Question 1

Based on intermolecular forces, which of the following will have the highest boiling point?

Accepted Answer

A)  SF4 
B)  AsF5 
C)  PF5 
D)  More information is needed to answer the question 
A)  SF4 
B)  AsF5 
C)  PF5 
D)  More information is needed to answer the question

Question 2

On the basis of your knowledge of bonding in liquids and solids, which of the following substances has the highest melting temperature?

Accepted Answer

A)  CH4 
B)  H2O 
C)  Br2 
D)  SO2 
E)  KBr 
A)  CH4 
B)  H2O 
C)  Br2 
D)  SO2 
E)  KBr

Question 3

The table below lists the ionic radii for the cations and anions in three ionic compounds.   Each compound has a cubic structure like NaCl, CsCl, or ZnS. Use the ratio of cation radius to anion radius to predict the structure formed (that of NaCl, CsCl, or ZnS). Then estimate the density of each compound. For ZnS structures, the holes occupied lie along the body diagonals of the unit cell so that 1/4 (body diagonal) = r+ + r-.

Accepted Answer

SnO₂: NaCl structure;

Question 4

Make a sketch to show the hydrogen bonding between two acetic acid molecules (HC2H3O2).

Accepted Answer

Question 5

The unit cell in this two-dimensional crystal contains __________ Xs and __________ Os.

Accepted Answer

A)  1, 4 
B)  1, 2 
C)  2, 1 
D)  1, 1 
E)  4, 1 
A)  1, 4 
B)  1, 2 
C)  2, 1 
D)  1, 1 
E)  4, 1

Question 6

What is the radius of the largest sphere that can be placed at the center of a face-centered cubic unit cell of a cubic closest-packed array of spheres if the spheres have diameters of 4.00 F1F1F1S1F1F1F10 102 pm?

Accepted Answer

A)  2.0 F1F1F1S1F1F1F10 102 pm 
B)  41.5 pm 
C)  83.0 pm 
D)  4.0 F1F1F1S1F1F1F10 102 pm 
E)  none of these 
A)  2.0 F1F1F1S1F1F1F10 102 pm 
B)  41.5 pm 
C)  83.0 pm 
D)  4.0 F1F1F1S1F1F1F10 102 pm 
E)  none of these

Question 7

Knowing that F1F1F1S1F1F1F10Hvap for water is 40.7 kJ/mol, calculate Pvap of water at 37°C.

Accepted Answer

A)  12.4 torr 
B)  52.6 torr 
C)  18.7 torr 
D)  6.90 torr 
E)  25.4 torr 
A)  12.4 torr 
B)  52.6 torr 
C)  18.7 torr 
D)  6.90 torr 
E)  25.4 torr

Question 8

Which of the following chemical species has the highest boiling point?

Accepted Answer

A)  H2 
B)  He 
C)  CH4 
D)  NO 
E)  N2 
A)  H2 
B)  He 
C)  CH4 
D)  NO 
E)  N2

Question 9

100. g of ice at 0°C is added to 300.0 g of water at 60°C. Assuming no transfer of heat to the surroundings, what is the temperature of the liquid water after all the ice has melted?

Accepted Answer

The answer of 100. g of ice at 0°C is...

Question 10

In the unit cell of sphalerite, Zn2+ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S2- ions. What is the number of formula units of ZnS in the unit cell?

Accepted Answer

A)  3 
B)  5 
C)  4 
D)  1 
E)  2 
A)  3 
B)  5 
C)  4 
D)  1 
E)  2

Question 11

KCl crystallizes in a structure like NaCl. The ionic radius of Na+ is 0.525 times the ionic radius of Cl- and 0.714 times the ionic radius of K+.
A) Estimate the ratio of the unit cell edge length for KCl to that for NaCl.
B) Estimate the ratio of the density of NaCl to that of KCl.

Accepted Answer

Question 12

Which statement regarding water is true?

Accepted Answer

A)  Liquid water is less dense than solid water. 
B)  Only covalent bonds are broken when ice melts. 
C)  Hydrogen bonds are stronger than covalent bonds. 
D)  Energy must be given off in order to break down the crystal lattice of ice to a liquid. 
E)  All of these statements are false. 
A)  Liquid water is less dense than solid water. 
B)  Only covalent bonds are broken when ice melts. 
C)  Hydrogen bonds are stronger than covalent bonds. 
D)  Energy must be given off in order to break down the crystal lattice of ice to a liquid. 
E)  All of these statements are false.

Question 13

Based on the phase diagram shown below, which of the following statements are correct? 
I. Sublimation occurs at a point in the transformation that falls along a straight line from point A to point F.
II. C and E represent points where the gas and liquid phases are in equilibrium.
III. (F1F1F1S1F1F1F10Hvap can be measured at point B).
IV. Molecules at point D have a greater average kinetic energy than those at point F.
V. The temperature at point E is called the critical temperature of the compound.

Accepted Answer

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

Question 14

Which of the following statements is(are) false? 
I.The hexagonal closest-packed structure is ABAB....
II.A body-centered cubic unit cell has four atoms per unit cell.
III.For unit cells having the same edge length, a simple cubic structure would have a smaller density than a body-centered cube.
IV.Atoms in a solid consisting of only one element would have six nearest neighbors if the crystal structure was a simple cubic array.

Accepted Answer

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

Question 15

The triple point of CO2 is at 5.2 atm and -57°C. Under atmospheric conditions present in a typical Boulder, Colorado, laboratory (P = 630 torr, T = 23°C), solid CO2 will

Accepted Answer

A)  remain solid. 
B)  melt. 
C)  boil. 
D)  sublime. 
A)  remain solid. 
B)  melt. 
C)  boil. 
D)  sublime.

Question 16

The molar volume of a certain form of solid lead is 18 cmS1U1P13S1S1P0/mol. Assuming cubic closest-packed structure, determine the following.
-The volume of a single cell

Accepted Answer

A)  1.20 F1F1F1S1F1F1F10 106 pm3 
B)  1.20 F1F1F1S1F1F1F10 108 pm3 
C)  1.20 F1F1F1S1F1F1F10 104 pm3 
D)  1.20 F1F1F1S1F1F1F10 102 pm3 
E)  none of these 
A)  1.20 F1F1F1S1F1F1F10 106 pm3 
B)  1.20 F1F1F1S1F1F1F10 108 pm3 
C)  1.20 F1F1F1S1F1F1F10 104 pm3 
D)  1.20 F1F1F1S1F1F1F10 102 pm3 
E)  none of these

Question 17

Pure rubidium crystallizes in a body-centered cubic lattice; the edge length of the unit cell is 562 pm. What is the density of rubidium in grams per cubic centimeter?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 18

A material is made from Al, Ga, and As. The mole fractions of these elements are 0.25, 0.26, and 0.49, respectively. This material would be

Accepted Answer

A)  an insulator. 
B)  an n-type semiconductor. 
C)  a metallic conductor because Al is present. 
D)  a p-type semiconductor. 
E)  none of these 
A)  an insulator. 
B)  an n-type semiconductor. 
C)  a metallic conductor because Al is present. 
D)  a p-type semiconductor. 
E)  none of these

Question 19

The normal boiling point of liquid X is less than that of Y, which is less than that of Z. Which of the following is the correct order of increasing vapor pressure of the three liquids at STP?

Accepted Answer

A)  Z, Y, X 
B)  Y, Z, X 
C)  X, Z, Y 
D)  Y, X, Z 
E)  X, Y, Z 
A)  Z, Y, X 
B)  Y, Z, X 
C)  X, Z, Y 
D)  Y, X, Z 
E)  X, Y, Z

Question 20

The heat of vaporization of a certain refrigerant is 148 J/g. Calculate the number of kilograms of refrigerant that must be evaporated to freeze a tray of 16 one-ounce (1 oz = 28 g) ice cubes starting with the water at 15°C. Heat capacity (water) = 4.184 J/g °C
F1F1F1S1F1F1F10Hfusion (water) = 333 J/g

Accepted Answer

A)  0.82 kg 
B)  1.2 kg 
C)  4.2 kg 
D)  1.1 kg 
E)  0.19 kg 
A)  0.82 kg 
B)  1.2 kg 
C)  4.2 kg 
D)  1.1 kg 
E)  0.19 kg

Based on intermolecular forces, which of the following will have the highest boiling point?

On the basis of your knowledge of bonding in liquids and solids, which of the following substances has the highest melting temperature?

Make a sketch to show the hydrogen bonding between two acetic acid molecules (HC₂H₃O₂).

The unit cell in this two-dimensional crystal contains Xs and Os.

What is the radius of the largest sphere that can be placed at the center of a face-centered cubic unit cell of a cubic closest-packed array of spheres if the spheres have diameters of 4.00  10² pm?

Knowing that H_vap for water is 40.7 kJ/mol, calculate P_vap of water at 37°C.

Which of the following chemical species has the highest boiling point?

100. g of ice at 0°C is added to 300.0 g of water at 60°C. Assuming no transfer of heat to the surroundings, what is the temperature of the liquid water after all the ice has melted?

In the unit cell of sphalerite, Zn²⁺ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S²^- ions. What is the number of formula units of ZnS in the unit cell?

KCl crystallizes in a structure like NaCl. The ionic radius of Na⁺ is 0.525 times the ionic radius of Cl^- and 0.714 times the ionic radius of K⁺. A) Estimate the ratio of the unit cell edge length for KCl to that for NaCl. B) Estimate the ratio of the density of NaCl to that of KCl.

Which statement regarding water is true?

The triple point of CO₂ is at 5.2 atm and -57°C. Under atmospheric conditions present in a typical Boulder, Colorado, laboratory (P = 630 torr, T = 23°C), solid CO₂ will

The molar volume of a certain form of solid lead is 18 cm³/mol. Assuming cubic closest-packed structure, determine the following. -The volume of a single cell

Pure rubidium crystallizes in a body-centered cubic lattice; the edge length of the unit cell is 562 pm. What is the density of rubidium in grams per cubic centimeter?

A material is made from Al, Ga, and As. The mole fractions of these elements are 0.25, 0.26, and 0.49, respectively. This material would be

The normal boiling point of liquid X is less than that of Y, which is less than that of Z. Which of the following is the correct order of increasing vapor pressure of the three liquids at STP?

The heat of vaporization of a certain refrigerant is 148 J/g. Calculate the number of kilograms of refrigerant that must be evaporated to freeze a tray of 16 one-ounce (1 oz = 28 g) ice cubes starting with the water at 15°C. Heat capacity (water) = 4.184 J/g °C H_fusion (water) = 333 J/g

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Exam 16: Liquids and Solids

Based on intermolecular forces, which of the following will have the highest boiling point?

On the basis of your knowledge of bonding in liquids and solids, which of the following substances has the highest melting temperature?

Make a sketch to show the hydrogen bonding between two acetic acid molecules (HC2H3O2).

The unit cell in this two-dimensional crystal contains __________ Xs and __________ Os.

What is the radius of the largest sphere that can be placed at the center of a face-centered cubic unit cell of a cubic closest-packed array of spheres if the spheres have diameters of 4.00  102 pm?

Knowing that Hvap for water is 40.7 kJ/mol, calculate Pvap of water at 37°C.

Which of the following chemical species has the highest boiling point?

100. g of ice at 0°C is added to 300.0 g of water at 60°C. Assuming no transfer of heat to the surroundings, what is the temperature of the liquid water after all the ice has melted?

In the unit cell of sphalerite, Zn2+ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S2- ions. What is the number of formula units of ZnS in the unit cell?

KCl crystallizes in a structure like NaCl. The ionic radius of Na+ is 0.525 times the ionic radius of Cl- and 0.714 times the ionic radius of K+. A) Estimate the ratio of the unit cell edge length for KCl to that for NaCl. B) Estimate the ratio of the density of NaCl to that of KCl.

Which statement regarding water is true?

The triple point of CO2 is at 5.2 atm and -57°C. Under atmospheric conditions present in a typical Boulder, Colorado, laboratory (P = 630 torr, T = 23°C), solid CO2 will

The molar volume of a certain form of solid lead is 18 cm3/mol. Assuming cubic closest-packed structure, determine the following. -The volume of a single cell

Pure rubidium crystallizes in a body-centered cubic lattice; the edge length of the unit cell is 562 pm. What is the density of rubidium in grams per cubic centimeter?

A material is made from Al, Ga, and As. The mole fractions of these elements are 0.25, 0.26, and 0.49, respectively. This material would be

The normal boiling point of liquid X is less than that of Y, which is less than that of Z. Which of the following is the correct order of increasing vapor pressure of the three liquids at STP?

The heat of vaporization of a certain refrigerant is 148 J/g. Calculate the number of kilograms of refrigerant that must be evaporated to freeze a tray of 16 one-ounce (1 oz = 28 g) ice cubes starting with the water at 15°C. Heat capacity (water) = 4.184 J/g °C Hfusion (water) = 333 J/g

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Make a sketch to show the hydrogen bonding between two acetic acid molecules (HC₂H₃O₂).

The unit cell in this two-dimensional crystal contains Xs and Os.

What is the radius of the largest sphere that can be placed at the center of a face-centered cubic unit cell of a cubic closest-packed array of spheres if the spheres have diameters of 4.00  10² pm?

Knowing that H_vap for water is 40.7 kJ/mol, calculate P_vap of water at 37°C.

In the unit cell of sphalerite, Zn²⁺ ions occupy half the tetrahedral holes in a face-centered cubic lattice of S²^- ions. What is the number of formula units of ZnS in the unit cell?

KCl crystallizes in a structure like NaCl. The ionic radius of Na⁺ is 0.525 times the ionic radius of Cl^- and 0.714 times the ionic radius of K⁺. A) Estimate the ratio of the unit cell edge length for KCl to that for NaCl. B) Estimate the ratio of the density of NaCl to that of KCl.

The triple point of CO₂ is at 5.2 atm and -57°C. Under atmospheric conditions present in a typical Boulder, Colorado, laboratory (P = 630 torr, T = 23°C), solid CO₂ will

The molar volume of a certain form of solid lead is 18 cm³/mol. Assuming cubic closest-packed structure, determine the following. -The volume of a single cell

The heat of vaporization of a certain refrigerant is 148 J/g. Calculate the number of kilograms of refrigerant that must be evaporated to freeze a tray of 16 one-ounce (1 oz = 28 g) ice cubes starting with the water at 15°C. Heat capacity (water) = 4.184 J/g °C H_fusion (water) = 333 J/g