Deck 7: Intermolecular Forces and the Phases of Matter

Question 1

The change of state from a liquid to a gas is called ________.

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

Answer 1

evaporation

Question 2

Which of the three phases of matter (solid, liquid, or gas) features particles in a fixed, rigid arrangement?

A) solid
B) liquid
C) gas
D) All three phases of matter have rigid arrangements of particles.

Answer 2

solid

Question 3

Between individual molecules of NO₂ in the solid state, which of the following types of intermolecular forces would you expect to be dominant?

A) hydrogen bonding
B) London forces
C) van der Waals forces
D) dipole-dipole forces

Answer 3

dipole-dipole forces

Question 4

The change of state from a solid to a gas is called ________.

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

Question 5

Which of the three phases of matter (solid, liquid, or gas) has particles moving at the highest average velocity?

A) solid
B) liquid
C) gas
D) The particles in all three phases have about the same average speed.

Question 6

Which of the following substances would you expect to be a liquid at room temperature, assuming that strong intermolecular forces need to be present to be a liquid at room temperature?

A) N₂
B) CS2
C) H₂
D) O₂

Question 7

Which of the three phases of matter (solid, liquid, or gas) has particles that are fast-moving and independent of each other?

A) solid
B) liquid
C) gas
D) All of the above feature loose arrangements of particles.

Question 8

Which of the following is not a solid at 0 °C?

A) salt
B) carbon dioxide
C) sugar
D) iron

Question 9

The change of state from a solid to a liquid is called ________.

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

Question 10

Which of the following sublimes?

A) sugar
B) iron
C) mothballs
D) margarine

Question 11

Which of the three phases of matter (solid, liquid, or gas) features particles that are no longer held together by intermolecular forces?

A) solid
B) liquid
C) gas
D) All three phases of matter will do this.

Question 12

A change of state from a gas to a liquid is called ________.

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

Question 13

Which of the following statements is true about intermolecular forces of attraction between molecules?

A) They tend to hold molecules together.
B) Cooling is responsible for the substance's liquefaction.
C) The solidification of a substance usually requires lower temperatures than in the case of liquefaction.
D) All of the above are true.

Question 14

Which of the following chemical substances would you expect to have the highest melting point?

A) water, H₂O
B) methyl alcohol, CH₃OH
C) nitrogen dioxide, NO₂
D) hydrogen sulfide, H₂S

Question 15

The term "normal" boiling point indicates ________.

A) the temperature at which a liquid evaporates under the atmospheric pressure found at sea level.
B) the temperature at which a liquid boils under the atmospheric pressure found at sea level.
C) the temperature at which a liquid boils under any pressure conditions
D) both A and B

Question 16

Which of the following chemical substances would you expect to have the lowest boiling point (you may consider molecular mass and the degree of intermolecular forces as primary controlling factors)?

A) CH₄
B) CH₃CH₃
C) CH₃CH₂CH₃
D) CH₃CH₂CH₂CH₃

Question 17

Which of the three phases of matter (solid, liquid, or gas) features particles that are easily compressible?

A) solid
B) liquid
C) gas
D) All three phases of matter are compressible.

Question 18

Which of the three phases of matter (solid, liquid, or gas) has particles separated by the least amount of distance?

A) solid
B) liquid
C) gas
D) The separation distance is about the same in all three phases.

Question 19

Which of the following does not sublime?

A) mothballs
B) iodine crystals
C) salt
D) dry ice

Question 20

Which of the following statements about London forces is correct?

A) London forces are also called dispersion forces.
B) London forces are relatively weakly attractive.
C) London forces occur between polar and nonpolar molecules.
D) All the above statements are true.

Question 21

Which of the following will have the highest boiling point?

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

Question 22

Which of the following will have the lowest boiling point?

A) H₂S
B) H₂Te
C) H₂Se
D) H₂O

Question 23

Which of the following chemical substances would you expect to exhibit hydrogen bonding?

A) NH₃
B) CH₃OH
C) HF
D) all of the above

Question 24

Which of the following intermolecular force is the strongest?

A) London forces
B) van der Waals forces
C) hydrogen bonding
D) dipole forces

Question 25

Which of the following will have the lowest boiling point?

A) CH₃OCH₃
B) CH₃CH₂OH
C) HOCH₂-CH₂OH
D) CH₃CH₃

Question 26

Polar molecules may exhibit ________.

A) London forces
B) hydrogen bonding
C) dipole-dipole forces
D) all of the above

Question 27

Which of the following does not have a dipole?

A) carbon tetrachloride
B) acetone
C) ammonia
D) water

Question 28

Which of the following influences the strength of the intermolecular forces?

A) distance between interacting molecules
B) relative orientation between interacting molecules
C) location of the molecule in a liquid or solid
D) All of the above influence the strength of the intermolecular forces.

Question 29

London forces are extremely weak for ________.

A) nitrogen gas
B) methane gas
C) oxygen gas
D) all of the above

Question 30

The force(s) responsible for holding the DNA molecule in a very long twisted zipper is ________.

A) hydrogen bonding
B) London forces
C) dipolar forces
D) interionic forces

Question 31

The strength of an O-H bond is about equal to ________ kJ/bond

A) 16
B) 50
C) 100
D) 400

Question 32

The strength of a hydrogen bond is about ________ percent of the strength of a normal O-H bond

A) 1
B) 4
C) 16
D) 50

Question 33

Which of the following chemical substances would you expect to exhibit hydrogen bonding?

A) methyl chloride, CH₃Cl
B) methyl alcohol, CH₃OH
C) octane, C₈H₁₈
D) methane, CH₄

Question 34

Nonpolar molecules may exhibit ________.

A) London forces
B) hydrogen bonding
C) dipolar forces
D) all of the above

Question 35

The main reason why carbon tetrabromide is a solid at room temperature when compared to carbon tetrachloride which is a liquid is because ________.

A) carbon tetrabromide is tetrahedral in shape.
B) carbon tetrachloride has the weaker London forces than carbon tetrabromide.
C) carbon tetrabromide may undergo hydrogen bonding.
D) all of the above

Question 36

To form hydrogen bonds, molecules must contain ________.

A) an N-H bond
B) an O-H bond
C) an H-F bond
D) at least one of the above mentioned bonds

Question 37

Which of the following will have the highest boiling point?

A) CH₃OCH₃
B) CH₃CH₂OH
C) HOCH₂-CH₂OH
D) CH₃CH₃

Question 38

Which of the following experiences the strongest London forces?

A) carbon tetrachloride
B) water
C) hydrogen
D) helium

Question 39

Which of the following chemical substances would you expect to have the highest boiling point (you may consider molecular mass and the degree of intermolecular hydrogen bonding as primary controlling factors)?

A) methane, CH₄
B) ammonia, NH₃
C) methyl alcohol, CH₃OH
D) ethyl alcohol, CH₃CH₂OH

Question 40

Which of the compounds below has a large permanent dipole?

A) methane
B) hydrogen
C) acetone
D) nitrogen

Question 41

The acetone molecule has a large dipole because of the electronegativity difference between carbon and oxygen.

Question 42

Which of the following can be called a non-molecular ionic solid?

A) water
B) sodium chloride
C) methane
D) hydrogen

Question 43

Which intermolecular force is important for the function of the antibiotic vancomycin?

A) London forces
B) van der Waals forces
C) hydrogen bonding
D) dipole forces

Question 44

The replacement of a single NH group on vancomycin causes the antibiotic to become ineffective.

Question 45

London forces become significant for large molecules with many atoms and many electrons.

Question 46

The terms "dispersion forces" and "London forces" are interchangeable.

Question 47

Which statement is true about network solids?

A) They have extremely high melting points.
B) They are covalent substances.
C) They are large network molecules held by covalent compounds.
D) All of the above are true.

Question 48

The attractive forces between carbon dioxide molecules are considerably stronger than those found in water molecules.

Question 49

Quartz contains atoms that are held together with hydrogen bonding.

Question 50

At the freezing point the molecules are effectively frozen in place.

Question 51

Water has a much higher boiling point than acetone due to the ability of water to undergo hydrogen bonding.

Question 52

The melting and freezing points are identical for the same compound.

Question 53

Which of the following may not be considered an ionic compound?

A) sodium chloride
B) magnesium oxide
C) ammonia
D) potassium bromide

Question 54

Molecular substances have a higher melting point than non-molecular substances

Question 55

Vancomycin is the first line of defense against bacteria.

Question 56

Polar molecules do not exhibit London forces.

Question 57

Solid carbon dioxide is also known as dry ice.

Question 58

The freezing point of dry ice is 0 °C.

Question 59

How does vancomycin function to kill bacteria?

A) destroys the bacterial DNA
B) interferes with cell wall construction
C) inhibits protein synthesis
D) prevents bacteria metabolism

Question 60

Which of these has the highest melting point?

A) diamond
B) iron
C) sodium
D) bromine

Question 61

Identify the following crystalline solids as ionic, molecular, or metallic.
silicon carbide, SiC, m.p.: 2700 °C

Question 62

Identify each of the compounds as molecular or non-molecular.

-sodium oxide

A)non-molecular
B)molecular

Question 63

Identify the following crystalline solids as ionic, molecular, or metallic.
copper (II) carbonate, CuCO₃ (or cupric carbonate)

Question 64

Identify the following crystalline solids as ionic, molecular, or metallic.
glucose, C₆H₁₂O₆

Question 65

Identify the following crystalline solids as ionic, molecular, or metallic.
sodium fluoride, NaF, m.p.: 993 °C

Question 66

Identify each of the compounds as molecular or non-molecular.

-methane

A)non-molecular
B)molecular

Question 67

Identify the following crystalline solids as ionic, molecular, or metallic.
chromium, Cr

Question 68

Identify each of the compounds as molecular or non-molecular.

-hydrogen

A)non-molecular
B)molecular

Question 69

Identify each of the compounds as molecular or non-molecular.

-graphite

A)non-molecular
B)molecular

Question 70

Identify each of the compounds as molecular or non-molecular.

-ammonia

A)non-molecular
B)molecular

Question 71

Identify the following crystalline solids as ionic, molecular, or metallic.
What is the general trend in terms of increasing melting point for ionic solids, molecular solids, and network covalent solids?

Question 72

Identify each of the compounds as molecular or non-molecular.

-silicon dioxide

A)non-molecular
B)molecular

Question 73

Quartz and diamond are non-molecular solids, where the atoms are held together with covalent bonds.

Question 74

Identify the following crystalline solids as ionic, molecular, or metallic.
ethanol, C₂H₆O, m.p.: -117 °C

Question 75

Identify the following crystalline solids as ionic, molecular, or metallic.
calcium chloride, CaCl₂

Question 76

Identify the following crystalline solids as ionic, molecular, or metallic.
niobium, Nb, m.p.: 2468 °C

Question 77

Identify the following crystalline solids as ionic, molecular, or metallic.
magnesium chloride, MgCl₂, m.p.: 714 °C

Question 78

Identify the following crystalline solids as ionic, molecular, or metallic.
iodine, I₂

Question 79

Identify each of the compounds as molecular or non-molecular.

-sodium chloride

A)non-molecular
B)molecular

Question 80

Identify each of the compounds as molecular or non-molecular.

-water

A)non-molecular
B)molecular