Question 1

Which of the following requires the smallest energy to separate the ions?

Accepted Answer

A)  CaF2 
B)  KF 
C)  NaF 
D)  MgF2 
E)  LiCl 
A)  CaF2 
B)  KF 
C)  NaF 
D)  MgF2 
E)  LiCl

Question 2

Identify the dominant intermolecular interaction(s) that must be overcome when solid CO2 sublimes and H2O melts.

Accepted Answer

Carbon dioxide is nonpolar, so

Question 3

Which liquid, water or ethanol, would you expect to have the higher surface tension and viscosity? Explain.

Accepted Answer

Water would have higher surface tension

Question 4

Molecular nitrogen (N2) interacts with water and is sparingly soluble in water due to ________

Accepted Answer

A)  dispersion forces. 
B)  dipole-induced dipole forces. 
C)  ion-dipole forces. 
D)  hydrogen bonding. 
E)  dipole-dipole forces. 
A)  dispersion forces. 
B)  dipole-induced dipole forces. 
C)  ion-dipole forces. 
D)  hydrogen bonding. 
E)  dipole-dipole forces.

Question 5

When two liquids mix completely in all proportions, they are ________

Accepted Answer

A)  soluble. 
B)  miscible. 
C)  insoluble. 
D)  solvated. 
E)  ubiquitous. 
A)  soluble. 
B)  miscible. 
C)  insoluble. 
D)  solvated. 
E)  ubiquitous.

Question 6

Sketch a phase diagram for water and correctly label all the parts (areas, lines, points, key temperatures).

Accepted Answer

Boiling points can also be cal

Question 7

Which statement about vapor pressure of a pure liquid is not correct?

Accepted Answer

A)  The vapor pressure is the pressure of the gas at a given temperature in equilibrium with its liquid phase. 
B)  The temperature at which the vapor pressure equals 760 torr is called the normal boiling point of the substance. 
C)  The vapor pressure increases with increasing temperature. 
D)  The vapor pressure increases with increasing surface area of the liquid. 
E)  Substances with weak intermolecular forces have high vapor pressures at a given temperature. 
A)  The vapor pressure is the pressure of the gas at a given temperature in equilibrium with its liquid phase. 
B)  The temperature at which the vapor pressure equals 760 torr is called the normal boiling point of the substance. 
C)  The vapor pressure increases with increasing temperature. 
D)  The vapor pressure increases with increasing surface area of the liquid. 
E)  Substances with weak intermolecular forces have high vapor pressures at a given temperature.

Question 8

Which is the dominant interaction between water molecules?

Accepted Answer

A)  ion-ion 
B)  ion-dipole 
C)  dipole-dipole 
D)  hydrogen bonding 
E)  dispersion or London forces 
A)  ion-ion 
B)  ion-dipole 
C)  dipole-dipole 
D)  hydrogen bonding 
E)  dispersion or London forces

Question 9

When sodium chloride dissolves in water, how do the water molecules orient around the ions?

Accepted Answer

A)  Water molecules are randomly oriented around the ions. 
B)  The hydrogen atoms point toward both the sodium and the chloride. 
C)  The oxygen atoms point toward both the sodium and the chloride. 
D)  Around sodium the hydrogen atoms point toward the sodium, and around chloride the oxygen atoms point toward the chloride. 
E)  Around sodium the oxygen atoms point toward the sodium, and around chloride the hydrogen atoms point toward the chloride. 
A)  Water molecules are randomly oriented around the ions. 
B)  The hydrogen atoms point toward both the sodium and the chloride. 
C)  The oxygen atoms point toward both the sodium and the chloride. 
D)  Around sodium the hydrogen atoms point toward the sodium, and around chloride the oxygen atoms point toward the chloride. 
E)  Around sodium the oxygen atoms point toward the sodium, and around chloride the hydrogen atoms point toward the chloride.

Question 10

Which of the following compounds would you most appropriately call hydrophobic?

Accepted Answer

A)  CH4 
B)  H2CO 
C)  CO 
D)  HCl 
E)  NaCl 
A)  CH4 
B)  H2CO 
C)  CO 
D)  HCl 
E)  NaCl

Question 11

Which statement about a hydrogen bond is not correct?

Accepted Answer

A)  Hydrogen bonds involve hydrogen bonded to carbon, nitrogen, oxygen, or fluorine. 
B)  In a hydrogen bond, the hydrogen atom on one molecule is attracted to unpaired electrons associated with nitrogen, oxygen, or fluorine on another molecule. 
C)  A hydrogen bond can be thought of as a very strong dipole-dipole interaction. 
D)  The presence of hydrogen bonds leads to anomalously high boiling points for liquids. 
E)  Hydrogen bonds stabilize the double helix structure of DNA. 
A)  Hydrogen bonds involve hydrogen bonded to carbon, nitrogen, oxygen, or fluorine. 
B)  In a hydrogen bond, the hydrogen atom on one molecule is attracted to unpaired electrons associated with nitrogen, oxygen, or fluorine on another molecule. 
C)  A hydrogen bond can be thought of as a very strong dipole-dipole interaction. 
D)  The presence of hydrogen bonds leads to anomalously high boiling points for liquids. 
E)  Hydrogen bonds stabilize the double helix structure of DNA.

Question 12

Which of the following statements correctly characterizes the rate of evaporation of a liquid?
I. Increases with increasing temperature because molecules have higher kinetic energies.
II. Increases with increasing surface area of the liquid because more molecules are located at the surface.
III. Decreases with stronger intermolecular forces because molecules are less able to escape from the surface of the liquid.

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I and II only 
E)  All three: I, II, and III 
A)  I only 
B)  II only 
C)  III only 
D)  I and II only 
E)  All three: I, II, and III

Question 13

Which alkane compound has the highest boiling point?

Accepted Answer

A)  C4H10 
B)  C5H12 
C)  C6H14 
D)  C7H16 
E)  C8H18 
A)  C4H10 
B)  C5H12 
C)  C6H14 
D)  C7H16 
E)  C8H18

Question 14

Which of the following compounds will have the strongest dipole-dipole interactions between its molecules?

Accepted Answer

A)  CF4 
B)  CH4 
C)  CH3F 
D)  CH2F2 
E)  CH3Cl 
A)  CF4 
B)  CH4 
C)  CH3F 
D)  CH2F2 
E)  CH3Cl

Question 15

Which of the following gases would you expect to have the largest van der Waals a constant value?

Accepted Answer

A)  Kr 
B)  N2 
C)  O2 
D)  H2 
E)  Ne 
A)  Kr 
B)  N2 
C)  O2 
D)  H2 
E)  Ne

Question 16

Define the term vapor pressure.

Accepted Answer

Vapor pressure is the pressure

Question 17

Which of the following statements does not correctly characterize the rate of evaporation of a liquid?
I. Increases with increasing temperature because molecules have higher kinetic energies.
II. Increases with increasing surface area of the liquid because more molecules are located at the surface.
III. Increases with stronger intermolecular forces because molecules in the liquid repel each other more.

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I and II only 
E)  II and III only 
A)  I only 
B)  II only 
C)  III only 
D)  I and II only 
E)  II and III only

Question 18

The phase diagram for carbon dioxide is shown below. What is the phase that exists at room temperature (22oC) and 100 atm pressure?

Accepted Answer

A)  gas 
B)  liquid 
C)  solid I 
D)  supercritical fluid 
E)  solid II 
A)  gas 
B)  liquid 
C)  solid I 
D)  supercritical fluid 
E)  solid II

Question 19

Of the two compounds shown below, one is slightly soluble in water and the other is insoluble in water. Identify the slightly soluble compound and explain why it is soluble in water.
I. ClCH2CH2Cl  
II. CHCl2CH3

Accepted Answer

A)  I because it can form hydrogen bonds with water at each end of the molecule. 
B)  I because it has stronger dispersion interactions with water. 
C)  II because it has stronger dipole-dipole interactions with water. 
D)  II because it has stronger dispersion interactions with water. 
E)  I because it is nonpolar. 
A)  I because it can form hydrogen bonds with water at each end of the molecule. 
B)  I because it has stronger dispersion interactions with water. 
C)  II because it has stronger dipole-dipole interactions with water. 
D)  II because it has stronger dispersion interactions with water. 
E)  I because it is nonpolar.

Question 20

Which is the dominant interaction between oxygen and nitrogen molecules in air?

Accepted Answer

A)  ion-ion 
B)  ion-dipole 
C)  dipole-dipole 
D)  hydrogen bonding 
E)  dispersion or London forces 
A)  ion-ion 
B)  ion-dipole 
C)  dipole-dipole 
D)  hydrogen bonding 
E)  dispersion or London forces

Which of the following requires the smallest energy to separate the ions?

Identify the dominant intermolecular interaction(s) that must be overcome when solid CO₂ sublimes and H₂O melts.

Which liquid, water or ethanol, would you expect to have the higher surface tension and viscosity? Explain.

Molecular nitrogen (N₂) interacts with water and is sparingly soluble in water due to ________

When two liquids mix completely in all proportions, they are ________

Sketch a phase diagram for water and correctly label all the parts (areas, lines, points, key temperatures).

Which statement about vapor pressure of a pure liquid is not correct?

Which is the dominant interaction between water molecules?

When sodium chloride dissolves in water, how do the water molecules orient around the ions?

Which of the following compounds would you most appropriately call hydrophobic?

Which statement about a hydrogen bond is not correct?

Which alkane compound has the highest boiling point?

Which of the following compounds will have the strongest dipole-dipole interactions between its molecules?

Which of the following gases would you expect to have the largest van der Waals a constant value?

Define the term vapor pressure.

The phase diagram for carbon dioxide is shown below. What is the phase that exists at room temperature (22^oC) and 100 atm pressure?

Of the two compounds shown below, one is slightly soluble in water and the other is insoluble in water. Identify the slightly soluble compound and explain why it is soluble in water. I. ClCH₂CH₂Cl II. CHCl₂CH₃

Which is the dominant interaction between oxygen and nitrogen molecules in air?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: the Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Solutions: Properties and Behavior

Solids: Structures and Applications

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

Filters

Exam 10: Intermolecular Forces: The Uniqueness of Water

Which of the following requires the smallest energy to separate the ions?

Identify the dominant intermolecular interaction(s) that must be overcome when solid CO2 sublimes and H2O melts.

Which liquid, water or ethanol, would you expect to have the higher surface tension and viscosity? Explain.

Molecular nitrogen (N2) interacts with water and is sparingly soluble in water due to ________

When two liquids mix completely in all proportions, they are ________

Sketch a phase diagram for water and correctly label all the parts (areas, lines, points, key temperatures).

Which statement about vapor pressure of a pure liquid is not correct?

Which is the dominant interaction between water molecules?

When sodium chloride dissolves in water, how do the water molecules orient around the ions?

Which of the following compounds would you most appropriately call hydrophobic?

Which statement about a hydrogen bond is not correct?

Which alkane compound has the highest boiling point?

Which of the following compounds will have the strongest dipole-dipole interactions between its molecules?

Which of the following gases would you expect to have the largest van der Waals a constant value?

Define the term vapor pressure.

The phase diagram for carbon dioxide is shown below. What is the phase that exists at room temperature (22oC) and 100 atm pressure?

Of the two compounds shown below, one is slightly soluble in water and the other is insoluble in water. Identify the slightly soluble compound and explain why it is soluble in water. I. ClCH2CH2Cl II. CHCl2CH3

Which is the dominant interaction between oxygen and nitrogen molecules in air?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: the Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Solutions: Properties and Behavior

Solids: Structures and Applications

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

Filters

Identify the dominant intermolecular interaction(s) that must be overcome when solid CO₂ sublimes and H₂O melts.

Molecular nitrogen (N₂) interacts with water and is sparingly soluble in water due to ________

The phase diagram for carbon dioxide is shown below. What is the phase that exists at room temperature (22^oC) and 100 atm pressure?

Of the two compounds shown below, one is slightly soluble in water and the other is insoluble in water. Identify the slightly soluble compound and explain why it is soluble in water. I. ClCH₂CH₂Cl II. CHCl₂CH₃