1. Chapter 10 Liquids and Solids

2. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–2 QUESTION

3. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–3 ANSWER 5)The vapor pressure of a liquid. Section 10.1 Intermolecular Forces (p. 426) Molecules at the surface of a liquid will be held tighter by stronger intermolecular forces, making it more difficult for them to escape into the vapor phase.

4. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–4 QUESTION

5. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–5 ANSWER 2 5)For its molar mass, water has a high boiling point. Section 10.1 Intermolecular Forces (p. 426) Without hydrogen bonds, HO would boil at a lower temperature than oxygen.

6. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–6 QUESTION

7. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–7 ANSWER 2 4)I Section 10.1 Intermolecular Forces (p. 426) The intermolecular forces for each of these halide molecules is the same, so that leaves molecular mass to determine the order of boiling points.

8. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–8 QUESTION

9. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–9 ANSWER 2 1) NaS Section 10.7 Ionic Solids (p. 456) Sodium sulfide is an ionic compound with very strong ionic bonding.

10. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–10 QUESTION

11. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–11 ANSWER 4 4)CH Section 10.1 Intermolecular Forces (p. 426) For hydrogen bonding to take place, the hydrogen atom must be bonded to oxygen, nitrogen or fluorine. Carbon does not have a large enough electronegativity.

12. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–12 QUESTION

13. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–13 ANSWER 2 3) N(s) Section 10.1 Intermolecular Forces (p. 426) Two identical atoms bonded together in a diatomic molecule cannot have a dipole since they share electrons equally.

14. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–14 QUESTION

15. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–15 ANSWER - 2)4 Section 10.4 Structure and Bonding in Metals (p. 436) Lead atoms form a facecentered cubic lattice.

16. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–16 QUESTION

17. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–17 ANSWER I 2 1)ce and water Section 10.9 Phase Diagrams (p. 467) Under these conditions, HO is in equilibrium between two phases.

18. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–18 QUESTION

19. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–19 ANSWER 4) intramolecular forces Section 10.1 Intermolecular Forces (p. 426) “Intra-” meaning within or inside of, as opposed to “inter-“ meaning between.

20. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–20 QUESTION

21. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–21 ANSWER 5)Condensation Section 10.9 Phase Diagrams (p. 467) Evaporation is process of a liquid changing into a gas. The opposite process, a gas changing into a liquid, is condensation.

22. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–22 QUESTION

23. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–23 ANSWER 1)Ag(s) Section 10.3 An Introduction to Structures and Types of Solids (p. 430) The bonding of metals is described as an electron “sea”. The valence electrons of the metal atoms can flow throughout the entire piece of metal they belong to giving metals their high electrical conductivity.

24. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–24 QUESTION

25. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–25 ANSWER 4) hard, high melting, a poor electrical conductor. Section 10.7 Ionic Solids (p. 456) Though ionic compounds consist entirely of charged particles, these ions are unable to shift positions within the lattice and thus, in solid form, ionic compounds have poor electrical

26. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–26 ANSWER (continued)

27. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–27 QUESTION

28. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–28 ANSWER 32 –– 23 4) diethyl ether, CHCHO Section 10.8 Vapor Pressure (p. 459) Diethyl ether boils first as the temperature increases, leading one to believe that its vapor pressure at any temperature is also the highest of the given group of compounds.

29. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–29 QUESTION

30. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–30 ANSWER 2)crystallization Section 10.8 Vapor Pressure (p. 459) As a substance crystallizes, generally from a liquid, but a gaseous starting point is possible, the molecules, atoms, or ions lose kinetic energy to allow for bonding. This kinetic energy is emitted as heat.

31. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–31 QUESTION

32. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–32 ANSWER.  2) 760 torr Section 10.8 Vapor Pressure (p. 459) 100.0C is the boiling point for water and at the boiling point the vapor pressure of water equals the atmospheric pressure.

33. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–33 QUESTION

34. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–34 QUESTION (continued)

35. Copyright © Houghton Mifflin Company. All rights reserved.CRS Question, 10–35 ANSWER 2 - 2)The diagram shows that the melting point of the solid increases with increasing pressure. Section 10.9 Phase Diagrams (p. 467) HO has a SL line that slants in the opposite direction. This allows ice to be liquified with a high enough pressure. Atthe base of a glacier, the pressure from thousands of feet of ice, liquefies the lowest layers of the glacier, allowing it to move.