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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


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.


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


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


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


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


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


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.


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.


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


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



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


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


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


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


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.


3. The viscosity of a liquid is determined in part by the strength of intermolecular forces.


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


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


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


56. Which of the following pure substances has the highest normal boiling point?A) HIB) HClC) HFD) H2SE) HBr


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.


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


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


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


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


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


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


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


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)


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


87. Which of the following pure substances has the highest normal melting point?A) KFB) KIC) NaFD) NaClE) NaI


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


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


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


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.


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


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.


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


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


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


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


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


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?


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?


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


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


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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