Test Bank Chapter 11 Intermolecular Forces & Liquids

Chemistry: Molecular Nature of Matter, 8e (Jespersen)

Chapter 11 Intermolecular Attractions and the Properties of Liquids and Solids

1) The term "London forces" is a synonym for

A) ion-ion forces.

B) permanent dipole-permanent dipole interactions.

C) hydrogen bonding.

D) instantaneous dipole-instantaneous dipole interactions.

E) instantaneous dipole-induced dipole interactions.

Diff: 1

Section: 11.1

2) Which molecule is most polarizable and subject to significant instantaneous dipole-induced dipole forces?

A) H3C–Br

B) H3C–Cl

C) H3C–F

D) H3C–H

E) H3C–I

Diff: 1

Section: 11.1

3) Which molecule is most polarizable and subject to the greatest instantaneous dipole-induced dipole forces?

A) CH4

B) C2H6

C) C3H8

D) C4H10

E) C5H12

Diff: 1

Section: 11.1

4) For small molecules of comparable molecular weight, which one of the following choices lists the intermolecular forces in the order of increasing strength?

A) hydrogen bonds < dipole-dipole forces < London forces

B) dipole-dipole forces < hydrogen bonds < London forces

C) London forces < hydrogen bonds < dipole-dipole forces

D) hydrogen bonds < London forces < dipole-dipole forces

E) London forces < dipole-dipole forces < hydrogen bonds

Diff: 1

Section: 11.1

5) What compound will not exhibit hydrogen bonding in the liquid state?

A) CH3—CH2—Br

B) CH3—CH2—NH2

C) CH3—CH2—CH2—OH

D) CH3—NH—CH3

E) NH2—OH

Diff: 1

Section: 11.1

6) Which covalent compound will exhibit hydrogen bonding in the liquid state?

A) CH2F2

B) Cl2NH

C) H2PCl

D) HBr

E) NCl3

Diff: 1

Section: 11.1

7) Which covalent compound will exhibit hydrogen bonding in the liquid state?

A) CCl2F2

B) H2PCl

C) HCl

D) NH2OH

E) NF3

Diff: 1

Section: 11.1

8) Which covalent compound will exhibit hydrogen bonding in the liquid state?

A) PH3

B) H2

C) CH4

D) NH3

E) H2S

Diff: 1

Section: 11.1

9) Which compound will have the strongest intermolecular forces?

A) CH3—CH2—H

B) CH3—CH2—O—H

C) CH3—CH2—PH2

D) CH3—CH2—S—H

E) CH3—CH2—Se—H

Diff: 1

Section: 11.1

10) Which compound will have the weakest intermolecular forces?

A) CH3—CH2—H

B) CH3—CH2—O—H

C) CH3—CH2—PH2

D) CH3—CH2—S—H

E) CH3—CH2—Se—H

Diff: 1

Section: 11.1

11) The strongest intermolecular forces between molecules of NO are

A) covalent bonds.

B) dipole-dipole interactions.

C) ionic bonds.

D) hydrogen bonds.

E) London forces.

Diff: 1

Section: 11.1

12) Which compound is expected to exhibit hydrogen bonding?

A) CH3—CH2—H

B) CH3—CH2—O—H

C) CH3—CH2—PH2

D) CH3—CH2—S—H

E) CH3—CH2—Se—H

Diff: 1

Section: 11.1

13) At 1.0 atm pressure, ice (solid H2O) floats in water instead of sinking. The reason for this is

A) when water freezes, it expands instead of contracting.

B) the fusion process is endothermic, therefore the solid will float.

C) the triple point has a lower temperature than the freezing point for water.

D) the critical temperature has a higher temperature than the normal boiling point.

E) the triple point corresponds to a pressure below 1 standard atmosphere.

Diff: 1

Section: 11.1

14) The property that measures or describes the magnitude of resistance to flow in a liquid is called

A) London forces.

B) malleability.

C) surface tension.

D) vapor pressure.

E) viscosity.

Diff: 1

Section: 11.1

15) Which causes surface tension?

A) more molecules present on a surface than within a liquid

B) a liquid forming as much surface area as possible

C) surface molecules having fewer molecular neighbors than interior molecules

D) a higher viscosity within a liquid than at the surface of a liquid

E) the largest average size molecules moving toward the surface of a liquid

Diff: 1

Section: 11.2

16) The presence of which intermolecular force would lead to the highest viscosity within a liquid?

A) dipole-dipole

B) London

C) dispersion

D) Hydrogen bonding

E) induced dipole

Diff: 1

Section: 11.2

17) When a liquid undergoes a change of state to a gas, the process is called

A) condensation.

B) deposition.

C) fusion.

D) sublimation.

E) evaporation.

Diff: 1

Section: 11.2

18) When a solid undergoes a change of state to a gas, the process is called

A) condensation.

B) deposition.

C) fusion.

D) sublimation.

E) evaporation.

Diff: 1

Section: 11.2

19) When a gas undergoes a change of state to a liquid, the process is called

A) condensation.

B) deposition.

C) fusion.

D) sublimation.

E) evaporation.

Diff: 1

Section: 11.2

20) Which of the following is not a factor that directly affects the viscosity of a liquid?

A) length of the molecule

B) polarizability

C) density

D) branching of molecule

E) temperature

Diff: 1

Section: 11.2

21) Which of the following organic liquids would best demonstrate wetting on a clean glass surface?

A) carbon tetrachloride (CCl4)

B) octane (C8H18)

C) hexane (C6H14)

D) ethylene glycol (HO—CH2—CH2—OH)

E) heptane (C7H16)

Diff: 2

Section: 11.2

22) Which of the following organic liquids would have the strongest surface tension?

A) ethanol (CH3-CH2-OH)

B) octane (C8H18)

C) hexane (C6H14)

D) ethylene glycol (HO-CH2-CH2-OH)

E) heptanes (C7H16)

Diff: 2

Section: 11.2

23) A liquid in a covered container is in equilibrium with its vapor. If the cover is removed, what is the immediate result?

A) The average kinetic energy increases.

B) The evaporation rate decreases.

C) The evaporation rate increases.

D) The condensation rate decreases.

E) The condensation rate increases.

Diff: 2

Section: 11.2

24) Which of the following liquids, at the same temperature, has the lowest vapor pressure?

A) CH3—CH2—F

B) CH3—CH2—CH3

C) CH3—CH2—CH2—CH3

D) CH3—CH2—O—H

E) CH3—O—CH3

Diff: 1

Section: 11.4

25) Which of the following liquids, at the same temperature, has the lowest vapor pressure?

A) CH3—Br

B) CH3—Cl

C) CH3—F

D) CH3—H

E) CH3—I

Diff: 1

Section: 11.4

26) Which of the following liquids, at the same temperature, has the highest vapor pressure?

A) CH3—CH2—H

B) CH3—O—CH3

C) CH3—CH2—CH2—CH3

D) CH3—CH2—CH3

E) CH3—CH2—S—H

Diff: 1

Section: 11.4

27) Which of the following liquids, at the same temperature, has the highest vapor pressure?

A) CH3—Br

B) CH3—Cl

C) CH3—F

D) CH3—H

E) CH3—I

Diff: 1

Section: 11.4

28) Which of the following liquids, at the same temperature, has the highest vapor pressure?

A) CH3—Hg—CH3

B) CH3—O—CH3

C) CH3—S—CH3

D) CH3—Se—CH3

E) CH3—Te—CH3

Diff: 1

Section: 11.4

29) The vapor pressure of a liquid increases with increasing temperature. The temperature at which the vapor pressure is equal to the prevailing outside atmospheric pressure is

A) the boiling point.

B) the flash point.

C) the vaporization point.

D) 100 °C.

E) the normal boiling point.

Diff: 1

Section: 11.5

30) Which of the following substances should have the highest boiling point?

A) CCl4

B) Cl2

C) Kr

D) CH3Cl

E) N2

Diff: 1

Section: 11.5

31) Which of the following substances should have the highest boiling point?

A) CCl4

B) CH4

C) Kr

D) CH3Cl

E) KCl

Diff: 2

Section: 11.5

32) The temperature at which the vapor pressure is equal to 1 atm, 760 torr, or 101,325 Pa is defined as

A) the melting point.

B) the flash point.

C) the vaporization point.

D) 100°C.

E) the normal boiling point.

Diff: 1

Section: 11.5

33) Which compound should have the lowest boiling point?

A) CH3—Br

B) CH3—Cl

C) CH3—F

D) CH3—H

E) CH3—I

Diff: 1

Section: 11.5

34) Which compound should have the lowest boiling point?

A) CH3—Hg—CH3

B) CH3—O—CH3

C) CH3—S—CH3

D) CH3—Se—CH3

E) CH3—Te—CH3

Diff: 1

Section: 11.5

35) Which compound should have the highest boiling point?

A) CH3—Br

B) CH3—Cl

C) CH3—F

D) CH3—H

E) CH3—I

Diff: 1

Section: 11.5

36) Which compound should have the highest boiling point?

A) CH3—Hg—CH3

B) CH3—O—CH3

C) CH3—S—CH3

D) CH3—Se—CH3

E) CH3—Te—CH3

Diff: 1

Section: 11.5

37) Which factor affects the normal boiling point of a liquid?

A) atmospheric pressure

B) rate of condensation

C) rate of evaporation

D) strength of the intermolecular forces

E) rate of temperature increase

Diff: 1

Section: 11.5

38) Which of the following would be expected to have the highest vapor pressure at room temperature?

A) ethanol, boiling point = 78°C

B) methanol, boiling point = 65°C

C) water, boiling point = 100°C

D) acetone, boiling point = 56°C

E) The vapor pressure of each of the liquids at room temperature would be the same.

Diff: 1

Section: 11.5

39) Which of the following would be expected to have the lowest vapor pressure at room temperature?

A) dimethyl sulfoxide, boiling point = 189°C

B) 1-pentanol, boiling point = 137°C

C) diethyl ether, boiling point = 34.6°C

D) acetone, boiling point = 56°C

E) The vapor pressure of each of the liquids at room temperature would be the same.

Diff: 1

Section: 11.5

40) Given the following substances and their normal boiling points, in °C:

C: 43.8°C D: 93.7°C M: 56.7°C T: 83.5°C R: 63.6°C

Which ranking correctly lists some of these substances in order of decreasing vapor pressure at 20°C?

A) C > R > D

B) D > T > R

C) R > M > D

D) C > D > M

E) D > R > M

Diff: 1

Section: 11.5

41) Given the following substances and their normal boiling points, in °C:

C: 43.8°C D: 93.7°C M: 56.7°C T: 83.5°C R: 63.6°C

Which ranking correctly lists some of these substances in order of increasing vapor pressure at 20°C?

A) C < R < D

B) D < R < C

C) R < T < D

D) C < D < M

E) D < M < R

Diff: 1

Section: 11.5

42) Given the following substances and their normal boiling points, in °C:

C: 43.8°C D: 93.7°C M: 56.7°C T: 83.5°C R: 63.6°C

Which ranking correctly lists some of these liquids in order of decreasing intermolecular forces at 20°C?

A) C > R > D

B) D > C > R

C) R > T > D

D) C > D > M

E) D > R > C

Diff: 1

Section: 11.5

43) Given the following substances and their normal boiling points, in °C:

C: 43.8°C D: 93.7°C M: 56.7°C T: 83.5°C R: 63.6°C

Which ranking correctly lists some of these liquids in order of increasing intermolecular forces at 20°C?

A) C < R < D

B) D < T < R

C) R < T < C

D) C < D < M

E) D < R < M

Diff: 1

Section: 11.5

44) In order to boil water, we need to supply heat. This is in order to

A) decrease the kinetic energy of the molecules.

B) disrupt ionic interactions.

C) disrupt hydrogen bonding.

D) decrease the potential energy of the molecules.

E) All of the above

Diff: 1

Section: 11.5

45) Benzene, C6H8, has an enthalpy of fusion of 127.4 J g-1 and its melting point temperature is 5.53°C. How much heat is required to transform 80.0 g of solid benzene at 5.53°C into liquid benzene, also at 5.53°C?

A) 705 J

B) 10.2 kJ

C) 14.4 kJ

D) 19.3 kJ

E) 22.3 kJ

Diff: 1

Section: 11.6

46) p-Xylene, C8H10, has an enthalpy of fusion of 158.3 J g-1 and its melting point temperature is 13.2°C. How much heat is required to transform 115 g of solid p-xylene at 13.2°C into liquid p-xylene, also at 13.2°C?

A) 1.52 kJ

B) 2.09 kJ

C) 18.2 kJ

D) 32.9 kJ

E) 41.8 kJ

Diff: 1

Section: 11.6

47) Benzophenone, C13H10O, has a heat of fusion of 98.45 J g-1 and its melting point temperature is 47.85°C. How much heat is required to transform 126 g of solid benzophenone at 47.85°C into liquid benzophenone, also at 47.85°C?

A) 4.71 kJ

B) 6.03 kJ

C) 12.4 kJ

D) 31.6 kJ

E) 40.4 kJ

Diff: 1

Section: 11.6

48) Substance A has a normal melting point of –25.0°C, a heat of fusion of 1200 J g-1; specific heats for the solid and the liquid are 3.00 and 6.20 J g-1 °C -1, respectively. How much heat will be required to change 150 grams of substance A from a solid at –40.0°C to a liquid at +70.0°C?

A) 1.52 × 105 J

B) 1.81 × 105 J

C) 2.21 × 103 J

D) 2.29 × 105 J

E) 2.75 × 105 J

Diff: 1

Section: 11.6

49) A solid with a molecular weight of 174.0 g/mol is at its melting point. If this solid requires 21.3 kJ of heat to melt 34.0 g, what is the molar heat of fusion of this solid (in kJ/mol)

A) 3.60 × 10-3 kJ/mol

B) 4.16 kJ/mol

C) 2.40 × 10-1 kJ/mol

D) 109 kJ/mol

E) 1.26 × 105 kJ/mol

Diff: 2

Section: 11.6

50) A solid with a molecular weight of 148.0 g/mol is already at its melting point. If 18.6 g of this solid requires 4.838 kJ of heat to melt it, what is the molar heat of fusion (in kJ/mol)?

A) 1.33 × 104 kJ/mol

B) 0.608 kJ/mol

C) 569 kJ/mol

D) 0.0260 kJ/mol

E) 38.4 kJ/mol

Diff: 2

Section: 11.6

51) 22.4 g of a solid with a molecular weight of 148.0 g/mol is at its melting point. If this solid requires 5.358 kJ of heat to melt it, what is the molar heat of fusion, in kJ/mol, for this solid?

A) 1.23 × 104 kJ/mol

B) 0.811 kJ/mol

C) 35.4 kJ/mol

D) 0.0282 kJ/mol

E) 1.78 × 104 kJ/mol

Diff: 2

Section: 11.6

52) Given the phase changes: condensation, freezing, fusion, sublimation, and vaporization. Which of these phase changes is/are endothermic?

A) condensation and freezing only

B) fusion only

C) fusion and vaporization only

D) fusion and sublimation only

E) sublimation, fusion, and vaporization only

Diff: 1

Section: 11.6

53) Supercooling is defined as

A) the extremely rapid cooling of a vapor to form a liquid.

B) the use of extremely cold refrigerants to achieve smaller crystal size when liquids are frozen.

C) the extremely rapid cooling of a liquid to form a softer crystalline solid.

D) the cooling of a liquid to a temperature below its melting point without solidification.

E) the cooling of a substance to absolute zero.

Diff: 1

Section: 11.6

54) Which of the following compounds should have the largest value for heat of vaporization (ΔHvap)?

A) CH3—Br

B) CH3—Cl

C) CH3—F

D) CH3—H

E) CH3—I

Diff: 1

Section: 11.6

55) Which of the following compounds should have the largest value for heat of fusion (ΔHfus)?

A) NH3

B) CH3—Cl

C) N2

D) HCl

Diff: 1

Section: 11.6

56) Dioxane, C4H8O2, has an enthalpy of fusion of 145.8 J g-1 and its melting point temperature is 11.0°C. How much heat is required to transform 142 g of solid dioxane, into liquid dioxane, at 11.0°C?

A) 1.60 kJ

B) 2.59 kJ

C) 20.7 kJ

D) 22.8 kJ

E) 40.3 kJ

Diff: 2

Section: 11.6

57) A substance, B, has a normal boiling point of +89.3°C, and a heat of vaporization of 260 J/g. How much heat is required to change 150 grams of B from a liquid at 89.3°C to a gas at 89.3°C?

A) 5.2 × 102 J

B) 3.9 × 104 J

C) 4.4 × 105 J

D) 1.1 × 105 J

E) 1.6 × 105 J

Diff: 2

Section: 11.6

58) Evaporation

A) is an endothermic process.

B) is an exothermic process.

C) involves breaking intermolecular forces.

D) decreases the temperature on the surface where it occurs.

E) A, C, and D

Diff: 2

Section: 11.6

59) An isobar is a line of constant pressure which runs parallel to the temperature axis on the phase diagram for a substance. As we vary temperature along an isobar that lies below the triple point, which process would never be observed?

A) decrease in volume

B) deposition

C) expansion

D) fusion

E) sublimation

Diff: 2

Section: 11.7

60) The triple point of a substance is the temperature and pressure at which

A) all three physical states cease to exist.

B) sublimation, fusion, and condensation are taking place simultaneously.

C) the solid will always float on the liquid for all substances.

D) the vapor pressure of the liquid is higher than the vapor pressure of the solid.

E) the vapor pressure of the solid is higher than the vapor pressure of the liquid.

Diff: 1

Section: 11.7

The following questions refer to the phase diagram below. Gas, liquid, and solid phases are all present, but not labeled.

61) At the temperature and pressure of point d, which statement below is true?

A) The substance will sublime.

B) There will be an equilibrium between the solid phase and the gaseous phase.

C) Vaporization and deposition will take place simultaneously.

D) Condensation and evaporation will take place simultaneously.

E) The substance will be a supercritical fluid.

Diff: 1

Section: 11.7

62) At the temperature and pressure of point e, which statement below is true?

A) The substance will sublime.

B) There will be an equilibrium between the solid phase and the gaseous phase.

C) Vaporization and deposition will take place simultaneously.

D) Melting and freezing will take place simultaneously.

E) Melting and vaporization will take place simultaneously.

Diff: 1

Section: 11.7

63) Starting at the temperature and pressure of b, if the temperature is increased at constant pressure, ultimately

A) the substance will sublime.

B) the substance will undergo fusion.

C) the substance will undergo deposition.

D) the substance will freeze.

E) the substance will be a supercritical fluid.

Diff: 1

Section: 11.7

64) Starting at the temperature and pressure of c, if the pressure is increased at constant temperature, ultimately

A) the substance will sublime.

B) the substance will undergo fusion.

C) the substance will undergo deposition.

D) the substance will freeze.

E) the substance will undergo condensation.

Diff: 1

Section: 11.7

The following questions refer to the phase diagram below.

65) What phase should this substance exist as, at a pressure of 1500 torr and a temperature of -20°C?

A) solid

B) liquid

C) gas

D) supercritical fluid

E) unable to tell

Diff: 1

Section: 11.7

66) What phase should this substance exist as, at a pressure of 2000 torr and a temperature of 20°C?

A) solid

B) liquid

C) gas

D) supercritical fluid

E) unable to tell

Diff: 1

Section: 11.7

67) What phase should this substance exist as, at a pressure of 2000 torr and a temperature of -70°C?

A) solid

B) liquid

C) gas

D) supercritical fluid

E) unable to tell

Diff: 1

Section: 11.7

68) Which of the following values of temperature and pressure most closely correspond to the triple point of this substance?

A) -21°C and 1000 torr

B) 0°C and 1000 torr.

C) -57°C and 740 torr

D) -50°C and 4500 torr

E) 0°C and 1760 torr

Diff: 1

Section: 11.7

69) Which compound cannot be liquefied by compression, at a temperature of 25.0°C?

A) C2H4, critical point: 9.9°C, 50.5 atm

B) CH3Cl, critical point: 144.0°C, 66.0 atm

C) C2H2, critical point: 35.5°C, 61.6 atm

D) C2H6, critical point: 32.2°C, 48.2 atm

E) SO2, critical point: 158.0°C, 78.0 atm

Diff: 1

Section: 11.7

70) The critical temperature of a substance is

A) always higher than the triple point temperature.

B) the temperature below which it cannot exist in the liquid state.

C) the temperature which is always higher than the Kelvin point.

D) the temperature below which it cannot be liquefied by increasing the pressure.

E) the temperature below which it cannot be supercooled.

Diff: 2

Section: 11.7

71) Which compound cannot be liquefied by compression, at a temperature of 25.0°C?

A) CH3Cl, critical point: 144.0°C, 66.0 atm

B) C2H2, critical point: 35.5°C, 61.6 atm

C) C2H6, critical point: 32.2°C, 48.2 atm

D) SiF4, critical point: -14.1°C, 36.7 atm

E) SO2, critical point: 158.0°C, 78.0 atm

Diff: 2

Section: 11.7

72) The normal boiling point of acetic acid, HC2H3O2, is 117.9°C, and its heat of vaporization is 39,690 J/mol. What is its vapor pressure at 100.0°C?

A) 423.2 torr

B) 479.7 torr

C) 586.6 torr

D) 616.2 torr

E) 694.4 torr

Diff: 2

Section: 11.9

73) Find the boiling temperature at 760 torr of an isomer of octane, C8H18, if its heat of vaporization is 38,210 J mol-1 and its vapor pressure at 110.0°C is 638.43 torr.

A) 111.52°C

B) 113.22°C

C) 115.00°C

D) 115.65°C

E) 118.30°C

Diff: 2

Section: 11.9

74) Hexane (C6H14) boils at 68.73°C at 760 torr. The heat of vaporization for hexane is

28.9 kJ/mol. What is the vapor pressure of hexane at 30°C?

A) 207 torr

B) 546 torr

C) 2786 torr

D) 759 torr

E) 2396 torr

Diff: 2

Section: 11.9

75) The normal boiling point of 2,3,4-trimethypentane, C8H18, is 113.47°C, and its heat of vaporization is 37,600 J mol-1. What is its vapor pressure at 105.5°C?

A) 479.7 torr

B) 586.6 torr

C) 594.1 torr

D) 616.2 torr

E) 694.4 torr

Diff: 2

Section: 11.9

76) Portions of how many different atoms are in one simple cubic unit cell?

A) 2

B) 3

C) 4

D) 6

E) 8

Diff: 2

Section: 11.10

77) Which type of lattice structures have lattice points on all of the faces?

A) simple cubic structures

B) base-centered structures

C) face-centered structures

D) body-centered structures

E) both body-centered and base-centered structures

Diff: 1

Section: 11.10

78) Which type of unit cell has lattice points at each corner, and one in the center of the cell?

A) face-centered cubic

B) simple cubic

C) body-centered cubic

D) edge-centered cubic

E) hexagonal-centered cubic

Diff: 1

Section: 11.10

79) In a one-element solid with a face-centered cubic structure, how many atoms are in one unit cell?

A) 1

B) 2

C) 3

D) 4

E) 5

Diff: 2

Section: 11.10

80) In a one-element solid with a simple cubic crystal structure, how many atoms are in one unit cell?

A) 1

B) 2

C) 3

D) 4

E) 5

Diff: 2

Section: 11.10

81) A new compound, boganium sulfide, has been discovered. X-ray crystallographic studies reveal that it has a cubic unit cell with a sulfide ion at each of the corner lattice points, a sulfide ion at the geometric center of the unit cell, and a boganium ion in the center of each of the cube faces in the unit cell. Based on this structure, the formula for the compound should be

A) Bo3S

B) Bo3S2

C) BoS

D) Bo2S3

E) BoS3

Diff: 2

Section: 11.10

82) What type of crystal lattice is found in a sample of table salt, NaCl?

A) simple cubic

B) base-centered cubic

C) body-centered cubic

D) face-centered cubic

E) orthorhombic-centered cubic

Diff: 2

Section: 11.10

83) How many atoms are contained in one unit cell of metallic tungsten, if it forms a face-centered cubic unit cell?

A) 2

B) 4

C) 8

D) 9

E) 14

Diff: 2

Section: 11.10

84) How many atoms are contained in one unit cell of metallic lanthanum, if it forms a body-centered cubic unit cell?

A) 2

B) 4

C) 8

D) 9

E) 14

Diff: 2

Section: 11.10

85) How many atoms are contained in one unit cell of metallic polonium, if it forms a simple cubic unit cell?

A) 1

B) 2

C) 4

D) 8

E) 14

Diff: 2

Section: 11.10

86) Crystals tend to have flat surfaces of particles that meet at angles characteristic of the substance. The particles may be

A) atoms only.

B) molecules or atoms, only.

C) atoms or ions, only.

D) molecules or ions, only.

E) molecules, atoms or ions.

Diff: 2

Section: 11.10

87) A new compound, voronium oxide, has been discovered. X-ray crystallographic studies reveal that it has a cubic unit cell with a voronium ion at each of the corner lattice points and an oxide ion in the geometric center of the unit cell. Based on this structure, the formula for the compound should be

A) Vr8O

B) Vr4O

C) Vr2O

D) VrO

E) VrO2

Diff: 2

Section: 11.10

88) A new compound, vitellium oxide, has been discovered. X-ray crystallographic studies reveal that it has a cubic unit cell with a vitellium ion at each of the corner lattice points, a vitellium ion at the geometric center of the unit cell, and an oxide ion in the center of each of the cube faces in the unit cell. Based on this structure, the correct formula should be

A) Vi3O

B) Vi3O2

C) ViO

D) Vi2O3

E) ViO3

Diff: 2

Section: 11.10

89) A unit cell of sodium chloride (face-centered cubic) consists of sodium and chloride ions. How many sodium ions are within this unit cell?

A) 1

B) 2

C) 3

D) 4

E) 8

Diff: 2

Section: 11.10

90) A unit cell of sodium chloride (face-centered cubic) consists of sodium and chloride ions. How many chloride ions are within this unit cell?

A) 1

B) 2

C) 3

D) 4

E) 8

Diff: 2

Section: 11.10

91) A unit cell of sodium chloride (face-centered cubic) consists of sodium and chloride ions. How many chloride ions are present in entirety within just one sodium chloride unit cell?

A) 0

B) 1

C) 2

D) 3

E) 4

Diff: 2

Section: 11.10

92) A unit cell of sodium chloride (face-centered cubic) consists of sodium and chloride ions. How many sodium ions are present in entirety within just one sodium chloride unit cell?

A) 0

B) 1

C) 2

D) 3

E) 4

Diff: 2

Section: 11.10

93) What lies in the geometric center of a unit cell of sodium chloride (face-centered cubic)?

A) a sodium ion

B) a chloride ion

C) a sodium atom

D) a chlorine atom

E) No atoms or ions lie in the geometric center of this unit cell,

Diff: 2

Section: 11.10

94) The unit cell below is best described as what type of crystal structure?

A) Body-centered cubic

B) Simple cubic

C) Trigonal

D) Face-centered cubic

E) Octahedral

Diff: 2

Section: 11.10

95) The unit cell below is best described as what type of crystal structure?

A) Body-centered cubic

B) Simple cubic

C) Trigonal

D) Face-centered cubic

E) Octahedral

Diff: 2

Section: 11.10

96) The unit cell below is best described as what type of crystal structure?

A) Body-centered cubic

B) Simple cubic

C) Trigonal

D) Face-centered cubic

E) Octahedral

Diff: 2

Section: 11.10

97) A technique used for determining the structure of a crystalline substance is

A) magnetic resonance imaging (MRI).

B) microwave spectroscopy.

C) infrared spectroscopy.

D) ultraviolet laser scattering.

E) x-ray diffraction.

Diff: 2

Section: 11.11

98) One of the solid forms of iron, called α-iron, crystallizes in a body-centered cubic lattice. If atomic planes of this form of iron are separated by 143.3 pm, at what angle would you find the first-order (n = 1) diffraction of 0.209 nm X-rays from these planes?

A) 43.2°

B) 21.4°

C) 23.4°

D) 0.817°

E) 46.8°

Diff: 2

Section: 11.11

99) X-ray radiation at a wavelength of 1.542 × 10-10 m is used to irradiate a metallic crystal. The X-rays are being reflected at an angle of 12.73°. If this reflection is a first order reflection

(n = 1), what is the distance between the planes of atoms in this metallic crystal?

A) 3.5 × 10-10 m

B) 9.5 × 10-10 m

C) 1.4 × 10-9 m

D) 4.7 × 10-10 m

E) 7.0 × 10-10 m

Diff: 2

Section: 11.11

100) X-ray diffraction measurements revealed that Ag crystallizes in a face-centered cubic lattice in which the unit cell edge length is 408.6 picometers. Calculate the atomic radius of the Ag atoms in this crystal, based on the usual assumption that the atoms are tightly packed in the unit cell.

A) 102.2 pm

B) 144.5 pm

C) 192.6 pm

D) 204.3 pm

E) 288.9 pm

Diff: 2

Section: 11.11

101) X-ray diffraction measurements revealed that α-Fe crystallizes in a face-centered cubic lattice in which the unit cell edge length is 286.6 picometers. Calculate the atomic radius of the Fe atoms in this crystal, based on the assumption that the atoms are tightly packed in the unit cell.

Hint: Find the length of the cell face diagonal using the Pythagorean theorem.

A) 71.7 pm

B) 101.3 pm

C) 124.1 pm

D) 143.3 pm

E) 248.2 pm

Diff: 3

Section: 11.11

102) X-ray diffraction measurements revealed that Cu crystallizes in a face-centered cubic lattice in which the unit cell edge length is 361.5 picometers. Calculate the atomic radius of the Cu atoms in this crystal, based on the assumption that the atoms are tightly packed in the unit cell.

Hint: Find the length of the cell face diagonal using the Pythagorean theorem.

A) 90.4 pm

B) 127.8 pm

C) 156.5 pm

D) 170.4 pm

E) 180.8 pm

Diff: 3

Section: 11.11

103) X-ray diffraction measurements revealed that Ni crystallizes in a face-centered cubic lattice in which the unit cell edge length is 352.4 picometers.Calculate the atomic radius of the Ni atoms in this crystal, based on the assumption that the atoms are tightly packed in the unit cell.

Hint: Find the length of the cell face diagonal using the Pythagorean theorem.

A) 88.1 pm

B) 124.6 pm

C) 152.6 pm

D) 166.1 pm

E) 176.2 pm

Diff: 3

Section: 11.11

104) X-ray diffraction measurements on a newly discovered crystalline form of element X revealed that X crystallizes in a body-centered cubic lattice in which the unit cell edge length is 304.6 picometers. Calculate the atomic radius of the X atoms in this crystal, based on the assumption that the atoms are tightly packed in the unit cell.

Hint: Find the length of the cell body diagonal using the Pythagorean theorem.

A) 76.2 pm

B) 107.7 pm

C) 131.9 pm

D) 175.9 pm

E) 215.4 pm

Diff: 3

Section: 11.11

105) X-ray diffraction measurements on a newly discovered crystalline form of Eu revealed that Eu crystallizes in a body-centered cubic lattice in which the unit cell edge length is 458.3 picometers. Calculate the atomic radius of the Eu atoms in this crystal, based on the assumption that the atoms are tightly packed in the unit cell.

Hint: Find the length of the cell body diagonal using the Pythagorean theorem.

A) 114.6 pm

B) 162.0 pm

C) 198.4 pm

D) 229.2 pm

E) 264.6 pm

Diff: 3

Section: 11.11

106) X-ray diffraction measurements on a newly discovered crystalline form of La

revealed that La crystallizes in a body-centered cubic lattice in which the unit cell edge length is 426.3 picometers. Calculate the atomic radius of the La atoms in this crystal, based on the assumption that the atoms are tightly packed in the unit cell.

Hint: Find the length of the cell body diagonal using the Pythagorean theorem.

A) 107 pm

B) 151 pm

C) 184.6 pm

D) 213 pm

E) 246 pm

Diff: 3

Section: 11.11

107) Gold crystallizes in a face-centered cubic lattice. How many unit cells are there in a gold sample whose mass is 1.50 grams? The atomic weight of gold is 196.97 g mol-1.

Hint: Use dimensional analysis and the number of atoms per unit cell.

A) 1.15 × 1021 unit cells

B) 2.29 × 1021 unit cells

C) 3.28 × 1020 unit cells

D) 4.58 × 1021 unit cells

E) 9.17 × 1021 unit cells

Diff: 3

Section: 11.11

108) Iron crystallizes in a body-centered cubic lattice. How many unit cells are in an iron sample whose mass is 1.50 grams? The molar mass of iron is 55.85 g mol-1.

Hint: Use dimensional analysis and the number of atoms per unit cell.

A) 1.80 × 1021 unit cells

B) 3.23 × 1022 unit cells

C) 4.04 × 1021 unit cells

D) 8.09 × 1021 unit cells

E) 1.62 × 1022 unit cells

Diff: 3

Section: 11.11

109) What is the mass of a sample of iron that has 5.00 × 1022 unit cells, if the iron crystallizes in a body-centered cubic lattice? The molar mass of iron is 55.85 g mol-1.

Hint: Use dimensional analysis and the number of atoms per unit cell.

A) 4.63 g

B) 9.27 g

C) 10.5 g

D) 2.32 g

E) 6.43 g

Diff: 3

Section: 11.11

110) What is the mass of a sample of silver that has 5.00 × 1022 unit cells, if the silver crystallizes in a face-centered cubic lattice? The molar mass of silver is 107.87 g mol-1

Hint: Use dimensional analysis and the number of atoms per unit cell.

A) 8.96 g

B) 14.2 g

C) 35.8 g

D) 71.6 g

E) 128.8 g

Diff: 3

Section: 11.11

111) Which set of properties below best describes solid ionic crystalline substances?

A) broad range of melting points, soft to hard, conductors in liquid and solid states

B) high melting points, brittle, nonconductors

C) high melting points, hard, not brittle, nonconductors

D) low melting points, soft, nonconductors

E) low melting points, soft, conductors in liquid and solid states

Diff: 1

Section: 11.12

112) Which set of properties below best describes metallic substances?

A) broad range of melting points, soft to hard, conductors in liquid and solid states

B) high melting points, brittle, nonconductors

C) high melting points, hard, not brittle, nonconductors

D) low melting points, soft, nonconductors

E) low melting points, soft, conductors in liquid and solid states

Diff: 1

Section: 11.12

113) Which set of properties below best describes molecular crystalline substances?

A) broad range of melting points, soft to hard, conductors in liquid and solid states

B) high melting points, brittle, nonconductors

C) high melting points, hard, not brittle, nonconductors

D) low melting points, soft, nonconductors

E) low melting points, soft, conductors in liquid and solid states

Diff: 1

Section: 11.12

114) Paradichlorobenzene is a white crystalline solid which is very soft, has a low melting point, and does not conduct electricity. Which category of substance does it most likely fit under?

A) ionic

B) molecular

C) metallic

D) covalent (network)

E) amorphous

Diff: 1

Section: 11.12

115) 1,3,6,8-Tetramethylnaphthlene is a white crystalline solid which is very soft, has a low melting point, and is a nonconductor of electricity. Which category of substance does it most likely fit under?

A) ionic

B) molecular

C) metallic

D) covalent (network)

E) amorphous

Diff: 1

Section: 11.12

116) Which one of the following substances is most likely composed of ions rather than distinct formula units, when it is in the solid state?

A) Al2O3, m.p. 2000°C, hard substance

B) CrO3, m.p. 196°C, soft substance

C) Mn2O7, m.p. 5.9°C, soft in solid state

D) OsO4, m.p. 40°C, soft substance

E) SeO3, m.p. 118°C, relatively soft

Diff: 1

Section: 11.12

117) Which one of the following substances is most likely composed of ions rather than distinct formula units, when it is in the solid state?

A) CaCl2, m.p. +772°C

B) SnCl4, m.p. -33°C

C) SbCl5, m.p. +2.8°C

D) TiCl4, m.p. -25°C

E) VCl4, m.p. -28°C

Diff: 1

Section: 11.12

118) A particular solid, crystalline substance has a high melting point and is very hard. It is a non-conductor of electricity, even in the molten state. Most likely, what type of solid is this substance?

A) an ionic crystal

B) an amorphous crystal

C) a molecular crystal

D) a covalent crystal

E) a metallic crystal

Diff: 1

Section: 11.12

119) Silicon carbide, which has the empirical formula SiC, melts at 2830°C and is nearly as hard as diamond. Which category of substance does silicon carbide most likely fit into?

A) ionic

B) molecular

C) metallic

D) covalent

E) amorphous

Diff: 1

Section: 11.12

120) Boron nitride has the empirical formula BN, melts at 2967°C and is nearly as hard as diamond. Which category of substance does boron nitride most likely fit into?

A) ionic

B) molecular

C) metallic

D) covalent

E) amorphous

Diff: 1

Section: 11.12

121) An unknown solid is soft and lustrous. It has a low melting point and conducts electricity well as a solid or liquid. What kind of crystal best describes this solid?

A) ionic

B) molecular

C) metallic

D) covalent

E) amorphous

Diff: 1

Section: 11.12

122) An unknown solid is soft and brittle with a low melting point. It does not conduct electricity in either the solid or liquid phase. What kind of crystal best describes this solid?

A) ionic

B) molecular

C) metallic

D) covalent

E) amorphous

Diff: 1

Section: 11.12

123) An unknown solid is hard and brittle with a high melting point. It does not conduct electricity as a solid, but does as a liquid. What kind of crystal best describes this solid?

A) ionic

B) molecular

C) metallic

D) covalent

E) amorphous

Diff: 1

Section: 11.12

124) An unknown solid is very hard with a very high melting point. It does not conduct electricity in either the solid or liquid phase. What kind of crystal best describes this solid?

A) ionic

B) molecular

C) metallic

D) covalent

E) amorphous

Diff: 1

Section: 11.12

125) Arrange these compounds in order of increasing intermolecular forces:

CCl4, GeCl4, SiCl4, SnCl4.

Diff: 1

Section: 11.1

126) Arrange these compounds in order of increasing intermolecular forces:

CBr4, CCl4, CF4, CH4, CI4.

Diff: 1

Section: 11.1

127) The ease with which the electron cloud of an atom or molecule is distorted is called the ________ of the atom or molecule.

Diff: 1

Section: 11.1

128) Arrange these compounds in order of increasing vapor pressure at 20°C:

CCl4, GeCl4, SiCl4, SnCl4.

Diff: 1

Section: 11.1

129) What are the characteristics that distinguish solids, liquids, and gases?

A complete answer will include a discussion of intermolecular forces and retention of shape and volume.

Diff: 1

Section: 11.1

130) Describe the essential features of a hydrogen bond.

Diff: 1

Section: 11.1

131) Will a nonpolar molecule will have the strongest intermolecular interaction with another nonpolar molecule, a polar molecule, or an ion in solution? Explain.

Diff: 1

Section: 11.1

132) What other molecular factors determine the viscosity of a liquid?

Diff: 1

Section: 11.1

133) Helium atoms do not combine to make diatomic helium molecules (He2), but He atoms do have a weak ________ intermolecular attraction to each other.

Diff: 1

Section: 11.1

134) Arrange the following compounds in order of increasing viscosity: methylene chloride (CH2Cl2); glycerin (C3H5(OH)3); 1,1-ethandiol (C2H4(OH)2); and acetone (C3H6O). Explain your reasoning.

Diff: 1

Section: 11.1

135) A low heat of vaporization indicates that a substance has ________ intermolecular forces in the liquid form.

Diff: 2

Section: 11.2

136) Which property of water allows some bugs to be able to walk on the surface of water?

Diff: 2

Section: 11.2

137) A liquid will evaporate at a given temperature until ________ is reached.

Diff: 1

Section: 11.2

138) Given this set of phase changes: condensation, freezing, fusion, sublimation, vaporization, which of these phase changes is/are exothermic?

Diff: 1

Section: 11.3

139) A high vapor pressure indicates that the substance has ________ intermolecular forces in the liquid form.

Diff: 2

Section: 11.4

140) Arrange these compounds in order of increasing vapor pressure at 20 °C:

CBr4, CCl4, CF4, CH4, CI4.

Diff: 1

Section: 11.4

141) A substance with a high boiling point has ________ intermolecular forces in the liquid form.

Diff: 2

Section: 11.5

142) The heating of a liquid above its boiling point temperature without boiling occurring is called ________.

Diff: 1

Section: 11.6

143) The heat capacity of liquid water is 4.18 J g-1 °C-1 and its heat of vaporization is 40.7 kJ/mol. From this information, ________ kJ of heat must be provided to convert 1.50 g of liquid water at 57°C into 1.50 g of steam at 100°C.

Diff: 2

Section: 11.6

144) Substances with higher vapor pressures at room temperature will have a ________ boiling point than substances with lower vapor pressures.

Diff: 1

Section: 11.7

145) Which of the following substances has the lowest boiling point?

N2, CCl4, CH3Cl, Cl2, H2O

Diff: 2

Section: 11.7

146) A solid chemical substance whose triple point pressure is 4.60 atmospheres will normally ________ when it is heated to a sufficiently high temperature in the open laboratory.

Diff: 1

Section: 11.7

The following questions refer to the basic phase diagram below with gas, liquid, and solid phases present and labeled.

147) If the substance starts at a pressure of 330 torr and -20°C and is heated at constant pressure to 20°C, what phase transition will occur?

Diff: 1

Section: 11.7

148) If the substance starts at a pressure of 500 torr and 105°C and is cooled to 50°C, what phase transition will occur?

Diff: 1

Section: 11.7

149) What phase of this substance exists at 760 torr and 50°C?

Diff: 1

Section: 11.7

150) What phase of this substance exists at 2.15 torr and 80°C?

Diff: 1

Section: 11.7

151) The triple point of this substance is at ________ atm and ________ °C.

Diff: 1

Section: 11.7

152) Above ________ °C, it is not possible for a liquid phase of this substance to exist.

Diff: 1

Section: 11.7

153) A liquid which is kept in a pressure container at a temperature above its critical temperature is called a ________.

Diff: 1

Section: 11.7

154) The pressure below which the liquid state of matter does not exist regardless of the temperature is called ________.

Diff: 1

Section: 11.7

155) The temperature above which only a solid state and a non-solid exists for a substance is called the ________.

Diff: 1

Section: 11.7

The following questions refer to the diagram below.

Pressure/atm

156) At what temperatures do the triple point and critical point occur?

Diff: 1

Section: 11.7

157) At what temperature and pressure will the species stop subliming (going from a solid to a gas)?

Diff: 1

Section: 11.7

158) How does the boiling point of this substance vary as the pressure on this substance increases?

Diff: 1

Section: 11.7

159) Does the curvature of the lines on this phase diagram look similar to those on the phase diagram of water? Why or why not?

Diff: 2

Section: 11.7

160) At what temperatures do the normal boiling and freezing points occur for this substance?

Diff: 2

Section: 11.7

161) Solid carbon dioxide never forms a liquid at a pressure of one atmosphere, instead, it sublimes when left open to the atmosphere. Why?

Diff: 2

Section: 11.7

162) Using Le Châtelier's Principle and what you know about phase transitions, explain how a person coming out of a swimming pool in Arizona on a 90°F day is more likely to become cold than someone getting out of a swimming pool in Florida on a 90°F day.

Diff: 2

Section: 11.8

163) Determine the shift in equilibrium that would result if 100 kJ of energy were added to water freezing at 0°C to form ice (H2O(s) ⇆ H2O(l)).

Diff: 1

Section: 11.8

164) Determine the shift in equilibrium that would result if 100 kJ of energy were removed from a system in which dry ice and CO2 gas were in equilibrium at the freezing point.

Diff: 1

Section: 11.8

165) Determine the shift in equilibrium that would result if 100 kJ of energy were added to ice melting at 0°C to form water (H2O(s) ⇆ H2O(l)).

Diff: 1

Section: 11.8

166) The vapor pressure of ethanol is 400 mmHg at 63.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is the vapor pressure of ethanol at 34.9°C?

Diff: 2

Section: 11.9

167) The molar enthalpy of vaporization of carbon disulfide is 26.74 kJ/mol, and its normal boiling point is 46°C. What is the vapor pressure of CS2 at 0°C?

Diff: 2

Section: 11.9

168) Tungsten metal (W) exists as a body-centered cubic structure. How many tungsten atoms are within a unit cell of tungsten metal?

Diff: 2

Section: 11.10

169) The atomic planes in a graphite crystal are separated by 335 pm. At what angle would you find the second-order (n = 2) diffraction of 0.154 nm X-rays from a graphite crystal?

Diff: 2

Section: 11.11

170) Describe the difference between molecular crystals and covalent crystals, in terms of types of bonding and physical properties.

Diff: 2

Section: 11.12

171) Osmium tetroxide, OsO4, forms a crystal that melts at 40°C. The liquid formed from this melting does not conduct electricity. What would be the best classification of this type of crystal?

Diff: 1

Section: 11.12

172) Boron nitride, BN3, melts at approximately 3000°C under high pressure. The material is almost as hard as diamond. What kind of crystal is boron nitride?

Diff: 1

Section: 11.12

173) Crystals of elemental sulfur are easily crushed, and melt at 113°C. Liquid sulfur does not conduct electricity. What kind of crystal is elemental sulfur?

Diff: 1

Section: 11.12

174) An unknown solid is hard, but malleable and melts at 1700°C. The liquid form conducts electricity. The solid form also conducts electricity. What kind of crystal is this?

Diff: 1

Section: 11.12

175) An unknown solid is hard, but brittle and melts at 3500°C. The liquid form of the unknown conducts electricity, but the solid form does not. What kind of crystal is the unknown?

Diff: 1

Section: 11.12

176) Above a substance's critical point, its gas phase becomes like a liquid and the liquid becomes like a gas.

Diff: 1

Section: 11.1

177) When a gas is below its critical temperature, application of sufficient pressure will cause the gas to become a liquid.

Diff: 1

Section: 11.1

178) Viscosity is determined only by the intermolecular attractive forces in a liquid.

Diff: 1

Section: 11.2

179) The surface tension of a liquid depends on the strength of the substance's intermolecular attractive forces.

Diff: 1

Section: 11.2

180) A cylinder contains a liquid which is in equilibrium with its vapor at 45.0°C. If the piston is moved down to constrict the volume of the cylinder without changing the temperature, the equilibrium vapor pressure of the liquid will increase.

Diff: 2

Section: 11.2

181) All substances have London forces.

Diff: 1

Section: 11.2

182) Amorphous solids are highly ordered crystals, and they must contain silicon or carbon to be classified as an amorphous solid.

Diff: 1

Section: 11.10

183) What is the difference between intermolecular interactions and intramolecular interactions in a molecule?

Diff: 2

Section: 11.1

184) During a rain storm, the surface of a car hood gets wet. If the car has a good polish or has recently been waxed, the water tends to bead or form drops, instead of evenly covering the surface. What does this say about the properties of water and the wax used to protect the car hood?

Diff: 2

Section: 11.1

185) Why would the coffee purchased in a to-go cup with a lid at the fast food takeout shop remain hot much longer than the coffee you pour into your ceramic cup at home?

Diff: 2

Section: 11.2

186) Why does CH3–CH2–O–H have a higher boiling point than CH3– O–CH3 even though they have the same formula, C2H6O?

Diff: 2

Section: 11.2

187) Explain how you could cause pure water to boil at a temperature of 25°C.

Diff: 1

Section: 11.5

188) A substance has a melting point of -25.0°C, an enthalpy of fusion of 1200 J g-1,and specific heats for the solid and the liquid are 3.00 and 6.20 J g-1 °C -1, respectively. How much energy is needed to change 150 grams of the substance from a solid at -40.0°C to a liquid at +70.0°C?

Diff: 2

Section: 11.6

189) A substance has a melting point of +25.0°C, an enthalpy of fusion of 1200 J g 1, and specific heats for the solid and the liquid are 3.00 and 6.20 J g-1 °C -1, respectively. How much energy is needed to change 150 grams of the substance from a solid at -40.0°C to a liquid at +70.0°C?

Diff: 2

Section: 11.6

190) A substance has a normal boiling point of +89.3 °C, an enthalpy of vaporization of

2600 J g-1, and specific heats for the liquid and the gas are 6.20 and 3.20 J g-1 °C -1, respectively. How much energy is needed to change 150 grams of the substance from a liquid at -10.0 °C to a gas at +129.0 °C?

Diff: 2

Section: 11.6

191) Based on the phase diagram of water, why can someone on ice skates can glide along the ice much more easily than someone in normal shoes?

Diff: 2

Section: 11.7

192) Keshon has an equation that gives the relationship between the air pressure at sea level, p0, and the air pressure, p, at a height, h (in meters), above sea level:

h = 4405 ln

He found a value for ΔΗvap of water, 41,108 J mol-1. Keshon has now challenged two other whiz kids in the class with this problem: Their weather app has given the barometric pressure at sea level as 30.18 inches of mercury. What is the temperature of the boiling water in a teapot at a mountain camp which is 2200 meters (about 7220 feet) above sea level?

Hint: Use the Clausius-Clapeyron equation and pay attention to units.

Diff: 3

Section: 11.9

193) Broken laboratory glass can sometimes be repaired by using heat to melt the glass pieces back together at the break or to melt shut a crack. Often the glass will crack easily at these repair joints, unless it undergoes a process called annealing. Annealing raises the temperature of the glass to just below the melting point and slowly lets it cool down to room temperature. After annealing, the glassware is often just like new. Using your knowledge of amorphous solids, why does annealing strengthen the glassware?

Diff: 2

Section: 11.10

194) Draw the unit cell for the following two-dimensional lattice.

Hint: Think about the repeating unit.

Diff: 3

Section: 11.10

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