Question 1

Consider the melting point of the following solids.Which of these solids is most likely a network solid?

Accepted Answer

A)  SiF4, -90oC
B)  CO2, -57oC
C)  BN, 3000oC
D)  KBr, 734oC
E)  GeBr4, 26oC

Question 2

Which substance has the highest melting point?

Accepted Answer

A)  Cu
B)  C6H14 
C)  Rn
D)  C (graphite) 
E)  I2

Question 3

Which of the following is not an attractive force that acts between the individual molecules of CH3OH?

Accepted Answer

A)  London dispersion forces
B)  dipole-dipole forces
C)  hydrogen-bonding forces
D)  covalent bonds
E)  none of these is correct

Question 4

What phase transition is occurring between points B and C on the heating curve?

Accepted Answer

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

Question 5

Identify the type of solid shown in the image.

Accepted Answer

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

Question 6

The atmospheric pressure on Mount Everest is about 0.30 atm.From the vapor pressure curve of propane, it can be seen the boiling point of propane at this elevation is about _________. oC B) -120oC C) -67oC D) -42oC E) 0oC" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  -137oC
B)  -120oC
C)  -67oC
D)  -42oC
E)  0oC

Question 7

Identify the type of solid shown in the image.

Accepted Answer

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

Question 8

Select the pair of substances which has the one with the higher equilibrium vapor pressure at a given temperature listed first.

Accepted Answer

A)  H2O, H2S
B)  CH3CH2OH, CH3OH
C)  CH3COCH3, CH3CH2CH2OH
D)  NH3, PH3 
E)  Br2, Cl2

Question 9

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

Accepted Answer

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

Question 10

Which of the following substances is most likely to be a gas at room temperature and atmospheric pressure?

Accepted Answer

A)  Cs
B)  SO2 
C)  I2 
D)  CCl4 
E)  Ni

Question 11

Which of the following statements regarding intermolecular forces is incorrect?

Accepted Answer

A)  An intermolecular force is an attractive force that operates between molecules.
B)  Bonding forces are much stronger than intermolecular forces.
C)  London dispersion forces occur in all atoms and molecules.
D)  London dispersion forces are the result of permanent dipoles in atoms or molecules.
E)  Molecules which have hydrogen bonded to F, O, or N can undergo hydrogen-bonding.

Question 12

Which of the following statements regarding the liquid state is incorrect?

Accepted Answer

A)  Liquids are about 1000 times denser than gases.
B)  Liquids are normally about 90-95% as dense as their corresponding solid.
C)  The viscosity of a liquid is a measure of its resistance to flow.
D)  Molecules with high intermolecular forces will have high surface tension.
E)  Surface tension increases as temperature increases.

Question 13

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

Accepted Answer

A)  melting point.
B)  boiling point.
C)  viscosity.
D)  vapor pressure.
E)  mass.

Question 14

Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5  °\degree° C to water at 24.0  °\degree° C.(Cwater = 4.18 J/g  °\degree° C; Cice = 2.03 J/g  °\degree° C; molar heat of fusion of ice = 6.01 x 103 J/mol)

Accepted Answer

A)  8.88 x 102 J
B)  1.17 x 104 J
C)  1.61 x 1010 J
D)  3.51 x 103 J
E)  1.61 x 104 J

Question 15

Which of the following molecules experience dipole-dipole forces?

Accepted Answer

A)  CO2 
B)  SO2 
C)  CCl4 
D)  H2S
E)  both SO2 and H2S

Question 16

Rank the following substances in order of increasing intermolecular forces: Ar, H2O, N2, O2

Accepted Answer

A)  Ar 2O 2 2 
B)  Ar 2O 2 2 
C)  H2O 2 2 
D)  N2 2 2O
E)  Ar 2 2 2O

Question 17

Which of the following statements is correct?

Accepted Answer

A)  The phase change from solid to liquid is exothermic.
B)  Liquids boil at lower than normal temperatures in Death Valley, since it is below sea level.
C)  A substance with a low boiling point would be expected to have a relatively low vapor pressure at a low temperature.
D)  The phase change from liquid to gas is exothermic.
E)  When a substance condenses, heat energy is given off.

Question 18

Network covalent substances have the highest melting points of all substances.

Accepted Answer

A) True 
 B)False

Question 19

Which of the following has the highest boiling point?

Accepted Answer

A)  H2 
B)  HF
C)  HCl
D)  HBr
E)  HI

Question 20

From the vapor pressure curve of acetone, it can be seen that the normal boiling point of acetone is about _________. oC B) 0oC C) 50oC D) 57oC E) 100oC" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  -50oC
B)  0oC
C)  50oC
D)  57oC
E)  100oC

Exam 10: The Liquid and Solid States

Which of the following substances is most likely to be a gas at room temperature and atmospheric pressure?

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Select the pair of substances which has the one with the higher equilibrium vapor pressure at a given temperature listed first.

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Identify the type of solid shown in the image.

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Which of the following is not an attractive force that acts between the individual molecules of CH3OH?

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

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Rank the following substances in order of increasing intermolecular forces: Ar, H2O, N2, O2

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

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Which substance has the highest melting point?

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Network covalent substances have the highest melting points of all substances.

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Which of the following statements regarding intermolecular forces is incorrect?

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The atmospheric pressure on Mount Everest is about 0.30 atm.From the vapor pressure curve of propane, it can be seen the boiling point of propane at this elevation is about _________.

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Which of the following statements is correct?

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From the vapor pressure curve of acetone, it can be seen that the normal boiling point of acetone is about _________.

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Identify the type of solid shown in the image.

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Which of the following molecules experience dipole-dipole forces?

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Consider the melting point of the following solids.Which of these solids is most likely a network solid?

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Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5 °\degree° C to water at 24.0 °\degree° C.(Cwater = 4.18 J/g °\degree° C; Cice = 2.03 J/g °\degree° C; molar heat of fusion of ice = 6.01 x 103 J/mol)

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Which of the following statements regarding the liquid state is incorrect?

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What phase transition is occurring between points B and C on the heating curve?

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Which of the following has the highest boiling point?

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Which of the following is not an attractive force that acts between the individual molecules of CH₃OH?

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Rank the following substances in order of increasing intermolecular forces: Ar, H₂O, N₂, O₂

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Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5 $\degree$ C to water at 24.0 $\degree$ C.(C_water = 4.18 J/g $\degree$ C; C_ice = 2.03 J/g $\degree$ C; molar heat of fusion of ice = 6.01 x 10³ J/mol)

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