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Chapter 11 - States of Matter: Liquids and Solids
1. Which of the following statements concerning liquids is incorrect?A) The volume of a liquid changes very little with pressure.B) Liquids are relatively incompressible.C) Liquid molecules move slowly compared to solids.D) Non-volatile liquids have low vapor pressures at room temperature.E) The molecules of a liquid are in constant random motion.
ANS: C PTS: 1 DIF: easy REF: 11.1OBJ: Compare a gas, a liquid, and a solid using a kinetic-molecular theory description.TOP: phases | liquid KEY: properties of liquidsMSC: general chemistry
2. Which of the following statements concerning solids, liquids and gases is/are correct?
1. The close contact of the particles in a solid prevents all possible motion, including vibrational motion.
2. Liquids and gases are both considered fluids.3. The postulate from kinetic-molecular theory that the particles in a gas are in
constant random motion is equally applicable to liquids, except the particles are more tightly packed in a gas.
A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 2 and 3
ANS: B PTS: 1 DIF: easy REF: 11.1OBJ: Compare a gas, a liquid, and a solid using a kinetic-molecular theory description.TOP: phases | liquid
3. What is the name for the following phase change?
I2(s) I2(g)
A) sublimationB) freezingC) vaporizationD) condensationE) melting
ANS: A PTS: 1 DIF: easy REF: 11.2OBJ: Define melting, freezing, vaporization, sublimation, and condensation.TOP: phases | phase transitions MSC: general chemistry
Test Bank General Chemistry, 10th edition 1
4. Which of the following processes is endothermic?
A) melting of iceB) condensation of waterC) deposition of carbon dioxideD) freezing of waterE) condensation of ammonia
ANS: A PTS: 1 DIF: moderate REF: 11.2OBJ: Define melting, freezing, vaporization, sublimation, and condensation.TOP: phases | phase transitions
5. The process represented by the equation C10H8(s) C10H8(g) isA) melting.B) liquefaction.C) sublimation.D) condensation.E) fusion.
ANS: C PTS: 1 DIF: easy REF: 11.2OBJ: Define melting, freezing, vaporization, sublimation, and condensation.TOP: phases | phase transitions MSC: general chemistry
6. When a solid undergoes a phase change to a gas, the process is calledA) fusion.B) condensation.C) melting.D) vaporization.E) sublimation.
ANS: E PTS: 1 DIF: easy REF: 11.2OBJ: Define melting, freezing, vaporization, sublimation, and condensation.TOP: phases | phase transitions MSC: general chemistry
7. A bottle is filled with a small amount of a volatile liquid and sealed. Sometime later it is observed that no liquid is evident in the sealed bottle. Which of the following statements would explain this observation?
A) More time is needed to establish equilibrium.B) Liquid and vapor are at equilibrium in the bottle.C) Too little liquid was added to achieve a liquid vapor equilibrium in the closed
system.D) The vapor state is favored when equilibrium is established.E) The liquid has undergone sublimation.
ANS: C PTS: 1 DIF: moderate REF: 11.2OBJ: Define vapor pressure. TOP: phases | phase transitionsKEY: vapor pressure MSC: general chemistry
Test Bank General Chemistry, 10th edition 2
8. Enough of a volatile liquid is placed in a closed container to achieve a liquid-vapor equilibrium at a fixed temperature. Which of the following statements regarding this system is/are correct once equilibrium is established?
1. Liquid molecules are no longer evaporating.2. The number of vapor molecules remains essentially constant.3. The partial pressure exerted by the vapor molecules is called the vapor
pressure of the liquid.
A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 2 and 3
ANS: E PTS: 1 DIF: moderate REF: 11.2OBJ: Define vapor pressure. TOP: phases | phase transitions
9. Enough of a volatile liquid is placed in a closed container to achieve a liquid-vapor equilibrium. Which of the following statements regarding this system is/are correct once equilibrium is established?
1. The rate of condensation is equal to the rate of evaporation.2. The fraction of molecules with enough energy to escape the liquid surface
depends on the liquid surface area.3. The vapor pressure is independent of the temperature.
A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1, 2, and 3
ANS: A PTS: 1 DIF: moderate REF: 11.2OBJ: Define vapor pressure. TOP: phases | phase transitions
10. If more ice is added to an ice-water mixture at equilibrium,A) the temperature will increase somewhat.B) the vapor pressure of the water will decrease.C) the temperature will decrease somewhat.D) the vapor pressure of the water will rise.E) the vapor pressure of the water will remain constant.
ANS: E PTS: 1 DIF: moderate REF: 11.2OBJ: Describe the process of reaching a dynamic equilibrium that involves the vaporization of a liquid and condensation of its vapor.TOP: phases | phase transitions KEY: vapor pressureMSC: general chemistry
Test Bank General Chemistry, 10th edition 3
11. Which of the following involves a change in temperature during the phase transition?
A) condensation of waterB) fusion of ethanolC) vaporization of waterD) all of the aboveE) none of the above
ANS: E PTS: 1 DIF: moderate REF: 11.2OBJ: Describe the process of reaching a dynamic equilibrium that involves the vaporization of a liquid and condensation of its vapor.TOP: phases | phase transitions
12. The boiling point of a liquid is
A) always the temperature at which the vapor pressure equals 760 mmHg (1 atm).B) always the temperature at which the liquid phase of a substance is in equilibrium
with the vapor phase.C) always the temperature at which the vapor pressure equals the pressure exerted on
the liquid.D) always equal to the vapor pressure of the liquid at a given temperature.E) independent of the pressure exerted on the liquid.
ANS: C PTS: 1 DIF: easy REF: 11.2OBJ: Define boiling point. TOP: phases | phase transitions
13. Which one of the following liquids would you expect to have the highest vapor pressure at room temperature? (all boiling points are normal boiling points)
A) n-pentane, b.p. = 36.1°CB) methanol, b.p. = 65.0°CC) carbon tetrachloride, b.p. = 76.7°CD) acetic acid, b.p. = 118°CE) mercury, b.p. = 357°C
ANS: A PTS: 1 DIF: moderate REF: 11.2OBJ: Define boiling point. TOP: phases | phase transitions
14. In which of the following processes will energy be evolved as heat?A) crystallizationB) meltingC) sublimationD) vaporizationE) none of these
ANS: A PTS: 1 DIF: easy REF: 11.2OBJ: Define heat (enthalpy) of fusion and heat (enthalpy) of vaporization.TOP: phases | phase transitions KEY: phase transition enthalpy changeMSC: general chemistry
Test Bank General Chemistry, 10th edition 4
15. Which of the following phase changes are endothermic?
A) vaporizationB) freezingC) liquifactionD) crystallizationE) condensation
ANS: A PTS: 1 DIF: easy REF: 11.2OBJ: Define heat (enthalpy) of fusion and heat (enthalpy) of vaporization.TOP: phases | phase transitions
16. The enthalpy of fusion of sodium is 2.60 kJ/mol. How many grams of sodium can be melted by adding 81.7 kJ of energy to the metal at its melting point?
A) 7.22 102 gB) 9.24 gC) 3.55 gD) 31.4 gE) 1.50 103 g
ANS: A PTS: 1 DIF: easy REF: 11.2OBJ: Calculate the heat required for a phase change of a given mass of substance. (Example 11.1) TOP: phases | phase transitions
17. Assume 12,500 J of energy is added to 2.0 moles (36 grams) of H2O as an ice sample at 0°C. The molar heat of fusion is 6.02 kJ/mol. The specific heat of liquid water is 4.18 J/g °C. The molar heat of vaporization is 40.6 kJ/mol. The resulting sample contains which of the following?A) water and water vaporB) ice and waterC) only waterD) only water vaporE) only ice
ANS: C PTS: 1 DIF: moderate REF: 11.2OBJ: Calculate the heat required for a phase change of a given mass of substance. (Example 11.1) TOP: phases | phase transitionsKEY: phase transition enthalpy change MSC: general chemistry
18. How much heat is released at constant pressure if a 14.0-L tank containing 56.0 atm of hydrogen sulfide gas condenses at its boiling point of -60.0oC? The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0oC. (R = 0.0821 L • atm/(K • mol))A) 1.17 102 JB) 2.98 106 JC) 4.17 102 JD) 1.87 104 JE) 8.38 105 J
Test Bank General Chemistry, 10th edition 5
ANS: E PTS: 1 DIF: moderate REF: 11.2OBJ: Calculate the heat required for a phase change of a given mass of substance. (Example 11.1) TOP: phases | phase transitionsKEY: phase transition enthalpy change MSC: general chemistry
19. What is the value of q when 8.21 g of water vaporizes at 373 K? The enthalpy of condensation of water at 373 K is –40.7 kJ/mol.A) –334 kJB) –18.5 kJC) 18.5 kJD) 334 kJE) 0.202 kJ
ANS: C PTS: 1 DIF: moderate REF: 11.2OBJ: Calculate the heat required for a phase change of a given mass of substance. (Example 11.1) TOP: phases | phase transitionsKEY: phase transition enthalpy change MSC: general chemistry
20. The vapor pressure of a liquid increases with increasing temperature. Which of the following statements best explains this relationship?A) All the molecules have greater kinetic energies.B) The number of gaseous molecules above the liquid remains constant, but these
molecules have greater average kinetic energy.C) The faster-moving molecules in the liquid exert a greater pressure.D) The intermolecular forces between the molecules decrease at higher temperatures.E) The average kinetic energy of molecules is greater; thus more molecules can enter
the gaseous state.
ANS: E PTS: 1 DIF: moderate REF: 11.2OBJ: Describe the general dependence of the vapor pressure (in P) on the temperature (T).TOP: phases | phase transitions KEY: vapor pressureMSC: general chemistry
21. The vapor pressure of a given liquid will increase ifA) the liquid is moved to a container in which its surface is very much larger.B) the volume of the liquid is increased.C) the temperature is increased.D) the volume of the vapor phase is increased.E) a more volatile liquid is added to the given liquid.
ANS: C PTS: 1 DIF: easy REF: 11.2OBJ: Describe the general dependence of the vapor pressure (in P) on the temperature (T).TOP: phases | phase transitions KEY: vapor pressureMSC: general chemistry
Test Bank General Chemistry, 10th edition 6
22. A particular compound has an enthalpy of vaporization of 28300 J/mol. At 281 K it has a vapor pressure of 101 mmHg. What is its vapor pressure at 301 K? (R = 8.31 J/(K· mol))A) 98.8 mmHgB) 123 mmHgC) 45.2 mmHgD) 226 mmHgE) 103 mmHg
ANS: D PTS: 1 DIF: moderate REF: 11.2OBJ: Calculate the vapor pressure at a given temperature. (Example 11.2)TOP: phases | phase transitions KEY: Clausius-Clapeyron equationMSC: general chemistry
23. A liquid has an enthalpy of vaporization of 30.8 kJ/mol. At 275 K it has a vapor pressure of 117 mmHg. What is the normal boiling point of this liquid? (R = 8.31 J/(K· mol))A) 293 KB) 319 KC) 275 KD) 259 KE) 241 K
ANS: B PTS: 1 DIF: moderate REF: 11.2OBJ: Calculate the vapor pressure at a given temperature. (Example 11.2)TOP: phases | phase transitions KEY: Clausius-Clapeyron equationMSC: general chemistry
24. In a certain mountain range, water boils at 94°C. What is the atmospheric pressure under these conditions? The enthalpy of vaporization of water at 100°C is 40.7 kJ/mol. (R = 8.31 J/(K · mol))A) 1760 mmHgB) 324 mmHgC) 613 mmHgD) 942 mmHgE) 329 mmHg
ANS: C PTS: 1 DIF: moderate REF: 11.2OBJ: Calculate the vapor pressure at a given temperature. (Example 11.2)TOP: phases | phase transitions KEY: Clausius-Clapeyron equationMSC: general chemistry
25. For a particular liquid, raising its temperature from 319 K to 337 K causes its vapor pressure to double. What is the enthalpy of vaporization of this liquid? (R = 8.31 J/(K · mol))A) 34.4 kJ/molB) 320 kJ/molC) 2.01 kJ/molD) 228 kJ/molE) 104 kJ/mol
Test Bank General Chemistry, 10th edition 7
ANS: A PTS: 1 DIF: difficult REF: 11.2OBJ: Calculate the heat of vaporization from vapor pressure. (Example 11.3)TOP: phases | phase transitions KEY: Clausius-Clapeyron equationMSC: general chemistry
26. Knowing that Hvap for water is 40.7 kJ/mol, calculate Pvap of water at 37°C.A) 52.7 torrB) 25.4 torrC) 18.7 torrD) 12.4 torrE) 6.90 torr
ANS: A PTS: 1 DIF: difficult REF: 11.2OBJ: Calculate the heat of vaporization from vapor pressure. (Example 11.3)TOP: phases | phase transitions KEY: Clausius-Clapeyron equationMSC: general chemistry
27. What is the enthalpy of vaporization of a compound that has a vapor pressure of 131 mmHg at 211 K and 2.23 mmHg at 177 K? (R = 8.31 J/(K· mol))A) 996 kJ/molB) 1.15 kJ/molC) 3.31 kJ/molD) 37.2 kJ/molE) 368 kJ/mol
ANS: D PTS: 1 DIF: moderate REF: 11.2OBJ: Calculate the heat of vaporization from vapor pressure. (Example 11.3)TOP: phases | phase transitions KEY: Clausius-Clapeyron equationMSC: general chemistry
28. In the accompanying phase diagram, a liquid can be present at combinations of temperature and pressure corresponding to points
A) A, C, G, and D.B) A, C, D, and F.C) A, B, C, and G.D) A and C only.E) G, C, D, and E.
Test Bank General Chemistry, 10th edition 8
ANS: B PTS: 1 DIF: moderate REF: 11.3OBJ: Define phase diagram. TOP: phases | phase transitionsKEY: phase diagram MSC: general chemistry
29. Which of the following statements concerning the accompanying phase diagram is false?
A) The solid is more dense than the liquid.B) Point C is the critical point of the substance.C) Point A is the triple point of the substance.D) The normal boiling point is above the triple point.E) The curve AD divides the solid region from the gas region.
ANS: A PTS: 1 DIF: moderate REF: 11.3OBJ: Define phase diagram. TOP: phases | phase transitions
30. Given the accompanying phase diagram, under what conditions will liquid be found in equilibrium with either solid or gas?
A) Anywhere along curve AB.B) Anywhere along curve AC.C) Anywhere along curve AD.D) Anywhere along curve AB and AC.E) Anywhere along curve AB and AD.
Test Bank General Chemistry, 10th edition 9
ANS: D PTS: 1 DIF: moderate REF: 11.3OBJ: Define phase diagram. TOP: phases | phase transitions
31. Choose the correct statement about the diagram below.
A) The diagram shows the triple point above 1 atm pressure.B) The diagram is qualitatively correct for water.C) The diagram shows that the melting point of the solid increases with increasing
pressure.D) The diagram could represent the phase diagram of CO2.E) None of the above statements is correct.
ANS: C PTS: 1 DIF: moderate REF: 11.3OBJ: Define phase diagram. TOP: phases | phase transitionsKEY: phase diagram MSC: general chemistry
32. From a consideration of the phase diagram below, a change from point M to point N corresponds to
A) sublimation.B) liquefaction.C) evaporation.D) condensation.E) freezing.
ANS: E PTS: 1 DIF: easy REF: 11.3OBJ: Define phase diagram. TOP: phases | phase transitionsKEY: phase diagram MSC: general chemistry
Test Bank General Chemistry, 10th edition 10
33. The triple point of iodine is at 90 torr and 115°C. This means that liquid I2A) cannot have a vapor pressure less than 90 torr.B) is more dense than I2(s).C) cannot exist at 1 atmosphere pressure.D) cannot exist above 115°C.E) can exist at pressure of 10 torr.
ANS: A PTS: 1 DIF: easy REF: 11.3OBJ: Define triple point. TOP: phases | phase transitionsKEY: phase diagram MSC: general chemistry
34. The critical point of CCl4 is 283°C and 45 atm pressure. Liquid CCl4 has a vapor pressure of 10.0 atm at 178°C. Which of the following statements must be true?A) Vapor and liquid can only be in equilibrium at one temperature—the normal
boiling point.B) Liquid CCl4 can exist at temperatures greater than 283°C if the pressure is greater
than 45 atm.C) Liquid and solid can only be in equilibrium at one temperature—the freezing point.D) The triple point of CCl4 must be less than 178°C.E) The normal boiling point of CCl4 must be greater than 178°C.
ANS: D PTS: 1 DIF: moderate REF: 11.3OBJ: Define triple point. TOP: phases | phase transitionsKEY: phase diagram | triple point MSC: general chemistry
35. Below is a phase diagram for a substance.
What is the name for point X on the diagram?A) boiling pointB) normal boiling pointC) triple pointD) melting pointE) critical point
ANS: C PTS: 1 DIF: easy REF: 11.3OBJ: Define triple point. TOP: phases | phase transitionsKEY: phase diagram | triple point MSC: general chemistry
Test Bank General Chemistry, 10th edition 11
36. Below is a phase diagram for a substance.
Which line represents the melting-point curve of the substance?A) R-XB) S-XC) X-ZD) S-ZE) M-N
ANS: A PTS: 1 DIF: easy REF: 11.3OBJ: Describe the melting-point curve and the vapor-pressure curves (for the liquid and the solid) in a phase diagram. TOP: phases | phase transitionsKEY: phase diagram | melting-point curve MSC: general chemistry
37. Below is a phase diagram for a substance.
Which line represents the vapor-pressure curve of the substance?A) S-ZB) X-ZC) S-XD) M-NE) R-X
ANS: B PTS: 1 DIF: easy REF: 11.3OBJ: Describe the melting-point curve and the vapor-pressure curves (for the liquid and the solid) in a phase diagram. TOP: phases | phase transitionsKEY: phase diagram | vapor pressure curve MSC: general chemistry
Test Bank General Chemistry, 10th edition 12
38. If the liquid of a pure substance has a lower density than the solid, what is the effect on the pressure-temperature phase diagram?A) The vapor-pressure curve arches upward.B) The normal melting point is above room temperature.C) The melting-point curve has a negative slope.D) The vapor-pressure curve arches downward.E) The melting-point curve has a positive slope.
ANS: E PTS: 1 DIF: moderate REF: 11.3OBJ: Describe the melting-point curve and the vapor-pressure curves (for the liquid and the solid) in a phase diagram. TOP: phases | phase transitionsKEY: phase diagram | melting-point curve MSC: general chemistry
39. Below is a phase diagram for a substance.
What is the name for point Z on the diagram?A) normal boiling point.B) critical point.C) melting point.D) boiling point.E) triple point.
ANS: B PTS: 1 DIF: easy REF: 11.3OBJ: Define critical temperature and critical pressure.TOP: phases | phase transitions KEY: phase diagramMSC: general chemistry
40. Which explanation best describes surface tension?A) Molecules at the surface of a liquid experience a net force towards the liquid's
interior.B) Molecules at the edges of a liquid adhere to the surface of the liquid's container.C) Molecules of a liquid tend to form a concave meniscus.D) Molecules of a liquid tend to resist flow.E) Molecules of a liquid have a very low vapor pressure.
ANS: A PTS: 1 DIF: easy REF: 11.4OBJ: Define surface tension. TOP: phases | liquidKEY: properties of liquids | surface tension MSC: general chemistry
Test Bank General Chemistry, 10th edition 13
41. If the diameter of a spherical water droplet is 100.0 m, how much energy is required to increase the diameter of the water droplet by 3.0 m? The surface tension of water is 1.0 10-3 J/m2.A) 3.1 10–11 JB) 1.9 10–12 JC) 2.8 10–14 JD) 7.7 10–12 JE) 3.3 10–11 J
ANS: B PTS: 1 DIF: moderate REF: 11.4OBJ: Define surface tension. TOP: phases | liquidKEY: properties of liquids | surface tension MSC: general chemistry
42. Which is the best reason for why water in a glass capillary has a concave meniscus, while mercury in a glass capillary has a convex meniscus?A) Mercury has a greater dispersion force than water.B) The water is attracted more strongly to the glass than the mercury is attracted to the
glass.C) The mercury is attracted more strongly to the glass than the water is attracted to the
glass.D) Water is a molecular compound while mercury is a metallic element.E) Water has a greater dispersion force than mercury.
ANS: B PTS: 1 DIF: easy REF: 11.4OBJ: Describe the phenomenon of capillary rise. TOP: phases | liquidKEY: properties of liquids | surface tension MSC: general chemistry
43. Which of the following forces is/are responsible for capillary action, a property of liquids?
1. attractive forces between the liquid and the capillary material2. surface tension of the liquid3. viscosity of the liquid
A) 1B) 2C) 3D) 1 and 2E) 1, 2, and 3
ANS: D PTS: 1 DIF: easy REF: 11.4OBJ: Describe the phenomenon of capillary rise. TOP: phases | liquidKEY: properties of liquids MSC: general chemistry
44. Which of the following concerning surface tension and viscosity is/are correct?
1. A molecule at the surface of a liquid experiences a net attractive force toward the interior of the liquid.
2. The surface tension of a liquid is unaffected by substances dissolved in the liquid.
Test Bank General Chemistry, 10th edition 14
3. The viscosity of a liquid is determined in part by the strength of intermolecular forces.
A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1 and 3
ANS: E PTS: 1 DIF: easy REF: 11.4OBJ: Describe the phenomenon of capillary rise. TOP: phases | liquid
45. The measure of the resistance to flow of a liquid isA) London forces.B) van der Waals forces.C) viscosity.D) vapor pressure.E) surface tension.
ANS: C PTS: 1 DIF: easy REF: 11.4OBJ: Define viscosity. TOP: phases | liquidKEY: properties of liquids | viscosity MSC: general chemistry
46. In which of the following substances are intermolecular forces of attraction absent?
A) HF(l)B) CCl4(l)C) NaCl(l)D) H2O(l)E) N2(l)
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Define London (dispersion) forces. TOP: phases | liquid
47. Which one of the following decreases as the strength of the attractive intermolecular forces increases?A) The normal boiling temperature.B) The vapor pressure of a liquid.C) The extent of deviations from the ideal gas law.D) The heat of vaporization.E) The sublimation temperature of a solid.
ANS: B PTS: 1 DIF: moderate REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
Test Bank General Chemistry, 10th edition 15
48. Which of the following compounds has the highest normal boiling point?A) CH3CH2CH2CH3
B) CH3ClC) CH3CH2OHD) CH3OCH3
E) CH3CH2CH3
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
49. Which of the following compounds has the highest vapor pressure at 25°C?A) CH3CH2OHB) CH3CH2CH2CH3
C) CH3OCH3
D) CH3CH2CH3
E) CH3CH2CH2Cl
ANS: D PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
50. Which of the following pure substances has the lowest normal boiling point?A) H2SB) NH3
C) H2OD) H2TeE) H2Se
ANS: A PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
51. Methane (CH4) is able to be liquefied at low temperatures due to which intermolecular force?
A) ionic bondingB) covalent bondingC) hydrogen bondingD) dipole–dipoleE) London dispersion
ANS: E PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid
Test Bank General Chemistry, 10th edition 16
52. Which compound has the lowest standard enthalpy of vaporization at 25°C?A) C6H14
B) C8H16
C) C5H12
D) C8H18
E) C7H16
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forces | London forcesMSC: general chemistry
53. Which of the following indicates the existence of strong intermolecular forces of attraction in a liquid?A) a very low critical temperatureB) a very low boiling pointC) a very low vapor pressureD) a very low viscosityE) a very low enthalpy of vaporization
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
54. Which of the following compounds has the lowest normal boiling point?A) CH3CH2CH2NH2
B) CH3CH2CH2FC) CH3CH2CH2OHD) CH3CH2COOHE) CH3CH(OH)CH3
ANS: B PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
55. Which of the following compounds is expected to have the lowest vapor pressure?A) CH3OCH3
B) CH3CH2FC) CH3CH2OHD) CH3CH2CH2CH3
E) CH3CH2CH3
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
Test Bank General Chemistry, 10th edition 17
56. Which of the following pure substances has the highest normal boiling point?A) HIB) HClC) HFD) H2SE) HBr
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
57. Why does hydrogen fluoride have an unusually high normal boiling point compared to the other hydrogen halides?A) The H-F bond in hydrogen fluoride is very strong.B) Hydrogen fluoride has very strong London dispersion forces.C) Hydrogen fluoride is capable of forming hydrogen bonds.D) Hydrogen fluoride is ionic.E) Hydrogen fluoride is covalent.
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
58. Which of the following pure substances has the lowest vapor pressure at 25°C?A) SbH3
B) NH3
C) PH3
D) AsH3
E) H2O
ANS: E PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
59. Which of the following pure substances has the highest vapor pressure at room temperature?A) Si3H8
B) Si2H6
C) Si2Cl6
D) Si4H10
E) SiH4
ANS: E PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forces | London forcesMSC: general chemistry
Test Bank General Chemistry, 10th edition 18
60. Which of the following pure substances has the highest standard enthalpy of vaporization at 25°C?A) H2OB) NH3
C) PH3
D) AsH3
E) SbH3
ANS: A PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
61. At 25°C, the vapor pressure of diethyl ether, (CH3CH2)2O, is higher than the vapor pressure of its isomer n-butanol, CH3CH2CH2CH2OH, becauseA) diethyl ether has a higher density than n-butanol.B) diethyl ether has weaker intermolecular forces than n-butanol.C) diethyl ether has a lower critical temperature than n-butanol.D) diethyl ether has a higher surface tension than n-butanol.E) diethyl ether has weaker intramolecular forces than n-butanol.
ANS: B PTS: 1 DIF: easy REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
62. Which of the following pure substances has an unusually high normal boiling point?A) CH3OCH3
B) CH3SHC) HClD) CH3NH2
E) CH3Cl
ANS: D PTS: 1 DIF: moderate REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
63. Rank the following molecules in order of increasing normal boiling point: CH3CH2OH, CH3CH2CH2OH, CH3CH2OCH3.A) lowest CH3CH2CH2OH, CH3CH2OCH3, CH3CH2OH highest.B) lowest CH3CH2OH, CH3CH2OCH3, CH3CH2CH2OH highest.C) lowest CH3CH2CH2OH, CH3CH2OH, CH3CH2OCH3 highest.D) lowest CH3CH2OCH3, CH3CH2OH, CH3CH2CH2OH highest.E) lowest CH3CH2OCH3, CH3CH2CH2OH, CH3CH2OH highest.
ANS: D PTS: 1 DIF: moderate REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
Test Bank General Chemistry, 10th edition 19
64. Rank the following in order of increasing normal boiling point: N2, O2, Br2, Xe.
A) N2 < O2 < Xe < Br2
B) O2 < N2 < Xe < Br2
C) Br2 < Xe < N2 < O2
D) N2 < O2 < Br2 < Xe E) Xe < Br2 < N2 < O2
ANS: A PTS: 1 DIF: moderate REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid
65. Which of the following concerning intermolecular forces is/are correct?
1. Intermolecular forces depend in part on the shape of a molecule.2. London forces contribute to the net forces of attraction found in all molecular
solids and liquids.3. Hydrogen bonding is a special category of dipole-dipole attractions.
A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1, 2, and 3
ANS: E PTS: 1 DIF: moderate REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid
66. In an experiment, 40.0 mmol of helium gas is collected over water. The total volume of gas collected is 0.224 L. Under similar conditions, the gas is collected over two other liquids, A and B. The total volume of gas collected over A and B are 0.222 L and 0.227 L, respectively. Which of the following statements is false?A) Liquid B boils at a higher temperature than waterB) Liquid A boils at a higher temperature than waterC) The vapor pressure of B is higher than that of AD) The vapor pressure of B is higher than that of waterE) Liquid A boils at a temperature higher than B
ANS: A PTS: 1 DIF: difficult REF: 11.5OBJ: Relate the properties of liquids to the intermolecular forces involved.TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
Test Bank General Chemistry, 10th edition 20
67. When two water molecule form a hydrogen bond, which atoms are involved in the interaction?A) Two hydrogens from one molecule and one hydrogen from the other moleculeB) An oxygen from one molecule and an oxygen from the other moleculeC) Two hydrogens from one molecule and one oxygen from the other moleculeD) A hydrogen from one molecule and a hydrogen from the other moleculeE) A hydrogen from one molecule and an oxygen from the other molecule
ANS: E PTS: 1 DIF: easy REF: 11.5OBJ: Define hydrogen bonding. TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
68. What is the maximum number of hydrogen bonds in which a water molecule could participate?A) 2B) 4C) 3D) 6E) 5
ANS: B PTS: 1 DIF: moderate REF: 11.5OBJ: Define hydrogen bonding. TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
69. Which pure substance exhibits hydrogen bonding?A) HNF2
B) B2H6
C) HBrD) H2SE) CaH2
ANS: A PTS: 1 DIF: easy REF: 11.5OBJ: Define hydrogen bonding. TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
70. Which of the following substances has the weakest intermolecular forces?A) I2
B) C8H18
C) SiH4
D) CH3CH2CH2CH2OHE) SbCl3
ANS: C PTS: 1 DIF: easy REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
Test Bank General Chemistry, 10th edition 21
71. Which of the following best describes carbon dioxide (CO2) at room temperature and pressure?A) ionic solidB) nonpolar molecular gasC) metallic solidD) polar molecular gasE) covalent network solid
ANS: B PTS: 1 DIF: easy REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | gas MSC: general chemistry
72. Which of the following pure substances may exhibit hydrogen bonding?A) CH3ClB) CH3OCH3
C) H2COD) N(CH3)3
E) H2NNH2
ANS: E PTS: 1 DIF: easy REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | liquidKEY: intermolecular forces | hydrogen bonding MSC: general chemistry
73. The strongest intermolecular forces present in a sample of pure I2 areA) London forces.B) dipole–dipole forces.C) metallic bonds.D) covalent network bonds.E) covalent bonds.
ANS: A PTS: 1 DIF: easy REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | liquid KEY: intermolecular forces | London forcesMSC: general chemistry
74. The strongest intermolecular forces between molecules of PH3 areA) hydrogen bonds.B) covalent bonds.C) ionic bonds.D) London forces.E) dipole–dipole attractions.
ANS: E PTS: 1 DIF: easy REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
Test Bank General Chemistry, 10th edition 22
75. The molecules in a sample of solid SO2 are attracted to each other by a combination ofA) H-bonding and ionic bonding.B) covalent bonding and dipole-dipole interactions.C) London forces and H-bonding.D) London forces and dipole-dipole interactions.E) none of these
ANS: D PTS: 1 DIF: moderate REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
76. Which of the following best describes silane (SiH4) at room temperature and pressure?A) ionic solidB) covalent network solidC) nonpolar molecular gasD) polar molecular gasE) metallic solid
ANS: C PTS: 1 DIF: moderate REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | gas MSC: general chemistry
77. Which of the following is the strongest intermolecular force present in dry ice, CO2(s)?A) covalent bondingB) hydrogen bondingC) ionic bondingD) London forcesE) metallic bonding
ANS: D PTS: 1 DIF: easy REF: 11.5OBJ: Identify the intermolecular forces in a substance. (Example 11.5)TOP: phases | liquid KEY: intermolecular forcesMSC: general chemistry
78. A solid has a very high melting point, is hard, and in the molten state is a non-conductor. The solid is most likely
A) a covalent network solid.B) a metallic solid.C) an amorphous solid.D) a molecular solid.E) an ionic solid.
ANS: A PTS: 1 DIF: easy REF: 11.6OBJ: Define molecular solid, metallic solid, ionic solid, and covalent network solid.TOP: phases | solid
Test Bank General Chemistry, 10th edition 23
79. Van der Waals forces must be broken to melt this type of solid.
A) A covalent network solid.B) A metallic solid.C) A molecular solid.D) An ionic solid.E) none of the above
ANS: C PTS: 1 DIF: easy REF: 11.6OBJ: Define molecular solid, metallic solid, ionic solid, and covalent network solid.TOP: phases | solid
80. Which substance can be described as cations bonded together by mobile electrons?A) S8(s)B) Ag(s)C) HCl(l)D) KCl(s)E) Kr(l)
ANS: B PTS: 1 DIF: easy REF: 11.6OBJ: Define molecular solid, metallic solid, ionic solid, and covalent network solid.TOP: phases | solid KEY: classification of solidsMSC: general chemistry
81. Which of the following best describes calcium hydride (CaH2) at room temperature and pressure?A) nonpolar molecular gasB) metallic solidC) ionic solidD) polar molecular gasE) covalent network solid
ANS: C PTS: 1 DIF: moderate REF: 11.6OBJ: Identify types of solids. (Example 11.7) TOP: phases | solidKEY: classification of solids MSC: general chemistry
82. Which of the following is not a covalent network solid?A) diamondB) silicon carbideC) quartzD) ironE) graphite
ANS: D PTS: 1 DIF: easy REF: 11.6OBJ: Identify types of solids. (Example 11.7) TOP: phases | solidKEY: classification of solids MSC: general chemistry
Test Bank General Chemistry, 10th edition 24
83. Which of the following is a molecular solid?A) NaClB) CH4
C) SiO2
D) C(graphite)E) C(diamond)
ANS: B PTS: 1 DIF: easy REF: 11.6OBJ: Identify types of solids. (Example 11.7) TOP: phases | solidKEY: classification of solids MSC: general chemistry
84. Which of the following is an ionic solid?A) SiO2(s)B) Ne(s)C) Na(s)D) CsF(s)E) CO2(s)
ANS: D PTS: 1 DIF: easy REF: 11.6OBJ: Identify types of solids. (Example 11.7) TOP: phases | solidKEY: classification of solids MSC: general chemistry
85. Which bonding interaction best describes the strongest intermolecular forces in AlH3?A) dipole–dipole forcesB) metallic bondingC) ionic bondingD) London dispersion forcesE) primarily hydrogen bonding
ANS: C PTS: 1 DIF: moderate REF: 11.6OBJ: Identify types of solids. (Example 11.7) TOP: phases | solidMSC: general chemistry
86. Which of the following is a molecular solid?A) carborundum, SiCB) quartzC) glassD) hydrogen chlorideE) potassium
ANS: D PTS: 1 DIF: easy REF: 11.6OBJ: Identify types of solids. (Example 11.7) TOP: phases | solidKEY: classification of solids MSC: general chemistry
87. Which of the following pure substances has the highest normal melting point?A) KFB) KIC) NaFD) NaClE) NaI
Test Bank General Chemistry, 10th edition 25
ANS: C PTS: 1 DIF: easy REF: 11.6OBJ: Relate the melting point of a solid to its structure. TOP: phases | solidKEY: properties of solids | melting point MSC: general chemistry
88. Which of the following pure substances has the lowest melting point?A) LiFB) RbFC) CsFD) KFE) NaF
ANS: C PTS: 1 DIF: easy REF: 11.6OBJ: Relate the melting point of a solid to its structure. TOP: phases | solidKEY: properties of solids | melting point MSC: general chemistry
89. Which of the following pure substances has the lowest melting point?A) Cs2OB) CsClC) CsBrD) CsIE) CsF
ANS: D PTS: 1 DIF: easy REF: 11.6OBJ: Relate the melting point of a solid to its structure. TOP: phases | solidKEY: properties of solids | melting point MSC: general chemistry
90. Which of the following pure substances has the highest melting point?A) CCl4
B) AlCl3
C) NCl3
D) LiClE) MgCl2
ANS: B PTS: 1 DIF: easy REF: 11.6OBJ: Relate the melting point of a solid to its structure. TOP: phases | solidKEY: properties of solids | melting point MSC: general chemistry
91. Which of the following pure substances has the highest melting point?A) KBrB) NaClC) NaFD) CsIE) LiF
ANS: E PTS: 1 DIF: moderate REF: 11.6OBJ: Relate the melting point of a solid to its structure. TOP: phases | solidKEY: properties of solids | melting point MSC: general chemistry
Test Bank General Chemistry, 10th edition 26
92. A low melting solid readily dissolves in water to give a nonconducting solution. The solid is most likely a
A) molecular solid.B) ionic solid.C) covalent network solid.D) weak base.E) metallic solid.
ANS: A PTS: 1 DIF: easy REF: 11.6OBJ: Relate the melting point of a solid to its structure. TOP: phases | solid
93. Which of the following pure substances is a solid at room temperature and pressure?A) NH3
B) PH3
C) SiH4
D) CH4
E) AlH3
ANS: E PTS: 1 DIF: easy REF: 11.6OBJ: Determine relative melting points based on types of solids. (Example 11.8)TOP: phases | solid KEY: properties of solids | melting pointMSC: general chemistry
94. Which of the following pure substances has the highest normal melting point?A) NO2
B) SiO2
C) CO2
D) P4O10
E) N2O5
ANS: B PTS: 1 DIF: easy REF: 11.6OBJ: Determine relative melting points based on types of solids. (Example 11.8)TOP: phases | solid KEY: properties of solids | melting pointMSC: general chemistry
95. Which of the following pure substances has the highest normal melting point?A) P4O10
B) P4O6
C) CO2
D) CaOE) Na2O
ANS: D PTS: 1 DIF: moderate REF: 11.6OBJ: Determine relative melting points based on types of solids. (Example 11.8)TOP: phases | solid KEY: properties of solids | melting pointMSC: general chemistry
Test Bank General Chemistry, 10th edition 27
96. Which of the following pure substances has the highest normal boiling point?A) H2OB) CF4
C) CsFD) CaF2
E) KF
ANS: D PTS: 1 DIF: moderate REF: 11.6OBJ: Determine relative melting points based on types of solids. (Example 11.8)TOP: phases | solid KEY: properties of solidsMSC: general chemistry
97. A certain solid substance that is very hard, has a high melting point, and is nonconducting unless melted is most likely to be:A) CO2
B) I2
C) H2OD) NaClE) Cu
ANS: D PTS: 1 DIF: easy REF: 11.6OBJ: Relate the hardness and electrical conductivity of a solid to its structure.TOP: phases | solid KEY: properties of solidsMSC: general chemistry
98. A solid crystal of NaCl isA) soft, low melting, a poor electrical conductor.B) soft, low melting, a good electrical conductor.C) hard, high melting, a good electrical conductor.D) hard, high melting, a poor electrical conductor.E) soft, high melting, a poor electrical conductor.
ANS: D PTS: 1 DIF: easy REF: 11.6OBJ: Relate the hardness and electrical conductivity of a solid to its structure.TOP: phases | solid KEY: properties of solidsMSC: general chemistry
99. Which of the following concerning the 2-D lattice provided below is/are correct?
1. One possible unit cell contains a single and a single .2. More than one unit cell which reproduces this lattice is possible.3. One possible unit cell contains four ’s and four ’s.
A) 1 only
Test Bank General Chemistry, 10th edition 28
B) 2 onlyC) 3 onlyD) 1 and 2E) 1, 2, and 3
ANS: D PTS: 1 DIF: moderate REF: 11.7OBJ: Define crystal lattice and unit cell of a crystal lattice. TOP: phases | solid
100. For a given pure metal which of the following cubic unit cells would result in the highest metal density?A) It depends on the identity of the metal.B) The density would be identical for all these cells if the edge length of each cell
were the same.C) A face-centered cubic cell.D) A simple cubic cell.E) A body-centered cubic cell.
ANS: C PTS: 1 DIF: moderate REF: 11.7OBJ: Define simple cubic unit cell, body-centered cubic unit cell, and face-centered cubic unit cell. TOP: phases | solidKEY: crystalline solids | cubic unit cell MSC: general chemistry
101. In any cubic lattice an atom lying at the corner of a unit cell is shared equally by how many unit cells?A) 1B) 16C) 2D) 4E) 8
ANS: E PTS: 1 DIF: easy REF: 11.7OBJ: Define simple cubic unit cell, body-centered cubic unit cell, and face-centered cubic unit cell. TOP: phases | solidKEY: crystalline solids | cubic unit cell MSC: general chemistry
102. The space-filling representation of a crystalline polonium provided below is an example of a _____ unit cell, which contains the equivalent of _____ atom(s) within a single unit cell.
Test Bank General Chemistry, 10th edition 29
A) simple cubic, 1 atomB) body centered cubic, 2 atomsC) face centered cubic, 4 atomsD) simple cubic, 8 atomsE) body centered cubic, 3 atoms
ANS: A PTS: 1 DIF: easy REF: 11.7OBJ: Define simple cubic unit cell, body-centered cubic unit cell, and face-centered cubic unit cell. TOP: phases | solid
103. The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. The unit cell contains a net:A) 2 anions and 3 cations.B) 2 anions and 2 cations.C) 5 anions and 3 cations.D) 3 anions and 4 cations.E) 5 anions and 6 cations.
ANS: A PTS: 1 DIF: easy REF: 11.7OBJ: Determine the number of atoms in a unit cell. (Example 11.9)TOP: phases | solid KEY: crystalline solids | cubic unit cellMSC: general chemistry
104. How many atoms are there in a cubic close-packed unit cell of aluminum?A) 4B) 6C) 1D) 8E) 2
ANS: A PTS: 1 DIF: easy REF: 11.8OBJ: Determine the number of atoms in a unit cell. (Example 11.9)TOP: phases | solidKEY: structures of crystalline solids | metallic solid MSC: general chemistry
105. How many atoms are there in a body-centered cubic unit cell of vanadium?A) 4B) 8C) 6D) 2E) 1
ANS: D PTS: 1 DIF: easy REF: 11.7OBJ: Determine the number of atoms in a unit cell. (Example 11.9)TOP: phases | solidKEY: structures of crystalline solids | metallic solid MSC: general chemistry
Test Bank General Chemistry, 10th edition 30
106. A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 196 pm and the density of the element is 1.55 g/cm3. How many atoms are there per unit cell?A) 4B) 6C) 8D) 1E) 2
ANS: A PTS: 1 DIF: moderate REF: 11.7OBJ: Determine the number of atoms in a unit cell. (Example 11.9)TOP: phases | solidKEY: structures of crystalline solids | metallic solid MSC: general chemistry
107. Which one of the following statements about solid Cu (face-centered cubic unit cell) is incorrect?A) It will conduct electricity.B) The length of a face diagonal is four times the Cu radius.C) The number of atoms surrounding each Cu atom is 12.D) The solid has a cubic closest-packed structure.E) There are two atoms per unit cell.
ANS: E PTS: 1 DIF: moderate REF: 11.8OBJ: Note the common structures (face-centered cubic and body-centered cubic) of metallic solids. TOP: phases | solidKEY: structures of crystalline solids | metallic solid MSC: general chemistry
108. Lithium chloride crystallizes in a face-centered cubic structure. The unit cell length is 5.14 10-8 cm. The chloride ions are touching each other along the face diagonal of the unit cell. The lithium ions fit into the holes between the chloride ions. How many chloride ions are there in this unit cell?A) 4B) 3C) 1D) 8E) 2
ANS: A PTS: 1 DIF: moderate REF: 11.8OBJ: Describe the three types of cubic structures of ionic solids.TOP: phases | solidKEY: structures of crystalline solids | ionic solid MSC: general chemistry
109. Assuming the following metals all have the same unit cell structure, which of the following would be expected to have the highest density: Sc, Ti, Mn, or Co?A) MnB) TiC) CoD) ScE) cannot be determined from the information given.
Test Bank General Chemistry, 10th edition 31
ANS: C PTS: 1 DIF: moderate REF: 11.9OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
110. The metal palladium crystallizes in a face-centered cubic lattice with an edge length of 388.8 pm. What is the density of palladium?A) 0.752 g/cm3
B) 3.01 g/cm3
C) 1.50 g/cm3
D) 6.01 g/cm3
E) 12.0 g/cm3
ANS: E PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
111. The metal gold, with an atomic radius of 144.2 pm, crystallizes in a face-centered cubic lattice. What is the density of gold?A) 9.65 g/cm3
B) 1.21 g/cm3
C) 4.82 g/cm3
D) 2.41 g/cm3
E) 19.3 g/cm3
ANS: E PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
112. A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 198 pm and the density of the element is 6.57 g/cm3. What is the identity of the metal?A) CuB) CaC) SrD) NiE) Yb
ANS: E PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)TOP: phases | solid KEY: structures of crystalline solidsMSC: general chemistry
Test Bank General Chemistry, 10th edition 32
113. Calcium crystallizes in a face-centered cubic lattice. The density of the element is 1.55 g/cm3. What is the volume of a single unit cell?
A) 1.72 10 22 cm3
B) 4.13 10 22 cm3
C) 1.07 10 25 cm3
D) 4.29 10 23 cm3
E) 1.03 10 22 cm3
ANS: A PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)TOP: phases | solid
114. Ytterbium crystallizes in a face-centered cubic lattice. The radius of ytterbium is 198 pm. What is the edge length of the unit cell?
A) 560 pmB) 396 pmC) 792 pmD) 420 pmE) 198 pm
ANS: A PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension given radius and unit cell. TOP: phases | solid
115. Lithium chloride crystallizes in a face-centered cubic structure. The unit cell length is 5.14 10-8 cm. The chloride ions are touching each other along the face diagonal of the unit cell. The lithium ions fit into the holes between the chloride ions. What is the mass of LiCl in a unit cell?A) 5.63 10-22 gB) 1.41 10-22 gC) 4.22 10-22 gD) 7.04 10-23 gE) 2.82 10-22 g
ANS: E PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
116. Lithium chloride crystallizes in a face-centered cubic structure. The unit cell length is 5.14 10-8 cm. The chloride ions are touching each other along the face diagonal of the unit cell. The lithium ions fit into the holes between the chloride ions. What is the density of the lithium chloride?A) 0.520 g/cm3
B) 2.82 g/cm3
C) 2.08 g/cm3
D) 3.11 g/cm3
E) 3.78 g/cm3
ANS: C PTS: 1 DIF: difficult REF: 11.9
Test Bank General Chemistry, 10th edition 33
OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
117. The metal iron crystallizes in a body-centered cubic lattice. If the density of iron is 7.87 g/cm3, what is the unit cell edge length?A) 287 pmB) 77.6 pmC) 75.0 pmD) 61.6 pmE) 228 pm
ANS: A PTS: 1 DIF: moderate REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
118. The metal barium crystallizes in a body-centered cubic lattice. If the radius of barium is 222 pm, what is the unit cell edge length?
A) 513 pmB) 444 pmC) 296 pmD) 222 pmE) 96.1 pm
ANS: A PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid
119. The metal cesium crystallizes in a body-centered cubic lattice. If the density of cesium is 1.88 g/cm3, what is the unit cell volume?A) 1.77 106 pm3
B) 2.35 104 pm3
C) 2.35 108 pm3
D) 1.17 108 pm3
E) 4.70 104 pm3
ANS: C PTS: 1 DIF: moderate REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
Test Bank General Chemistry, 10th edition 34
120. Sodium crystallizes in the body-centered cubic system. If the edge of the unit cell is 430 pm, what is the radius of a sodium atom in picometers?
A) 186 pmB) 744 pmC) 992 pmD) 859 pmE) 80.5 pm
ANS: A PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and edge-length. (Example 11.11)TOP: phases | solid
121. Copper crystallizes with a face-centered cubic unit cell. If the edge length of the unit cell is 362 pm, what is the radius of a copper atom in picometers?
A) 128 pmB) 512 pmC) 1020 pmD) 296 pmE) 45.3 pm
ANS: A PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and edge-length. (Example 11.11)TOP: phases | solid
122. What is the simplest formula of the compound represented by the unit cell provided below?
A) AB3
B) AB2
C) ABD) A2B4
E) A2B6
ANS: A PTS: 1 DIF: difficult REF: 11.9OBJ: Determine the number of atoms in a unit cell. (Example 11.9)TOP: phases | solid
Test Bank General Chemistry, 10th edition 35
123. A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 125 pm and the density of the element is 8.91 g/cm3. What is the volume of the unit cell?A) 8.18 106 pm3
B) 1.12 109 pm3
C) 4.42 107 pm3
D) 1.95 106 pm3
E) 3.27 107 pm3
ANS: C PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
124. A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 214 pm and the density of the element is 2.63 g/cm3. What is the molar volume of the metal?A) 98.9 cm3/molB) 24.7 cm3/molC) 86.6 cm3/molD) 33.4 cm3/molE) 0.380 cm3/mol
ANS: D PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
125. The metal cesium crystallizes in a body-centered cubic lattice. If the density of cesium is 1.88 g/cm3, what is the atomic volume of cesium?A) 1.60 104 pm3
B) 7.99 103 pm3
C) 3.99 107 pm3
D) 6.01 105 pm3
E) 7.98 107 pm3
ANS: E PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
126. The metal barium crystallizes in a body-centered cubic lattice. If the density of barium is 3.51 g/cm3, what is the atomic radius of barium?A) 15.1 pmB) 174 pmC) 42.5 pmD) 19.0 pmE) 219 pm
Test Bank General Chemistry, 10th edition 36
ANS: E PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
127. Lithium chloride crystallizes in a face-centered cubic structure. The unit cell length is 5.14 10-8 cm. The chloride ions are touching each other along the face diagonal of the unit cell. The lithium ions fit into the holes between the chloride ions. What is the radius of the chloride ion?A) 2.52 10-8 cmB) 1.82 10-8 cmC) 2.56 10-8 cmD) 1.45 10-8 cmE) 2.82 10-8 cm
ANS: B PTS: 1 DIF: difficult REF: 11.9OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11)TOP: phases | solid KEY: calculations with unit cell dimensionsMSC: general chemistry
128. Which of the following statements concerning the determination of crystal structure by x-ray diffraction is incorrect?A) X-rays are reflected from the repeating planes of an ordered crystal lattice.B) A diffraction pattern reveals the locations of the electrons in a crystal.C) Analysis of a diffraction pattern reveals the structure of a crystal.D) X-rays undergo constructive and destructive interference upon reflection in a
crystal lattice.E) A diffraction pattern from a crystal depends on the incident angle of the x-rays.
ANS: B PTS: 1 DIF: easy REF: 11.10OBJ: Note that diffraction of x rays from a crystal gives information about the positions of atoms in the crystal. TOP: phases | solid KEY: x-ray diffractionMSC: general chemistry
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