Question 1

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

Accepted Answer

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

Question 2

Choose the substance with the lowest viscosity in the liquid phase.

Accepted Answer

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

Question 3

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

Accepted Answer

A)  Ne 2 2 
B)  Cl2 2 2 2 2 2 
E)  Ne 2 2 
A)  Ne 2 2 
B)  Cl2 2 2 2 2 2 
E)  Ne 2 2

Question 4

Which of the following is considered an ionic solid?

Accepted Answer

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

Question 5

From the phase diagram of benzene given below, predict the temperature at triple point.

Accepted Answer

The answer of From the phase diagram of benzene given...

Question 6

Identify the type of solid for AgCl.

Accepted Answer

A)  metallic atomic solid 
B)  ionic solid 
C)  nonbonding atomic solid 
D)  molecular solid 
E)  networking atomic solid 
A)  metallic atomic solid 
B)  ionic solid 
C)  nonbonding atomic solid 
D)  molecular solid 
E)  networking atomic solid

Question 7

How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point if its ΔvapH is 24.3 kJ mol-1?

Accepted Answer

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

Question 8

Ethanol (     OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ mol-1. The specific heats of solid and liquid ethanol are 0.97 J g-1 °C-1 and 2.3 J g-1 °C-1, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -145 °C to liquid ethanol at -60 °C?

Accepted Answer

A)  6.58 
B)  9.96 
C)  8.88 
D)  3859 
E)  -13.56 
A)  6.58 
B)  9.96 
C)  8.88 
D)  3859 
E)  -13.56

Question 9

Match the following.
-LiI + H2O

Accepted Answer

A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond 
A) dipole-dipole forces 
B) ion-dipole forces 
C) H2 + H2O 
D) dispersion forces 
E) hydrogen bonding
F)ionic bond

Question 10

Identify the compound that does not have dipole-dipole forces as its strongest force.

Accepted Answer

A)  CH2Cl2 
B)  CH3OCH3 
C)  CH3Br 
D)  HCCl3 
E)  CO2 
A)  CH2Cl2 
B)  CH3OCH3 
C)  CH3Br 
D)  HCCl3 
E)  CO2

Question 11

Choose the substance with the lowest boiling point.

Accepted Answer

A)  Diethyl ether 
B)  Ethanol 
C)  Methanol 
D)  Propanol 
E)  Butanol 
A)  Diethyl ether 
B)  Ethanol 
C)  Methanol 
D)  Propanol 
E)  Butanol

Question 12

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

Accepted Answer

A)  H2 
B)  SO2 
C)  NH3 
D)  CF4 
E)  BCl3 
A)  H2 
B)  SO2 
C)  NH3 
D)  CF4 
E)  BCl3

Question 13

The forces between polar molecules is known as ________.

Accepted Answer

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

Question 14

Cesium has a radius of 272 pm and crystallizes in a body-centred cubic structure. What is the edge length of the unit cell?

Accepted Answer

A)  314 pm 
B)  385 pm 
C)  544 pm 
D)  628 pm 
A)  314 pm 
B)  385 pm 
C)  544 pm 
D)  628 pm

Question 15

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

Accepted Answer

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

Question 16

Choose the substance with the highest boiling point.

Accepted Answer

A)  CH4 
B)  KI 
C)  CS2 
D)  HF 
E)  I2 
A)  CH4 
B)  KI 
C)  CS2 
D)  HF 
E)  I2

Question 17

Choose the substance with the highest surface tension in the liquid phase.

Accepted Answer

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

Question 18

Which pairs of substances would form homogeneous solutions when combined?

Accepted Answer

A)  CH2Cl2 and water 
B)  Diethyl ether and water 
C)  Glucose and water 
D)  CCl4 and water 
A)  CH2Cl2 and water 
B)  Diethyl ether and water 
C)  Glucose and water 
D)  CCl4 and water

Question 19

Assign the appropriate labels to the phase diagram shown below.

Accepted Answer

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 
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 20

Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ mol-1. How much heat could be removed by 20.0 g of ethyl chloride?

Accepted Answer

A)  8.18 kJ 
B)  341 kJ 
C)  528 kJ 
D)  3410 kJ 
A)  8.18 kJ 
B)  341 kJ 
C)  528 kJ 
D)  3410 kJ

Exam 11: Liquids, Solids, and Intermolecular Forces

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

Choose the substance with the lowest viscosity in the liquid phase.

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

Which of the following is considered an ionic solid?

From the phase diagram of benzene given below, predict the temperature at triple point.

Identify the type of solid for AgCl.

How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point if its ΔvapH is 24.3 kJ mol-1?

Ethanol ( OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ mol-1. The specific heats of solid and liquid ethanol are 0.97 J g-1 °C-1 and 2.3 J g-1 °C-1, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -145 °C to liquid ethanol at -60 °C?

Match the following. -LiI + H2O

Identify the compound that does not have dipole-dipole forces as its strongest force.

Choose the substance with the lowest boiling point.

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

The forces between polar molecules is known as ________.

Cesium has a radius of 272 pm and crystallizes in a body-centred cubic structure. What is the edge length of the unit cell?

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

Choose the substance with the highest boiling point.

Choose the substance with the highest surface tension in the liquid phase.

Which pairs of substances would form homogeneous solutions when combined?

Assign the appropriate labels to the phase diagram shown below.

Ethyl chloride, C2H5Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ mol-1. How much heat could be removed by 20.0 g of ethyl chloride?

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

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

Place the following substances in order of increasing boiling point. Ne Cl₂O₂

How much energy is required to vaporize 158 g of butane (C₄H₁₀) at its boiling point if its Δ_vapH is 24.3 kJ mol^-1?

Ethanol ( OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ mol^-1. The specific heats of solid and liquid ethanol are 0.97 J g^-1 °C^-1 and 2.3 J g^-1 °C^-1, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -145 °C to liquid ethanol at -60 °C?

Match the following. -LiI + H₂O

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

Ethyl chloride, C₂H₅Cl, is used as a local anesthetic. It works by cooling tissue as it vaporizes; its heat of vaporization is 26.4 kJ mol^-1. How much heat could be removed by 20.0 g of ethyl chloride?