LT 11.1 Practice Test

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1 point

1. The principal source of the difference in the normal boiling points of ICl (97°C; molecular mass 162 amu) and Br₂ (59°C; molecular mass 160 amu) is both dipole-dipole interactions and London dispersion forces.

1 point

True

False

Clear selection

2. The boiling points of normal hydrocarbons are higher than those of branched hydrocarbons of similar molecular weight because the London-dispersion forces between normal hydrocarbons are greater than those between branched hydrocarbons.

1 point

True

False

Clear selection

3. Heats of vaporization are greater than heats of fusion.

1 point

True

False

Clear selection

4. Under ordinary conditions, a substance will sublime rather than melt if its triple point occurs at a pressure above atmospheric pressure.

1 point

True

False

Clear selection

5. In liquids, the attractive intermolecular forces are __________.

1 point

very weak compared with kinetic energies of the molecules

strong enough to hold molecules relatively close together

strong enough to keep the molecules confined to vibrating about their fixed lattice points

not strong enough to keep molecules from moving past each other

strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other

Clear selection

6. As a solid element melts, the atoms become __________ and they have __________ attraction for one another.

1 point

more separated; more

more separated; less

closer together; more

closer together; less

larger; greater

Clear selection

7. A gas is __________ and assumes __________ of its container whereas a liquid is __________ and assumes __________ of its container.

1 point

compressible; the volume and shape; not compressible; the shape of a portion

compressible; the shape; not compressible; the volume and shape

compressible; the volume and shape; compressible; the volume

condensed; the volume and shape; condensed; the volume and shape

condensed; the shape; compressible; the volume and shape

Clear selection

8. Together, liquids and solids constitute __________ phases of matter.

1 point

the compressible

the fluid

the condensed

all of the

the disordered

Clear selection

9. Which statement is true about liquids but not true about solids?

1 point

They flow and are highly ordered

They are highly ordered and not compressible

They flow and are compressible

They assume both the volume and the shape of their containers.

They flow and are not compressible.

Clear selection

10. The strongest interparticle attractions exist between particles of a __________ and the weakest interparticle attractions exist between particles of a __________.

1 point

solid; liquid

solid; gas

liquid; gas

liquid; solid

gas; solid

Clear selection

11. Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point?

1 point

CH₃CH₂CH₃

CH₃OCH₃

CH₃Cl

CH₃CHO

CH₃CN

Clear selection

12. Of the following substances, only __________ has London dispersion forces as its only intermolecular force.

1 point

CH₃OH

NH₃

H₂S

CH₄

HCl

Clear selection

13. Of the following substances, only __________ has London dispersion forces as the only intermolecular force.

1 point

CH₃OH

NH₃

H₂S

HCl

Clear selection

14. Which one of the following should have the lowest boiling point?

1 point

PH₃

H₂S

HCl

SiH₄

H₂O

Clear selection

15. Of the following substances, __________ has the highest boiling point.

1 point

H₂O

CO₂

CH₄

NH₃

Clear selection

16. Of the following, __________ has the highest boiling point.

1 point

N₂

Br₂

H₂

Cl₂

O₂

Clear selection

17. In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces?

1 point

CH₄

C₅H₁₁OH

C₆H₁₃NH₂

CH₃OH

CO₂

Clear selection

18. Which of the following has dispersion forces as its only intermolecular force?

1 point

CH₄

HCl

C₆H₁₃NH₂

NaCl

CH₃Cl

Clear selection

19. Which one of the following exhibits dipole-dipole attraction between molecules?

1 point

XeF₄

AsH₃

CO₂

BCl₃

Cl₂

Clear selection

21. Which one of the following has the highest boiling point?

1 point

C₂Br₆

C₂F₆

C₂I₆

C₂Cl₆

C₂H₆

Clear selection

22. What is the predominant intermolecular force in CBr₄?

1 point

dispersion forces

ion-dipole attraction

ionic bonding

dipole-dipole attraction

hydrogen-bonding

Clear selection

23. The intermolecular force(s) responsible for the fact that CH₄ has the lowest boiling point in the set is/are __________.

1 point

hydrogen bonding

dipole-dipole interactions

dispersion forces

mainly hydrogen bonding but also dipole-dipole interactions

mainly London-dispersion forces but also dipole-dipole interactions

Clear selection

24. Elemental iodine (I₂) is a solid at room temperature. What is the major attractive force that exists among different I₂ molecules in the solid?

1 point

dispersion forces

dipole-dipole rejections

ionic-dipole interactions

covalent-ionic interactions

dipole-dipole attractions

Clear selection

25. Hydrogen bonding is a special case of __________.

1 point

London-dispersion forces

ion-dipole attraction

dipole-dipole attractions

ion-ion interactions

none of the above

Clear selection

26. Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?

1 point

Clear selection

27. Which one of the following substances will not have hydrogen bonding as one of its intermolecular forces?

1 point

Clear selection

28. What intermolecular force is responsible for the fact that ice is less dense than liquid water?

1 point

London dispersion forces

dipole-dipole forces

ion-dipole forces

hydrogen bonding

ionic bonding

Clear selection

29. The predominant intermolecular force in (CH₃)₂NH is __________.

1 point

London dispersion forces

ion-dipole forces

ionic bonding

dipole-dipole forces

hydrogen bonding

Clear selection

30. C₁₂H₂₆ molecules are held together by __________.

1 point

ion-ion interactions

hydrogen bonding

ion-dipole interactions

dipole-dipole interactions

dispersion forces

Clear selection

31. Which of the following molecules has hydrogen bonding as its only intermolecular force?

1 point

H₂O

C₆H₁₃NH₂

C₅H₁₁OH

None

all of the above exhibit dispersion forces.

Clear selection

36. Which statements about viscosity are true?

(i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii) Viscosity increases as intermolecular forces increase

1 point

(i) only

(ii) and (iii)

(i) and (iii)

none

all

Clear selection

37. The shape of a liquid's meniscus is determined by __________.

1 point

the viscosity of the liquid

the type of material the container is made of

the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container

the amount of hydrogen bonding in the liquid

the volume of the liquid

Clear selection

38. Viscosity is __________.

1 point

the "skin" on a liquid surface caused by intermolecular attraction

the resistance to flow

the same as density

inversely proportional to molar mass

unaffected by temperature

Clear selection

39. How high a liquid will rise up a narrow tube as a result of capillary action depends on __________.

1 point

the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube

and gravity

gravity alone

only the magnitude of adhesive forces between the liquid and the tube

the viscosity of the liquid

only the magnitude of cohesive forces in the liquid

Clear selection

40. The property responsible for the "beading up" of water is __________.

1 point

density

viscosity

vapor pressure

surface tension

hydrogen bonding

Clear selection

41. The substance with the largest heat of vaporization is __________.

1 point

I₂

Br₂

Cl₂

F₂

O₂

Clear selection

42. Of the following, __________ is an exothermic process.

1 point

melting

subliming

freezing

boiling

All of the above are exothermic

Clear selection

43. The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.3 J/mol • K. The conversion of 50.0 g of ice at 0.00°C to liquid water at 22.0°C requires __________ kJ of heat.

1 point

3.8 × 10²

21.3

17.2

0.469

Insufficient data are given.

Clear selection

Use for problems 44-48

44. The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the __________ segment corresponds to the heat capacity of the liquid of the substance.

1 point

Clear selection

45. The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the __________ segment corresponds to the heat capacity of the gas.

1 point

Clear selection

46. The heating curve shown was generated by measuring the heat flow and temperature of a solid as it was heated. The heat flow into the sample in the segment __________ will yield the value of the ΔHvap of this substance.

1 point

Clear selection

47. The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the __________ segment corresponds to the heat capacity of the solid.

1 point

Clear selection

48. The heating curve shown was generated by measuring the heat flow and temperature of a solid as it was heated. The heat flow into the sample in the segment __________ will yield the value of the ΔHfus of this substance.

1 point

Clear selection

49. Of the following, __________ should have the highest critical temperature.

1 point

CBr₄

CCl₄

CF₄

CH₄

H₂

Clear selection

50. Heat of sublimation can be approximated by adding together __________ and __________.

1 point

heat of fusion; heat of condensation

heat of fusion; heat of vaporization

heat of freezing (solidification); heat of condensation

heat of freezing (solidification); heat of vaporization

heat of deposition; heat of vaporization

Clear selection

51. Which of the following statements is false?

1 point

The absolute value of the heat of sublimation is equal to the absolute value of the heat of deposition.

The heat of sublimation is equal to the sum of the heat of vaporization and the heat of melting.

The heat of sublimation is equal to the sum of the heat of vaporization and the heat of freezing.

The absolute value of the heat of sublimation is equal to the absolute value of the sum of the heat of condensation and the heat of freezing.

The absolute value of the heat of deposition is equal to sum of the absolute value of the heat of vaporization and the absolute value of the heat of freezing.

Clear selection

52. The phase changes B → C and D → E are not associated with temperature increases because the heat energy is used up to __________.

1 point

increase distances between molecules

break intramolecular bonds

rearrange atoms within molecules

increase the velocity of molecules

increase the density of the sample

Clear selection

53. Based on the information in the table above, which compound has the strongest intermolecular forces?

1 point

Argon

Benzene

Ethanol

Water

Methane

Clear selection

55. Calculate the enthalpy change associated with the conversion of 25.0 grams of ice at -4.00°C to water vapor at 110.0°C. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H₂O, ΔHfus = 6.01 kJ/mol and ΔHvap = 40.67 kJ/mol.

1 point

64.8 kJ

75.9 kJ

1.11 × 10⁴ kJ

1.12 × 10⁴ kJ

1.00 × 10⁵ kJ

Clear selection

56. Large intermolecular forces in a substance are manifested by __________.

1 point

low vapor pressure

high boiling point

high heats of fusion and vaporization

high critical temperatures and pressures

all of the above

Clear selection

57. A substance that expands to fill its container yet has a density approaching that of a liquid, and that can behave as a solvent is called a(n) __________.

1 point

plasma

gas

liquid

amorphous solid

supercritical fluid and gas

Clear selection

58. The critical temperature and pressure of CS₂ are 279°C and 78 atm, respectively. At temperatures above 279°C and pressures above 78 atm, CS₂ can only occur as a __________.

1 point

solid

liquid

liquid and gas

gas

supercritical fluid

Clear selection

59. The enthalpy change for converting 1.00 mol of ice at -50.0°C to water at 70.0°C is___________ kJ.

The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H₂O, ΔHfus = 6.01 kJ/mol and ΔHvap = 40.67 kJ/mol.

1 point

12.28

6.41

13.16

7154

9.40

Clear selection

60. The enthalpy change for converting 10.0 g of ice at -25.0°C to water at 80.0°C is __________ kJ.

The specific heats of ice, water, and steam are and respectively. For H₂O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol.

1 point

12.28

6.16

3870

7.21

9.88

Clear selection

61. The fluorocarbon C₂Cl₃F₃ has a normal boiling point of 47.6°C. The specific heats of and C₂Cl₃F₃(g) are 0.91 J/g-K and 0.67 J/g-K, respectively. The heat of vaporization of the compound is 27.49 kJ/mol. The heat required to convert 50.0 g of the compound from the liquid at 5.0°C to the gas at 80.0°C is __________ kJ.

1 point

8.19

1454

30.51

3031

10.36

Clear selection

62. Ethanol (C₂H₅OH) melts at -114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135°C to liquid ethanol at -50°C?

1 point

207.3

-12.7

6.91

4192

9.21

Clear selection

63. Of the following, __________ is the most volatile.

1 point

CBr₄

CCl₄

CF₄

CH₄

C₆H₁₄

Clear selection

64. A volatile liquid is one that __________.

1 point

is highly flammable

is highly viscous

is highly hydrogen-bonded

is highly cohesive

readily evaporates

Clear selection

65. In general, the vapor pressure of a substance increases as __________ increases.

1 point

surface tension

molecular weight

hydrogen bonding

viscosity

temperature

Clear selection

66. The vapor pressure of any substance at its normal boiling point is

1 point

1 Pa

1 torr

1 atm

equal to atmospheric pressure

equal to the vapor pressure of water

Clear selection

67. Volatility and vapor pressure are __________.

1 point

inversely proportional to one another

directly proportional to one another

not related

the same thing

both independent of temperature

Clear selection

68. Some things take longer to cook at high altitudes than at low altitudes because __________.

1 point

water boils at a lower temperature at high altitude than at low altitude

water boils at a higher temperature at high altitude than at low altitude

heat isn't conducted as well in low density air

natural gas flames don't burn as hot at high altitudes

there is a higher moisture content in the air at high altitude

Clear selection

69. The vapor pressure of a liquid __________.

1 point

increases linearly with increasing temperature

increases nonlinearly with increasing temperature

decreases linearly with increasing temperature

decreases nonlinearly with increasing temperature

is totally unrelated to its molecular structure

Clear selection

Use for problems 70-72

70. Based on the figure above, the boiling point of diethyl ether under an external pressure of 1.32 atm is __________°C.

1 point

Clear selection

71. Based on the figure above, the boiling point of ethyl alcohol under an external pressure of 0.0724 atm is __________°C.

1 point

Clear selection

72. Based on the figure above, the boiling point of water under an external pressure of 0.316 atm atm is __________°C.

1 point

Clear selection

Use for problems 73-74

73. On the phase diagram shown above, segment __________ corresponds to the conditions of temperature and pressure under which the solid and the gas of the substance are in equilibrium.

1 point

Clear selection

74. On the phase diagram shown above, the coordinates of point __________ correspond to the critical temperature and pressure.

1 point

Clear selection

75. The phase diagram of a substance is given above. The region that corresponds to the solid phase is __________.

1 point

x and y

Clear selection

76. The normal boiling point of the substance with the phase diagram shown above is __________°C.

1 point

Clear selection

Use for problems 77-78

77. The phase diagram of a substance is shown above. The area labeled __________ indicates the gas phase for the substance.

1 point

y and z

Clear selection

78. According to the phase diagram shown above, the normal boiling point of this substance is __________°C.

1 point

-3

Clear selection

79. The phase diagram of a substance is given above, This substance is a __________ at 25°C and 1.0 atm.

1 point

solid

liquid

gas

supercritical fluid

crystal

Clear selection

80. On a phase diagram, the critical pressure is __________.

1 point

the pressure required to melt a solid

the pressure below which a substance is a solid at all temperatures

the pressure above which a substance is a liquid at all temperatures

the pressure at which a liquid changes to a gas

the pressure required to liquefy a gas at its critical temperature

Clear selection

81. On a phase diagram, the critical temperature is __________.

1 point

the temperature below which a gas cannot be liquefied

the temperature above which a gas cannot be liquefied

the temperature at which all three states are in equilibrium

the temperature required to melt a solid

the temperature required to cause sublimation of a solid

Clear selection

82. On a phase diagram, the melting point is the same as __________.

1 point

the triple point

the critical point

the freezing point

the boiling point

the vapor-pressure curve

Clear selection

83. When the phase diagram for a substance has a solid-liquid phase boundary line that has a negative slope (leans to the left), the substance __________.

1 point

can go from solid to liquid within a small temperature range via the application of pressure

sublimes rather than melts under ordinary conditions

cannot go from solid to liquid by application of pressure at any temperature

cannot be liquefied above its triple point

melts rather than sublimes under ordinary conditions

Clear selection

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