Question 1

Rank the following substances in order of increasing boiling point: O2, Ne, Ar, H2

Accepted Answer

A)  O2 2 
B)  O2 2 
C)  H2 2 
D)  H2 2 
E)  Ar 2 2

Question 2

Which of the following statements regarding intermolecular forces is incorrect?

Accepted Answer

A)  Hydrogen bonding is the strongest of the intermolecular forces for substances of similar molar mass.
B)  London dispersion forces are present in all atoms and molecules.
C)  Dipole-dipole forces increase with increasing molecular size.
D)  Bonding forces are much stronger than intermolecular forces.
E)  Hydrogen bonding is the reason for the abnormally high boiling point of water.

Question 3

Which of the following molecules experience dipole-dipole forces?

Accepted Answer

A)  NO2 
B)  CO2 
C)  CBr4 
D)  SO3 
E)  all of these choices are correct

Question 4

The forces that hold CO2 together in the solid state are:

Accepted Answer

A)  ionic bonds.
B)  dipole-dipole forces.
C)  London dispersion forces only.
D)  covalent bonds.
E)  attractions between nuclei and delocalized valence electrons. C

Question 5

Arrange the following substances in order of increasing boiling point: N2, H2, NH3, PH3

Accepted Answer

A)  H2 < N2 < PH3 <  NH3 
B)  N2 < H2 < PH3 <  NH3 
C)  H2 < N2 < NH3 <  PH3 
D)  N2 < PH3 <  NH3 < H2 
E)  NH3 < PH3 <  N2 < H2  A

Question 6

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except:

Accepted Answer

A)  density.
B)  boiling point.
C)  surface tension.
D)  melting point.
E)  mass.

Question 7

Rank the following substances in order of increasing boiling point: F2, Ne, He, Cl2

Accepted Answer

A)  F2 2 
B)  F2 2 
C)  F2 2 
D)  He 2 2 
E)  Cl2 2 < Ne < He

Question 8

The pictured change of state occurs at constant temperature even though heat is being removed.Where does this change of state occur on the cooling curve?

Accepted Answer

A)  AB
B)  BC
C)  CD
D)  DE
E)  EF

Question 9

Which choice correctly lists the intermolecular forces present in CH3NH2?

Accepted Answer

A)  London forces only
B)  dipole-dipole forces only
C)  London forces, dipole-dipole forces, and hydrogen bonding
D)  dipole-dipole forces and hydrogen bonding
E)  hydrogen bonding only

Question 10

A solid substance has a moderate melting point, is fairly soft, and is a nonconductor.This substance is probably a(n)  ________ solid.

Accepted Answer

A)  metallic
B)  ionic
C)  network
D)  nonpolar molecular
E)  polar molecular

Question 11

Three phases of water are shown in the figure.List the terms used to identify the phase changes indicated by the arrows.

Accepted Answer

A)  A = sublimation, B = vaporization, C = freezing
B)  A = vaporization, B = condensation, C = melting
C)  A = vaporization, B = deposition, C = melting
D)  A = sublimation, B = condensation, C = freezing
E)  A = condensation, B = sublimation, C = freezing

Question 12

Rank the following substances in order of increasing intermolecular forces: He, HF, F2, Ne

Accepted Answer

A)  He 2 
B)  He 2 
C)  He 2 
D)  He 2  
E)  HF 2 < He C

Question 13

Identify the type of solid shown in the image.

Accepted Answer

A)  metallic
B)  ionic
C)  network
D)  nonpolar molecular
E)  polar molecular

Question 14

Which of the following substances can participate in hydrogen bonding?

Accepted Answer

A)  CH4 
B)  HF
C)  CH3COCH3 
D)  SiH4 
E)  all of these choices are correct

Question 15

Calculate the amount of heat energy required to convert 55.0 g of water at 62.5oC to steam at 124.0  °\degree° C.(Cwater = 4.18 J/g  °\degree° C; Csteam = 2.02 J/g  °\degree° C; molar heat of vaporization of liquid water = 4.07 x 104 J/mol)

Accepted Answer

A)  2.25 x 103 kJ
B)  1.23 x 102 kJ
C)  0.862 kJ
D)  1.35 x 102 kJ
E)  2.67 kJ

Question 16

Which of the following statements is correct?

Accepted Answer

A)  At the melting point of a substance, the solid, liquid, and gas phases are all in equilibrium.
B)  The freezing point and the melting point of a substance are the same.
C)  There is no fundamental difference in the melting process for covalent substances and ionic substances.
D)  When iodine vapor cools at atmospheric pressure, it condenses to the liquid state.
E)  In order for a substance to go from the liquid phase to the gas phase, it must give off energy to the surroundings.

Question 17

Calculate the amount of heat energy required to melt 25.0 g of ice at 0.0  °\degree° C.(molar heat of fusion of ice = 6.01 x 103 J/mol)

Accepted Answer

A)  1.50 x 102 kJ
B)  8.34 kJ
C)  4.33 kJ
D)  7.50 x 102 kJ
E)  1.50 x 10-1 kJ

Question 18

What phase transition is occurring between points D and E on the heating curve?

Accepted Answer

A)  melting
B)  freezing
C)  evaporation
D)  sublimation
E)  deposition

Question 19

A solid substance has a high melting point, is hard, brittle, and conducts electricity when molten.This substance is probably a(n) ________ solid.

Accepted Answer

A)  metallic
B)  ionic
C)  network
D)  nonpolar molecular
E)  polar molecular

Question 20

Identify the type of solid shown in the image.

Accepted Answer

A)  metallic
B)  ionic
C)  network
D)  molecular
E)  amorphous

Exam 10: The Liquid and Solid States

Rank the following substances in order of increasing boiling point: O2, Ne, Ar, H2

Correct AnswerverifiedShow Answer

Which of the following statements regarding intermolecular forces is incorrect?

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Which of the following molecules experience dipole-dipole forces?

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The forces that hold CO2 together in the solid state are:

Correct AnswerverifiedC

Arrange the following substances in order of increasing boiling point: N2, H2, NH3, PH3

Correct AnswerverifiedA

The physical properties of a substance influenced by the strength of intermolecular forces include all of the following except:

Correct AnswerverifiedShow Answer

Rank the following substances in order of increasing boiling point: F2, Ne, He, Cl2

Correct AnswerverifiedShow Answer

The pictured change of state occurs at constant temperature even though heat is being removed.Where does this change of state occur on the cooling curve?

Correct AnswerverifiedShow Answer

Which choice correctly lists the intermolecular forces present in CH3NH2?

Correct AnswerverifiedShow Answer

A solid substance has a moderate melting point, is fairly soft, and is a nonconductor.This substance is probably a(n) ________ solid.

Correct AnswerverifiedShow Answer

Three phases of water are shown in the figure.List the terms used to identify the phase changes indicated by the arrows.

Correct AnswerverifiedShow Answer

Rank the following substances in order of increasing intermolecular forces: He, HF, F2, Ne

Correct AnswerverifiedC

Identify the type of solid shown in the image.

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Which of the following substances can participate in hydrogen bonding?

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Calculate the amount of heat energy required to convert 55.0 g of water at 62.5oC to steam at 124.0 °\degree° C.(Cwater = 4.18 J/g °\degree° C; Csteam = 2.02 J/g °\degree° C; molar heat of vaporization of liquid water = 4.07 x 104 J/mol)

Correct AnswerverifiedShow Answer

Which of the following statements is correct?

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Calculate the amount of heat energy required to melt 25.0 g of ice at 0.0 °\degree° C.(molar heat of fusion of ice = 6.01 x 103 J/mol)

Correct AnswerverifiedShow Answer

What phase transition is occurring between points D and E on the heating curve?

Correct AnswerverifiedShow Answer

A solid substance has a high melting point, is hard, brittle, and conducts electricity when molten.This substance is probably a(n) ________ solid.

Correct AnswerverifiedShow Answer

Identify the type of solid shown in the image.

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Rank the following substances in order of increasing boiling point: O₂, Ne, Ar, H₂

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The forces that hold CO₂ together in the solid state are:

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C

Arrange the following substances in order of increasing boiling point: N₂, H₂, NH_3,PH₃

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A

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Rank the following substances in order of increasing boiling point: F₂, Ne, He, Cl₂

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Which choice correctly lists the intermolecular forces present in CH₃NH₂?

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Rank the following substances in order of increasing intermolecular forces: He, HF, F₂, Ne

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C

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Calculate the amount of heat energy required to convert 55.0 g of water at 62.5^oC to steam at 124.0 $\degree$ C.(C_water = 4.18 J/g $\degree$ C; C_steam = 2.02 J/g $\degree$ C; molar heat of vaporization of liquid water = 4.07 x 10⁴ J/mol)

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Calculate the amount of heat energy required to melt 25.0 g of ice at 0.0 $\degree$ C.(molar heat of fusion of ice = 6.01 x 10³ J/mol)

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