Deck 7: Intermolecular Forces and the Phases of Matter

Question 1

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.

Answer 1

gas

Question 2

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 forces

Answer 2

dipole forces

Question 3

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

Answer 3

water, H₂O

Question 4

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.

Question 5

Which of the following sublimes?

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

Question 6

Which of the three phases of matter (solid, liquid, or gas)has particles that are in a loose, changeable arrangement but do not completely fill the volume of a given container?

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

Question 7

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

A)NH₃
B)CH₃OH
C)HF
D)all of the above

Question 8

The solid to gas conversion is called ________.

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

Question 9

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 10

The gas to liquid change of state is called ________.

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

Question 11

The term "normal" boiling point indicates ________.

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

Question 12

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

A)They tend to stick 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 13

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 14

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 15

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

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

Question 16

Nonpolar molecules may exhibit ________.

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

Question 17

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 18

Which of the following does not sublime?

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

Question 19

The liquid to gas change of state is called ________.

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

Question 20

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 21

Which of the following will have the lowest boiling point?

A)H₂S
B)H₂Te
C)H₂Se
D)H₂O

Question 22

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

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

Question 23

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 24

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 25

Which of these has the highest melting point?

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

Question 26

Which of the following will have the highest boiling point?

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

Question 27

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 28

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

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

Question 29

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

Question 30

London forces are extremely weak for ________.

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

Question 31

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 32

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

A)carbon tetrabromide is tetrahedral in shape
B)carbon tetrachloride has a higher molecular weight
C)carbon tetrabromide may undergo hydrogen bonding
D)all of the above

Question 33

Which of the following will have the highest boiling point?

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

Question 34

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

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

Question 35

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 36

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

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

Question 37

Which of the following experiences the strongest London forces?

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

Question 38

Polar molecules may exhibit ________.

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

Question 39

Which of the following intermolecular force is the strongest?

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

Question 40

Which of the following does not have a dipole?

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

Question 41

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

Question 42

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

Question 43

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

Question 44

Identify the following crystalline solids as ionic, molecular, or metallic.
calcium chloride, CaC1₂

Question 45

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

Question 46

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

Question 47

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

Question 48

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

Question 49

Vancomycin is the first line of defense against bacteria.

Question 50

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

Question 51

The reason why quartz has a high melting point is hydrogen bonding.

Question 52

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent.
magnesium chloride, MgC1₂, m.p.: 714 °C

Question 53

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent.
silicon carbide, SiC, m.p.: 2700 °C

Question 54

Solid carbon dioxide is also known as dry ice.

Question 55

Quartz and diamond are non-molecular covalent substances.

Question 56

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

Question 57

The main reason why water has a much higher boiling point than acetone is the ability of water to undergo hydrogen bonding.

Question 58

Polar molecules do not exhibit London forces.

Question 59

The freezing point of dry ice is 0 °C.

Question 60

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

Question 64

Match the description of processes that appear in the questions with the corresponding change of states in the list below.

Question 65

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent.
sodium fluoride, NaF, m.p.: 993 °C

Question 66

Match each temperatures in the questions with the processes described in the list below.

Question 68

Match each of the substances in the questions with the STRONGEST type of bonding that it exhibits from the list below.

Question 69

What is the general trend in terms of increasing melting point for ionic solids, molecular solids, and network covalent solids?

Question 70

Identify each of the compounds in the left column as molecular or non-molecular.

Question 71

Based upon the formulas and melting points, decide whether each of the following crystalline substances should be classified as ionic, molecular, metallic or network covalent.
ethanol, C₂H₆O, m.p.: -117 °C