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Test 1 Review

Chem 2

QuestionAnswer
As a solid element melts, the atoms become __________ and they have __________ attraction for one another. more separated, less
The strongest interparticle attractions exist between particles of a __________ and the weakest interparticle attractions exist between particles of a __________. solid, gas
Which one of the following exhibits dipole-dipole attraction between molecules? PH3
Of the following substances, only __________ has London dispersion forces as its only intermolecular force. CH4
Which one of the following should have the lowest boiling point? CH4
Of the following substances, __________ has the highest boiling point. H2O
What is the predominant intermolecular force in CBr4? London-dispersion forces
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. ion-dipole
Which of the following has dispersion forces as its only intermolecular force? CH4
The predominant intermolecular force in (CH3)2NH is __________. hydrogen bonding
What types of intermolecular forces exist between HI and H2S? dispersion forces and dipole-dipole
What types of intermolecular forces exist between NH3 and CBr4? dispersion forces and dipole-induced dipole forces
Which compound has the strongest intermolecular forces? CI4
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. T/F FALSE
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. T/F TRUE
Heats of vaporization are greater than heats of fusion. T/F TRUE
Under ordinary conditions, a substance will sublime rather than melt if its triple point occurs at a pressure above atmospheric pressure. T/F TRUE
Molecules containing only single bonds do not exhibit liquid-crystal behavior because free rotation can occur around single bonds making these molecules flexible. T/F TRUE
Of the following, __________ is the most volatile. CH4
A saturated solution __________. contains dissolved solute in equilibrium with undissolved solute
The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the __________. weak solvation of Na+ and Cl- by C6H6
The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the __________. weak solvation of Na+ and Cl- by C6H6
Which one of the following substances would be the most soluble in CCl4? C10H2^2
Which of the following substances is more likely to dissolve in CH3OH? CH3CH2OH
Which one of the following is most soluble in water? CH3OH
Which of the following statements is false? The weaker the attraction between the solute and solvent molecules, the greater the solubility.
A 0.100 m solution of which one of the following solutes will have the lowest vapor pressure? Al(ClO4)3
Of the following, a 0.1 M aqueous solution of __________ will have the highest freezing point. sucrose
A sample of potassium chlorate (15.0 g) is dissolved in 201 g of water at 70°C, with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0°C and no precipitate is observed. This solution is __________. unsaturated
As a gaseous element condenses, the atoms become __________ and they have __________ attraction for one another. closer together, more
Which one of the following exhibits dipole-dipole attraction between molecules? AsH3
Which one of the following should have the lowest boiling point? SiH4
Of the following substances, __________ has the highest boiling point. HOCH2CH2OH
The predominant intermolecular force in CH3CH2OH is __________. hydrogen bonding
The intermolecular fore(s) responsible for the fact that CH4 has the lowest boiling point in the set CH4, SiH4, GeH4, SnH4 is/are ____. london dispersion forces
What intermolecular force is responsible for the fact that ice is less dense than liquid in water? hydrogen bonding
The predominant intermolecular force in AsH3 is __________. dipole-dipole forces
Which of the following molecules has hydrogen bonding as its ONLY intermolecular force? none of the above exhibit dispersion forces.
What type(s) of intermolecular forces exist between Br2 and CCl4? dispersion forces
Which types of intermolecular forces exist between PH3 and N2? dispersion forces and dipole-induced dipole forces
____ is the energy required to expand the surface area of a liquid by a unit amount of area. surface tension
Viscosity is ____. the resistance to flow
Of the following, ____ is an exothermic process. freezing
Of the following, __________ is the least volatile. CBr4
A subsaturated solution ____. is one with a higher concentration than the solubility.
In a saturated solution of a salt in water, ____. the rate of crystallization = the rate of dissolution.
A solution with a concentration higher than the solubility is ____. is supersaturated
Which one of the following substances would be the least soluble in CCl4? NaCl
Which one of the following is least soluble in water? CH3CH2CH2CH2CH2OH
Pressure has an appreciable effect on the solubility of ____ in liquids. gases
Which one of the following concentration units varies with temperature? molarity
A 0.100 M solution of which one of the following solutes will have the highest vapor pressure? sucrose
Of the following, a 0.1 M aqueous solution of __________ will have the lowest freezing point. Al(NO3)3
Which one of the following solutes has a limiting van't Hoff factor (i) of 3 when dissolved in water? Na2SO4
A sample potassium nitrate (49.0 g) dissolved in 101 g water at 100 °C, with precautions to avoid evaporation of water. The solution is cooled to 30.0 °C and no precipitate is observed. The solution is ____. supersaturated
Created by: aarell82
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