Question 1

Which compound should have the highest boiling point?

Accepted Answer

A) CH3-Br 
B) CH3-Cl 
C) CH3-F 
D) CH3-H 
E) CH3-I 
A) CH3-Br 
B) CH3-Cl 
C) CH3-F 
D) CH3-H 
E) CH3-I

Question 2

Silicon carbide, which has the empirical formula SiC, melts at 2830°C and is nearly as hard as diamond. Which category of substance does silicon carbide most likely fit into?

Accepted Answer

A) ionic 
B) molecular 
C) metallic 
D) covalent 
E) amorphous 
A) ionic 
B) molecular 
C) metallic 
D) covalent 
E) amorphous

Question 3

Which type of unit cell has lattice points at each corner, and one in the center of the cell?

Accepted Answer

A) face-centered cubic 
B) simple cubic 
C) body-centered cubic 
D) edge-centered cubic 
E) hexagonal-centered cubic 
A) face-centered cubic 
B) simple cubic 
C) body-centered cubic 
D) edge-centered cubic 
E) hexagonal-centered cubic

Question 4

Osmium tetroxide, OsO4, forms a crystal that melts at 40°C. The liquid formed from this melting does not conduct electricity. What would be the best classification of this type of crystal?

Accepted Answer

Question 5

Based on the phase diagram of water, why can someone on ice skates can glide along the ice much more easily than someone in normal shoes?

Accepted Answer

According to the phase diagram for water

Question 6

Determine the shift in equilibrium that would result if 100 kJ of energy were added to water freezing at 0°C to form ice (H2O(s)⇆ H2O(l)).

Accepted Answer

Shift to t

Question 7

Which molecule is most polarizable and subject to the greatest instantaneous dipole-induced dipole forces?

Accepted Answer

A) CH4 
B) C2H6 
C) C3H8 
D) C4H10 
E) C5H12  
A) CH4 
B) C2H6 
C) C3H8 
D) C4H10 
E) C5H12

Question 8

Which of the following liquids, at the same temperature, has the highest vapor pressure?

Accepted Answer

A) CH3-Br 
B) CH3-Cl 
C) CH3-F 
D) CH3-H 
E) CH3-I 
A) CH3-Br 
B) CH3-Cl 
C) CH3-F 
D) CH3-H 
E) CH3-I

Question 9

X-ray diffraction measurements revealed that Ag crystallizes in a face-centered cubic lattice in which the unit cell edge length is 408.6 picometers. Calculate the atomic radius of the Ag atoms in this crystal, based on the usual assumption that the atoms are tightly packed in the unit cell.

Accepted Answer

A) 102.2 pm 
B) 144.5 pm 
C) 192.6 pm 
D) 204.3 pm 
E) 288.9 pm 
A) 102.2 pm 
B) 144.5 pm 
C) 192.6 pm 
D) 204.3 pm 
E) 288.9 pm

Question 10

A high vapor pressure indicates that the substance has ________ intermolecular forces in the liquid form.

Accepted Answer

The answer of A high vapor pressure indicates that the...

Question 11

The vapor pressure of a liquid increases with increasing temperature. The temperature at which the vapor pressure is equal to the prevailing outside atmospheric pressure is

Accepted Answer

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

Question 12

Draw the unit cell for the following two-dimensional lattice.   Hint: Think about the repeating unit.

Accepted Answer

The answer of Draw the unit cell for the following...

Question 13

The pressure below which the liquid state of matter does not exist regardless of the temperature is called ________.

Accepted Answer

the critic

Question 14

Which factor affects the normal boiling point of a liquid?

Accepted Answer

A) atmospheric pressure 
B) rate of condensation 
C) rate of evaporation 
D) strength of the intermolecular forces 
E) rate of temperature increase 
A) atmospheric pressure 
B) rate of condensation 
C) rate of evaporation 
D) strength of the intermolecular forces 
E) rate of temperature increase

Question 15

Determine the shift in equilibrium that would result if 100 kJ of energy were removed from a system in which dry ice and CO2 gas were in equilibrium at the freezing point.

Accepted Answer

More solid

Question 16

Which type of lattice structures have lattice points on all of the faces?

Accepted Answer

A) simple cubic structures 
B) base-centered structures 
C) face-centered structures 
D) body-centered structures 
E) both body-centered and base-centered structures 
A) simple cubic structures 
B) base-centered structures 
C) face-centered structures 
D) body-centered structures 
E) both body-centered and base-centered structures

Question 17

An unknown solid is hard, but brittle and melts at 3500°C. The liquid form of the unknown conducts electricity, but the solid form does not. What kind of crystal is the unknown?

Accepted Answer

The answer of An unknown solid is hard, but brittle...

Question 18

Substance A has a normal melting point of -25.0°C, a heat of fusion of 1200 J g-1; specific heats for the solid and the liquid are 3.00 and 6.20 J g-1 °C -1, respectively. How much heat will be required to change 150 grams of substance A from a solid at -40.0°C to a liquid at +70.0°C?

Accepted Answer

A) 1.52 × 105 J 
B) 1.81 × 105 J 
C) 2.21 × 103 J 
D) 2.29 × 105 J 
E) 2.75 × 105 J 
A) 1.52 × 105 J 
B) 1.81 × 105 J 
C) 2.21 × 103 J 
D) 2.29 × 105 J 
E) 2.75 × 105 J

Question 19

An unknown solid is hard, but malleable and melts at 1700°C. The liquid form conducts electricity. The solid form also conducts electricity. What kind of crystal is this?

Accepted Answer

The answer of An unknown solid is hard, but malleable...

Question 20

The unit cell below is best described as what type of crystal structure?

Accepted Answer

A) Body-centered cubic 
B) Simple cubic 
C) Trigonal 
D) Face-centered cubic 
E) Octahedral 
A) Body-centered cubic 
B) Simple cubic 
C) Trigonal 
D) Face-centered cubic 
E) Octahedral

Exam 12: Intermolecular Attractions and the Properties of Liquids and Solids

Which compound should have the highest boiling point?

Silicon carbide, which has the empirical formula SiC, melts at 2830°C and is nearly as hard as diamond. Which category of substance does silicon carbide most likely fit into?

Which type of unit cell has lattice points at each corner, and one in the center of the cell?

Osmium tetroxide, OsO4, forms a crystal that melts at 40°C. The liquid formed from this melting does not conduct electricity. What would be the best classification of this type of crystal?

Based on the phase diagram of water, why can someone on ice skates can glide along the ice much more easily than someone in normal shoes?

Determine the shift in equilibrium that would result if 100 kJ of energy were added to water freezing at 0°C to form ice (H2O(s)⇆ H2O(l)).

Which molecule is most polarizable and subject to the greatest instantaneous dipole-induced dipole forces?

Which of the following liquids, at the same temperature, has the highest vapor pressure?

X-ray diffraction measurements revealed that Ag crystallizes in a face-centered cubic lattice in which the unit cell edge length is 408.6 picometers. Calculate the atomic radius of the Ag atoms in this crystal, based on the usual assumption that the atoms are tightly packed in the unit cell.

A high vapor pressure indicates that the substance has ________ intermolecular forces in the liquid form.

The vapor pressure of a liquid increases with increasing temperature. The temperature at which the vapor pressure is equal to the prevailing outside atmospheric pressure is

Draw the unit cell for the following two-dimensional lattice. Hint: Think about the repeating unit.

The pressure below which the liquid state of matter does not exist regardless of the temperature is called ________.

Which factor affects the normal boiling point of a liquid?

Determine the shift in equilibrium that would result if 100 kJ of energy were removed from a system in which dry ice and CO2 gas were in equilibrium at the freezing point.

Which type of lattice structures have lattice points on all of the faces?

An unknown solid is hard, but brittle and melts at 3500°C. The liquid form of the unknown conducts electricity, but the solid form does not. What kind of crystal is the unknown?

Substance A has a normal melting point of -25.0°C, a heat of fusion of 1200 J g-1; specific heats for the solid and the liquid are 3.00 and 6.20 J g-1 °C -1, respectively. How much heat will be required to change 150 grams of substance A from a solid at -40.0°C to a liquid at +70.0°C?

An unknown solid is hard, but malleable and melts at 1700°C. The liquid form conducts electricity. The solid form also conducts electricity. What kind of crystal is this?

The unit cell below is best described as what type of crystal structure?

A Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Mixtures at the Molecular Level: Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Solubility and Simultaneous Equilibria

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

Osmium tetroxide, OsO₄, forms a crystal that melts at 40°C. The liquid formed from this melting does not conduct electricity. What would be the best classification of this type of crystal?

Determine the shift in equilibrium that would result if 100 kJ of energy were added to water freezing at 0°C to form ice (H₂O(s)⇆ H₂O(l)).

Determine the shift in equilibrium that would result if 100 kJ of energy were removed from a system in which dry ice and CO₂ gas were in equilibrium at the freezing point.

Substance A has a normal melting point of -25.0°C, a heat of fusion of 1200 J g^-1; specific heats for the solid and the liquid are 3.00 and 6.20 J g^-1 °C^-1, respectively. How much heat will be required to change 150 grams of substance A from a solid at -40.0°C to a liquid at +70.0°C?