Question 1

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 2

Arrange the following compounds in order of increasing viscosity:
I.1-propanol,CH3CH2CH2OH;
II.1,2-propanediol,CH3CH(OH)CH2OH;
III.1,2,3-propanetriol, (glycerol),HOCH2CH(OH)CH2OH.

Accepted Answer

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

Question 3

Lithium crystallizes in a body-centred cubic structure.What is the coordination number of each atom?

Accepted Answer

A) 4 
B) 6 
C) 8 
D) 12 
A) 4 
B) 6 
C) 8 
D) 12

Question 4

Which probably has the highest boiling point at 1.00 atm pressure?

Accepted Answer

A) H2NCH2CH2NH2  
B) CH3CH2CH2NH2  
C) (CH3)2CHNH2  
D) CH3CH2NHCH3  
E) (CH3)3N 
A) H2NCH2CH2NH2  
B) CH3CH2CH2NH2  
C) (CH3)2CHNH2  
D) CH3CH2NHCH3  
E) (CH3)3N

Question 5

Three types of holes of the cubic closest packed structure are:

Accepted Answer

A) trigonal,tetrahedral and octahedral 
B) tetrahedral,pyramidal and octahedral 
C) tetrahedral,bipyramidal and octahedral 
D) cubic,tetrahedral,and octahedral 
E) tetragonal,tetrahedral and octahedral 
A) trigonal,tetrahedral and octahedral 
B) tetrahedral,pyramidal and octahedral 
C) tetrahedral,bipyramidal and octahedral 
D) cubic,tetrahedral,and octahedral 
E) tetragonal,tetrahedral and octahedral

Question 6

When the vapor pressure of a liquid equals atmospheric pressure,the temperature of the liquid equals ________.

Accepted Answer

A) 100 °C 
B) the boiling point 
C) the normal boiling point 
D) the vaporization point 
E) the sublimation point 
A) 100 °C 
B) the boiling point 
C) the normal boiling point 
D) the vaporization point 
E) the sublimation point

Question 7

Given the following information,calculate ΔH° (in kcal mol-1)for: 
Cl(g)+ e- → Cl-(g)

Accepted Answer

A) + 83 kcal mol-1 
B) -83 kcal mol-1 
C) 161 kcal mol-1 
D) -112 kcal mol-1 
E) 190 kcal mol-1 
A) + 83 kcal mol-1 
B) -83 kcal mol-1 
C) 161 kcal mol-1 
D) -112 kcal mol-1 
E) 190 kcal mol-1

Question 8

A 0.90 g sample of liquid water was introduced into an evacuated 2.00 L flask,which was then sealed and heated to 37 °C.What percentage,by mass,of the water remained as liquid? [Vapor pressure of water at 37 °C = 48.2 Torr.]

Accepted Answer

A) 10% 
B) 18% 
C) 82% 
D) 90% 
E) 0% 
A) 10% 
B) 18% 
C) 82% 
D) 90% 
E) 0%

Question 9

The phenomenon in which a steel needle can,with proper care,be made to float on the surface of some water illustrates a property of liquids known as:

Accepted Answer

A) compressibility 
B) polarizability 
C) surface tension 
D) triple point 
E) viscosity 
A) compressibility 
B) polarizability 
C) surface tension 
D) triple point 
E) viscosity

Question 10

CHS1U1B14 S1U1B0probably has a lower boiling point at 1 atm than SnHS1U1B14S1U1B0.

Accepted Answer

A) True 
 B)False

Question 11

Under which of the following conditions will vaporization best occur?

Accepted Answer

A) high mass,large surface area,high kinetic energy 
B) weak forces between molecules,high kinetic energy,large surface area 
C) high molecular energy,small surface area 
D) low kinetic energy,strong molecular forces,large surface area 
E) small surface area,low kinetic energy,low molecular mass 
A) high mass,large surface area,high kinetic energy 
B) weak forces between molecules,high kinetic energy,large surface area 
C) high molecular energy,small surface area 
D) low kinetic energy,strong molecular forces,large surface area 
E) small surface area,low kinetic energy,low molecular mass

Question 12

The heat of fusion for napthalene (C10H8)is 18.98 kJ/mol and for sodium is 2.60 kJ/mol.The amount of heat that would melt 37.0 grams of napthalene would melt how many grams of sodium?

Accepted Answer

A) 0.909 g 
B) 1510 g 
C) 28.3 g 
D) 48.4 g 
E) 270.g 
A) 0.909 g 
B) 1510 g 
C) 28.3 g 
D) 48.4 g 
E) 270.g

Question 13

According to the phase diagram given,which of the following statements is INCORRECT?

Accepted Answer

A) At the temperature and pressure of point 1,W exists as a three-phase equilibrium system. 
B) At the temperature of point 2,a pressure of 500 Torr will cause W to liquefy. 
C) If the system is maintained at the temperature of point 3 while pressure is decreased,more W will vaporize. 
D) If W is maintained at the pressure of point 4 while the temperature is increased to 80 °C,the liquid will vaporize. 
E) The existence of liquid W at -40 °C and 500 Torr represents the metastable condition of "supercooling." 
A) At the temperature and pressure of point 1,W exists as a three-phase equilibrium system. 
B) At the temperature of point 2,a pressure of 500 Torr will cause W to liquefy. 
C) If the system is maintained at the temperature of point 3 while pressure is decreased,more W will vaporize. 
D) If W is maintained at the pressure of point 4 while the temperature is increased to 80 °C,the liquid will vaporize. 
E) The existence of liquid W at -40 °C and 500 Torr represents the metastable condition of "supercooling."

Question 14

The property that causes water to have a concave meniscus but mercury to have a convex meniscus is ________.

Accepted Answer

A) heat of vaporization 
B) sublimation 
C) surface tension 
D) vapor pressure 
E) critical point 
A) heat of vaporization 
B) sublimation 
C) surface tension 
D) vapor pressure 
E) critical point

Question 15

Which of the substances below would produce the hardest crystals?

Accepted Answer

A) SiC 
B) Xe 
C) Cu 
D) KNO3  
E) H2O 
A) SiC 
B) Xe 
C) Cu 
D) KNO3  
E) H2O

Question 16

Given the following information,calculate ΔH° (in kcal mol-1)for: LiCl(s)→ Cl-(g)+ Li+(g)

Accepted Answer

A) +73 kcal mol-1 
B) +148 kcal mol-1 
C) +216 kcal mol-1 
D) -96 kcal mol-1 
E) -49 kcal mol-1 
A) +73 kcal mol-1 
B) +148 kcal mol-1 
C) +216 kcal mol-1 
D) -96 kcal mol-1 
E) -49 kcal mol-1

Question 17

A liquid has a molar heat of vaporization of 22.7 kJ/mol.Its normal boiling point is 459 K.What is the vapor pressure,in mmHg,at 70 °C?

Accepted Answer

A) 102 mmHg 
B) 7.48 mmHg 
C) 56.8 mmHg 
D) 742 mmHg 
E) 580 mmHg 
A) 102 mmHg 
B) 7.48 mmHg 
C) 56.8 mmHg 
D) 742 mmHg 
E) 580 mmHg

Question 18

Vaporization occurs more readily with:

Accepted Answer

A) increased temperature,increased surface area,decreased volume 
B) increased temperature,increased surface area,increased intramolecular forces 
C) increased temperature,decreased surface area,decreased intermolecular forces 
D) increased temperature,increased surface area,decreased intermolecular forces 
E) decreased temperature,decreased surface area,decreased intermolecular forces 
A) increased temperature,increased surface area,decreased volume 
B) increased temperature,increased surface area,increased intramolecular forces 
C) increased temperature,decreased surface area,decreased intermolecular forces 
D) increased temperature,increased surface area,decreased intermolecular forces 
E) decreased temperature,decreased surface area,decreased intermolecular forces

Question 19

There are no types of crystalline solids that are held together by:

Accepted Answer

A) dipole-dipole interactions 
B) ionic attractions 
C) hydrogen bonds 
D) covalent bonds 
E) pi bonds only 
A) dipole-dipole interactions 
B) ionic attractions 
C) hydrogen bonds 
D) covalent bonds 
E) pi bonds only

Question 20

Which has the smallest dipole-dipole forces?

Accepted Answer

A) CH3Cl  
B) HBr  
C) O2 
D) NO  
A) CH3Cl  
B) HBr  
C) O2 
D) NO

Exam 12: Intermolecular Forces: Liquids and Solids

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

Arrange the following compounds in order of increasing viscosity: I.1-propanol,CH3CH2CH2OH; II.1,2-propanediol,CH3CH(OH)CH2OH; III.1,2,3-propanetriol, (glycerol),HOCH2CH(OH)CH2OH.

Lithium crystallizes in a body-centred cubic structure.What is the coordination number of each atom?

Which probably has the highest boiling point at 1.00 atm pressure?

Three types of holes of the cubic closest packed structure are:

When the vapor pressure of a liquid equals atmospheric pressure,the temperature of the liquid equals ________.

Given the following information,calculate ΔH° (in kcal mol-1)for: Cl(g)+ e- → Cl-(g)

A 0.90 g sample of liquid water was introduced into an evacuated 2.00 L flask,which was then sealed and heated to 37 °C.What percentage,by mass,of the water remained as liquid? [Vapor pressure of water at 37 °C = 48.2 Torr.]

The phenomenon in which a steel needle can,with proper care,be made to float on the surface of some water illustrates a property of liquids known as:

CH4 probably has a lower boiling point at 1 atm than SnH4.

Under which of the following conditions will vaporization best occur?

The heat of fusion for napthalene (C10H8)is 18.98 kJ/mol and for sodium is 2.60 kJ/mol.The amount of heat that would melt 37.0 grams of napthalene would melt how many grams of sodium?

According to the phase diagram given,which of the following statements is INCORRECT?

The property that causes water to have a concave meniscus but mercury to have a convex meniscus is ________.

Which of the substances below would produce the hardest crystals?

Given the following information,calculate ΔH° (in kcal mol-1)for: LiCl(s)→ Cl-(g)+ Li+(g)

A liquid has a molar heat of vaporization of 22.7 kJ/mol.Its normal boiling point is 459 K.What is the vapor pressure,in mmHg,at 70 °C?

Vaporization occurs more readily with:

There are no types of crystalline solids that are held together by:

Which has the smallest dipole-dipole forces?

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

Arrange the following compounds in order of increasing viscosity: I.1-propanol,CH₃CH₂CH₂OH; II.1,2-propanediol,CH₃CH(OH)CH₂OH; III.1,2,3-propanetriol, (glycerol),HOCH₂CH(OH)CH₂OH.

Given the following information,calculate ΔH° (in kcal mol^-1)for: Cl(g)+ e^- → Cl^-(g)

CH₄probably has a lower boiling point at 1 atm than SnH₄.

The heat of fusion for napthalene (C₁₀H₈)is 18.98 kJ/mol and for sodium is 2.60 kJ/mol.The amount of heat that would melt 37.0 grams of napthalene would melt how many grams of sodium?

Given the following information,calculate ΔH° (in kcal mol^-1)for: LiCl(s)→ Cl^-(g)+ Li⁺(g)