Deck 11: Liquids, Solids, and Intermolecular Forces

Question 1

Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force.

A)H₂
B)SO₂
C)NH₃
D)CF₄
E)BCl₃

Answer 1

SO₂

Question 2

Choose the pair of substances that are most likely to form a homogeneous solution.

A)NaCl and Hg
B)C₃H₈ and C₂H₅OH
C)LiF and C₆H₁₄
D)Br₂ and PF₃
E)NH₃ and CH₃OH

Answer 2

NH₃ and CH₃OH

Question 3

Identify the characteristics of a liquid.

A)indefinite shape and volume
B)indefinite shape,but definite volume
C)definite shape and volume
D)none of the above
E)all of the above

Answer 3

indefinite shape,but definite volume

Question 4

Give the change in condition to go from a liquid to a gas.

A)Increase heat or reduce pressure.
B)Increase heat or increase pressure.
C)Cool or reduce pressure.
D)Cool or increase pressure.
E)None of the above

Question 5

What type of intermolecular force causes the dissolution of NaCl in water?

A)hydrogen bonding
B)dipole-dipole forces
C)ion-dipole force
D)dispersion forces
E)None of the above

Question 6

Place the following compounds in order of increasing strength of intermolecular forces.
CH₄ CH₃CH₂CH₃ CH₃CH₃

A)CH₃CH₂CH₃ < CH₄ < CH₃CH₃
B)CH₃CH₂CH₃ < CH₃CH₃ < CH₄
C)CH₃CH₃ < CH₄ < CH₃CH₂CH₃
D)CH₄ < CH₃CH₂CH₃ < CH₃CH₃
E)CH₄ < CH₃CH₃ < CH₃CH₂CH₃

Question 7

Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force.

A)SCl₂
B)C₂H₆
C)CH₃OH
D)CH₂F₂
E)None of the above compounds exhibit hydrogen bonding.

Question 8

Identify the phase in which the water molecules are closest together.

A)gas
B)dry ice
C)solid
D)liquid

Question 9

What is the strongest type of intermolecular force present in CHF₃?

A)ion-dipole
B)dispersion
C)hydrogen bonding
D)dipole-dipole
E)None of the above

Question 10

Place the following compounds in order of decreasing strength of intermolecular forces.
I.CH₃CH₂CH₂CH₂CH₂CH₃
II.(CH₃)₃CCH₃
III.(CH₃)₃CCH₂CH₃

A)III > II > I
B)I > III > II
C)I > II > III
D)II > III > I
E)III > I > II

Question 11

Identify the weakest type of intermolecular forces.

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

Question 12

What is the strongest type of intermolecular force present in H₂?

A)ion-dipole
B)dipole-dipole
C)dispersion
D)hydrogen bonding
E)None of the above

Question 13

Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force.

A)Cl₂
B)CO
C)HF
D)NaCl
E)All of these have intermolecular forces stronger than dispersion.

Question 14

Choose the pair of substances that are most likely to form a homogeneous solution.

A)C₆H₁₄ and C₁₀H₂₀
B)LiBr and C₅H₁₂
C)N₂O₄ and NH₄Cl
D)C₆H₁₄ and H₂O
E)None of the pairs above will form a homogeneous solution.

Question 15

Place the following compounds in order of increasing strength of intermolecular forces.
CO₂ F₂ NH₂CH₃

A)NH₂CH₃ < CO₂ < F₂
B)F₂ < NH₂CH₃ < CO₂
C)NH₂CH₃ < F₂ < CO₂
D)F₂ < CO₂ < NH₂CH₃
E)CO₂ < NH₂CH₃ < F₂

Question 16

Choose the pair of substances that are most likely to form a homogeneous solution.

A)CCl₄ and SCl₂
B)NF₃ and SO₂
C)CO and C₆H₆
D)NH₂CH₃ and CH₄
E)None of the pairs above will form a homogeneous solution.

Question 17

Which of the following statements is true?

A)Intermolecular forces are generally stronger than bonding forces.
B)Until a certain point,the potential energy of molecules decrease as they get closer to one another.
C)Energy is given off when the attraction between two molecules is broken.
D)Increasing the pressure on a solid usually causes it to become a liquid.
E)None of the above are true.

Question 18

Place the following compounds in order of decreasing strength of intermolecular forces.
HF O₂ CO₂

A)HF > CO₂ > O₂
B)HF > O₂ > CO₂
C)O₂ > CO₂ > HF
D)CO₂ > HF > O₂
E)CO₂ > O₂ > HF

Question 19

What is the strongest type of intermolecular force present in NH₂CH₃?

A)dispersion
B)dipole-dipole
C)hydrogen bonding
D)ion-dipole
E)None of the above

Question 20

Choose the substance with the highest surface tension.

A)HOCH₂CH₂OH
B)CH₂F₂
C)CH₃CH₂F
D)CH₃CH₂OH
E)CH₃CH₂CH₃

Question 21

Which of the following statements is true?

A)Vapor pressure increases with temperature.
B)Hydrogen bonds are stronger than covalent bonds.
C)Intermolecular forces hold the atoms in molecules together.
D)Dispersion forces are generally stronger than dipole-dipole forces.
E)None of the above are true.

Question 22

Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.

A)absolute temperature
B)definite temperature
C)fluid temperature
D)critical temperature
E)solid temperature

Question 23

Choose the substance with the highest boiling point.

A)CH₄
B)KI
C)CS₂
D)HF
E)I₂

Question 24

Choose the substance with the lowest surface tension.

A)CH₃SH
B)CH₃CH₂CH₂CH₃
C)C₆H₆
D)H₂O
E)(CH₃)₂CO

Question 25

How much energy is required to vaporize 48.7 g of dichloromethane (CH₂Cl₂)at its boiling point,if its ΔH_vap is 31.6 kJ/mol?

A)31.2 kJ
B)6.49 kJ
C)55.1 kJ
D)15.4 kJ
E)18.1 kJ

Question 26

Place the following substances in order of increasing boiling point.
Ne Cl₂ O₂

A)Ne < Cl₂ < O₂
B)Cl₂ < O₂ < Ne
C)O₂ < Cl₂ < Ne
D)Cl₂ < Ne < O₂
E)Ne < O₂ < Cl₂

Question 27

How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH)at its boiling point,if its ΔH_vap is 40.5 kJ/mol?

A)86.7 kJ
B)11.5 kJ
C)18.9 kJ
D)52.8 kJ
E)39.9 kJ

Question 28

Place the following substances in order of decreasing vapor pressure at a given temperature.
PF₅ BrF₃ CF₄

A)BrF₃ > PF₅ > CF₄
B)BrF₃ > CF₄ > PF₅
C)PF₅ > BrF₃ > CF₄
D)CF₄ > BrF₃ > PF₅
E)CF₄ > PF₅ > BrF₃

Question 29

Choose the substance with the lowest boiling point.

A)H₂S
B)NBr₃
C)F₂
D)CF₂H₂
E)H₂O₂

Question 30

Which of the following substances would you predict to have the highest ΔH_vap?

A)CH₃Cl
B)HCl
C)HOCH₂CH₂OH
D)CH₃CH₂OH
E)CH₃CH₂CH₂CH₃

Question 31

Place the following substances in order of increasing boiling point.
CH₃CH₂OH Ar CH₃OCH₃

A)Ar < CH₃OCH₃ < CH₃CH₂OH
B)CH₃CH₂OH < Ar < CH₃OCH₃
C)CH₃CH₂OH < CH₃OCH₃ < Ar
D)CH₃OCH₃ < Ar < CH₃CH₂OH
E)Ar < CH₃CH₂OH < CH₃OCH₃

Question 32

Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube.

A)capillary action
B)viscosity
C)surface tension
D)density
E)None of the above

Question 33

Choose the substance with the lowest vapor pressure at a given temperature.

A)CO₂
B)BeCl₂
C)BF₃
D)He
E)PF₅

Question 34

Place the following substances in order of increasing vapor pressure at a given temperature.
SF₆ SiH₄ SF₄

A)SF₆ < SiH₄ < SF₄
B)SiH₄ < SF₄ < SF₆
C)SF₆ < SF₄ < SiH₄
D)SF₄ < SF₆ < SiH₄
E)SiH₄ < SF₆ < SF₄

Question 35

Choose the substance with the lowest viscosity.

A)Cl₃CCCl₃
B)Cl₂CHCH₂Cl
C)Cl₂CHCHCl₂
D)ClCH₂CH₂Cl
E)Cl₃CCHCl₂

Question 36

How much energy is required to vaporize 158 g of butane (C₄H₁₀)at its boiling point,if its ΔH_vap is 24.3 kJ/mol?

A)15.1 kJ
B)66.1 kJ
C)89.4 kJ
D)11.2 kJ
E)38.4 kJ

Question 37

Choose the substance with the highest viscosity.

A)(CH₃CH₂)₂CO
B)C₂H₄Cl₂
C)HOCH₂CH₂CH₂CH₂OH
D)CF₄
E)C₆H₁₄

Question 38

Choose the substance with the highest vapor pressure at a given temperature.

A)SiS₂
B)RbCl
C)CH₃SCH₃
D)BF₃
E)SbH₃

Question 39

Which of the following substances would you predict to have the highest ΔH_vap?

A)Xe
B)C₆H₆
C)SiF₄
D)Br₂
E)N₂

Question 40

Which substance below has the strongest intermolecular forces?

A)A₂X,ΔH_vap = 39.6 kJ/mol
B)BY₂,ΔH_vap = 26.7 kJ/mol
C)C₃X₂,ΔH_vap = 36.4 kJ/mol
D)DX₂,ΔH_vap = 23.3 kJ/mol
E)EY₃,ΔH_vap = 21.5 kJ/mol

Question 41

Give the phase transition that occurs as the temperature of dry ice increases.

A)from solid to gas
B)from gas to solid
C)from liquid to gas
D)from liquid to solid
E)from solid to liquid

Question 42

Determine ΔH_vap for a compound that has a measured vapor pressure of 24.3 torr at 273 K and 135 torr at 325 K.

A)41 kJ/mol
B)79 kJ/mol
C)24 kJ/mol
D)13 kJ/mol
E)34 kJ/mol

Question 43

Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35°C and has a ΔH_vap of 32.1 kJ/mol.

A)255 K
B)368 K
C)412 K
D)390.K
E)466 K

Question 44

Determine the vapor pressure (in mm Hg)of a substance at 29°C,whose normal boiling point is 76°C and has a ΔH_vap of 38.7 kJ/mol.

A)80 mm Hg
B)13 mm Hg
C)21 mm Hg
D)48 mm Hg
E)96 mm Hg

Question 45

Place the following substances in order of decreasing boiling point.
H₂O N₂ CO

A)CO > H₂O > N₂
B)N₂ > CO > H₂O
C)H₂O > CO > N₂
D)CO > N₂ > H₂O
E)N₂ > H₂O > CO

Question 46

Assign the appropriate labels to the phase diagram shown below.

A)A = liquid,B = solid,C = gas,D = critical point
B)A = gas,B = solid,C = liquid,D = triple point
C)A = gas,B = liquid,C = solid,D = critical point
D)A = solid,B = gas,C = liquid,D = supercritical fluid
E)A = liquid,B = gas,C = solid,D = triple point

Question 47

Why is water an extraordinary substance?

A)Water has a low molar mass,yet it is a liquid at room temperature.
B)Water is the main solvent within living organisms.
C)Water has an exceptionally high specific heat capacity.
D)Water has strong hydrogen bonding.
E)All of the above

Question 48

Consider the phase diagram shown.Choose the statement below that is true.

A)The triple point of this substance occurs at a temperature of 31°C.
B)At 10 atm of pressure,there is no temperature where the liquid phase of this substance would exist.
C)The solid phase of this substance is higher in density than the liquid phase.
D)The line separating the solid and liquid phases represents the ΔH_vap.
E)None of the above are true.

Question 49

Place the following substances in order of decreasing vapor pressure at a given temperature.
BeF₂ CH₃OH OF₂

A)CH₃OH > OF₂ > BeF₂
B)BeF₂ > OF₂ > CH₃OH
C)OF₂ > CH₃OH > BeF₂
D)OF₂ > BeF₂ > CH₃OH
E)BeF₂ > CH₃OH > OF₂

Question 50

How much energy must be removed from a 94.4 g sample of benzene (molar mass = 78.11 g/mol)at 322.0 K to solidify the sample and lower the temperature to 205.0 K? The following physical data may be useful.
ΔH_vap = 33.9 kJ/mol
ΔH_fus = 9.8 kJ/mol
C_liq = 1.73 J/g°C
C_gas = 1.06 J/g°C
C_sol = 1.51 J/g°C
T_melting = 279.0 K
T_boiling = 353.0 K

A)17.6 kJ
B)11.8 kJ
C)70.2 kJ
D)10.5 kJ
E)29.4 kJ

Question 51

Define sublimation.

A)The phase transition from solid to gas.
B)The phase transition from gas to solid.
C)The phase transition from gas to liquid.
D)The phase transition from liquid to gas.
E)The phase transition from liquid to solid.

Question 52

How much energy must be removed from a 125 g sample of benzene (molar mass = 78.11 g/mol)at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful.
ΔH_vap = 33.9 kJ/mol
ΔH_fus = 9.8 kJ/mol
C_liq = 1.73 J/g°C
C_gas = 1.06 J/g°C
C_sol = 1.51 J/g°C
T_melting = 279.0 K
T_boiling = 353.0 K

A)38.9 kJ
B)95.4 kJ
C)67.7 kJ
D)54.3 kJ
E)74.4 kJ

Question 53

Place the following substances in order of decreasing boiling point.
N₂ O₂ H₂

A)O₂ > H₂ > N₂
B)N₂ > H₂ > O₂
C)N₂ > O₂ > H₂
D)O₂ > N₂ > H₂
E)H₂ > N₂ > O₂

Question 54

Determine the vapor pressure (in torr)of a substance at 36°C,whose normal boiling point is 84°C and has a ΔH_vap of 22.1 kJ/mol.

A)239 torr
B)31.8 torr
C)41.8 torr
D)147 torr
E)98 torr

Question 55

Identify triple point.

A)The temperature,pressure,and density for a gas.
B)The temperature at which the boiling point equals the melting point.
C)The temperature and pressure where liquid,solid,and gas are equally stable and are in equilibrium.
D)The temperature that is unique for a substance.
E)The temperature at which the solid and liquid co-exist.

Question 56

How much energy is required to heat 87.1 g acetone (molar mass = 58.08 g/mol)from a solid at -154.0°C to a liquid at -42.0°C? The following physical data may be useful.
ΔH_fus = 7.27 kJ/mol
C_liq = 2.16 J/g°C
C_gas = 1.29 J/g°C
C_sol = 1.65 J/g°C
T_melting = -95.0°C

A)8.48 kJ
B)18.5 kJ
C)32.2 kJ
D)29.4 kJ
E)9.97 kJ

Question 57

Place the following substances in order of increasing vapor pressure at a given temperature.
NF₃ NH₃ BCl₃

A)NH₃ < NF₃ < BCl₃
B)NF₃ < NH₃ < BCl₃
C)BCl₃ < NF₃ < NH₃
D)NH₃ < BCl₃ < NF₃
E)BCl₃ < NH₃ < NF₃

Question 58

Consider the phase diagram below.If the dashed line at 1 atm of pressure is followed from 100 to 500°C,what phase changes will occur (in order of increasing temperature)?

A)condensation,followed by vaporization
B)sublimation,followed by deposition
C)vaporization,followed by deposition
D)fusion,followed by vaporization
E)No phase change will occur under the conditions specified.

Question 59

Define fusion.

A)The phase transition from solid to gas.
B)The phase transition from gas to solid.
C)The phase transition from gas to liquid.
D)The phase transition from liquid to solid.
E)The phase transition from solid to liquid.

Question 60

How much energy is required to heat 36.0 g H₂O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful.
ΔH_vap = 40.7 kJ/mol
C_liq = 4.18 J/g°C
C_gas = 2.01 J/g°C
C_sol = 2.09 J/g°C
T_melting = 0°C
T_boiling = 100°C

A)63.5 kJ
B)87.7 kJ
C)10.9 kJ
D)52.7 kJ
E)91.7 kJ

Question 61

Explain why the bolling point of water is so much higher than other compounds of similar molecular weight.

Question 62

Match the following.
CH₃CH₃

A)dipole-dipole forces
B)dispersion forces
C)ion-dipole forces
D)ionic bond
E)hydrogen bonding

Question 63

Why does the temperature of a substance stay constant during a phase change such as vaporization?

Question 64

Vanadium crystallizes in a body-centered cubic structure and has an atomic radius of 131 pm.Determine the density of vanadium,if the edge length of a bcc structure is 4r/
.

A)3.06 g/cm³
B)12.2 g/cm³
C)6.11 g/cm³
D)2.77 g/cm³
E)8.46 g/cm³

Question 65

If all of the following are in solid phase,which is considered a non-bonding atomic solid?

A)Ne
B)Fe
C)I₂
D)Ca
E)Li

Question 66

Define viscosity.

Question 67

Match the following.
CH₂F₂

A)dipole-dipole forces
B)dispersion forces
C)ion-dipole forces
D)ionic bond
E)hydrogen bonding

Question 68

Which of the following is considered a molecular solid?

A)Cu
B)NH₄NO₃
C)I₂
D)Xe
E)None of these is a molecular solid.

Question 69

Match the following.
CH₃OH

A)dipole-dipole forces
B)dispersion forces
C)ion-dipole forces
D)ionic bond
E)hydrogen bonding

Question 70

Why is the ΔH_vap higher than ΔH_fus for any given compound?

Question 71

Match the following.
LiI

A)dipole-dipole forces
B)dispersion forces
C)ion-dipole forces
D)ionic bond
E)hydrogen bonding

Question 72

Which of the following substances should have the highest melting point?

A)CO₂
B)SrS
C)Xe
D)F₂
E)MgO

Question 73

A metal crystallizes in a face centered cubic structure and has a density of 11.9 g/cm³.If the radius of the metal atom is 138 pm,what is the identity of the metal?

A)At
B)Pd
C)Mn
D)Fe
E)Cr

Question 74

Determine the radius of an Al atom (in pm)if the density of aluminum is 2.71 g/cm³.Aluminum crystallizes in a face centered cubic structure with an edge length of 2
R.

A)143 pm
B)227 pm
C)96 pm
D)172 pm
E)193 pm

Question 75

Match the following.
LiI + H₂O

A)dipole-dipole forces
B)dispersion forces
C)ion-dipole forces
D)ionic bond
E)hydrogen bonding

Question 76

Why do O,F and N,when bonded to H,form such strong intermolecular attractions to neighboring molecules? Make sure to be specific.

Question 77

Which of the following is considered an atomic solid?

A)Br₂
B)CsCl
C)N₂
D)Nb
E)None of these is an atomic solid.

Question 78

Define dynamic equilibrium as it relates to vapor pressure.

Question 79

Which of the following is considered an ionic solid?

A)(NH₄)₂CO₃
B)CCl₄
C)SeBr₂
D)XeF₄
E)None of these is an ionic solid.

Question 80

Which of the following substances should have the highest melting point?

A)Fe
B)Ne
C)Xe
D)N₂
E)CO