Question 1

Which of the molecules in the figure has hydrogen bonding in the pure liquid state?

Accepted Answer

A) I only 
B) II only 
C) III only 
D) II and III 
E) I and II 
A) I only 
B) II only 
C) III only 
D) II and III 
E) I and II

Question 2

Which of the following substances can participate in hydrogen bonding?

Accepted Answer

A) SiH4  
B) CH2Cl2  
C) H2O 
D) PH3  
E) both H2O and PH3  
A) SiH4  
B) CH2Cl2  
C) H2O 
D) PH3  
E) both H2O and PH3

Question 3

The forces that hold NH3 together in the solid state are:

Accepted Answer

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

Question 4

Which of the following molecules experience dipole-dipole forces?

Accepted Answer

A) NO 
B) Cl2  
C) CH4  
D) SiH4  
E) all of these 
A) NO 
B) Cl2  
C) CH4  
D) SiH4  
E) all of these

Question 5

A solid substance has a high melting point, is hard, and is a good conductor of both heat and electricity.It is also malleable and ductile.This substance is probably a(n) ________ solid.

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 6

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

Question 7

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

Accepted Answer

A) SiO2, 1610oC 
B) SiC, 2700oC 
C) BN, 3000oC 
D) KBr, 734oC 
E) GeBr4, 26oC 
A) SiO2, 1610oC 
B) SiC, 2700oC 
C) BN, 3000oC 
D) KBr, 734oC 
E) GeBr4, 26oC

Question 8

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

Accepted Answer

A) Ni 
B) Hg 
C) CO2  
D) C7H16  
E) CBr4  
A) Ni 
B) Hg 
C) CO2  
D) C7H16  
E) CBr4

Question 9

Arrange the following substances in order of increasing boiling point: CH3OH, CH4, CH3CH2OH, HOCH2CH2OH

Accepted Answer

A) CH3OH < CH4 < CH3CH2OH < HOCH2CH2OH 
B) CH4 < CH3OH < CH3CH2OH < HOCH2CH2OH 
C) CH4 < CH3OH < HOCH2CH2OH < CH3CH2OH 
D) CH3OH < CH4 < HOCH2CH2OH < CH3CH2OH 
E) HOCH2CH2OH < CH3CH2OH < CH3OH < CH4  
A) CH3OH < CH4 < CH3CH2OH < HOCH2CH2OH 
B) CH4 < CH3OH < CH3CH2OH < HOCH2CH2OH 
C) CH4 < CH3OH < HOCH2CH2OH < CH3CH2OH 
D) CH3OH < CH4 < HOCH2CH2OH < CH3CH2OH 
E) HOCH2CH2OH < CH3CH2OH < CH3OH < CH4

Question 10

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

Accepted Answer

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

Question 11

The diagram represents the physical state of a substance.Where does this physical 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 12

Which of the following has the highest vapor pressure at a given temperature?

Accepted Answer

A) CH4  
B) CF4  
C) CCl4  
D) CBr4  
E) CI4  
A) CH4  
B) CF4  
C) CCl4  
D) CBr4  
E) CI4

Question 13

Which of the molecules in the figure has hydrogen bonding in the pure liquid state?

Accepted Answer

A) I only 
B) II only 
C) III only 
D) II and III 
E) I and II 
A) I only 
B) II only 
C) III only 
D) II and III 
E) I and II

Question 14

One would expect that water is more viscous than C2H6, due to differences in intermolecular forces.

Accepted Answer

A) True 
 B)False

Question 15

Which of the following substances can participate in hydrogen bonding?

Accepted Answer

A) CH4  
B) CHCl3  
C) H2S 
D) NH3  
E) both H2S and NH3  
A) CH4  
B) CHCl3  
C) H2S 
D) NH3  
E) both H2S and NH3

Question 16

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

Question 17

Which of the following statements is correct?

Accepted Answer

A) When the temperature of a sample of liquid is increased, the molecules move faster, but there is no change in the vapor pressure of the sample. 
B) The melting point of metallic sodium is 97.8oC, so at a temperature of 25oC, it is a liquid. 
C) If you cook an egg on a mountain, it will require a short cooking time, due to the high elevation. 
D) When liquids evaporate, it requires an input of energy from the surroundings, so the surroundings become warm. 
E) Nitrogen gas has a boiling point of -196oC, so if it is cooled to -200oC, it condenses. 
A) When the temperature of a sample of liquid is increased, the molecules move faster, but there is no change in the vapor pressure of the sample. 
B) The melting point of metallic sodium is 97.8oC, so at a temperature of 25oC, it is a liquid. 
C) If you cook an egg on a mountain, it will require a short cooking time, due to the high elevation. 
D) When liquids evaporate, it requires an input of energy from the surroundings, so the surroundings become warm. 
E) Nitrogen gas has a boiling point of -196oC, so if it is cooled to -200oC, it condenses.

Question 18

Which of the following is not one of the classifications into which solids can be organized?

Accepted Answer

A) metallic 
B) ionic 
C) molecular 
D) liquid crystals 
E) network 
A) metallic 
B) ionic 
C) molecular 
D) liquid crystals 
E) network

Question 19

Which substance has the highest melting point?

Accepted Answer

A) Mn 
B) C8H18  
C) Ar 
D) C (diamond) 
E) Br2  
A) Mn 
B) C8H18  
C) Ar 
D) C (diamond) 
E) Br2

Question 20

Calculate the amount of heat energy required to evaporate 55.0 g of water at 100.0 $\degree$C.(molar heat of vaporization of liquid water = 4.07 x 104 J/mol)

Accepted Answer

A) 1.24 x 102 kJ 
B) 2.24 x 103 kJ 
C) 4.03 x 104 kJ 
D) 1.24 x 108 kJ 
E) 2.43 x 10-2 kJ 
A) 1.24 x 102 kJ 
B) 2.24 x 103 kJ 
C) 4.03 x 104 kJ 
D) 1.24 x 108 kJ 
E) 2.43 x 10-2 kJ

Which of the molecules in the figure has hydrogen bonding in the pure liquid state?

Which of the following substances can participate in hydrogen bonding?

The forces that hold NH₃ together in the solid state are:

Which of the following molecules experience dipole-dipole forces?

A solid substance has a high melting point, is hard, and is a good conductor of both heat and electricity.It is also malleable and ductile.This substance is probably a(n) ________ solid.

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

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

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

Arrange the following substances in order of increasing boiling point: CH₃OH, CH₄, CH₃CH₂OH, HOCH₂CH₂OH

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

The diagram represents the physical state of a substance.Where does this physical state occur on the cooling curve?

Which of the following has the highest vapor pressure at a given temperature?

Which of the molecules in the figure has hydrogen bonding in the pure liquid state?

One would expect that water is more viscous than C₂H₆, due to differences in intermolecular forces.

Which of the following substances can participate in hydrogen bonding?

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?

Which of the following statements is correct?

Which of the following is not one of the classifications into which solids can be organized?

Which substance has the highest melting point?

Calculate the amount of heat energy required to evaporate 55.0 g of water at 100.0 $\degree$ C.(molar heat of vaporization of liquid water = 4.07 x 10⁴ J/mol)

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 molecules in the figure has hydrogen bonding in the pure liquid state?

Which of the following substances can participate in hydrogen bonding?

The forces that hold NH3 together in the solid state are:

Which of the following molecules experience dipole-dipole forces?

A solid substance has a high melting point, is hard, and is a good conductor of both heat and electricity.It is also malleable and ductile.This substance is probably a(n) ________ solid.

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

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

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

Arrange the following substances in order of increasing boiling point: CH3OH, CH4, CH3CH2OH, HOCH2CH2OH

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

The diagram represents the physical state of a substance.Where does this physical state occur on the cooling curve?

Which of the following has the highest vapor pressure at a given temperature?

Which of the molecules in the figure has hydrogen bonding in the pure liquid state?

One would expect that water is more viscous than C2H6, due to differences in intermolecular forces.

Which of the following substances can participate in hydrogen bonding?

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?

Which of the following statements is correct?

Which of the following is not one of the classifications into which solids can be organized?

Which substance has the highest melting point?

Calculate the amount of heat energy required to evaporate 55.0 g of water at 100.0 °\degree° C.(molar heat of vaporization of liquid water = 4.07 x 104 J/mol)

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

The forces that hold NH₃ together in the solid state are:

Arrange the following substances in order of increasing boiling point: CH₃OH, CH₄, CH₃CH₂OH, HOCH₂CH₂OH

One would expect that water is more viscous than C₂H₆, due to differences in intermolecular forces.

Calculate the amount of heat energy required to evaporate 55.0 g of water at 100.0 $\degree$ C.(molar heat of vaporization of liquid water = 4.07 x 10⁴ J/mol)