Question 1

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

Question 2

Identify the type of solid shown in the image.

Accepted Answer

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

Question 3

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 _________.

Accepted Answer

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

Question 4

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

Question 5

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. 
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 6

Which of the following has the highest boiling point?

Accepted Answer

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

Question 7

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. 
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 8

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

Question 9

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

Question 10

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

Question 11

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

Question 12

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 
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 13

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

Accepted Answer

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

Question 14

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

Accepted Answer

A) True 
 B)False

Question 15

Which substance has the highest melting point?

Accepted Answer

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

Question 16

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

Question 17

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

Question 18

Which of the following molecules experience dipole-dipole forces?

Accepted Answer

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

Question 19

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. 
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 20

Identify the type of solid shown in the image.

Accepted Answer

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

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

Identify the type of solid shown in the image.

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 _________.

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

Which of the following statements regarding intermolecular forces is incorrect?

Which of the following has the highest boiling point?

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

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

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

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

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

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)

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

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

Which substance has the highest melting point?

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?

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

Which of the following molecules experience dipole-dipole forces?

Which of the following statements is correct?

Identify the type of solid shown in the image.

Matter and Energy

Atoms, Ions, and the Periodic Table

Chemical Compounds

Chemical Composition

Chemical Reactions and Equations

Quantities in Chemical Reactions

Electron Structure of the Atom

Chemical Bonding

The Gaseous State

Solutions

Reaction Rates and Chemical Equilibrium

Acids and Bases

Oxidation-Reduction Reactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

Exam 10: The Liquid and Solid States

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

Identify the type of solid shown in the image.

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 _________.

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

Which of the following statements regarding intermolecular forces is incorrect?

Which of the following has the highest boiling point?

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

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

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

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

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

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)

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

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

Which substance has the highest melting point?

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?

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

Which of the following molecules experience dipole-dipole forces?

Which of the following statements is correct?

Identify the type of solid shown in the image.

Matter and Energy

Atoms, Ions, and the Periodic Table

Chemical Compounds

Chemical Composition

Chemical Reactions and Equations

Quantities in Chemical Reactions

Electron Structure of the Atom

Chemical Bonding

The Gaseous State

Solutions

Reaction Rates and Chemical Equilibrium

Acids and Bases

Oxidation-Reduction Reactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

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

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

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)