Question 1

Which type of bonding does Sr form upon solidification?

Accepted Answer

A) covalent network 
B) ionic 
C) metallic 
D) molecular 
A) covalent network 
B) ionic 
C) metallic 
D) molecular

Question 2

Which combination of "type of solid" and specific example is INCORRECT?

Accepted Answer

A) ionic/"table salt" 
B) metallic/copper wire 
C) molecular/"dry ice" 
D) network covalent/iodine 
E) network covalent/silicon carbide 
A) ionic/"table salt" 
B) metallic/copper wire 
C) molecular/"dry ice" 
D) network covalent/iodine 
E) network covalent/silicon carbide

Question 3

The process in which a gas is transformed into a solid is called ________.

Accepted Answer

A) vaporization 
B) condensation 
C) solidification 
D) deposition 
E) fusion 
A) vaporization 
B) condensation 
C) solidification 
D) deposition 
E) fusion

Question 4

How many H- ions are around each Na+ ion in NaH,which has a cubic unit cell with H- ions on each corner and each face?

Accepted Answer

A) 1 
B) 4 
C) 6 
D) 8 
A) 1 
B) 4 
C) 6 
D) 8

Question 5

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

Accepted Answer

A) At the temperature and pressure of point 1,substance U exists as a three-phase equilibrium system. 
B) At the temperature and pressure of point 2,substance U exists as a one-phase gaseous system. 
C) At the temperature and pressure of point 3,substance U exists as a two-phase system. 
D) If the U(s)⇔ U(l)system is maintained at the temperature of point 4 while pressure is decreased steadily to about 300 Torr,more U will freeze. 
E) There are no conditions of temperature and pressure under which solid U will vaporize without melting first. 
A) At the temperature and pressure of point 1,substance U exists as a three-phase equilibrium system. 
B) At the temperature and pressure of point 2,substance U exists as a one-phase gaseous system. 
C) At the temperature and pressure of point 3,substance U exists as a two-phase system. 
D) If the U(s)⇔ U(l)system is maintained at the temperature of point 4 while pressure is decreased steadily to about 300 Torr,more U will freeze. 
E) There are no conditions of temperature and pressure under which solid U will vaporize without melting first.

Question 6

Given the data below,determine the normal boiling point of liquid Rb.
P1 = 400 mmHg,t1 = 620 °C,ΔvapH = 78.5 kJ/mol

Accepted Answer

A) 374 °C 
B) 920 °C 
C) 647 °C 
D) 951 °C 
E) 678 °C 
A) 374 °C 
B) 920 °C 
C) 647 °C 
D) 951 °C 
E) 678 °C

Question 7

Which of the following forms an ionic solid?

Accepted Answer

A) Cu 
B) C2H5NH2 
C) NH4NO3 
D) NO2 
A) Cu 
B) C2H5NH2 
C) NH4NO3 
D) NO2

Question 8

List the following ionic compounds in order of increasing solubility in water:
RbI,CaO,KCl

Accepted Answer

A) RbI,CaO,KCl 
B) KCl,CaO,RbI 
C) KCl,RbI,CaO 
D) CaO,KCl,RbI 
E) RbI,KCl,CaO 
A) RbI,CaO,KCl 
B) KCl,CaO,RbI 
C) KCl,RbI,CaO 
D) CaO,KCl,RbI 
E) RbI,KCl,CaO

Question 9

Gold crystallizes in a face-centred cubic structure.What is the edge length of the unit cell if the atomic radius of gold is 144 pm?

Accepted Answer

A) 204 pm 
B) 288 pm 
C) 333 pm 
D) 407 pm 
A) 204 pm 
B) 288 pm 
C) 333 pm 
D) 407 pm

Question 10

Which of the following statements concerning molecules in the liquid state is true?

Accepted Answer

A) Cohesive forces are not important. 
B) The molecules contract to fit the size of the container. 
C) The molecules have no motion. 
D) The molecules are in a patterned (oriented)arrangement. 
E) The molecules are mobile and relatively close together. 
A) Cohesive forces are not important. 
B) The molecules contract to fit the size of the container. 
C) The molecules have no motion. 
D) The molecules are in a patterned (oriented)arrangement. 
E) The molecules are mobile and relatively close together.

Question 11

Which probably has the lowest boiling point at 1.0 atm pressure?

Accepted Answer

A) PbH4  
B) SnH4  
C) SiH4  
D) GeH4  
E) CH4  
A) PbH4  
B) SnH4  
C) SiH4  
D) GeH4  
E) CH4

Question 12

The enthalpy of fusion is:

Accepted Answer

A) the quantity of heat required to melt one mole of a solid 
B) the quantity of heat released when a solid melts 
C) the quantity of heat when two elements are fused together to produce binary compound 
D) the quantity of heat required to fuse two atomic nuclei 
E) the quantity of heat released when an organic compound burns in an atmosphere of pure oxygen 
A) the quantity of heat required to melt one mole of a solid 
B) the quantity of heat released when a solid melts 
C) the quantity of heat when two elements are fused together to produce binary compound 
D) the quantity of heat required to fuse two atomic nuclei 
E) the quantity of heat released when an organic compound burns in an atmosphere of pure oxygen

Question 13

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

Accepted Answer

A) -633 kcal mol-1 
B) -450 kcal mol-1 
C) -71 kcal mol-1 
D) -696 kcal mol-1 
E) +712 kcal mol-1 
A) -633 kcal mol-1 
B) -450 kcal mol-1 
C) -71 kcal mol-1 
D) -696 kcal mol-1 
E) +712 kcal mol-1

Question 14

Consider a parallelepiped with all edges being equal in length.There is an atom at each corner and one in the center.This is a simple cubic cell.

Accepted Answer

A) True 
 B)False

Question 15

Which of the following describe the critical point of a liquid?
I.the temperature and pressure at which a liquid's meniscus disappears
II.the point where the vapor pressure curve intersects the fusion temperature curve
III.the highest temperature and pressure at which a liquid can exist
IV.the highest temperature at which it is possible to obtain a liquid from its vapor by increasing pressure

Accepted Answer

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

Question 16

The heat of deposition equals the negative of the heat of sublimation.

Accepted Answer

A) True 
 B)False

Question 17

Which of the following keeps the rate of vaporization unchanged?

Accepted Answer

A) closing container lid 
B) increasing forces between molecules 
C) increasing mass of molecule 
D) decreasing temperature 
E) decreasing surface area 
A) closing container lid 
B) increasing forces between molecules 
C) increasing mass of molecule 
D) decreasing temperature 
E) decreasing surface area

Question 18

A compound of iron and sulfur crystallizes in a lattice pattern described as cubic closest packed sulfide ions,with iron ions in all octahedral sites.What is its empirical formula?

Accepted Answer

A) FeS 
B) FeS2  
C) Fe3S4  
D) Fe2S 
E) Fe2S3  
A) FeS 
B) FeS2  
C) Fe3S4  
D) Fe2S 
E) Fe2S3

Question 19

The relationship between the vapor pressure of a liquid and temperature can be expressed by the Clausius-Clapeyron equation:
Ln[P2/P1] = [ΔvapH/R] × [1/T1 - 1/T2]
Ethanol (C2H5OH)has a normal boiling point of 78.3 °C and,with ΔvapH = 39.3 kJ/mol.What is the vapor pressure of ethanol at 50.0 °C?

Accepted Answer

A) 118 Torr 
B) 234 Torr 
C) 354 Torr 
D) 485 Torr 
E) 670 Torr 
A) 118 Torr 
B) 234 Torr 
C) 354 Torr 
D) 485 Torr 
E) 670 Torr

Question 20

The maximum temperature at which a gas can be liquefied is just below the ________.

Accepted Answer

A) boiling temperature 
B) critical temperature 
C) melting temperature 
D) normal temperature 
E) superheating temperature 
A) boiling temperature 
B) critical temperature 
C) melting temperature 
D) normal temperature 
E) superheating temperature

Exam 12: Intermolecular Forces: Liquids and Solids

Which type of bonding does Sr form upon solidification?

Which combination of "type of solid" and specific example is INCORRECT?

The process in which a gas is transformed into a solid is called ________.

How many H- ions are around each Na+ ion in NaH,which has a cubic unit cell with H- ions on each corner and each face?

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

Given the data below,determine the normal boiling point of liquid Rb. P1 = 400 mmHg,t1 = 620 °C,ΔvapH = 78.5 kJ/mol

Which of the following forms an ionic solid?

List the following ionic compounds in order of increasing solubility in water: RbI,CaO,KCl

Gold crystallizes in a face-centred cubic structure.What is the edge length of the unit cell if the atomic radius of gold is 144 pm?

Which of the following statements concerning molecules in the liquid state is true?

Which probably has the lowest boiling point at 1.0 atm pressure?

The enthalpy of fusion is:

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

Consider a parallelepiped with all edges being equal in length.There is an atom at each corner and one in the center.This is a simple cubic cell.

The heat of deposition equals the negative of the heat of sublimation.

Which of the following keeps the rate of vaporization unchanged?

A compound of iron and sulfur crystallizes in a lattice pattern described as cubic closest packed sulfide ions,with iron ions in all octahedral sites.What is its empirical formula?

The maximum temperature at which a gas can be liquefied is just below the ________.

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

How many H^- ions are around each Na⁺ ion in NaH,which has a cubic unit cell with H^- ions on each corner and each face?

Given the data below,determine the normal boiling point of liquid Rb. P₁ = 400 mmHg,t₁ = 620 °C,Δ_vapH = 78.5 kJ/mol

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