heats of phase change (vaporization, fusion). What should
the signs be?
14. What properties of the "sea" model explain why some metals have stronger bonds than others?
15. Which metals should be the best conductors? Why?
16. Describe the general trend in melting and boiling points as molecular weight increases. What other
factors affect melting and boiling points?
17. What is required for the formation of a hydrogen bond?
18. Explain why dispersion forces are greater in a long straight molecule than in a highly-branched,
compact molecule.
19. In what ways would the development of superconductors revolutionize technology to improve our life
style? What is the major stumbling block to the achievement of this technology on a large scale?
20. Discuss the relative stabilities of the carbon compounds, graphite and diamond. Refer to the phase
diagram in your explanation.
Questions and Exercises: 13,15,19,21,23,27,33,35,37,46,71,75,81,87,89,91,93
Lab Work: Experiment -- Triple Point of Dry Ice (ditto) -- *Bring Pliers
Experiment -- Vapor Pressure of Water (ditto)