Deck 6: Intermolecular Forces Attractions Between Particles

Question 1

The relative energies strengths) of the intermolecular forces present in each of five different pure substances are shown in the figure below.Which substance has the highest melting point?

A)a
B)b
C)c
D)d
E)e

Answer 1

b

Question 2

Ion-dipole forces always require

A)an ion and a water molecule.
B)a cation and a water molecule.
C)an anion and a polar molecule.
D)an ion and a polar molecule.
E)a polar and a nonpolar molecule.

Answer 2

an ion and a polar molecule.

Question 3

Which molecule below exhibits the weakest dispersion forces?

A)O₂
B)P₄
C)Br₂
D)I₂
E)Xe

Answer 3

O₂

Question 4

Which compound below has the highest boiling point?

A)CCl₄
B)CI₄
C)CF₄
D)CH₄
E)CBr₄

Question 5

Arrange the following compounds in order of increasing dispersion interactions: CCl₄, CH₄, CF₄.

A)CH₄ $\lt$ CF4 $\lt$ CCL₄
B)CCL₄ $\lt$ CH₄ $\lt$ CF4
C)CF4 $\lt$ CH₄ $\lt$ CCL₄
D)CCL₄ $\lt$ CF4 $\lt$ CH₄
E)CH₄ $\lt$ CCL₄ $\lt$ CF4

Question 6

Which statement below regarding London dispersion forces is FALSE?

A)Electrons in one molecule can experience attractions to nuclei in a neighboring nonbonded molecule.
B)Temporary dipoles can arise when electrons are temporarily asymmetrically redistributed around the nucleus of an atom or within a bond.
C)As electron cloud size increases, the strength of London dispersion forces increases.
D)The dipole moments associated with London dispersion forces are long-lasting.
E)Temporary dipoles can induce dipoles in other particles.

Question 7

The relative energies strengths) of the intermolecular forces present in each of five different pure substances are shown in the figure below.Which substance has the lowest melting point?

A)a
B)b
C)c
D)d
E)e

Question 8

Polarizability refers to

A)the ease with which the electron cloud of an atom or molecule can be distorted.
B)the magnitude of the dipole moment of a molecule.
C)the ease with which a hydrogen bond can form.
D)the perturbation in electron density because of hydrogen bonding.
E)the ability to transmit polarized light.

Question 9

Which molecule below has the highest polarizability?

A)N₂
B)O₂
C)F₂
D)Br₂
E)I₂

Question 10

The relative energies strengths) of the intermolecular forces present in each of four different pure substances are shown in the figure below.Which substance is most likely to be a solid at room temperature?

A)a
B)b
C)c
D)d
E)e

Question 11

The relative energies (strengths) of the intermolecular forces between five different substances are shown in the figure below.Which substance has the highest boiling point?

A)a
B)b
C)c
D)d
E)e

Question 12

Which type of intermolecular interaction exists for all compounds?

A)ion-ion
B)dipole-dipole
C)London dispersion
D)hydrogen bonding
E)dipole-induced dipole

Question 13

The relative energies strengths) of the intermolecular forces between five different substances are shown in the figure below.Which substance has the lowest boiling point?

A)a
B)b
C)c
D)d
E)e

Question 14

Which statement below is FALSE?

A)The more electrons in an atom, the more likely it is that they will be asymmetrically distributed.
B)The more electrons in an atom, the stronger the London dispersion forces it can experience.
C)Larger atoms may experience larger temporary dipoles.
D)Atoms of elements lower in a group of the periodic table probably experience larger London dispersion forces.
E)As the strength of temporary dipoles decreases within a substance, the boiling point increases.

Question 15

Which straight-chain alkane below has the highest boiling point?

A)CH₄
B)C₆H₁₂
C)C₈H₁₈
D)C₂H₆
E)C₄H₁₀

Question 16

Which molecule below exhibits the greatest dispersion forces?

A)CH₃CH₃
B)CH₃CH₂CH₃
C)C₂H₂
D)CH₄
E)CH₃CH₂CH₂CH₃

Question 17

Dispersion forces are due to

A)permanent dipoles.
B)temporary dipoles.
C)hydrogen bonding.
D)ionic interactions.
E)protons.

Question 18

The relative energies strengths) of the intermolecular forces present in each of four different pure substances are shown in the figure below.Which substance is most likely to be a gas at room temperature?

A)a
B)b
C)c
D)d
E)e

Question 19

Viscosity is a measure of a substance's

A)ability to resist changes in its surface area.
B)resistance to flow.
C)surface tension.
D)compressibility.
E)color.

Question 20

Which straight-chain alkane below would you predict to be the most viscous? All are liquids exhibiting the general bonding pattern CH₃-(CH₂ )_n-CH₃ .

A)C₁₂H₂₆
B)C₁₀H₂₂
C)C₅H₁₂
D)C₆H₁₄
E)C₉H₂₀

Question 21

Which compound below will exhibit hydrogen bonding with itself in the liquid state?

A)CH₃OCH₃
B)CH₃COCH₃
C)CH₃CH₂NH₂
D)H₂CO
E)CH₃F

Question 22

When two liquids mix completely in all proportions, they are

A)soluble.
B)miscible.
C)immiscible.
D)solvated.
E)ubiquitous.

Question 23

The dipole moments of HCl and of HBr are 1.08 D and 0.82 D, respectively.The boiling point of HBr is higher than that of HCl.This is probably because HBr has

A)fewer electrons.
B)larger London dispersion interactions.
C)hydrogen bonding.
D)larger dipole-dipole interactions.
E)more ionic character.

Question 24

Which compound below is capable of dipole-dipole interactions?

A)CF₄
B)CS₂
C)PCl₃
D)SF₆
E)BF₃

Question 25

Which statement below is FALSE?

A)When an ionic compound dissolves in water, the ions interact with the permanent dipoles of the water molecules.
B)Water molecules orient such that their oxygen atoms point toward an anion in solution.
C)Liquid ammonia, NH₃, like water, could experience ion-dipole interactions with dissolved ions.
D)Water molecules in the inner sphere of hydration of an ion are involved in ion-dipole interactions.
E)Hydrated ions are stabilized by the surrounding water molecules.

Question 26

For a molecule to exhibit dipole-dipole interactions, it must

A)have a temporary dipole moment.
B)have a hydrogen bound to an oxygen, nitrogen, or fluorine.
C)have a permanent dipole moment.
D)be an ion.
E)have three or more atoms.

Question 27

Which pair of compounds below lists the molecule with the stronger dipole-dipole forces first?

A)CH₂Br₂ and CH₂Cl₂
B)C₃H₈ and CH₃CN
C)CH₃)₃N and CH₃)₃P
D)CH₃)₂S and CH₃)₂O
E)CH₃F and CHF₃

Question 28

Which statement below regarding hydrogen bonding is FALSE?

A)Hydrogen bonds can form between like or unlike molecules.
B)Hydrogen bonds are intermediate in strength between covalent bonds and dipole-dipole forces.
C)Hydrogen bonding is irreversible.
D)Hydrogen must be directly bonded to F, N, or O to participate in hydrogen bonding.
E)Hydrogen bonding plays a key role in the shapes of molecules.

Question 29

Which gaseous compound below is likely to condense at the highest temperature (gas $\rightarrow$ liquid)?

A)NH₃
B)NF₃
C)CF₄
D)PH₃
E)PF₃

Question 30

Dipole-dipole interactions typically are not as strong as ion-dipole interactions because

A)ion-dipole interactions involve partial charges caused by the equal sharing of electrons by atoms forming a bond.
B)dipole-dipole interactions involve the complete transfer of charge between atoms.
C)ion-dipole interactions involve only the partial transfer of charge between atoms.
D)ion-dipole interactions always involve water.
E)dipole-dipole interactions involve only partial charges caused by unequal sharing of electrons by atoms forming a bond.

Question 31

Which compound below would you predict can experience only dispersion forces?

A)SF₄
B)NO₂
C)CCl₄
D)H₂CO
E)NF₃

Question 32

A hydration sphere forms around an ion in aqueous solution due to

A)ion-dipole interactions.
B)ion-hydrogen-bonding interactions.
C)dispersion forces.
D)dipole-dipole interactions.
E)ion-induced dipole interactions.

Question 33

When an ion is dissolved in water, which intermolecular forces are in effect: ion-dipole forces, dipole-dipole forces, and/or London dispersion forces?

A)London dispersion forces
B)dipole-dipole forces
C)ion-dipole forces
D)ion-dipole forces and London dispersion forces
E)ion-dipole forces, dipole-dipole forces, and London dispersion forces

Question 34

You are interested in determining the solubility of ionic compounds in solvents other than water, and you decide to try liquid ammonia, NH₃.Which statement below regarding your experiment is probably true?

A)The hydrogen ions in ammonia have partial negative charges and can stabilize Na^- in solution.
B)The molecular dipole moment is too small to effectively interact with ions.
C)The hydrogen atoms in ammonia would orient toward both ions equally.
D)The lone pair of electrons on nitrogen in ammonia can act in a way similar to the lone pairs on oxygen in water.
E)Ion-dipole interactions exist only in water.

Question 35

Based on their boiling points,which compound below will have the largest dipole-dipole interaction?

A)propane 231 K)
B)dimethyl ether 248 K)
C)acetonitrile 355 K)
D)methyl chloride 249 K)
E)butane 135 K)

Question 36

When sodium chloride dissolves in water, how do the water molecules orient around the ions?

A)Water molecules are randomly oriented around the ions.
B)The hydrogen atoms point toward both the sodium and the chloride ions.
C)The oxygen atoms point toward both the sodium ions and the chloride ions.
D)The hydrogen atoms point toward the sodium ions, and the oxygen atoms point toward the chloride ions.
E)The oxygen atoms point toward the sodium ions, and the hydrogen atoms point toward the chloride ions.

Question 37

Which compound below is likely to have the highest boiling point?

A)CH₃CF₃
B)CH₃CN
C)CH₃)₂CO
D)CH₃CH₂SH
E)CH₃CH₂OH

Question 38

Which compound below will have the strongest dipole-dipole interactions between its molecules?

A)CF₄
B)CO₂
C)CH₃F
D)H₂CO
E)CH₃Cl

Question 39

Which is the strongest interaction for substances with similar mass?

A)ion-dipole
B)hydrogen bonding
C)dipole-dipole
D)London dispersion
E)ion-induced dipole

Question 40

Which compound below is capable of hydrogen bonding with itself in the liquid state?

A)CHCl₃
B)H₂CO
C)HCN
D)BeH₂
E)CH₃OH

Question 41

Which pair of compounds below is most likely to be miscible?

A)CCl₄ and Br₂
B)Br₂ and HCl
C)HF and CCl₄
D)H₂O and CH₃CH₂CH₂CH₃
E)CCl₄ and NH₃

Question 42

Stearic acid, a fatty acid commonly found in animal fat, has a condensed chemical formula of CH₃(CH₂)₁₆COOH.It is a common component of soaps and detergents.Which stataement below is FALSE?

A)The -COOH group would experience hydrogen bonding with water.
B)The long alkane "tail," CH₃(CH₂)₁₆^-, is hydrophobic.
C)Stearic acid and water are probably miscible.
D)Stearic acid would probably dissolve in nonpolar solvents such as hexane, C₆H₁₄.
E)Stearic acid contains hydrophilic and hydrophobic regions.

Question 43

Molecular nitrogen (N₂) interacts with water and is sparingly soluble in water due to

A)dispersion forces.
B)dipole-induced dipole forces.
C)ion-dipole forces.
D)hydrogen bonding.
E)dipole-dipole forces.

Question 44

Which compound below would you expect to be most soluble in water?

A)CF₄
B)CCl₄
C)CH₂Cl₂
D)CH₄
E)CH₃OH

Question 45

Suppose a solution that is 70% isopropyl alcohol and 30% water by mass has a density of 0.785 g/mL.Which statement below regarding this solution is true? Isopropyl alcohol has a condensed formula of CH₃)₂CHOH and a molar mass of 60.09 g/mol.

A)Isopropyl alcohol is the solvent.
B)Isopropyl alcohol can hydrogen bond with water and with itself.
C)100 mL of this solution would have a mass of 785 grams.
D)The number of moles of isopropyl alcohol is greater than the number of moles of water present.
E)The solution will separate over time because the intermolecular forces between water molecules are so strong.

Question 46

Which choice below is not equal to a standard atmosphere (atm)?

A)1013 mb
B)10⁵ Pa
C)101.3 kPa
D)1.013 * 10⁵ N/m²
E)the average pressure at sea level

Question 47

Which alcohol should be most soluble in a nonpolar solvent such as hexane, C₆H₁₄?

A)CH₃OH
B)CH₃CH₂OH
C)CH₃CH₂CH₂OH
D)CH₃CH₂CH₂CH₂OH
E)CH₃CH₂CH₂CH₂CH₂OH

Question 48

A substance that is will be insoluble in water, but a substance that is will be soluble in water.

A)hydrophobic; immiscible
B)hydrophilic; hydrophobic
C)hydrophilic; miscible
D)hydrophobic; hydrophilic
E)miscible; immiscible

Question 49

At the critical point,

A)all the liquid has evaporated.
B)the densities of the solid and liquid are the same.
C)the densities of the solid and the gas are the same.
D)the densities of the gas and the liquid are the same.
E)a critical mass has been reached.

Question 50

At the point marked with a dot on the phase diagram, the solid will

A)be indistinguishable from the gas.
B)boil.
C)melt.
D)sublime.
E)freeze.

Question 51

Which statement below regarding the physical state of a substance is true?

A)All substances expand as they melt or boil.
B)The physical state observed is largely independent of attractive forces between the substance's constituent particles.
C)The physical state observed depends only on temperature.
D)The solid and liquid phases are unaffected by changes in pressure.
E)Changes in temperature cause changes in the energies of the substance's constituent particles.

Question 52

Which statement below is true?

A)Nonpolar molecules can dissolve in polar solvents.
B)Gases are soluble only in nonpolar solvents.
C)Ionic compounds cannot dissolve in any solvent other than water.
D)Polar molecules cannot dissolve in nonpolar solvents.
E)Solubility depends only slightly on the strength of solute-solute attractive forces.

Question 53

Which compound below would you most appropriately call hydrophobic?

A)CH₄
B)H₂CO
C)CO
D)HCl
E)NaCl

Question 54

Hydrophilic substances

A)are immiscible in water.
B)are insoluble in water.
C)are soluble in water.
D)are soluble in nonpolar solvents.
E)generally do not hydrogen bond.

Question 55

A phase diagram shows the states of a substance as a function of and .

A)pressure; volume
B)volume; temperature
C)pressure; temperature
D)concentration; temperature
E)density; pressure

Question 56

Which compound below would be most soluble in benzene, C₆H₆?

A)H₂O
B)H₂COH)₂
C)PCl₃
D)CCl₄
E)CH₃CH₂OH

Question 57

The solubility of a compound may depend on many factors, including

A)solute-solvent interactions.
B)solute-solute interactions.
C)solvent-solvent interactions.
D)physical parameters such as temperature.
E)all of the items listed.

Question 58

You decide to experiment with carbon disulfide CS₂) as a solvent.Which statement below is probably true? Carbon disulfide is a colorless liquid with a density of 1.261 g/mL and a molar mass of 76.14 g/mol.

A)CS₂ is probably a good solvent for alkanes carbon-hydrogen molecules containing only single bonds).
B)Water is probably miscible with CS₂.
C)For a substance to dissolve in CS₂, dipole-dipole interactions between CS₂ molecules would have to be broken.
D)Solutes that experience hydrogen bonding should dissolve readily in CS₂.
E)Nonpolar gases such as N₂ and O₂ are probably completely insoluble in CS₂.

Question 59

Which pair of compounds below is most likely to be immiscible?

A)Br₂ and C₆H₆
B)H₂O and CH₃CH₂OH
C)CCl₄ and H₂CO
D)CH₃OH and CH₃CH₂OH
E)H₂O and NH₃

Question 60

At the triple point of a substance,

A)three phases are present in equilibrium.
B)the solid completely sublimes.
C)the gas completely condenses to a liquid.
D)only the solid and liquid are in equilibrium.
E)only one phase appears to be present.

Question 61

Consider the phase diagram for a substance shown here.The solid phase is than the liquid phase.

A)more dense
B)less dense
C)more massive
D)less massive
E)hotter

Question 62

Which statement below best explains why the density of water decreases as it is cooled from 4.0 $\degree$ C to its normal freezing point?

A)Water molecules decrease in size as they cool because energy is released.
B)A regular, repeating network of hydrogen bonds between water molecules is formed.
C)Water molecules become more rigid as they cool.
D)Hydrogen bonds in liquid water are longer than they are in ice.
E)All substances contract just before freezing.

Question 63

The temperature at point b in the phase diagram below is the _______

A)critical point.
B)triple point.
C)transition point.
D)normal freezing point.
E)normal boiling point.

Question 64

Arrange the following molecules in order of increasing boiling point: CH₂Cl₂, CH₃OH, CH₃CH₃, CH₃F

Question 65

Point c in the phase diagram below is the _______

A)critical point.
B)triple point.
C)transition point.
D)normal freezing point.
E)normal boiling point.

Question 66

Which statement below about the following phase diagram is FALSE?

A)The solid phase is more dense than the liquid phase.
B)D is the normal boiling point.
C)The melting point decreases as pressure increases.
D)The normal melting point is at a lower temperature than the triple point.
E)E, F, and G label in that order the solid, liquid, and gas phases.

Question 67

Which statement below regarding capillary action is FALSE?

A)Capillary action refers to the rise of a liquid in a narrow tube.
B)The molecules can move in opposition to gravity.
C)The molecules in the liquid are attracted to each other.
D)An external force is required to cause the movement of the liquid.
E)The phenomenon is caused by both adhesive and cohesive forces.

Question 68

Difluoromethane (CH₂F₂) has a dipole moment of 1.93 D and a boiling point of -52 $\degree$ C.Dichloromethane (CH₂Cl₂) has a dipole moment of 1.60 D and a boiling point of 40 $\degree$ C.Why is the boiling point of dichloromethane so much higher than that of difluoromethane?

Question 69

Which liquid below will have the highest surface tension?

A)acetonitrile, CH₃CN
B)acetone, CH₃)₂CO
C)water, H₂O
D)ethanol, CH₂CH₂OH
E)ethylene glycol, HOCH₂CH₂OH

Question 70

The temperature at point a in the phase diagram below is the

A)critical point.
B)triple point.
C)transition point.
D)normal freezing point.
E)normal boiling point.

Question 71

Water forms a concave meniscus in a glass tube because

A)the cohesive forces between water molecules are larger than the adhesive forces between water molecules and the glass wall.
B)the adhesive forces between water molecules and the glass wall are larger than the cohesive forces between water molecules.
C)water molecules form hydrogen bonds with each other.
D)water molecules repel each other.
E)the glass wall is wet.

Question 72

Why does HI boil at a higher temperature than HBr even though the dipole moment of HBr 0.82 D) is larger than that of HI 0.38 D)?

Question 73

Which of the following ions would you predict experiences the strongest ion-dipole forces in water: Na⁺, K⁺, Mg²⁺, Ca²⁺, Br^-, or I ^-? State your reasoning.

Question 74

The boiling points of group IVA hydrides increases in the order CH₄ $\lt$ SiH₄ $\lt$ GeH₄ $\lt$ SnH₄.Which molecule experiences the strongest attractive forces and why?

Question 75

Point d in the phase diagram below is the _______

A)critical point.
B)triple point.
C)transition point.
D)normal freezing point.
E)normal boiling point.

Question 76

Explain why the boiling point of nitrogen (N₂, 77 K) is much lower than that of carbon monoxide (CO, 84 K) even though both have the same number of electrons and protons and nearly the same mass.

Question 77

What structural characteristics must a molecule have in order to hydrogen bond?

Question 78

Arrange the following in order of increasing boiling point: Xe, Ar, Ne, F₂, and Br₂.Explain the reason for your ranking

Question 79

Why do the strengths of dispersion interactions generally increase with the molar mass of the compound?

Question 80

The resistance of a liquid to an increase in its surface area is

A)surface tension.
B)viscosity.
C)capillary action.
D)a meniscus.
E)density.