Chemistry Chapter 11

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The strongest interparticle attractions exist between particles of a __________ and the weakest interparticle attractions exist between particles of a __________.
A) solid, liquid
B) solid, gas
C) liquid, gas
D) liquid, solid
E) gas, solid

B

Which one of the following exhibits dipole-dipole attraction between molecules? 

A) XeF4
B) AsH3
C) CO2
D) BCl3
E) Cl2

B

Hydrogen bonding is a special case of __________.
A) London-dispersion forces
B) ion-dipole attraction
C) dipole-dipole attractions
D) ion-ion interactions
E) none of the above

C

When NaCl dissolves in water, aqueous Na+ and Cl- ions result. The force of attraction that exists between Na+ and H2O is called a(n) __________ interaction.
A) dipole-dipole
B) ion-ion
C) hydrogen bonding
D) ion-dipole
E) London dispersion force

D

Of the following substances, only __________ has London dispersion forces as its only intermolecular force.
A) CH3OH
B) NH3
C) H2S
D) CH4
E) HCl

D

What is the predominant intermolecular force in ?
A) London-dispersion forces
B) ion-dipole attraction
C) ionic bonding
D) dipole-dipole attraction
E) hydrogen-bonding

A

Of the following substances, only __________ has London dispersion forces as the only intermolecular force.
A) CH3OH
B) NH3
C) H2S
D) Kr
E) HCl

D

Which of the following has dispersion forces as its only intermolecular force? 

A) CH4
B) HCl
C) C6H13NH2
D) NaCl
E) CH3Cl

A

Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists among different I2 molecules in the solid?
A) London dispersion forces
B) dipole-dipole rejections
C) ionic-dipole interactions
D) covalent-ionic interactions
E) dipole-dipole attractions

A

The predominant intermolecular force in CH3 -NH-CH3 is __________. 

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

E

C12H26 molecules are held together by __________.
A) ion-ion interactions
B) hydrogen bonding
C) ion-dipole interactions
D) dipole-dipole interactions
E) dispersion forces

E

Which of the following has hydrogen bonding as its only intermolecular force?
A) HF
B) H2O
C) C6H13NH2
D) C5H11OH
E) None, all exhibit dispersion forces.

E

Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?




Diagrams here

D

Which one of the following substances will not have hydrogen bonding as one of its intermolecular forces?

Diagrams here

A

The ease with which the charge distribution in a molecule can be distorted by an external electrical field is called the __________.
A) electronegativity
B) hydrogen bonding
C) polarizability
D) volatility
E) viscosity

C

__________ are particularly polarizable.
A) Small nonpolar molecules
B) Small polar molecules
C) Large nonpolar molecules
D) Large polar molecules
E) Large molecules, regardless of their polarity

E

In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces?

A) CH4
B) C5H11OH
C) C6H13NH2
D) CH3OH
E) CO2

D

Based on the following information, which compound has the strongest intermolecular forces?
Substance ΔHvap (kJ/mol)
Argon (Ar) 6.3
Benzene (C6H6) 31.0
Ethanol (C2H5OH) 39.3
Water (H2O) 40.8
Methane (CH4) 9.2


A) Argon
B) Benzene
C) Ethanol
D) Water
E) Methane

D

Based on molecular mass and dipole moment of the five compounds in this table, which should have the highest boiling point?

A) CH3CH2CH3
B) CH3OCH3
C) CH3Cl
D) CH3CHO
E) CH3CN

E

Which one of the following should have the lowest boiling point?
A) PH3
B) H2S
C) HCl
D) SiH4
E) H2O

D

Of the following substances, __________ has the highest boiling point.
A) H2O
B) CO2
C) CH4
D) Kr
E) NH3

A

Of the following, __________ has the highest boiling point.
A) N2
B) Br2
C) H2
D) Cl2
E) O2

B

Which one of the following derivatives of ethane has the highest boiling point?
A) C2Br6
B) C2F6
C) C2I6
D) C2Cl6
E) C2H6

C

The intermolecular force(s) responsible for the fact that CH4 has the lowest boiling point in the set CH4, SiH4, GeH4, SnH4 is/are __________.
A) Hydrogen bonding
B) dipole-dipole interactions
C) London dispersion forces
D) Mainly hydrogen bonding but also dipole-dipole interactions
E) Mainly London-dispersion forces but also dipole-dipole interactions

C

What intermolecular force is responsible for ice being less dense than liquid water?
A) London dispersion forces
B) dipole-dipole forces
C) ion-dipole forces
D) Hydrogen bonding
E) Ionic bonding

D

What types of intermolecular forces exist between HI and H2S?
A) dipole-dipole and ion-dipole
B) dispersion forces, dipole-dipole, and ion-dipole
C) dispersion forces, hydrogen bonding, dipole-dipole, and ion-dipole
D) dispersion forces and dipole-dipole
E) dispersion forces, dipole-dipole, and hydrogen bonding

D

What type(s) of intermolecular forces exist between Br2 and CCl4?
A) dispersion forces
B) dispersion forces and ion-dipole
C) dispersion forces and dipole-dipole
D) dispersion forces, ion-dipole, and dipole-dipole
E) None. Since both are gases at room temperature, they do not interact with each other.

A

Of the following, __________ is an exothermic process.
A) melting
B) subliming
C) freezing
D) boiling
E) All are exothermic.

C

Which of the following is NOT a phase change?
A) melting
B) diffusion
C) sublimation
D) vaporization

B

The direct change of a substance from a solid to a gas is called _____.
A) boiling
B) evaporation
C)sublimation
D) condensation

C

The escape of gas molecules from the surface of an uncontained liquid is known as _____.
A) evaporation
B) condensation
C)boiling
D) sublimation

A

The first particles to evaporate from a liquid are _____.
A) those with the lowest kinetic energy
B) those farthest from the surface of the liquid
C) those with the highest kinetic energy

C

Which of the following will evaporate the fastest?
A) water at 20°C
B) water at 40°C
C) water at 0°C
D) all of the above evaporate at the same rate.

B

A volatile liquid is one that __________.
A) is highly flammable
B) is highly viscous
C) is highly hydrogen-bonded
D) is highly cohesive
E) readily evaporates

E

Volatility and vapor pressure are __________.
A) inversely proportional to one another
B) directly proportional to one another
C) not related
D) the same thing
E) both independent of temperature

B

If a liquid is sealed in a container and kept at constant temperature, how does its vapor pressure change over time? 

A)It rises at first, then remains constant.
B)It rises at first, then falls.
C)It rises continuously.

A

An increase in the temperature of a contained liquid _____.
A) has no effect on the kinetic energy of the liquid
B) causes fewer particles to escape the surface of the liquid
C) decreases the vapor pressure of the liquid
D) causes the vapor pressure above the liquid to increase

D

When the vapor pressure of a liquid equals the atmospheric pressure, the liquid _____.
A) freezes
B) boils
C)condenses
D) No change is observed.

B

Water could be made to boil at 105°C instead of 100°C by _____.
A) increasing the air pressure on the water
B ) decreasing the air pressure above the water
C) decreasing the pressure on the water
D) applying a great deal of heat

A

Some things take longer to cook at high altitudes than at low altitudes because _____.
A) water boils at a lower temperature at high altitude than at low altitude
B) water boils at a higher temperature at high altitude than at low altitude
C) heat isn't conducted as well in low density air
D) natural gas flames don't burn as hot at high altitudes
E) there is a higher moisture content in the air at high altitude

A

What is the pressure when a liquid is boiling at its normal boiling point?
A)505 kPa
B) 101 kPa
C) 202 kPa
D) 0 kPa

B

Based on this figure, the boiling point of diethyl ether under an external pressure of 1.32 atm is _______°C. 

A) 10
B) 20
C) 30
D) 40
E) 0

D

Based on this figure, the boiling point of ethyl alcohol under an external pressure of 50 torr is _____°C.
A) 80
B) 60
C) 70
D) 40
E) 20

E

Based on this figure, the boiling point of water under an external pressure of 0.316 atm is ____ °C. 

A) 70
B) 40
C) 60
D) 80
E) 90

A

The phase diagram of a substance is shown to the right. The region that corresponds to the solid phase is _____.
A) w
B) x
C) y
D) z
E) x and y

A

On the phase diagram shown to the right, segment __________ corresponds to the conditions of temperature and pressure under which the solid and the gas of the substance are in equilibrium.
A) AB
B) AC
C) AD
D) CD
E) BC

B

On the phase diagram shown to the right, the coordinates of point ________ correspond to the critical temperature and pressure.
A) A
B) B
C) C
D) D
E) E

B

The normal boiling point of the substance with the phase diagram shown to the right is about _____°C.
A) 10
B) 20
C) 30
D) 40
E) 50

D

In this phase diagram, the area labeled ________ indicates the gas phase for the substance.
A) w
B) x
C) y
D) z
E) y and z

C

According to this phase diagram, the normal boiling point of this substance is _______°C.
A) -3
B) 10
C) 29
D) 38
E) 0

C

In this phase diagram, the substance is a __________ at 25 °C and 1.0 atm.
A) solid
B) liquid
C) gas
D) supercritical fluid
E) crystal

B

On a phase diagram, the melting point is the same as the __________.
A) triple point
B) critical point
C) freezing point
D) boiling point
E) vapor-pressure curve

C

A gas is __________ and assumes __________ of its container whereas a liquid is __________ and assumes __________ of its container.
A) compressible, the volume and shape, not compressible, the shape of a portion
B) compressible, the shape, not compressible, the volume and shape
C) compressible, the volume and shape, compressible, the volume
D) condensed, the volume and shape, condensed, the volume and shape
E) condensed, the shape, compressible, the volume and shape

A

In liquids, the attractive intermolecular forces are __________.
A) very weak compared with kinetic energies of the molecules
B) strong enough to hold molecules relatively close together
C) strong enough to keep the molecules confined to vibrating about their fixed lattice points
D) not strong enough to keep molecules from moving past each other
E) strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other

E

Which of the following is not a type of solid? 

A) ionic
B) molecular
C) supercritical
D) metallic
E) covalent-network

C

As a solid element melts, the atoms become __________ and they have __________ attraction for one another.
A) more separated, more
B) more separated, less
C) closer together, more
D) closer together, less
E) larger, greater

B

Together, liquids and solids constitute __________ phases of matter.
A) the compressible
B) the fluid
C) the condensed
D) all of the
E) the disordered

C

Which statement is true about liquids but not true about solids?
A) They flow and are highly ordered.
B) They are highly ordered and not compressible.
C) They flow and are compressible.
D) They assume both the volume and the shape of their containers.
E) They flow and are not compressible.

C

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