1) Crystalline solids __________.
A) have their particles arranged randomly
B) have highly ordered structures
C) are usually very soft
D) exist only at high temperatures
E) exist only at very low temperatures
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
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
As a gaseous element condenses, the atoms become __________ and they have __________ attraction for one another.
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
6) Together, liquids and solids constitute __________ phases of matter.
A) the compressible
B) the fluid
C) the condensed
D) all of the
E) the disordered
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.
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
9) Which one of the following exhibits dipole-dipole attraction between molecules?
A) XeF4
B) AsH3
C) CO2
D) BCl3
E) Cl2
10) Which one of the following exhibits dipole-dipole attraction between molecules?
A) PH3
B) CCl4
C) Br2
D) CO2
E) C10H22
Of the following substances, only __________ has London dispersion forces as its only intermolecular force.
A) CH3OH
B) NH3
C) H2S
D) CH4
E) HCl
A) H2O
C) HF
D) CH3COOH
E) PH3
Of the following substances, only __________ has London dispersion forces as the only intermolecular force.
D) Kr
Which one of the following should have the lowest boiling point?
B) H2S
C) HCl
D) SiH4
E) H2O
C) NH3
D) HCl
E) CH4
Of the following substances, __________ has the highest boiling point.
B) CO2
C) CH4
E) NH3
A) CH3CH2OH
B) C2H6
C) N2
D) F2
E) HOCH2CH2OH
Of the following, __________ has the highest boiling point.
A) N2
B) Br2
C) H2
D) Cl2
E) O2
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
Which of the following has dispersion forces as its only intermolecular force?
B) HCl
D) NaCl
E) CH3Cl
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
__________ 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,
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
Which one of the following derivatives of ethane has the highest boiling point?
A) C2Br6
B) C2F6
C) C2I6
D) C2Cl6
E) C2H6
What is the predominant intermolecular force in CBr4?
A) London-dispersion forces
B) ion-dipole attraction
C) ionic bonding
D) dipole-dipole attraction
E) hydrogen-bonding
What is the predominant intermolecular force in CH3CH2OH?
D) induced dipole-dipole attraction
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
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
Hydrogen bonding is a special case of __________.
C) dipole-dipole attractions
D) ion-ion interactions
E) none of the above
Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?
What intermolecular force is responsible for the fact that ice is less dense than liquid water?
B) dipole-dipole forces
C) ion-dipole forces
D) hydrogen bonding
E) ionic bonding
The predominant intermolecular force in (CH3)2NH is __________.
B) ion-dipole forces
D) dipole-dipole forces
E) hydrogen bonding
The predominant intermolecular force in AsH3 is __________.
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 ion-dipole
What type(s) of intermolecular forces exist between Cl2 and CO3-2?
A) dispersion forces
B) dispersion forces and ion-dipole
C) dispersion forces, ion-dipole, and induced dipole - induced dipole
D) dispersion forces and ion-induced dipole
E) dispersion forces, ion-dipole, dipole-dipole, and ion-induced dipole
What types of intermolecular forces exist between NH3 and CBr4?
A) dispersion forces and dipole-dipole forces
B) dispersion forces and dipole-induced dipole forces
C) dispersion forces and hydrogen bonds
D) dispersion forces, hydrogen bonds, and induced dipole-induced dipole forces
E) dispersion forces, hydrogen bonds, and dipole-induced dipole forces
What types of intermolecular forces exist between PH3 and N2?
Which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii) Viscosity increases as intermolecular forces increase.
A) (i) only
B) (ii) and (iii)
C) (i) and (iii)
D) none
E) all
The shape of a liquid's meniscus is determined by __________.
A) the viscosity of the liquid
B) the type of material the container is made of
C) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container
D) the amount of hydrogen bonding in the liquid
E) the volume of the liquid
Viscosity is __________.
A) the "skin" on a liquid surface caused by intermolecular attraction
B) the resistance to flow
C) the same as density
D) inversely proportional to molar mass
E) unaffected by temperature
How high a liquid will rise up a narrow tube as a result of capillary action depends on __________.
A) the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube, and gravity
B) gravity alone
C) only the magnitude of adhesive forces between the liquid and the tube
D) the viscosity of the liquid
E) only the magnitude of cohesive forces in the liquid
The property responsible for the "beading up" of water is __________.
A) density
B) viscosity
C) vapor pressure
D) surface tension
Heat of sublimation can be approximated by adding together __________ and __________.
A) heat of fusion, heat of condensation
B) heat of fusion, heat of vaporization
C) heat of freezing (solidification), heat of condensation
D) heat of freezing (solidification), heat of vaporization
E) heat of deposition, heat of vaporization
Which of the following statements is false?
A) The absolute value of the heat of sublimation is equal to the absolute value of the heat of deposition.
B) The heat of sublimation is equal to the sum of the heat of vaporization and the heat of melting.
C) The heat of sublimation is equal to the sum of the heat of vaporization and the heat of freezing.
D) The absolute value of the heat of sublimation is equal to the absolute value of the sum of the heat of condensation and the heat of freezing.
E) The absolute value of the heat of deposition is equal to sum of the absolute value of the heat of vaporization and the absolute value of the heat of freezing.
The phase changes B → C and D → E are not associated with temperature increases because the heat energy is used up to __________.
A) increase distances between molecules
B) break intramolecular bonds
C) rearrange atoms within molecules
D) increase the velocity of molecules
E) increase the density of the sample
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
Large intermolecular forces in a substance are manifested by __________.
A) low vapor pressure
B) high boiling point
C) high heats of fusion and vaporization
D) high critical temperatures and pressures
E) all of the above
The critical temperature and pressure of CS2 are 279°C and 78 atm, respectively. At temperatures above 279°C and pressures above 78 atm, CS2 can only occur as a __________.
A) solid
B) liquid
C) liquid and gas
D) gas
E) supercritical fluid
The substance with the largest heat of vaporization is __________.
A) I2
C) Cl2
Of the following, __________ is an exothermic process.
A) melting
B) subliming
C) freezing
D) boiling
E) All of the above are exothermic.
Of the following, __________ should have the highest critical temperature.
A) CBr4
C) CF4
E) H2
Of the following, __________ is the most volatile.
E) C6H14
Of the following, __________ is the least volatile.
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
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
The vapor pressure of a liquid __________.
A) increases linearly with increasing temperature
B) increases nonlinearly with increasing temperature
C) decreases linearly with increasing temperature
D) decreases nonlinearly with increasing temperature
E) is totally unrelated to its molecular structure
When the phase diagram for a substance has a solid-liquid phase boundary line that has a negative slope (leans to the left), the substance __________.
A) can go from solid to liquid, within a small temperature range, via the application of pressure
B) sublimes rather than melts under ordinary conditions
C) cannot go from solid to liquid by application of pressure at any temperature
D) cannot be liquefied above its triple point
E) melts rather than sublimes under ordinary conditions
The predominant intermolecular force in CaBr2 is __________.
Which of the following is most likely to exhibit liquid-crystalline behavior?
A) CH3CH2-C(CH3)2-CH2CH3
B) CH3CH2CH2CH2CH2CH2CH2CH3
C) CH3CH2CH2CH2CH2-Na+
D)
E)
Which of the following characteristics would prevent liquid crystal behavior?
A) long axial structure
B) ionic configuration
C) carbon-carbon single bonds
D) double bonding
E) polar groups
Molecules with only single bonds do not generally exhibit liquid-crystalline properties because __________.
A) molecules without multiple bonds lack the rigidity necessary for alignment
B) molecules without multiple bonds are too small to exhibit liquid-crystalline properties
C) molecules with only single bonds are gases
D) molecules with only single bonds are too big to exhibit liquid-crystalline properties
E) molecules without multiple bonds lack the flexibility necessary for alignment
Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point?
A) CH3CH2CH3
B) CH3OCH3
C) CH3Cl
D) CH3CHO
E) CH3CN
The normal boiling point of the substance with the phase diagram shown above is __________°C.
A) 10
B) 20
C) 30
D) 40
E) 50
In general, intramolecular forces determine the __________ properties of a substance and intermolecular forces determine its __________ properties.
A) Physical, Chemical
B) Chemical, Physical
The direct conversion of a solid to a gas is called __________.
A) Evaporation
B) Vaporization
C) Sublimation
D) Condensation
E) Deposition
The boiling points of normal hydrocarbons are higher than those of branched hydrocarbons of similar molecular weight because the London-dispersion forces between normal hydrocarbons are greater than those between branched hydrocarbons.
True
False
The principal source of the difference in the normal boiling points of ICl (97°C; molecular mass 162 amu) and Br2 (59°C; molecular mass 160 amu) is both dipole-dipole interactions and London dispersion forces.
Heats of vaporization are greater than heats of fusion.
Under ordinary conditions, a substance will sublime rather than melt if its triple point occurs at a pressure above atmospheric pressure.
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