AP Chem Chapter 13 HomeworkMultiple Choice Identify the choice that best completes the statement or answers the question. ____ 1. Which one of the following statements does not describe the general properties of liquids accurately? a. Liquids have characteristic volumes that do not change greatly with changes in temperature. (Assuming that the liquid is not vaporized.) b. Liquids have characteristic volumes that do not change greatly with changes in pressure. c. Liquids diffuse only very slowly when compared to solids. d. The liquid state is highly disordered compared to the solid state. e. Liquids have high densities compared to gases. 2. Identify which property liquids do not have in common with solids. a. rigid shape b. volumes do not change significantly with pressure c. hydrogen bonding forces can be significant d. practically incompressible e. volumes do not change significantly with temperature 3. Which one of the following statements does not describe the general properties of solids accurately? a. Solids have characteristic volumes that do not change greatly with changes in temperature. b. Solids have characteristic volumes that do not change greatly with changes in pressure. c. Solids diffuse only very slowly when compared to liquids and gases. d. Solids are not fluid. e. Most solids have high vapor pressures at room temperature. 4. Which of the following interactions are the strongest? a. hydrogen bonding force b. ion-ion interactions c. permanent dipole force d. dispersion force e. London force 5. The boiling points of the halogens increase in the order F2 < Cl2 < Br2 < I2 due to the resulting increasing __________ interactions. a. ion-dipole b. hydrogen-bonding c. ion-ion d. dispersion forces e. permanent dipole-dipole 6. For which of the following would permanent dipole-dipole interactions play an important role in determining physical properties in the liquid state? a. BF3 b. ClF c. BeCl2 d. F2 e. CCl4 7. For which of the following would dispersion forces be the most important factor in determining physical properties in the liquid state? ____ ____ ____ ____ ____ ____ dispersion force ____ ____ 10. e. C8H17NH2 b. II. dispersion force e. e. c. a. IV.a. C7H14 . V. ion-ion interaction b. III. d. c. and IV I. dispersion force. dispersion force c. V. IV and V II and V ____ 11. IV. a. II. and V I. II. b. permanent dipole force d. e. and III III. dispersion force. hydrogen bonding force. permanent dipole force. permanent dipole force. and III II. dispersion force e. Which liquid would have the highest viscosity at room temperature? a. Ar Li2SO4 SiF4 Br2 NH3 I. III. and no others? I. d. III. d. ion-ion interaction b. Which response includes all of the following substances that can exhibit hydrogen bonding. and IV ____ 12. and V III and V I. ____ H2O NaCl F2 HF NH4Cl 8. Which response correctly identifies all the interactions that might affect the properties of BrI? a. Which response correctly identifies all the interactions that might affect the properties of BF3? a. IV. hydrogen bonding force. dispersion force 9. dispersion force c. In which of the following would dispersion forces be the only significant factors in determining boiling point? I. c. II. III. IV. b. H2 CH4 NH3 SiH4 HF II and V I. permanent dipole force d. b. Which statement is false? a. molar heat of vaporization ____ 15. vapor pressure e. 170 g/mol e. C3H8 c. boiling point c. 895 g/mol d. 62 g/mol ____ 14. H2O. C12H26. b. density d. Which one of the following statements does not describe the general properties of liquids accurately? a. 114 g/mol c. the vapor pressure of the liquid decreases. 18 g/mol b. c. Gasoline. Liquids with strong cohesive forces have high heats of vaporization. C6H14 ____ 16. C2H6 d. Which of the following boils at the highest temperature? a. Vegetable oil. Which one of the following would have the highest molar heat of vaporization? a. Ethylene glycol. CH3NH2 b. C5H12 e. Which property is not affected by strength of intermolecular forces? a. In the absence of a phase change. Vapor pressures of liquids at a given temperature differ greatly. b. All other factors being equal. d. CH3NH2 ____ 13. and these differences in vapor pressure are due to the nature of the molecules in different liquids. C9H18 d. The normal boiling point of a liquid is the temperature at which the vapor pressure of the liquid becomes equal to exactly 760 torr. e. . In the liquid state the close spacing of molecules leads to large intermolecular forces that are strongly dependent on the nature of the molecules involved. C4H10 d. H2S ____ 17. c. Liquids are practically incompressible. ____ 18. SiH4 e. C8H18. the viscosity of a liquid increases as temperature decreases. As the temperature of a liquid is increased. e. C2H6 b. Vaporization of liquids can occur below their normal boiling points at one atmosphere pressure. CH4 c. The shape of a meniscus depends on the difference between the strengths of cohesive forces and adhesive forces. viscosity b. if adhesive forces are strong.c. C5H12 e. HO-CH2-CH2-OH. Mineral oil. capillary action is likely to occur less readily than if adhesive forces are weak. d. Which liquid would evaporate most quickly at room temperature? a. 0 C. Which substance would be expected to have the highest heat of vaporization? a.solid and vapor are in equilibrium. c. the molecules get closer and closer together as they solidify.____ 19. e. CH3OCH3 e. c. a. e. vaporization d. sublimation c. b.liquid and gas (vapor) are in equilibrium. ____ 23. d. A sketch of the phase diagram (not to scale) of water is given below. C2H6 d. Line AB is the melting curve . a. F2 b. 700 torr 450 torr 100 torr 80 torr 55 torr ____ 20. liquid. Point A is the triple point . Some solids can be converted directly to the vapor phase by heating. condensation e. CCl4 c. Line AC is the vapor pressure curve . d. The process is called __________.7 kJ/mol. The slope of line AB is negative showing that as the liquid is cooled.solid. fusion b. b. Using the Clausius-Clapeyron equation determine the vapor pressure of water at 50. . Which statement is false? a. and vapor are at equilibrium. Line AD is the sublimation curve . The molar heat of vaporization of water is 40.solid and liquid are in equilibrium. distillation ____ 22. A sketch of a phase diagram is given below. CH2OHCH2OH ____ 21. The units that occupy the lattice points are positive ions. A sketch of the phase diagram (not to scale) of water is given below. The melting points of metallic solids vary over a large range.Which statement about this diagram is not true? a. c. then the temperature remains constant until all of the ice is melted into liquid. ____ 24. Which one of the following statements is not applicable to metallic solids? a. four e. Increasing temperature at constant pressure can cause the liquid to vaporize. b. d. three d. Which statement concerning the path (broken line) is false? a. b. Increasing pressure at constant temperature can cause liquid to freeze. d. e. If heat is added to the ice at point E. c. how many atoms are contained in a unit cell? a. The hardness of metallic solids varies from quite soft to quite hard. Increasing temperature at constant pressure can cause the solid to sublime. e. the temperature of the ice increases until line AB is reached. At point E the water is all solid (ice). b. d. the temperature will remain constant as the liquid water vaporizes. . Metallic solids conduct electric current well. c. Once all the ice has melted (at the intersection of the broken line and line AB) the temperature of the water increases as heat is added until point F is reached. ____ 25. one b. two c. Another way to vaporize all of the liquid water at point F is to increase the pressure. The binding forces in metallic solids are shared electron pairs. In a body-centered cubic lattice. If more heat is added upon reaching point F. Increasing pressure at constant temperature can melt the solid. five ____ 26. e. Increasing pressure at constant temperature can cause deposition of solid from gas. nickel c. sucrose. The binding forces in molecular solids are dispersion forces or dispersion forces and dipole-dipole interactions. ammonium chloride d. silicon carbide. Which one of the following is a metallic solid? a. b. Molecular solids are usually excellent conductors of electric current. sodium chloride ____ 34. CH4 ____ 33. Which of the following. copper c. d. phosphorus trichloride d. sucrose. ammonium chloride d. e. graphite b. Molecular solids have relatively low melting points. neon ____ 31. C e. c. Which one of the following statements is not applicable to molecular solids? a. Which one of the following is an ionic solid? a. Which type of solid is expected for SO2? a. nickel c. ____ 28. C12H22O11 ____ 29. CO2 d. K2SO4 b. metallic d. nickel d. diamond b. sulfur c. ionic c. magnesium fluoride e.____ 27. graphite b. Cr c. Which one of the following is a covalent solid? a. Molecular solids are soft compared to covalent solids. in the solid state. SiC e. covalent b. SiC e. would be an example of a molecular crystal? a. Which one of the following substances is incorrectly matched with the kind of solid it forms? Substance Kind of Solid . molecular e. hypersaturated ____ 32. Which one of the following is classified as a covalent solid? a. silicon carbide. sulfur trioxide b. iodine e. The units that occupy the lattice points are molecules. C12H22O11 ____ 30. e. KCl. c. The lattice of a metallic solid is defined by the position of the metal nuclei. NaF. Molten KBr should be a good conductor of electricity. should not sublime readily. e. Silicon carbide. The interactions among the molecules in molecular solids are generally stronger than those among the particles that define either covalent or ionic lattices. d. e. Which of the following compounds would be expected to have the highest melting point? a. MgF2. Arrange the following ionic compounds in order of increasing melting points. Which of the following statements regarding properties of solids is not expected to be correct? a. Solid sodium should be a good conductor of electricity. HF a. NaF ____ 38. Diamond should have a high melting point. e. BaI2 e. c.a. SiC. c. d. Molecular solids generally have lower melting points than covalent solids. NaI a. b. d. NaF < NaBr < NaI < MgF2 < AlF3 NaBr < NaI < NaF < AlF3 < MgF2 MgF2 < AlF3 < NaF < NaI < NaBr AlF3 < MgF2 < NaF < NaBr < NaI NaI < NaBr < NaF < MgF2 < AlF3 ____ 39. Substances have properties that are related to their structures. b. Metallic solids exhibit a wide range of melting points. NaBr. Solid CaF2 should have a low melting point. d. BaF2 b. AlF3. sulfur dioxide graphite calcium bromide lithium methane molecular covalent ionic ionic molecular ____ 35. ____ 37. b. e. ____ 36. H2O. Arrange the following in order of increasing melting points. Most molecular solids melt at lower temperatures than metallic solids. b. Which statement is false? a. BaBr2 d. He. BaCl2 c. d. b. c. He < H2O < HF < KCl H2O < HF < He < KCl KCl < H2O < HF < He He < HF < H2O < KCl H2O < He < KCl < HF . and the valence electrons are distributed over the lattice as a whole. c. 3s and 4s . 3s and 3p b. a. 3p and 3d e.____ 40. 3s and 3d c. 3d and 4s d. The conduction band of magnesium is thought to result from the combination of molecular orbitals resulting from overlap of __________ atomic orbitals. 16. 21. 34. 35. 2.AP Chem Chapter 13 Homework Answer Section MULTIPLE CHOICE 1. 5. 40. ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: C A E B D B C D E C D A B C E A B C C E B E E E B B D D C C D D C D E D A E D A PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 1 TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: TOP: Kinetic-Molecular Description of Liquids and Solids Kinetic-Molecular Description of Liquids and Solids Kinetic-Molecular Description of Liquids and Solids Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes Intermolecular Attractions and Phase Changes The Liquid State The Liquid State Heat Transfer Involving Liquids Heat Transfer Involving Liquids Sublimation Phase Diagrams (P vs. 17. 33. 37. 32. 10. 20. 30. 27. 19. 28. 18. 6. T) Phase Diagrams (P vs. 14. T) Structures of Crystals Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Bonding in Solids Band Theory of Metals . 9. 31. 26. T) Phase Diagrams (P vs. 8. 12. 24. 22. 13. 11. 15. 23. 3. 4. 29. 39. 7. 36. 38. 25.
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