Question 1

Define the terms hydrophobic and hydrophilic.

Accepted Answer

Hydrophobic describes a substa

Question 2

Which best describes the intermolecular forces present in NH3?

Accepted Answer

A) dispersion forces only 
B) hydrogen bonding and dispersion forces 
C) dipole-dipole, hydrogen bonding, and dispersion forces 
D) dipole-dipole forces only 
E) ion-dipole and dispersion forces 
A) dispersion forces only 
B) hydrogen bonding and dispersion forces 
C) dipole-dipole, hydrogen bonding, and dispersion forces 
D) dipole-dipole forces only 
E) ion-dipole and dispersion forces

Question 3

The pressure inside a bottle of carbonated beverage decreases when it is cooled in a refrigerator. What is the main reason for this change?

Accepted Answer

A) The solubility of carbon dioxide is higher at the lower temperature. 
B) Some carbon dioxide condenses to form a liquid phase. 
C) The volume of the vapor contracts. 
D) The volume of the liquid contracts. 
E) The volume of the bottle contracts. 
A) The solubility of carbon dioxide is higher at the lower temperature. 
B) Some carbon dioxide condenses to form a liquid phase. 
C) The volume of the vapor contracts. 
D) The volume of the liquid contracts. 
E) The volume of the bottle contracts.

Question 4

Which of the following compounds will not possess dipole-dipole interactions between its molecules?

Accepted Answer

A) HBr 
B) CO2 
C) PH3 
D) NO 
E) SCl2 
A) HBr 
B) CO2 
C) PH3 
D) NO 
E) SCl2

Question 5

The relative energies (strengths) of the intermolecular forces present in each of four different pure gases are shown in the figure below. Which gas will show the smallest deviation from ideal gas behavior?

Accepted Answer

A) a 
B) b 
C) c 
D) d 
A) a 
B) b 
C) c 
D) d

Question 6

Which of the following gases would be expected to most likely deviate from ideal gas behavior? Briefly explain your reasoning.
CH4, N2, and NH3

Accepted Answer

NH₃ The gas most likely to deviate from i

Question 7

The Henry's law constant (mol/L · atm) for carbon dioxide dissolving in water is 3.50 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 mol/(L atm) at 20F1F1F1S1F1F1F10C. Calculate the molar concentration of carbon dioxide in a soda can where the air pressure is 2.45 atm. The mole fraction of carbon dioxide in air is 0.0397.

Accepted Answer

A) 1.4   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
B) 3.4   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
C) 2.7   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
D) 8.2   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
E) 8.6   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
A) 1.4   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
B) 3.4   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
C) 2.7   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
D) 8.2   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
E) 8.6   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M

Question 8

Point d in the phase diagram below is the ________

Accepted Answer

A) critical point. 
B) triple point. 
C) transition point. 
D) normal freezing point. 
E) normal boiling point. 
A) critical point. 
B) triple point. 
C) transition point. 
D) normal freezing point. 
E) normal boiling point.

Question 9

A solute is most likely to be highly soluble in a solvent if the solute is ________ and the solvent is ________.

Accepted Answer

A) nonpolar; ionic 
B) polar; nonpolar 
C) polar; polar 
D) nonpolar; polar 
E) ionic; nonpolar 
A) nonpolar; ionic 
B) polar; nonpolar 
C) polar; polar 
D) nonpolar; polar 
E) ionic; nonpolar

Question 10

Given the van der Waals a constant values for the following gases, which gas has the lowest boiling point?

Accepted Answer

A) CO2 a   F1F1F1S1F1F1F103.64 L2 · atm/mol   
B) Ar a   F1F1F1S1F1F1F101.36 L2 · atm/mol   
C) CCl4 a   F1F1F1S1F1F1F1019.75 L2 · atm/mol   
D) HBr a   F1F1F1S1F1F1F104.51 L2 · atm/mol   
E) CO a   F1F1F1S1F1F1F101.51 L2 · atm/mol   
A) CO2 a   F1F1F1S1F1F1F103.64 L2 · atm/mol   
B) Ar a   F1F1F1S1F1F1F101.36 L2 · atm/mol   
C) CCl4 a   F1F1F1S1F1F1F1019.75 L2 · atm/mol   
D) HBr a   F1F1F1S1F1F1F104.51 L2 · atm/mol   
E) CO a   F1F1F1S1F1F1F101.51 L2 · atm/mol

Question 11

Of all the noble gases, ________ has the strongest intermolecular force and hence the highest boiling point.

Accepted Answer

A) He 
B) Ne 
C) Ar 
D) Kr 
E) Xe 
A) He 
B) Ne 
C) Ar 
D) Kr 
E) Xe

Question 12

Which of the substances a-d in the following figure has the weakest intermolecular forces?

Accepted Answer

A) a 
B) b 
C) c 
D) d 
A) a 
B) b 
C) c 
D) d

Question 13

The density of water decreases as it is cooled from 4.0F1F1F1S1F1F1F10C to freezing because ________

Accepted Answer

A) water molecules decrease in size as they cool because energy is released. 
B) a network of hydrogen bonds between water molecules is formed. 
C) water molecules become more rigid as they cool. 
D) hydrogen bonds in liquid water are longer than they are in ice. 
E) all substances contract just before freezing. 
A) water molecules decrease in size as they cool because energy is released. 
B) a network of hydrogen bonds between water molecules is formed. 
C) water molecules become more rigid as they cool. 
D) hydrogen bonds in liquid water are longer than they are in ice. 
E) all substances contract just before freezing.

Question 14

Henry's law constant (mol/L · atm) for oxygen dissolving in blood is 3.74 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 mol/L · atm at body temperature, 37F1F1F1S1F1F1F10C. Calculate the molar concentration of oxygen in blood for an alpine climber where the atmospheric pressure is 0.45 atm. The mole fraction of oxygen in air is 0.209.

Accepted Answer

A) 7.8   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
B) 3.5   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
C) 2.3   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
D) 1.3   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
E) 0.11 M 
A) 7.8   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
B) 3.5   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 M 
C) 2.3   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
D) 1.3   F1F1F1S1F1F1F1010F1F1F1S1F1F1F102 M 
E) 0.11 M

Question 15

Of all the noble gases, ________ has the weakest intermolecular force and hence the lowest boiling point.

Accepted Answer

A) He 
B) Ne 
C) Ar 
D) Kr 
E) Xe 
A) He 
B) Ne 
C) Ar 
D) Kr 
E) Xe

Question 16

At the triple point of a substance, ________

Accepted Answer

A) three phases are present in equilibrium. 
B) the solid sublimes. 
C) the gas condenses to a liquid. 
D) solid and liquid are in equilibrium. 
E) only one phase appears to be present. 
A) three phases are present in equilibrium. 
B) the solid sublimes. 
C) the gas condenses to a liquid. 
D) solid and liquid are in equilibrium. 
E) only one phase appears to be present.

Question 17

Which of the following diagrams best shows a set of polar molecules interacting through dipole-dipole interactions?

Accepted Answer

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

Question 18

Which of the following representations best shows the formation of an instantaneous dipole moment between two nonpolar molecules?

Accepted Answer

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

Question 19

A hydration sphere forms around an ion in aqueous solution due to ________

Accepted Answer

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

Question 20

The solubility of any gas in a liquid can always be increased by ________

Accepted Answer

A) increasing the temperature. 
B) using a solvent that can form hydrogen bonds. 
C) using a solvent that is nonpolar. 
D) decreasing the pressure of the gas above the solvent. 
E) increasing the pressure of the gas above the solvent. 
A) increasing the temperature. 
B) using a solvent that can form hydrogen bonds. 
C) using a solvent that is nonpolar. 
D) decreasing the pressure of the gas above the solvent. 
E) increasing the pressure of the gas above the solvent.

Exam 10: Intermolecular Forces: The Uniqueness of Water

Define the terms hydrophobic and hydrophilic.

Which best describes the intermolecular forces present in NH3?

The pressure inside a bottle of carbonated beverage decreases when it is cooled in a refrigerator. What is the main reason for this change?

Which of the following compounds will not possess dipole-dipole interactions between its molecules?

The relative energies (strengths) of the intermolecular forces present in each of four different pure gases are shown in the figure below. Which gas will show the smallest deviation from ideal gas behavior?

Which of the following gases would be expected to most likely deviate from ideal gas behavior? Briefly explain your reasoning. CH4, N2, and NH3

The Henry's law constant (mol/L · atm) for carbon dioxide dissolving in water is 3.50  102 mol/(L atm) at 20C. Calculate the molar concentration of carbon dioxide in a soda can where the air pressure is 2.45 atm. The mole fraction of carbon dioxide in air is 0.0397.

Point d in the phase diagram below is the ________

A solute is most likely to be highly soluble in a solvent if the solute is ________ and the solvent is ________.

Given the van der Waals a constant values for the following gases, which gas has the lowest boiling point?

Of all the noble gases, ________ has the strongest intermolecular force and hence the highest boiling point.

Which of the substances a-d in the following figure has the weakest intermolecular forces?

The density of water decreases as it is cooled from 4.0C to freezing because ________

Henry's law constant (mol/L · atm) for oxygen dissolving in blood is 3.74  102 mol/L · atm at body temperature, 37C. Calculate the molar concentration of oxygen in blood for an alpine climber where the atmospheric pressure is 0.45 atm. The mole fraction of oxygen in air is 0.209.

Of all the noble gases, ________ has the weakest intermolecular force and hence the lowest boiling point.

At the triple point of a substance, ________

Which of the following diagrams best shows a set of polar molecules interacting through dipole-dipole interactions?

Which of the following representations best shows the formation of an instantaneous dipole moment between two nonpolar molecules?

A hydration sphere forms around an ion in aqueous solution due to ________

The solubility of any gas in a liquid can always be increased by ________

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: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Which best describes the intermolecular forces present in NH₃?

Which of the following gases would be expected to most likely deviate from ideal gas behavior? Briefly explain your reasoning. CH₄, N₂, and NH₃

The Henry's law constant (mol/L · atm) for carbon dioxide dissolving in water is 3.50  10^² mol/(L atm) at 20C. Calculate the molar concentration of carbon dioxide in a soda can where the air pressure is 2.45 atm. The mole fraction of carbon dioxide in air is 0.0397.

A solute is most likely to be highly soluble in a solvent if the solute is and the solvent is .

Henry's law constant (mol/L · atm) for oxygen dissolving in blood is 3.74  10^² mol/L · atm at body temperature, 37C. Calculate the molar concentration of oxygen in blood for an alpine climber where the atmospheric pressure is 0.45 atm. The mole fraction of oxygen in air is 0.209.