Question 1

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 2

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 3

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

Accepted Answer

A) True 
 B)False

Question 4

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

Accepted Answer

A) Most polymers, such as rubbers and plastics, are amorphous. 
B) Minerals, such as quartz and amethyst, are crystalline solids. 
C) Solids normally do not flow. 
D) The particles of a solid are held in a rigid, 3-dimensional array. 
E) The arrangement of the particles in a crystal lattice is called space packing. 
A) Most polymers, such as rubbers and plastics, are amorphous. 
B) Minerals, such as quartz and amethyst, are crystalline solids. 
C) Solids normally do not flow. 
D) The particles of a solid are held in a rigid, 3-dimensional array. 
E) The arrangement of the particles in a crystal lattice is called space packing.

Question 5

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

Question 6

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 7

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 8

Rank the following substances in order of increasing intermolecular forces: Ne, NH3, H2, O2

Accepted Answer

A) Ne 3 2 2 
B) Ne 3 2 2 
C) NH3 2 2 2 2 3 
E) H2 2 3 
A) Ne 3 2 2 
B) Ne 3 2 2 
C) NH3 2 2 2 2 3 
E) H2 2 3

Question 9

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 10

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

Accepted Answer

A) 1.50 × 102 kJ 
B) 8.34 kJ 
C) 4.33 kJ 
D) 7.50 × 102 kJ 
E) 1.50 × 10−1 kJ 
A) 1.50 × 102 kJ 
B) 8.34 kJ 
C) 4.33 kJ 
D) 7.50 × 102 kJ 
E) 1.50 × 10−1 kJ

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

Detergents are used to increase the surface tension of water, so that it will stay in the shape of a droplet.

Accepted Answer

A) True 
 B)False

Question 13

Explain why a container of liquid can begin to boil with no added heat if the air above the liquid is removed using a vacuum pump by filling in the blanks in the following statements: The ________ of a liquid is the temperature at which its ________ equals the atmospheric pressure on the sample. If the pressure is ________ sufficiently, the vapor pressure of the liquid will be greater than the pressure in the system, and the liquid will begin to boil.

Accepted Answer

The boiling point of a liquid is the tem

Question 14

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 15

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 16

What phase change is occurring in the figure, and is it endothermic or exothermic?

Accepted Answer

A) melting; exothermic 
B) freezing; endothermic 
C) freezing; exothermic 
D) melting; endothermic 
E) condensation; endothermic 
A) melting; exothermic 
B) freezing; endothermic 
C) freezing; exothermic 
D) melting; endothermic 
E) condensation; endothermic

Question 17

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

Question 18

Which of the following molecules experience dipole-dipole forces?

Accepted Answer

A) NO2 
B) CO2 
C) CBr4 
D) SO3 
E) F2 
A) NO2 
B) CO2 
C) CBr4 
D) SO3 
E) F2

Question 19

Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5°C to water at 24.0°C. (Cwater = 4.184 J/g°C; Cice = 2.03 J/g°C; molar heat of fusion of ice = 6.01 × 103 J/mol)

Accepted Answer

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

Question 20

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

Identify the type of solid shown in the image.

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

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

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

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

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

Which of the following substances can participate in hydrogen bonding?

Rank the following substances in order of increasing intermolecular forces: Ne, NH₃, H₂, O₂

Which of the following molecules experience dipole-dipole forces?

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

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

Detergents are used to increase the surface tension of water, so that it will stay in the shape of a droplet.

Which of the following statements regarding intermolecular forces is incorrect?

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

What phase change is occurring in the figure, and is it endothermic or exothermic?

The forces that hold CO₂ together in the solid state are

Which of the following molecules experience dipole-dipole forces?

Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5°C to water at 24.0°C. (C_water = 4.184 J/g°C; C_ice = 2.03 J/g°C; molar heat of fusion of ice = 6.01 × 10³ J/mol)

Which of the following substances can participate in hydrogen bonding?

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

Identify the type of solid shown in the image.

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

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

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

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

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

Which of the following substances can participate in hydrogen bonding?

Rank the following substances in order of increasing intermolecular forces: Ne, NH3, H2, O2

Which of the following molecules experience dipole-dipole forces?

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

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

Detergents are used to increase the surface tension of water, so that it will stay in the shape of a droplet.

Which of the following statements regarding intermolecular forces is incorrect?

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

What phase change is occurring in the figure, and is it endothermic or exothermic?

The forces that hold CO2 together in the solid state are

Which of the following molecules experience dipole-dipole forces?

Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5°C to water at 24.0°C. (Cwater = 4.184 J/g°C; Cice = 2.03 J/g°C; molar heat of fusion of ice = 6.01 × 103 J/mol)

Which of the following substances can participate in hydrogen bonding?

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

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

Rank the following substances in order of increasing intermolecular forces: Ne, NH₃, H₂, O₂

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

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

The forces that hold CO₂ together in the solid state are

Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5°C to water at 24.0°C. (C_water = 4.184 J/g°C; C_ice = 2.03 J/g°C; molar heat of fusion of ice = 6.01 × 10³ J/mol)