General Chemistry 10th Edition by Darrell Ebbing Steven D. Gammon test bank

General Chemistry  10th Edition by Darrell Ebbing Steven D. Gammon  test bank
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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: 11.1
OBJ: Compare a gas, a liquid, and a solid using a kinetic-molecular theory description.
TOP: phases | liquid KEY: properties of liquids
MSC: 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 only
B)
2 only
C)
3 only
D)
1 and 2
E)
2 and 3

ANS: B PTS: 1 DIF: easy REF: 11.1
OBJ: 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)
sublimation
B)
freezing
C)
vaporization
D)
condensation
E)
melting

ANS: A PTS: 1 DIF: easy REF: 11.2
OBJ: Define melting, freezing, vaporization, sublimation, and condensation.
TOP: phases | phase transitions MSC: general chemistry

4. Which of the following processes is endothermic?
A)
melting of ice
B)
condensation of water
C)
deposition of carbon dioxide
D)
freezing of water
E)
condensation of ammonia

ANS: A PTS: 1 DIF: moderate REF: 11.2
OBJ: Define melting, freezing, vaporization, sublimation, and condensation.
TOP: phases | phase transitions

5. The process represented by the equation C10H8(s) C10H8(g) is
A)
melting.
B)
liquefaction.
C)
sublimation.
D)
condensation.
E)
fusion.

ANS: C PTS: 1 DIF: easy REF: 11.2
OBJ: 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 called
A)
fusion.
B)
condensation.
C)
melting.
D)
vaporization.
E)
sublimation.

ANS: E PTS: 1 DIF: easy REF: 11.2
OBJ: 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: 11.2
OBJ: Define vapor pressure. TOP: phases | phase transitions
KEY: 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.

A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
2 and 3

ANS: E PTS: 1 DIF: moderate REF: 11.2
OBJ: 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 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3

ANS: A PTS: 1 DIF: moderate REF: 11.2
OBJ: 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: 11.2
OBJ: 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 pressure
MSC: general chemistry

11. Which of the following involves a change in temperature during the phase transition?
A)
condensation of water
B)
fusion of ethanol
C)
vaporization of water
D)
all of the above
E)
none of the above

ANS: E PTS: 1 DIF: moderate REF: 11.2
OBJ: 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: 11.2
OBJ: 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. = 36.1C
B)
methanol, b.p. = 65.0C
C)
carbon tetrachloride, b.p. = 76.7C
D)
acetic acid, b.p. = 118C
E)
mercury, b.p. = 357C

ANS: A PTS: 1 DIF: moderate REF: 11.2
OBJ: Define boiling point. TOP: phases | phase transitions

14. In which of the following processes will energy be evolved as heat?
A)
crystallization
B)
melting
C)
sublimation
D)
vaporization
E)
none of these

ANS: A PTS: 1 DIF: easy REF: 11.2
OBJ: Define heat (enthalpy) of fusion and heat (enthalpy) of vaporization.
TOP: phases | phase transitions KEY: phase transition enthalpy change
MSC: general chemistry

15. Which of the following phase changes are endothermic?
A)
vaporization
B)
freezing
C)
liquifaction
D)
crystallization
E)
condensation

ANS: A PTS: 1 DIF: easy REF: 11.2
OBJ: 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)
g
B)
9.24 g
C)
3.55 g
D)
31.4 g
E)
g

ANS: A PTS: 1 DIF: easy REF: 11.2
OBJ: 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 0C. 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 vapor
B)
ice and water
C)
only water
D)
only water vapor
E)
only ice

ANS: C PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the heat required for a phase change of a given mass of substance. (Example 11.1) TOP: phases | phase transitions
KEY: 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 J
B)
2.98 106 J
C)
4.17 102 J
D)
1.87 104 J
E)
8.38 105 J

ANS: E PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the heat required for a phase change of a given mass of substance. (Example 11.1) TOP: phases | phase transitions
KEY: 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 kJ
B)
18.5 kJ
C)
18.5 kJ
D)
334 kJ
E)
0.202 kJ

ANS: C PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the heat required for a phase change of a given mass of substance. (Example 11.1) TOP: phases | phase transitions
KEY: 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: 11.2
OBJ: Describe the general dependence of the vapor pressure (in P) on the temperature (T).
TOP: phases | phase transitions KEY: vapor pressure
MSC: general chemistry

21. The vapor pressure of a given liquid will increase if
A)
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: 11.2
OBJ: Describe the general dependence of the vapor pressure (in P) on the temperature (T).
TOP: phases | phase transitions KEY: vapor pressure
MSC: 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 mmHg
B)
123 mmHg
C)
45.2 mmHg
D)
226 mmHg
E)
103 mmHg

ANS: D PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the vapor pressure at a given temperature. (Example 11.2)
TOP: phases | phase transitions KEY: Clausius-Clapeyron equation
MSC: 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 K
B)
319 K
C)
275 K
D)
259 K
E)
241 K

ANS: B PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the vapor pressure at a given temperature. (Example 11.2)
TOP: phases | phase transitions KEY: Clausius-Clapeyron equation
MSC: general chemistry

24. In a certain mountain range, water boils at 94C. What is the atmospheric pressure under these conditions? The enthalpy of vaporization of water at 100C is 40.7 kJ/mol. (R = 8.31 J/(K  mol))
A)
1760 mmHg
B)
324 mmHg
C)
613 mmHg
D)
942 mmHg
E)
329 mmHg

ANS: C PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the vapor pressure at a given temperature. (Example 11.2)
TOP: phases | phase transitions KEY: Clausius-Clapeyron equation
MSC: 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/mol
B)
320 kJ/mol
C)
2.01 kJ/mol
D)
228 kJ/mol
E)
104 kJ/mol

ANS: A PTS: 1 DIF: difficult REF: 11.2
OBJ: Calculate the heat of vaporization from vapor pressure. (Example 11.3)
TOP: phases | phase transitions KEY: Clausius-Clapeyron equation
MSC: general chemistry

26. Knowing that Hvap for water is 40.7 kJ/mol, calculate Pvap of water at 37C.
A)
52.7 torr
B)
25.4 torr
C)
18.7 torr
D)
12.4 torr
E)
6.90 torr

ANS: A PTS: 1 DIF: difficult REF: 11.2
OBJ: Calculate the heat of vaporization from vapor pressure. (Example 11.3)
TOP: phases | phase transitions KEY: Clausius-Clapeyron equation
MSC: 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/mol
B)
1.15 kJ/mol
C)
3.31 kJ/mol
D)
37.2 kJ/mol
E)
368 kJ/mol

ANS: D PTS: 1 DIF: moderate REF: 11.2
OBJ: Calculate the heat of vaporization from vapor pressure. (Example 11.3)
TOP: phases | phase transitions KEY: Clausius-Clapeyron equation
MSC: 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: 11.3
OBJ: Define phase diagram. TOP: phases | phase transitions
KEY: 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: 11.3
OBJ: 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: 11.3
OBJ: 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: 11.3
OBJ: Define phase diagram. TOP: phases | phase transitions
KEY: 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: 11.3
OBJ: Define phase diagram. TOP: phases | phase transitions
KEY: phase diagram MSC: general chemistry

33. The triple point of iodine is at 90 torr and 115C. This means that liquid I2
A)
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 115C.
E)
can exist at pressure of 10 torr.

ANS: A PTS: 1 DIF: easy REF: 11.3
OBJ: Define triple point. TOP: phases | phase transitions
KEY: phase diagram MSC: general chemistry

34. The critical point of CCl4 is 283C and 45 atm pressure. Liquid CCl4 has a vapor pressure of 10.0 atm at 178C. Which of the following statements must be true?
A)
Vapor and liquid can only be in equilibrium at one temperaturethe normal boiling point.
B)
Liquid CCl4 can exist at temperatures greater than 283C if the pressure is greater than 45 atm.
C)
Liquid and solid can only be in equilibrium at one temperaturethe freezing point.
D)
The triple point of CCl4 must be less than 178C.
E)
The normal boiling point of CCl4 must be greater than 178C.

ANS: D PTS: 1 DIF: moderate REF: 11.3
OBJ: Define triple point. TOP: phases | phase transitions
KEY: 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 point
B)
normal boiling point
C)
triple point
D)
melting point
E)
critical point

ANS: C PTS: 1 DIF: easy REF: 11.3
OBJ: Define triple point. TOP: phases | phase transitions
KEY: phase diagram | triple point MSC: general chemistry

36. Below is a phase diagram for a substance.

Which line represents the melting-point curve of the substance?
A)
R-X
B)
S-X
C)
X-Z
D)
S-Z
E)
M-N

ANS: A PTS: 1 DIF: easy REF: 11.3
OBJ: Describe the melting-point curve and the vapor-pressure curves (for the liquid and the solid) in a phase diagram. TOP: phases | phase transitions
KEY: phase diagram | melting-point curve MSC: general chemistry

37. Below is a phase diagram for a substance.

Which line represents the vapor-pressure curve of the substance?
A)
S-Z
B)
X-Z
C)
S-X
D)
M-N
E)
R-X

ANS: B PTS: 1 DIF: easy REF: 11.3
OBJ: Describe the melting-point curve and the vapor-pressure curves (for the liquid and the solid) in a phase diagram. TOP: phases | phase transitions
KEY: 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: 11.3
OBJ: Describe the melting-point curve and the vapor-pressure curves (for the liquid and the solid) in a phase diagram. TOP: phases | phase transitions
KEY: phase diagram | melting-point curve MSC: general chemistry

39. Below is a phase diagram for a substance.

What is the name for point Z on the diagram?
A)
normal boiling point.
B)
critical point.
C)
melting point.
D)
boiling point.
E)
triple point.

ANS: B PTS: 1 DIF: easy REF: 11.3
OBJ: Define critical temperature and critical pressure.
TOP: phases | phase transitions KEY: phase diagram
MSC: general chemistry

40. Which explanation best describes surface tension?
A)
Molecules at the surface of a liquid experience a net force towards the liquids interior.
B)
Molecules at the edges of a liquid adhere to the surface of the liquids 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: 11.4
OBJ: Define surface tension. TOP: phases | liquid
KEY: 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 1011 J
B)
1.9 1012 J
C)
2.8 1014 J
D)
7.7 1012 J
E)
3.3 1011 J

ANS: B PTS: 1 DIF: moderate REF: 11.4
OBJ: Define surface tension. TOP: phases | liquid
KEY: 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: 11.4
OBJ: Describe the phenomenon of capillary rise. TOP: phases | liquid
KEY: 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 material

2.
surface tension of the liquid

3.
viscosity of the liquid

A)
1
B)
2
C)
3
D)
1 and 2
E)
1, 2, and 3

ANS: D PTS: 1 DIF: easy REF: 11.4
OBJ: Describe the phenomenon of capillary rise. TOP: phases | liquid
KEY: 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.

A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1 and 3

ANS: E PTS: 1 DIF: easy REF: 11.4
OBJ: Describe the phenomenon of capillary rise. TOP: phases | liquid

45. The measure of the resistance to flow of a liquid is
A)
London forces.
B)
van der Waals forces.
C)
viscosity.
D)
vapor pressure.
E)
surface tension.

ANS: C PTS: 1 DIF: easy REF: 11.4
OBJ: Define viscosity. TOP: phases | liquid
KEY: 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: 11.5
OBJ: 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: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces
MSC: general chemistry

48. Which of the following compounds has the highest normal boiling point?
A)
CH3CH2CH2CH3
B)
CH3Cl
C)
CH3CH2OH
D)
CH3OCH3
E)
CH3CH2CH3

ANS: C PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: intermolecular forces | hydrogen bonding MSC: general chemistry

49. Which of the following compounds has the highest vapor pressure at 25C?
A)
CH3CH2OH
B)
CH3CH2CH2CH3
C)
CH3OCH3
D)
CH3CH2CH3
E)
CH3CH2CH2Cl

ANS: D PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces
MSC: general chemistry

50. Which of the following pure substances has the lowest normal boiling point?
A)
H2S
B)
NH3
C)
H2O
D)
H2Te
E)
H2Se

ANS: A PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: 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 bonding
B)
covalent bonding
C)
hydrogen bonding
D)
dipoledipole
E)
London dispersion

ANS: E PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid

52. Which compound has the lowest standard enthalpy of vaporization at 25C?
A)
C6H14
B)
C8H16
C)
C5H12
D)
C8H18
E)
C7H16

ANS: C PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces | London forces
MSC: general chemistry

53. Which of the following indicates the existence of strong intermolecular forces of attraction in a liquid?
A)
a very low critical temperature
B)
a very low boiling point
C)
a very low vapor pressure
D)
a very low viscosity
E)
a very low enthalpy of vaporization

ANS: C PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces
MSC: general chemistry

54. Which of the following compounds has the lowest normal boiling point?
A)
CH3CH2CH2NH2
B)
CH3CH2CH2F
C)
CH3CH2CH2OH
D)
CH3CH2COOH
E)
CH3CH(OH)CH3

ANS: B PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: intermolecular forces | hydrogen bonding MSC: general chemistry

55. Which of the following compounds is expected to have the lowest vapor pressure?
A)
CH3OCH3
B)
CH3CH2F
C)
CH3CH2OH
D)
CH3CH2CH2CH3
E)
CH3CH2CH3

ANS: C PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces
MSC: general chemistry

56. Which of the following pure substances has the highest normal boiling point?
A)
HI
B)
HCl
C)
HF
D)
H2S
E)
HBr

ANS: C PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: intermolecular forces | hydrogen bonding MSC: general chemistry

57. Why does hydrogen fluoride have an unusually high normal boiling point compared to the other hydrogen halides?
A)
The H-F bond in hydrogen fluoride is very strong.
B)
Hydrogen fluoride has very strong London dispersion forces.
C)
Hydrogen fluoride is capable of forming hydrogen bonds.
D)
Hydrogen fluoride is ionic.
E)
Hydrogen fluoride is covalent.

ANS: C PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: intermolecular forces | hydrogen bonding MSC: general chemistry

58. Which of the following pure substances has the lowest vapor pressure at 25C?
A)
SbH3
B)
NH3
C)
PH3
D)
AsH3
E)
H2O

ANS: E PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: 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: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces | London forces
MSC: general chemistry

60. Which of the following pure substances has the highest standard enthalpy of vaporization at 25C?
A)
H2O
B)
NH3
C)
PH3
D)
AsH3
E)
SbH3

ANS: A PTS: 1 DIF: easy REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: intermolecular forces | hydrogen bonding MSC: general chemistry

61. At 25C, the vapor pressure of diethyl ether, (CH3CH2)2O, is higher than the vapor pressure of its isomer n-butanol, CH3CH2CH2CH2OH, because
A)
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: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces
MSC: general chemistry

62. Which of the following pure substances has an unusually high normal boiling point?
A)
CH3OCH3
B)
CH3SH
C)
HCl
D)
CH3NH2
E)
CH3Cl

ANS: D PTS: 1 DIF: moderate REF: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid
KEY: 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: 11.5
OBJ: Relate the properties of liquids to the intermolecular forces involved.
TOP: phases | liquid KEY: intermolecular forces
MSC: 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: 11.5 OBJ: 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 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3 ANS: E PTS: 1 DIF: moderate REF: 11.5 OBJ: 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 water B) Liquid A boils at a higher temperature than water C) The vapor pressure of B is higher than that of A D) The vapor pressure of B is higher than that of water E) Liquid A boils at a temperature higher than B ANS: A PTS: 1 DIF: difficult REF: 11.5 OBJ: Relate the properties of liquids to the intermolecular forces involved. TOP: phases | liquid KEY: intermolecular forces MSC: 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 molecule B) An oxygen from one molecule and an oxygen from the other molecule C) Two hydrogens from one molecule and one oxygen from the other molecule D) A hydrogen from one molecule and a hydrogen from the other molecule E) A hydrogen from one molecule and an oxygen from the other molecule ANS: E PTS: 1 DIF: easy REF: 11.5 OBJ: Define hydrogen bonding. TOP: phases | liquid KEY: intermolecular forces | hydrogen bonding MSC: general chemistry 68. What is the maximum number of hydrogen bonds in which a water molecule could participate? A) 2 B) 4 C) 3 D) 6 E) 5 ANS: B PTS: 1 DIF: moderate REF: 11.5 OBJ: Define hydrogen bonding. TOP: phases | liquid KEY: intermolecular forces | hydrogen bonding MSC: general chemistry 69. Which pure substance exhibits hydrogen bonding? A) HNF2 B) B2H6 C) HBr D) H2S E) CaH2 ANS: A PTS: 1 DIF: easy REF: 11.5 OBJ: Define hydrogen bonding. TOP: phases | liquid KEY: 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) CH3CH2CH2CH2OH E) SbCl3 ANS: C PTS: 1 DIF: easy REF: 11.5 OBJ: Identify the intermolecular forces in a substance. (Example 11.5) TOP: phases | liquid KEY: intermolecular forces MSC: general chemistry 71. Which of the following best describes carbon dioxide (CO2) at room temperature and pressure? A) ionic solid B) nonpolar molecular gas C) metallic solid D) polar molecular gas E) covalent network solid ANS: B PTS: 1 DIF: easy REF: 11.5 OBJ: 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) CH3Cl B) CH3OCH3 C) H2CO D) N(CH3)3 E) H2NNH2 ANS: E PTS: 1 DIF: easy REF: 11.5 OBJ: Identify the intermolecular forces in a substance. (Example 11.5) TOP: phases | liquid KEY: intermolecular forces | hydrogen bonding MSC: general chemistry 73. The strongest intermolecular forces present in a sample of pure I2 are A) London forces. B) dipoledipole forces. C) metallic bonds. D) covalent network bonds. E) covalent bonds. ANS: A PTS: 1 DIF: easy REF: 11.5 OBJ: Identify the intermolecular forces in a substance. (Example 11.5) TOP: phases | liquid KEY: intermolecular forces | London forces MSC: general chemistry 74. The strongest intermolecular forces between molecules of PH3 are A) hydrogen bonds. B) covalent bonds. C) ionic bonds. D) London forces. E) dipoledipole attractions. ANS: E PTS: 1 DIF: easy REF: 11.5 OBJ: Identify the intermolecular forces in a substance. (Example 11.5) TOP: phases | liquid KEY: intermolecular forces MSC: general chemistry 75. The molecules in a sample of solid SO2 are attracted to each other by a combination of A) 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: 11.5 OBJ: Identify the intermolecular forces in a substance. (Example 11.5) TOP: phases | liquid KEY: intermolecular forces MSC: general chemistry 76. Which of the following best describes silane (SiH4) at room temperature and pressure? A) ionic solid B) covalent network solid C) nonpolar molecular gas D) polar molecular gas E) metallic solid ANS: C PTS: 1 DIF: moderate REF: 11.5 OBJ: 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 bonding B) hydrogen bonding C) ionic bonding D) London forces E) metallic bonding ANS: D PTS: 1 DIF: easy REF: 11.5 OBJ: Identify the intermolecular forces in a substance. (Example 11.5) TOP: phases | liquid KEY: intermolecular forces MSC: 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: 11.6 OBJ: 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: 11.6 OBJ: 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: 11.6 OBJ: Define molecular solid, metallic solid, ionic solid, and covalent network solid. TOP: phases | solid KEY: classification of solids MSC: general chemistry 81. Which of the following best describes calcium hydride (CaH2) at room temperature and pressure? A) nonpolar molecular gas B) metallic solid C) ionic solid D) polar molecular gas E) covalent network solid ANS: C PTS: 1 DIF: moderate REF: 11.6 OBJ: Identify types of solids. (Example 11.7) TOP: phases | solid KEY: classification of solids MSC: general chemistry 82. Which of the following is not a covalent network solid? A) diamond B) silicon carbide C) quartz D) iron E) graphite ANS: D PTS: 1 DIF: easy REF: 11.6 OBJ: Identify types of solids. (Example 11.7) TOP: phases | solid KEY: classification of solids MSC: general chemistry 83. Which of the following is a molecular solid? A) NaCl B) CH4 C) SiO2 D) C(graphite) E) C(diamond) ANS: B PTS: 1 DIF: easy REF: 11.6 OBJ: Identify types of solids. (Example 11.7) TOP: phases | solid KEY: classification of solids MSC: general chemistry 84. Which of the following is an ionic solid? A) SiO2(s) B) Ne(s) C) Na(s) D) CsF(s) E) CO2(s) ANS: D PTS: 1 DIF: easy REF: 11.6 OBJ: Identify types of solids. (Example 11.7) TOP: phases | solid KEY: classification of solids MSC: general chemistry 85. Which bonding interaction best describes the strongest intermolecular forces in AlH3? A) dipoledipole forces B) metallic bonding C) ionic bonding D) London dispersion forces E) primarily hydrogen bonding ANS: C PTS: 1 DIF: moderate REF: 11.6 OBJ: Identify types of solids. (Example 11.7) TOP: phases | solid MSC: general chemistry 86. Which of the following is a molecular solid? A) carborundum, SiC B) quartz C) glass D) hydrogen chloride E) potassium ANS: D PTS: 1 DIF: easy REF: 11.6 OBJ: Identify types of solids. (Example 11.7) TOP: phases | solid KEY: classification of solids MSC: general chemistry 87. Which of the following pure substances has the highest normal melting point? A) KF B) KI C) NaF D) NaCl E) NaI ANS: C PTS: 1 DIF: easy REF: 11.6 OBJ: Relate the melting point of a solid to its structure. TOP: phases | solid KEY: properties of solids | melting point MSC: general chemistry 88. Which of the following pure substances has the lowest melting point? A) LiF B) RbF C) CsF D) KF E) NaF ANS: C PTS: 1 DIF: easy REF: 11.6 OBJ: Relate the melting point of a solid to its structure. TOP: phases | solid KEY: properties of solids | melting point MSC: general chemistry 89. Which of the following pure substances has the lowest melting point? A) Cs2O B) CsCl C) CsBr D) CsI E) CsF ANS: D PTS: 1 DIF: easy REF: 11.6 OBJ: Relate the melting point of a solid to its structure. TOP: phases | solid KEY: 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) LiCl E) MgCl2 ANS: B PTS: 1 DIF: easy REF: 11.6 OBJ: Relate the melting point of a solid to its structure. TOP: phases | solid KEY: properties of solids | melting point MSC: general chemistry 91. Which of the following pure substances has the highest melting point? A) KBr B) NaCl C) NaF D) CsI E) LiF ANS: E PTS: 1 DIF: moderate REF: 11.6 OBJ: Relate the melting point of a solid to its structure. TOP: phases | solid KEY: 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: 11.6 OBJ: 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: 11.6 OBJ: Determine relative melting points based on types of solids. (Example 11.8) TOP: phases | solid KEY: properties of solids | melting point MSC: 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: 11.6 OBJ: Determine relative melting points based on types of solids. (Example 11.8) TOP: phases | solid KEY: properties of solids | melting point MSC: general chemistry 95. Which of the following pure substances has the highest normal melting point? A) P4O10 B) P4O6 C) CO2 D) CaO E) Na2O ANS: D PTS: 1 DIF: moderate REF: 11.6 OBJ: Determine relative melting points based on types of solids. (Example 11.8) TOP: phases | solid KEY: properties of solids | melting point MSC: general chemistry 96. Which of the following pure substances has the highest normal boiling point? A) H2O B) CF4 C) CsF D) CaF2 E) KF ANS: D PTS: 1 DIF: moderate REF: 11.6 OBJ: Determine relative melting points based on types of solids. (Example 11.8) TOP: phases | solid KEY: properties of solids MSC: 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) H2O D) NaCl E) Cu ANS: D PTS: 1 DIF: easy REF: 11.6 OBJ: Relate the hardness and electrical conductivity of a solid to its structure. TOP: phases | solid KEY: properties of solids MSC: general chemistry 98. A solid crystal of NaCl is A) 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: 11.6 OBJ: Relate the hardness and electrical conductivity of a solid to its structure. TOP: phases | solid KEY: properties of solids MSC: 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 only C) 3 only D) 1 and 2 E) 1, 2, and 3 ANS: D PTS: 1 DIF: moderate REF: 11.7 OBJ: 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: 11.7 OBJ: Define simple cubic unit cell, body-centered cubic unit cell, and face-centered cubic unit cell. TOP: phases | solid KEY: 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) 1 B) 16 C) 2 D) 4 E) 8 ANS: E PTS: 1 DIF: easy REF: 11.7 OBJ: Define simple cubic unit cell, body-centered cubic unit cell, and face-centered cubic unit cell. TOP: phases | solid KEY: 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 atom B) body centered cubic, 2 atoms C) face centered cubic, 4 atoms D) simple cubic, 8 atoms E) body centered cubic, 3 atoms ANS: A PTS: 1 DIF: easy REF: 11.7 OBJ: 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: 11.7 OBJ: Determine the number of atoms in a unit cell. (Example 11.9) TOP: phases | solid KEY: crystalline solids | cubic unit cell MSC: general chemistry 104. How many atoms are there in a cubic close-packed unit cell of aluminum? A) 4 B) 6 C) 1 D) 8 E) 2 ANS: A PTS: 1 DIF: easy REF: 11.8 OBJ: Determine the number of atoms in a unit cell. (Example 11.9) TOP: phases | solid KEY: 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) 4 B) 8 C) 6 D) 2 E) 1 ANS: D PTS: 1 DIF: easy REF: 11.7 OBJ: Determine the number of atoms in a unit cell. (Example 11.9) TOP: phases | solid KEY: 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) 4 B) 6 C) 8 D) 1 E) 2 ANS: A PTS: 1 DIF: moderate REF: 11.7 OBJ: Determine the number of atoms in a unit cell. (Example 11.9) TOP: phases | solid KEY: 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: 11.8 OBJ: Note the common structures (face-centered cubic and body-centered cubic) of metallic solids. TOP: phases | solid KEY: 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) 4 B) 3 C) 1 D) 8 E) 2 ANS: A PTS: 1 DIF: moderate REF: 11.8 OBJ: Describe the three types of cubic structures of ionic solids. TOP: phases | solid KEY: 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) Mn B) Ti C) Co D) Sc E) cannot be determined from the information given. ANS: C PTS: 1 DIF: moderate REF: 11.9 OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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: 11.9 OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: general chemistry 111. The metal gold, with an atomic radius of 144.2 pm, crystallizes in a face-centered cubic lattice. What is the density of gold? A) 9.65 g/cm3 B) 1.21 g/cm3 C) 4.82 g/cm3 D) 2.41 g/cm3 E) 19.3 g/cm3 ANS: E PTS: 1 DIF: difficult REF: 11.9 OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: general chemistry 112. A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 198 pm and the density of the element is 6.57 g/cm3. What is the identity of the metal? A) Cu B) Ca C) Sr D) Ni E) Yb ANS: E PTS: 1 DIF: difficult REF: 11.9 OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10) TOP: phases | solid KEY: structures of crystalline solids MSC: 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) cm3 B) cm3 C) cm3 D) cm3 E) cm3 ANS: A PTS: 1 DIF: difficult REF: 11.9 OBJ: 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 pm B) 396 pm C) 792 pm D) 420 pm E) 198 pm ANS: A PTS: 1 DIF: difficult REF: 11.9 OBJ: 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 g B) 1.41 10-22 g C) 4.22 10-22 g D) 7.04 10-23 g E) 2.82 10-22 g ANS: E 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 dimensions MSC: general chemistry 116. Lithium chloride crystallizes in a face-centered cubic structure. The unit cell length is 5.14  10-8 cm. The chloride ions are touching each other along the face diagonal of the unit cell. The lithium ions fit into the holes between the chloride ions. What is the density of the lithium chloride? A) 0.520 g/cm3 B) 2.82 g/cm3 C) 2.08 g/cm3 D) 3.11 g/cm3 E) 3.78 g/cm3 ANS: C PTS: 1 DIF: difficult REF: 11.9 OBJ: Calculate atomic mass from unit-cell dimension and density. (Example 11.10) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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 pm B) 77.6 pm C) 75.0 pm D) 61.6 pm E) 228 pm ANS: A PTS: 1 DIF: moderate REF: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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 pm B) 444 pm C) 296 pm D) 222 pm E) 96.1 pm ANS: A PTS: 1 DIF: difficult REF: 11.9 OBJ: 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: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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? A) 186 pm B) 744 pm C) 992 pm D) 859 pm E) 80.5 pm ANS: A PTS: 1 DIF: difficult REF: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and edge-length. (Example 11.11) TOP: phases | solid 121. Copper crystallizes with a face-centered cubic unit cell. If the edge length of the unit cell is 362 pm, what is the radius of a copper atom in picometers? A) 128 pm B) 512 pm C) 1020 pm D) 296 pm E) 45.3 pm ANS: A PTS: 1 DIF: difficult REF: 11.9 OBJ: 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) AB D) A2B4 E) A2B6 ANS: A PTS: 1 DIF: difficult REF: 11.9 OBJ: 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: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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/mol B) 24.7 cm3/mol C) 86.6 cm3/mol D) 33.4 cm3/mol E) 0.380 cm3/mol ANS: D PTS: 1 DIF: difficult REF: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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 pm B) 174 pm C) 42.5 pm D) 19.0 pm E) 219 pm ANS: E PTS: 1 DIF: difficult REF: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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 cm B) 1.82 10-8 cm C) 2.56 10-8 cm D) 1.45 10-8 cm E) 2.82 10-8 cm ANS: B PTS: 1 DIF: difficult REF: 11.9 OBJ: Calculate unit-cell dimension from unit-cell type and density. (Example 11.11) TOP: phases | solid KEY: calculations with unit cell dimensions MSC: 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: 11.10 OBJ: 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 diffraction MSC: general chemistry

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