Sale!

Chemistry The Central Science 12th Edition Brown LeMay Bursten Test Bank

$80.00 $12.99

Chemistry The Central Science 12th Edition Brown LeMay Bursten Test Bank

ISBN-13: 9780321696724

Description

Chemistry The Central Science 12th Edition Brown LeMay Bursten Test Bank

ISBN-13: 9780321696724

 

 

Be the best nurse you can be:

Nursing test banks are legit and very helpful. This test bank on this page can be downloaded immediately after you checkout today.

Here is the definition of nursing

Its true that you will receive the entire legit test bank for this book and it can happen today regardless if its day or night. We have made the process automatic for you so that you don’t have to wait.

We encourage you to purchase from only a trustworthy provider:

Our site is one of the most confidential websites on the internet. We maintain no logs and guarantee it. Our website is also encrypted with an SSL on the entire website which will show on your browser with a lock symbol. This means not a single person can view any information.

Have any comments or suggestions?

When you get your file today you will be able to open it on your device and start studying for your class right now.

Remember, this is a digital download that is automatically given to you after you checkout today.

Free Nursing Test Questions:

Chemistry: The Central Science, 12e (Brown et al.)

Chapter 11   Liquids and Intermolecular Forces

 

11.1   Multiple-Choice Questions

 

1) Crystalline solids __________.

  1. A) have their particles arranged randomly
  2. B) have highly ordered structures
  3. C) are usually very soft
  4. D) exist only at high temperatures
  5. E) exist only at very low temperatures

Answer:  B

Diff: 1      Page Ref: Sec. 11.1

 

2) In liquids, the attractive intermolecular forces are __________.

  1. A) very weak compared with kinetic energies of the molecules
  2. B) strong enough to hold molecules relatively close together
  3. C) strong enough to keep the molecules confined to vibrating about their fixed lattice points
  4. D) not strong enough to keep molecules from moving past each other
  5. E) strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other

Answer:  E

Diff: 2      Page Ref: Sec. 11.1

 

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

  1. A) more separated, more
  2. B) more separated, less
  3. C) closer together, more
  4. D) closer together, less
  5. E) larger, greater

Answer:  B

Diff: 2      Page Ref: Sec. 11.1

 

4) As a gaseous element condenses, the atoms become __________ and they have __________ attraction for one another.

  1. A) more separated, more
  2. B) more separated, less
  3. C) closer together, more
  4. D) closer together, less
  5. E) larger, greater

Answer:  C

Diff: 2      Page Ref: Sec. 11.1

 

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

  1. A) compressible, the volume and shape, not compressible, the shape of a portion
  2. B) compressible, the shape, not compressible, the volume and shape
  3. C) compressible, the volume and shape, compressible, the volume
  4. D) condensed, the volume and shape, condensed, the volume and shape
  5. E) condensed, the shape, compressible, the volume and shape

Answer:  A

Diff: 1      Page Ref: Sec. 11.1

 

6) Together, liquids and solids constitute __________ phases of matter.

  1. A) the compressible
  2. B) the fluid
  3. C) the condensed
  4. D) all of the
  5. E) the disordered

Answer:  C

Diff: 1      Page Ref: Sec. 11.1

 

7) Which statement is true about liquids but not true about solids?

  1. A) They flow and are highly ordered.
  2. B) They are highly ordered and not compressible.
  3. C) They flow and are compressible.
  4. D) They assume both the volume and the shape of their containers.
  5. E) They flow and are not compressible.

Answer:  E

Diff: 2      Page Ref: Sec. 11.1

 

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

  1. A) solid, liquid
  2. B) solid, gas
  3. C) liquid, gas
  4. D) liquidRemember,lid
  5. E) gasRemember,lid

Answer:  B

Diff: 1      Page Ref: Sec. 11.1

9) Which one of the following exhibits dipole-dipole attraction between molecules?

  1. A) XeF4
  2. B) AsH3
  3. C) CO2
  4. D) BCl3
  5. E) Cl2

Answer:  B

Diff: 3      Page Ref: Sec. 11.2

 

10) Which one of the following exhibits dipole-dipole attraction between molecules?

  1. A) PH3
  2. B) CCl4
  3. C) Br2
  4. D) CO2
  5. E) C10H22

Answer:  A

Diff: 3      Page Ref: Sec. 11.2

 

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

  1. A) CH3OH
  2. B) NH3
  3. C) H2S
  4. D) CH4
  5. E) HCl

Answer:  D

Diff: 2      Page Ref: Sec. 11.2

 

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

  1. A) H2O
  2. B) CCl4
  3. C) HF
  4. D) CH3COOH
  5. E) PH3

Answer:  B

Diff: 2      Page Ref: Sec. 11.2

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

  1. A) CH3OH
  2. B) NH3
  3. C) H2S
  4. D) Kr
  5. E) HCl

Answer:  D

Diff: 2      Page Ref: Sec. 11.2

 

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

  1. A) PH3
  2. B) H2S
  3. C) HCl
  4. D) SiH4
  5. E) H2O

Answer:  D

Diff: 3      Page Ref: Sec. 11.2

 

15) Which one of the following should have the lowest boiling point?

  1. A) CH3OH
  2. B) H2S
  3. C) NH3
  4. D) HCl
  5. E) CH4

Answer:  E

Diff: 3      Page Ref: Sec. 11.2

 

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

  1. A) H2O
  2. B) CO2
  3. C) CH4
  4. D) Kr
  5. E) NH3

Answer:  A

Diff: 3      Page Ref: Sec. 11.2

17) Of the following substances, __________ has the highest boiling point.

  1. A) CH3CH2OH
  2. B) C2H6
  3. C) N2
  4. D) F2
  5. E) HOCH2CH2OH

Answer:  E

Diff: 3      Page Ref: Sec. 11.2

 

18) Of the following, __________ has the highest boiling point.

  1. A) N2
  2. B) Br2
  3. C) H2
  4. D) Cl2
  5. E) O2

Answer:  B

Diff: 3      Page Ref: Sec. 11.2

 

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

  1. A) CH4
  2. B) C5H11OH
  3. C) C6H13NH2
  4. D) CH3OH
  5. E) CO2

Answer:  D

Diff: 3      Page Ref: Sec. 11.2

 

20) Which of the following has dispersion forces as its only intermolecular force?

  1. A) CH4
  2. B) HCl
  3. C) C6H13NH2
  4. D) NaCl
  5. E) CH3Cl

Answer:  A

Diff: 2      Page Ref: Sec. 11.2

21) When NaCl dissolves in water, aqueous Na+ and Cl- ions result. The force of attraction that exists between Na+ and H2O is called a(n) __________ interaction.

  1. A) dipole-dipole
  2. B) ion-ion
  3. C) hydrogen bonding
  4. D) ion-dipole
  5. E) London dispersion force

Answer:  D

Diff: 2      Page Ref: Sec. 11.2

 

22) __________ are particularly polarizable.

  1. A) Small nonpolar molecules
  2. B) Small polar molecules
  3. C) Large nonpolar molecules
  4. D) Large polar molecules
  5. E) Large molecules, regardless of their polarity,

Answer:  E

Diff: 2      Page Ref: Sec. 11.2

 

23) The ease with which the charge distribution in a molecule can be distorted by an external electrical field is called the __________.

  1. A) electronegativity
  2. B) hydrogen bonding
  3. C) polarizability
  4. D) volatility
  5. E) viscosity

Answer:  C

Diff: 1      Page Ref: Sec. 11.2

 

24) Which one of the following derivatives of ethane has the highest boiling point?

  1. A) C2Br6
  2. B) C2F6
  3. C) C2I6
  4. D) C2Cl6
  5. E) C2H6

Answer:  C

Diff: 2      Page Ref: Sec. 11.2

25) What is the predominant intermolecular force in CBr4?

  1. A) London-dispersion forces
  2. B) ion-dipole attraction
  3. C) ionic bonding
  4. D) dipole-dipole attraction
  5. E) hydrogen-bonding

Answer:  A

Diff: 2      Page Ref: Sec. 11.2

 

26) What is the predominant intermolecular force in CH3CH2OH?

  1. A) London-dispersion forces
  2. B) ion-dipole attraction
  3. C) ionic bonding
  4. D) induced dipole-dipole attraction
  5. E) hydrogen-bonding

Answer:  E

Diff: 2      Page Ref: Sec. 11.2

 

27) The intermolecular force(s) responsible for the fact that CH4 has the lowest boiling point in the set CH4, SiH4, GeH4, SnH4 is/are __________.

  1. A) hydrogen bonding
  2. B) dipole-dipole interactions
  3. C) London dispersion forces
  4. D) mainly hydrogen bonding but also dipole-dipole interactions
  5. E) mainly London-dispersion forces but also dipole-dipole interactions

Answer:  C

Diff: 2      Page Ref: Sec. 11.2

 

28) 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. A) London dispersion forces
  2. B) dipole-dipole rejections
  3. C) ionic-dipole interactions
  4. D) covalent-ionic interactions
  5. E) dipole-dipole attractions

Answer:  A

Diff: 2      Page Ref: Sec. 11.2

 

29) Hydrogen bonding is a special case of __________.

  1. A) London-dispersion forces
  2. B) ion-dipole attraction
  3. C) dipole-dipole attractions
  4. D) ion-ion interactions
  5. E) none of the above

Answer:  C

Diff: 1      Page Ref: Sec. 11.2

 

30) Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?

 

  1. A)

 

  1. B)

 

  1. C)

 

  1. D)

 

  1. E)

 

Answer:  D

Diff: 2      Page Ref: Sec. 11.2

 

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

  1. A)

 

  1. B)

 

 

  1. C)

 

  1. D)

 

  1. E)

 

Answer:  A

Diff: 2      Page Ref: Sec. 11.2

 

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

  1. A) London dispersion forces
  2. B) dipole-dipole forces
  3. C) ion-dipole forces
  4. D) hydrogen bonding
  5. E) ionic bonding

Answer:  D

Diff: 1      Page Ref: Sec. 11.2

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

  1. A) London dispersion forces
  2. B) ion-dipole forces
  3. C) ionic bonding
  4. D) dipole-dipole forces
  5. E) hydrogen bonding

Answer:  E

Diff: 2      Page Ref: Sec. 11.2

 

34) The predominant intermolecular force in AsH3 is __________.

  1. A) London dispersion forces
  2. B) ion-dipole forces
  3. C) ionic bonding
  4. D) dipole-dipole forces
  5. E) hydrogen bonding

Answer:  D

Diff: 2      Page Ref: Sec. 11.2

 

35) C12H26 molecules are held together by __________.

  1. A) ion-ion interactions
  2. B) hydrogen bonding
  3. C) ion-dipole interactions
  4. D) dipole-dipole interactions
  5. E) dispersion forces

Answer:  E

Diff: 2      Page Ref: Sec. 11.2

 

36) Which of the following molecules has hydrogen bonding as its only intermolecular force?

  1. A) HF
  2. B) H2O
  3. C) C6H13NH2
  4. D) C5H11OH
  5. E) None, all of the above exhibit dispersion forces.

Answer:  E

Diff: 2      Page Ref: Sec. 11.2

37) Which of the following molecules has hydrogen bonding as its only intermolecular force?

  1. A) NH3
  2. B) H2O
  3. C) C3H7OH
  4. D) HOCH2CH2OH
  5. E) None, all of the above exhibit dispersion forces.

Answer:  E

Diff: 2      Page Ref: Sec. 11.2

 

38) What types of intermolecular forces exist between HI and H2S?

  1. A) dipole-dipole and ion-dipole
  2. B) dispersion forces, dipole-dipole, and ion-dipole
  3. C) dispersion forces, hydrogen bonding, dipole-dipole, and ion-dipole
  4. D) dispersion forces and dipole-dipole
  5. E) dispersion forces, dipole-dipole, and ion-dipole

Answer:  D

Diff: 3      Page Ref: Sec. 11.2

 

39) What type(s) of intermolecular forces exist between Br2 and CCl4?

  1. A) dispersion forces
  2. B) dispersion forces and ion-dipole
  3. C) dispersion forces and dipole-dipole
  4. D) dispersion forces, ion-dipole, and dipole-dipole
  5. E) None. Since both are gases at room temperature, they do not interact with each other.

Answer:  A

Diff: 3      Page Ref: Sec. 11.2

 

40) What type(s) of intermolecular forces exist between Cl2 and CO3-2?

  1. A) dispersion forces
  2. B) dispersion forces and ion-dipole
  3. C) dispersion forces, ion-dipole, and induced dipole – induced dipole
  4. D) dispersion forces and ion-induced dipole
  5. E) dispersion forces, ion-dipole, dipole-dipole, and ion-induced dipole

Answer:  D

Diff: 3      Page Ref: Sec. 11.2

41) What types of intermolecular forces exist between NH3 and CBr4?

  1. A) dispersion forces and dipole-dipole forces
  2. B) dispersion forces and dipole-induced dipole forces
  3. C) dispersion forces and hydrogen bonds
  4. D) dispersion forces, hydrogen bonds, and induced dipole-induced dipole forces
  5. E) dispersion forces, hydrogen bonds, and dipole-induced dipole forces

Answer:  B

Diff: 3      Page Ref: Sec. 11.2

 

42) What types of intermolecular forces exist between PH3 and N2?

  1. A) dispersion forces and dipole-dipole forces
  2. B) dispersion forces and dipole-induced dipole forces
  3. C) dispersion forces and hydrogen bonds
  4. D) dispersion forces, hydrogen bonds, and induced dipole-induced dipole forces
  5. E) dispersion forces, hydrogen bonds, and dipole-induced dipole forces

Answer:  B

Diff: 3      Page Ref: Sec. 11.2

 

43) __________ is the energy required to expand the surface area of a liquid by a unit amount of area.

  1. A) Viscosity
  2. B) Surface tension
  3. C) Volatility
  4. D) Meniscus
  5. E) Capillary action

Answer:  B

Diff: 2      Page Ref: Sec. 11.3

 

44) 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. A) (i) only
  2. B) (ii) and (iii)
  3. C) (i) and (iii)
  4. D) none
  5. E) all

Answer:  E

Diff: 3      Page Ref: Sec. 11.3

45) The shape of a liquid’s meniscus is determined by __________.

  1. A) the viscosity of the liquid
  2. B) the type of material the container is made of
  3. C) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container
  4. D) the amount of hydrogen bonding in the liquid
  5. E) the volume of the liquid

Answer:  C

Diff: 2      Page Ref: Sec. 11.3

 

46) Viscosity is __________.

  1. A) the “skin” on a liquid surface caused by intermolecular attraction
  2. B) the resistance to flow
  3. C) the same as density
  4. D) inversely proportional to molar mass
  5. E) unaffected by temperature

Answer:  B

Diff: 2      Page Ref: Sec. 11.3

 

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

  1. A) the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube, and gravity
  2. B) gravity alone
  3. C) only the magnitude of adhesive forces between the liquid and the tube
  4. D) the viscosity of the liquid
  5. E) only the magnitude of cohesive forces in the liquid

Answer:  A

Diff: 2      Page Ref: Sec. 11.3

 

48) The property responsible for the “beading up” of water is __________.

  1. A) density
  2. B) viscosity
  3. C) vapor pressure
  4. D) surface tension
  5. E) hydrogen bonding

Answer:  D

Diff: 2      Page Ref: Sec. 11.3

 

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

  1. A) heat of fusion, heat of condensation
  2. B) heat of fusion, heat of vaporization
  3. C) heat of freezing (solidification), heat of condensation
  4. D) heat of freezing (solidification), heat of vaporization
  5. E) heat of deposition, heat of vaporization

Answer:  B

Diff: 2      Page Ref: Sec. 11.4

 

50) Which of the following statements is false?

  1. A) The absolute value of the heat of sublimation is equal to the absolute value of the heat of deposition.
  2. B) The heat of sublimation is equal to the sum of the heat of vaporization and the heat of melting.
  3. C) The heat of sublimation is equal to the sum of the heat of vaporization and the heat of freezing.
  4. D) 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.
  5. E) 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.

Answer:  C

Diff: 3      Page Ref: Sec. 11.4

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

  1. A) increase distances between molecules
  2. B) break intramolecular bonds
  3. C) rearrange atoms within molecules
  4. D) increase the velocity of molecules
  5. E) increase the density of the sample

Answer:  A

Diff: 3      Page Ref: Sec. 11.4

 

52) Based on the following information, which compound has the strongest intermolecular forces?

 

Substance                                                                   ΔHvap(kJ/mol)

                                    Argon (Ar)                                                                             6.3

Benzene (C6H6)                                                                     31.0

Ethanol (C2H5OH)                                                                 39.3

Water (H2O)                                                                           40.8

Methane (CH4)                                                                       9.2

 

  1. A) Argon
  2. B) Benzene
  3. C) Ethanol
  4. D) Water
  5. E) Methane

Answer:  D

Diff: 2      Page Ref: Sec. 11.4

53) Which compound has the strongest intermolecular forces?

  1. A) CBr4
  2. B) C12H26
  3. C) CI4
  4. D) N2
  5. E) O2

Answer:  C

Diff: 2      Page Ref: Sec. 11.4

 

54) Large intermolecular forces in a substance are manifested by __________.

  1. A) low vapor pressure
  2. B) high boiling point
  3. C) high heats of fusion and vaporization
  4. D) high critical temperatures and pressures
  5. E) all of the above

Answer:  E

Diff: 2      Page Ref: Sec. 11.4

 

55) 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. A) plasma
  2. B) gas
  3. C) liquid
  4. D) amorphous solid
  5. E) supercritical fluid and gas

Answer:  E

Diff: 2      Page Ref: Sec. 11.4

 

56) 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. A) solid
  2. B) liquid
  3. C) liquid and gas
  4. D) gas
  5. E) supercritical fluid

Answer:  E

Diff: 2      Page Ref: Sec. 11.4

57) The substance with the largest heat of vaporization is __________.

  1. A) I2
  2. B) Br2
  3. C) Cl2
  4. D) F2
  5. E) O2

Answer:  A

Diff: 3      Page Ref: Sec. 11.4

 

58) Of the following, __________ is an exothermic process.

  1. A) melting
  2. B) subliming
  3. C) freezing
  4. D) boiling
  5. E) All of the above are exothermic.

Answer:  C

Diff: 2      Page Ref: Sec. 11.4

 

59) Of the following, __________ should have the highest critical temperature.

  1. A) CBr4
  2. B) CCl4
  3. C) CF4
  4. D) CH4
  5. E) H2

Answer:  A

Diff: 3      Page Ref: Sec. 11.4

 

60) Of the following, __________ is the most volatile.

  1. A) CBr4
  2. B) CCl4
  3. C) CF4
  4. D) CH4
  5. E) C6H14

Answer:  D

Diff: 3      Page Ref: Sec. 11.5

 

61) Of the following, __________ is the least volatile.

  1. A) CBr4
  2. B) CCl4
  3. C) CF4
  4. D) CH4
  5. E) C6H14

Answer:  A

Diff: 3      Page Ref: Sec. 11.5

 

62) A volatile liquid is one that __________.

  1. A) is highly flammable
  2. B) is highly viscous
  3. C) is highly hydrogen-bonded
  4. D) is highly cohesive
  5. E) readily evaporates

Answer:  E

Diff: 1      Page Ref: Sec. 11.5

 

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

  1. A) surface tension
  2. B) molecular weight
  3. C) hydrogen bonding
  4. D) viscosity
  5. E) temperature

Answer:  E

Diff: 1      Page Ref: Sec. 11.5

 

64) The vapor pressure of any substance at its normal boiling point is

  1. A) 1 Pa
  2. B) 1 torr
  3. C) 1 atm
  4. D) equal to atmospheric pressure
  5. E) equal to the vapor pressure of water

Answer:  C

Diff: 1      Page Ref: Sec. 11.5

 

65) Volatility and vapor pressure are __________.

  1. A) inversely proportional to one another
  2. B) directly proportional to one another
  3. C) not related
  4. D) the same thing
  5. E) both independent of temperature

Answer:  B

Diff: 2      Page Ref: Sec. 11.5

 

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

  1. A) water boils at a lower temperature at high altitude than at low altitude
  2. B) water boils at a higher temperature at high altitude than at low altitude
  3. C) heat isn’t conducted as well in low density air
  4. D) natural gas flames don’t burn as hot at high altitudes
  5. E) there is a higher moisture content in the air at high altitude

Answer:  A

Diff: 2      Page Ref: Sec. 11.5

 

67) The vapor pressure of a liquid __________.

  1. A) increases linearly with increasing temperature
  2. B) increases nonlinearly with increasing temperature
  3. C) decreases linearly with increasing temperature
  4. D) decreases nonlinearly with increasing temperature
  5. E) is totally unrelated to its molecular structure

Answer:  B

Diff: 2      Page Ref: Sec. 11.5

 

68) The slope of a plot of the natural log of the vapor pressure of a substance versus 1/T is __________.

  1. A) ΔHvap
  2. B) -ΔHvap
  3. C)
  4. D)
  5. E)

Answer:  D

Diff: 4      Page Ref: Sec. 11.5

 

69) On a phase diagram, the critical pressure is __________.

  1. A) the pressure required to melt a solid
  2. B) the pressure below which a substance is a solid at all temperatures
  3. C) the pressure above which a substance is a liquid at all temperatures
  4. D) the pressure at which a liquid changes to a gas
  5. E) the pressure required to liquefy a gas at its critical temperature

Answer:  E

Diff: 2      Page Ref: Sec. 11.6

70) On a phase diagram, the critical temperature is __________.

  1. A) the temperature below which a gas cannot be liquefied
  2. B) the temperature above which a gas cannot be liquefied
  3. C) the temperature at which all three states are in equilibrium
  4. D) the temperature required to melt a solid
  5. E) the temperature required to cause sublimation of a solid

Answer:  B

Diff: 2      Page Ref: Sec. 11.6

 

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

  1. A) the triple point
  2. B) the critical point
  3. C) the freezing point
  4. D) the boiling point
  5. E) the vapor-pressure curve

Answer:  C

Diff: 1      Page Ref: Sec. 11.6

 

72) 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. A) can go from solid to liquid, within a small temperature range, via the application of pressure
  2. B) sublimes rather than melts under ordinary conditions
  3. C) cannot go from solid to liquid by application of pressure at any temperature
  4. D) cannot be liquefied above its triple point
  5. E) melts rather than sublimes under ordinary conditions

Answer:  A

Diff: 2      Page Ref: Sec. 11.6

 

73) The predominant intermolecular force in CaBr2 is __________.

  1. A) London-dispersion forces
  2. B) ion-dipole forces
  3. C) ionic bonding
  4. D) dipole-dipole forces
  5. E) hydrogen bonding

Answer:  C

Diff: 2      Page Ref: Sec. 11.7

74) Which of the following is most likely to exhibit liquid-crystalline behavior?

  1. A) CH3CH2-C(CH3)2-CH2CH3

 

  1. B) CH3CH2CH2CH2CH2CH2CH2CH3

 

  1. C) CH3CH2CH2CH2CH2-Na+

 

  1. D)
  2. E)

Answer:  E

Diff: 2      Page Ref: Sec. 11.7

 

75) Which of the following characteristics would prevent liquid crystal behavior?

  1. A) long axial structure
  2. B) ionic configuration
  3. C) carbon-carbon single bonds
  4. D) double bonding
  5. E) polar groups

Answer:  B

Diff: 1      Page Ref: Sec. 11.7

 

76) In the smectic A liquid-crystalline phase, __________.

  1. A) the molecules are aligned along their long axes, with no ordering with respect to the ends of the molecules
  2. B) the molecules are arranged in sheets, with their long axes parallel and their ends aligned as well
  3. C) the molecules are aligned with their long axes tilted with respect to a line perpendicular to the plane in which the molecules are stacked
  4. D) disk-shaped molecules are aligned through a stacking of the disks in layers
  5. E) the molecules are oriented in a totally random fashion

Answer:  B

Diff: 2      Page Ref: Sec. 11.7

77) In the __________ liquid crystalline phase, the component molecules exhibit only one dimensional ordering.

  1. A) nematic
  2. B) smectic A
  3. C) smectic B
  4. D) smectic C
  5. E) cholesteric

Answer:  A

Diff: 5      Page Ref: Sec. 11.7

 

78) In the ________ liquid crystalline phase, the component molecules are aligned along their long axis and are arranged in layers with the molecules in each plane twisted slightly in relation to the molecules in the planes above and below.

  1. A) nematic
  2. B) smectic A
  3. C) smectic B
  4. D) smectic C
  5. E) cholesteric

Answer:  E

Diff: 5      Page Ref: Sec. 11.7

 

79) Cholesteric liquid crystals are colored because __________.

  1. A) each molecule is a chromophore
  2. B) of the slight twist between layers
  3. C) of the large spacing between layers
  4. D) of the large number of conjugated bonds
  5. E) all of the molecules contain multiple benzene rings

Answer:  B

Diff: 1      Page Ref: Sec. 11.7

 

80) Molecules with only single bonds do not generally exhibit liquid-crystalline properties because __________.

  1. A) molecules without multiple bonds lack the rigidity necessary for alignment
  2. B) molecules without multiple bonds are too small to exhibit liquid-crystalline properties
  3. C) molecules with only single bonds are gases
  4. D) molecules with only single bonds are too big to exhibit liquid-crystalline properties
  5. E) molecules without multiple bonds lack the flexibility necessary for alignment

Answer:  A

Diff: 1      Page Ref: Sec. 11.7

81) For a given substance that exhibits liquid-crystalline properties, the transition from solid to liquid-crystal state occurs __________.

  1. A) over a range of temperatures between the melting point of the solid and the boiling point of the liquid
  2. B) at the melting point of the solid
  3. C) over a range of temperatures that includes the melting point of the solid
  4. D) at a well defined temperature above the melting point of the solid
  5. E) at a well defined temperature below the melting point of the solid

Answer:  B

Diff: 1      Page Ref: Sec. 11.7

 

82) For a given substance that exhibits liquid-crystalline properties, the liquid-crystalline state exists __________.

  1. A) at one particular temperature below the melting point of the solid
  2. B) in a range of temperatures below the melting point of the solid
  3. C) at one particular temperature above the melting point of the solid
  4. D) in a range of temperatures above the melting point of the solid
  5. E) in a range of temperatures from below the melting point to above the melting point

Answer:  D

Diff: 2      Page Ref: Sec. 11.7

 

11.2   Bimodal Questions

 

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

 

 

 

  1. A) CH3CH2CH3
  2. B) CH3OCH3
  3. C) CH3Cl
  4. D) CH3CHO
  5. E) CH3CN

Answer:  E

Diff: 3      Page Ref: Sec. 11.2

 

2) 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. A) AB
  2. B) BC
  3. C) CD
  4. D) DE
  5. E) EF

Answer:  C

Diff: 1      Page Ref: Sec. 11.4

 

3) 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. A) AB
  2. B) BC
  3. C) CD
  4. D) DE
  5. E) EF

Answer:  A

Diff: 1      Page Ref: Sec. 11.4

4) 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. A) AB
  2. B) BC
  3. C) CD
  4. D) DE
  5. E) EF

Answer:  E

Diff: 1      Page Ref: Sec. 11.4

 

5) 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. A) AB
  2. B) BC
  3. C) CD
  4. D) DE
  5. E) EF

Answer:  D

Diff: 2      Page Ref: Sec. 11.4

 

6) 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 ΔHfusion of this substance.

  1. A) AB
  2. B) BC
  3. C) CD
  4. D) DE
  5. E) EF

Answer:  B

Diff: 2      Page Ref: Sec. 11.4

7) 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. A) AB
  2. B) AC
  3. C) AD
  4. D) CD
  5. E) BC

Answer:  B

Diff: 2      Page Ref: Sec. 11.6

 

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

  1. A) A
  2. B) B
  3. C) C
  4. D) D
  5. E) E

Answer:  B

Diff: 2      Page Ref: Sec. 11.6

 

9) On the phase diagram shown above, the coordinates of point __________ correspond to the triple point.

  1. A) A
  2. B) B
  3. C) C
  4. D) D
  5. E) E

Answer:  A

Diff: 2      Page Ref: Sec. 11.6

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

  1. A) w
  2. B) x
  3. C) y
  4. D) z
  5. E) x and y

Answer:  A

Diff: 2      Page Ref: Sec. 11.6

 

 

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

  1. A) 10
  2. B) 20
  3. C) 30
  4. D) 40
  5. E) 50

Answer:  D

Diff: 2      Page Ref: Sec. 11.6

12) The normal melting point of the substance with the phase diagram shown above is __________°C.

  1. A) 15
  2. B) 25
  3. C) 35
  4. D) 45
  5. E) 55

Answer:  A

Diff: 2      Page Ref: Sec. 11.6

 

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

  1. A) w
  2. B) x
  3. C) y
  4. D) z
  5. E) y and z

Answer:  C

Diff: 2      Page Ref: Sec. 11.6

 

14) The phase diagram of a substance is shown above. The area labeled __________ indicates the solid phase for the substance.

  1. A) w
  2. B) x
  3. C) y
  4. D) z
  5. E) y and z

Answer:  A

Diff: 2      Page Ref: Sec. 11.6

15) The phase diagram of a substance is shown above. The area labeled __________ indicates the liquid phase for the substance.

  1. A) w
  2. B) x
  3. C) y
  4. D) z
  5. E) y and z

Answer:  B

Diff: 2      Page Ref: Sec. 11.6

 

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

  1. A) -3
  2. B) 10
  3. C) 29
  4. D) 38
  5. E) 0

Answer:  C

Diff: 2      Page Ref: Sec. 11.6

 

17) According to the phase diagram shown above, the normal melting point of this substance is __________°C.

  1. A) -13
  2. B) 10
  3. C) 29
  4. D) 38
  5. E) 0

Answer:  E

Diff: 2      Page Ref: Sec. 11.6

 

18) A __________ liquid crystal has the least order and is the most liquid-like.

  1. A) nematic
  2. B) smectic
  3. C) cholesteric
  4. D) smectic B
  5. E) smectic C

Answer:  A

Diff: 1      Page Ref: Sec. 11.7

19) Which type of liquid crystal is colored and changes color with temperature?

  1. A) nematic
  2. B) smectic A
  3. C) cholesteric
  4. D) smectic B
  5. E) smectic C

Answer:  C

Diff: 1      Page Ref: Sec. 11.7

 

11.3   Algorithmic Questions

 

1) 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. A) 12.28
  2. B) 6.41
  3. C) 13.16
  4. D) 7154
  5. E) 9.40

Answer:  C

Diff: 3      Page Ref: Sec. 11.4

 

2) 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 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. A) 12.28
  2. B) 6.16
  3. C) 3870
  4. D) 7.21
  5. E) 9.88

Answer:  D

Diff: 3      Page Ref: Sec. 11.4

 

3) 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 10.0°C requires __________ kJ of heat.

  1. A) 2110
  2. B) 18.8
  3. C) 2.11
  4. D) 16.7
  5. E) Insufficient data are given.

Answer:  B

Diff: 3      Page Ref: Sec. 11.4

4) Calculate the enthalpy change (in kJ) associated with the conversion of 25.0 grams of ice at -4.00°C to water vapor at 106.0°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. A) 64.8
  2. B) 75.8
  3. C) 11000
  4. D) 12000
  5. E) 112

Answer:  B

Diff: 3      Page Ref: Sec. 11.4

 

5) 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. A) 207.3
  2. B) -12.7
  3. C) 6.91
  4. D) 4192
  5. E) 9.21

Answer:  C

Diff: 4      Page Ref: Sec. 11.4

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

  1. A) 10
  2. B) 20
  3. C) 30
  4. D) 40
  5. E) 0

Answer:  D

Diff: 3      Page Ref: Sec. 11.5

 

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

  1. A) 80
  2. B) 60
  3. C) 70
  4. D) 40
  5. E) 20

Answer:  E

Diff: 3      Page Ref: Sec. 11.5

8) Based on the figure above, the boiling point of water under an external pressure of 0.493 atm is __________°C.

  1. A) 80
  2. B) 40
  3. C) 60
  4. D) 70
  5. E) 90

Answer:  A

Diff: 3      Page Ref: Sec. 11.5

 

9) The phase diagram of a substance is given above. This substance is a __________ at -10°C and 1.0 atm.

  1. A) liquid
  2. B) solid
  3. C) gas
  4. D) supercritical fluid
  5. E) crystal

Answer:  B

Diff: 2      Page Ref: Sec. 11.6

 

11.4   Short Answer Questions

 

1) In general, intramolecular forces determine the __________ properties of a substance and intermolecular forces determine its __________ properties.

Answer:  chemical, physical

Diff: 2      Page Ref: Sec. 11.1

 

2) London Dispersion Forces tend to __________ in strength with increasing molecular weight.

Answer:  increase

Diff: 1      Page Ref: Sec. 11.2

3) The direct conversion of a solid to a gas is called __________.

Answer:  sublimation

Diff: 1      Page Ref: Sec. 11.4

 

4) The initial discovery of a liquid crystal resulted from studies on what compound?

Answer:  cholesteryl benzoate

Diff: 2      Page Ref: Sec. 11.7

 

11.5   True/False Questions

 

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.

Answer:  FALSE

Diff: 2      Page Ref: Sec. 11.2

 

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.

Answer:  TRUE

Diff: 2      Page Ref: Sec. 11.2

 

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

Answer:  TRUE

Diff: 1      Page Ref: Sec. 11.4

 

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

Answer:  TRUE

Diff: 2      Page Ref: Sec. 11.6

 

5) Molecules containing only single bonds do not exhibit liquid-crystal behavior because free rotation can occur around single bonds making these molecules flexible.

Answer:  TRUE

Diff: 2      Page Ref: Sec. 11.7

 

Reviews

There are no reviews yet.

Be the first to review “Chemistry The Central Science 12th Edition Brown LeMay Bursten Test Bank”

Your email address will not be published. Required fields are marked *