Question 1

Based on the phase diagram shown below, how will the melting point of the substance change if the pressure is increased above 1 atm

Accepted Answer

A)  The melting point will decrease. 
B)  The melting point will remain the same. 
C)  The melting point will increase. 
D)  The substance will not melt at pressures of 1 atm and above; instead, the solid sublimes to form the gas phase. 
A)  The melting point will decrease. 
B)  The melting point will remain the same. 
C)  The melting point will increase. 
D)  The substance will not melt at pressures of 1 atm and above; instead, the solid sublimes to form the gas phase.

Question 2

Suppose the atoms in a two-dimensional crystal have the following arrangement:   How many atoms are in one unit cell
A) One
B) Two
C) Three
D) Four
E) None of the above

Accepted Answer

A) True 
 B)False

Question 3

Which of following can form hydrogen bonds with water molecules
(1) Na+ (2) CH3COOH (3) C2H6 (4) CH3NH2

Accepted Answer

A)  (1) and (2) 
B)  (1) and (3) 
C)  (2) and (3) 
D)  (2) and (4) 
E)  (3) and (4) 
A)  (1) and (2) 
B)  (1) and (3) 
C)  (2) and (3) 
D)  (2) and (4) 
E)  (3) and (4)

Question 4

All intermolecular forces must be overcome in order for a substance to undergo a phase change from a solid to a liquid.

Accepted Answer

A) True 
 B)False

Question 5

Calculate the amount of enthalpy required to heat 25.0 g of solid benzene (C6H6) at -10$\circ$C to liquid benzene at 20.0$\circ$C. Thermodynamic data for benzene: specific heat of solid benzene = 1.52 J/g·$\circ$C; specific heat of liquid benzene = 1.73 J/g·$\circ$C; melting point = 5.5$\circ$C; $\Delta$Hfus = 9.9 kJ/mol.

Accepted Answer

A)  3.8 kJ 
B)  4.1 kJ 
C)  4.4 kJ 
D)  4.7 kJ 
E)  None of the above 
A)  3.8 kJ 
B)  4.1 kJ 
C)  4.4 kJ 
D)  4.7 kJ 
E)  None of the above

Question 6

MgO has the same crystal structure as NaCl, face-centered cubic. How many oxide ions surround each Mg2+ ion as nearest neighbors

Accepted Answer

A)  4 
B)  6 
C)  8 
D)  10 
E)  12 
A)  4 
B)  6 
C)  8 
D)  10 
E)  12

Question 7

Which one of the following crystallizes in a metallic lattice

Accepted Answer

A)  C 
B)  NaMnO4 
C)  K 
D)  LiClO4 
E)  K2Cr2O7 
A)  C 
B)  NaMnO4 
C)  K 
D)  LiClO4 
E)  K2Cr2O7

Question 8

The molar enthalpy of vaporization of carbon disulfide is 26.74 kJ/mol, and its normal boiling point is 46$\circ$C. What is the vapor pressure of CS2 at 0$\circ$C

Accepted Answer

A)  4160 torr 
B)  447 torr 
C)  313 torr 
D)  139 torr 
E)  5.47 torr 
A)  4160 torr 
B)  447 torr 
C)  313 torr 
D)  139 torr 
E)  5.47 torr

Question 9

Indicate all the types of intermolecular forces of attraction in SO2(l).

Accepted Answer

A)  Dispersion and Dipole-dipole 
B)  Dipole-dipole and Ionic 
C)  Ion-dipole and Hydrogen bonding 
D)  Hydrogen bonding and Dispersion 
E)  Dispersion 
A)  Dispersion and Dipole-dipole 
B)  Dipole-dipole and Ionic 
C)  Ion-dipole and Hydrogen bonding 
D)  Hydrogen bonding and Dispersion 
E)  Dispersion

Question 10

The vapor pressure of a liquid in a closed container depends upon

Accepted Answer

A)  the amount of liquid. 
B)  the surface area of the liquid. 
C)  the volume of the container. 
D)  the temperature. 
E)  none of the above. 
A)  the amount of liquid. 
B)  the surface area of the liquid. 
C)  the volume of the container. 
D)  the temperature. 
E)  none of the above.

Question 11

Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20$\circ$C to convert it to liquid water at 60.0$\circ$C. Given: specific heat (ice) = 2.1 J/g·$\circ$C; specific heat (water) = 4.18 J/g·$\circ$C; $\Delta$Hfus = 6.0 kJ/mol.

Accepted Answer

A)  63 kJ 
B)  7.5 J 
C)  420 J 
D)  2,900 J 
E)  6,300 J 
A)  63 kJ 
B)  7.5 J 
C)  420 J 
D)  2,900 J 
E)  6,300 J

Question 12

Which of the following is not true with regard to water

Accepted Answer

A)  Water has a high heat capacity. 
B)  Water has an unusually high boiling point. 
C)  Water can form hydrogen bonds. 
D)  Ice is more dense than liquid water. 
E)  Water is a polar molecule. 
A)  Water has a high heat capacity. 
B)  Water has an unusually high boiling point. 
C)  Water can form hydrogen bonds. 
D)  Ice is more dense than liquid water. 
E)  Water is a polar molecule.

Question 13

Indicate all the types of intermolecular forces of attraction in SF4(g).

Accepted Answer

A)  Dispersion and Dipole-dipole 
B)  Dipole-dipole and Ionic 
C)  Ion-dipole and Hydrogen bonding 
D)  Hydrogen bonding and Dispersion 
E)  Dispersion 
A)  Dispersion and Dipole-dipole 
B)  Dipole-dipole and Ionic 
C)  Ion-dipole and Hydrogen bonding 
D)  Hydrogen bonding and Dispersion 
E)  Dispersion

Question 14

Which of the following would be expected to have the highest vapor pressure at room temperature

Accepted Answer

A)  ethanol, bp = 78$\circ$C 
B)  methanol, bp = 65$\circ$C 
C)  water, bp = 100$\circ$C 
D)  acetone, bp = 56$\circ$C 
A)  ethanol, bp = 78$\circ$C 
B)  methanol, bp = 65$\circ$C 
C)  water, bp = 100$\circ$C 
D)  acetone, bp = 56$\circ$C

Question 15

W(s) is classified as a/an

Accepted Answer

A)  metallic crystal. 
B)  covalent solid. 
C)  molecular crystal. 
D)  amorphous solid. 
E)  ionic crystal. 
A)  metallic crystal. 
B)  covalent solid. 
C)  molecular crystal. 
D)  amorphous solid. 
E)  ionic crystal.

Question 16

Which one of the following substances is expected to have the highest boiling point

Accepted Answer

A)  Br2 
B)  Cl2 
C)  F2 
D)  I2 
A)  Br2 
B)  Cl2 
C)  F2 
D)  I2

Question 17

Iron crystallizes in a body-centered cubic unit. The edge of this cell is 287 pm. What is the density of iron

Accepted Answer

A)  7.86 g/cm3 
B)  7.66 g/cm3 
C)  7.46 g/cm3 
D)  7.26 g/cm3 
E)  None of the above 
A)  7.86 g/cm3 
B)  7.66 g/cm3 
C)  7.46 g/cm3 
D)  7.26 g/cm3 
E)  None of the above

Question 18

The liquid phase exists at the point labeled b.

Accepted Answer

A) True 
 B)False

Question 19

BaCl2 crystallizes such that the Ba2+ ions are in a face-centered cubic arrangement and the Cl- ions are in the holes of the lattice (fluorite structure). How many Cl- ions are present in one unit cell of this crystal

Accepted Answer

A)  1 
B)  2 
C)  4 
D)  6 
E)  8 
A)  1 
B)  2 
C)  4 
D)  6 
E)  8

Question 20

Suppose the atoms in a two-dimensional crystal have the following arrangement:   What is the coordination number of each atom in this crystal

Accepted Answer

A)  Two 
B)  Four 
C)  Six 
D)  Eight 
E)  None of the above 
A)  Two 
B)  Four 
C)  Six 
D)  Eight 
E)  None of the above

Exam 11: Intermolecular Forces and Liquids and Solids

Based on the phase diagram shown below, how will the melting point of the substance change if the pressure is increased above 1 atm

Suppose the atoms in a two-dimensional crystal have the following arrangement: How many atoms are in one unit cell A) One B) Two C) Three D) Four E) None of the above

Which of following can form hydrogen bonds with water molecules (1) Na+ (2) CH3COOH (3) C2H6 (4) CH3NH2

All intermolecular forces must be overcome in order for a substance to undergo a phase change from a solid to a liquid.

MgO has the same crystal structure as NaCl, face-centered cubic. How many oxide ions surround each Mg2+ ion as nearest neighbors

Which one of the following crystallizes in a metallic lattice

The molar enthalpy of vaporization of carbon disulfide is 26.74 kJ/mol, and its normal boiling point is 46 ∘\circ∘ C. What is the vapor pressure of CS2 at 0 ∘\circ∘ C

Indicate all the types of intermolecular forces of attraction in SO2(l).

The vapor pressure of a liquid in a closed container depends upon

Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20 ∘\circ∘ C to convert it to liquid water at 60.0 ∘\circ∘ C. Given: specific heat (ice) = 2.1 J/g· ∘\circ∘ C; specific heat (water) = 4.18 J/g· ∘\circ∘ C; Δ\DeltaΔ Hfus = 6.0 kJ/mol.

Which of the following is not true with regard to water

Indicate all the types of intermolecular forces of attraction in SF4(g).

Which of the following would be expected to have the highest vapor pressure at room temperature

W(s) is classified as a/an

Which one of the following substances is expected to have the highest boiling point

Iron crystallizes in a body-centered cubic unit. The edge of this cell is 287 pm. What is the density of iron

The liquid phase exists at the point labeled b.

BaCl2 crystallizes such that the Ba2+ ions are in a face-centered cubic arrangement and the Cl- ions are in the holes of the lattice (fluorite structure). How many Cl- ions are present in one unit cell of this crystal

Suppose the atoms in a two-dimensional crystal have the following arrangement: What is the coordination number of each atom in this crystal

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Mass Relationships in Chemical Reactions

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Physical Properties of Solutions

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Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

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Filters

Which of following can form hydrogen bonds with water molecules (1) Na⁺ (2) CH₃COOH (3) C₂H₆ (4) CH₃NH₂

MgO has the same crystal structure as NaCl, face-centered cubic. How many oxide ions surround each Mg²⁺ ion as nearest neighbors

The molar enthalpy of vaporization of carbon disulfide is 26.74 kJ/mol, and its normal boiling point is 46^$\circ$C. What is the vapor pressure of CS₂ at 0^$\circ$C

Indicate all the types of intermolecular forces of attraction in SO₂(l).

Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20^$\circ$C to convert it to liquid water at 60.0^$\circ$C. Given: specific heat (ice) = 2.1 J/g·^$\circ$C; specific heat (water) = 4.18 J/g·^$\circ$C; $\Delta$ H_fus = 6.0 kJ/mol.

Indicate all the types of intermolecular forces of attraction in SF₄(g).

BaCl₂ crystallizes such that the Ba²⁺ ions are in a face-centered cubic arrangement and the Cl^- ions are in the holes of the lattice (fluorite structure). How many Cl^- ions are present in one unit cell of this crystal