Question 1

A substance that is ________ will be insoluble in water, but a substance that is ________ will be soluble in water.

Accepted Answer

A) hydrophobic; immiscible 
B) immiscible; hydrophobic 
C) hydrophilic; miscible 
D) hydrophobic; hydrophilic 
E) miscible; immiscible 
A) hydrophobic; immiscible 
B) immiscible; hydrophobic 
C) hydrophilic; miscible 
D) hydrophobic; hydrophilic 
E) miscible; immiscible

Question 2

A phase diagram shows the states of a substance as a function of ________ and ________.

Accepted Answer

A) pressure; volume 
B) volume; temperature 
C) pressure; temperature 
D) concentration; temperature 
E) density; pressure 
A) pressure; volume 
B) volume; temperature 
C) pressure; temperature 
D) concentration; temperature 
E) density; pressure

Question 3

Indicate which of the following molecules exhibits the greatest dispersion forces.

Accepted Answer

A) CH3CH3 
B) CH3CH2CH3 
C) C2H2 
D) CH4 
E) CH3CH2CH2CH3 
A) CH3CH3 
B) CH3CH2CH3 
C) C2H2 
D) CH4 
E) CH3CH2CH2CH3

Question 4

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice.
(A) CCl4 or CHCl3
(B) CH3OH or C5H11OH
(C) NaF or MgO

Accepted Answer

(A) CHCl₃, because it has a dipole moment

Question 5

Given the van der Waals a constant values for the following gases, which gas has the greatest intermolecular forces?

Accepted Answer

A) N2 a   F1F1F1S1F1F1F101.35 L2 · atm/mol   
B) O2 a   F1F1F1S1F1F1F101.36 L2 · atm/mol   
C) NH3 a   F1F1F1S1F1F1F104.25 L2 · atm/mol   
D) CH4 a   F1F1F1S1F1F1F102.27 L2 · atm/mol   
E) SO2 a   F1F1F1S1F1F1F106.71 L2 · atm/mol   
A) N2 a   F1F1F1S1F1F1F101.35 L2 · atm/mol   
B) O2 a   F1F1F1S1F1F1F101.36 L2 · atm/mol   
C) NH3 a   F1F1F1S1F1F1F104.25 L2 · atm/mol   
D) CH4 a   F1F1F1S1F1F1F102.27 L2 · atm/mol   
E) SO2 a   F1F1F1S1F1F1F106.71 L2 · atm/mol

Question 6

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 7

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.

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 8

Hydrophilic substances ________

Accepted Answer

A) are immiscible in water. 
B) are insoluble in water. 
C) are soluble in water. 
D) are hydrated. 
E) generally do not hydrogen bond. 
A) are immiscible in water. 
B) are insoluble in water. 
C) are soluble in water. 
D) are hydrated. 
E) generally do not hydrogen bond.

Question 9

Which is the dominant interaction between chloroform (CHCl3) 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 10

Boiling points increase in the order HCl F1F1F1S1F1F1F10 HBr F1F1F1S1F1F1F10 HI because ________ contribute to the intermolecular interactions.

Accepted Answer

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

Question 11

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 12

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 13

Which is the dominant interaction that explains the high melting point of table salt, NaCl?

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 14

The vapor pressure of a liquid increases with increasing temperature because ________

Accepted Answer

A) more molecules can escape from the liquid because their average kinetic energy is greater. 
B) the number of gas molecules above the liquid does not change but their average kinetic energy increases. 
C) the molecules in the liquid move faster and exert a greater pressure. 
D) the ideal gas law states that the pressure is proportional to the temperature. 
E) molecules interact less strongly at higher temperatures. 
A) more molecules can escape from the liquid because their average kinetic energy is greater. 
B) the number of gas molecules above the liquid does not change but their average kinetic energy increases. 
C) the molecules in the liquid move faster and exert a greater pressure. 
D) the ideal gas law states that the pressure is proportional to the temperature. 
E) molecules interact less strongly at higher temperatures.

Question 15

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 16

Sublimation occurs in going from region ________

Accepted Answer

A) I to II. 
B) I to III. 
C) II to III. 
D) III to II. 
E) III to I. 
A) I to II. 
B) I to III. 
C) II to III. 
D) III to II. 
E) III to I.

Question 17

Which molecule has the largest dipole?

Accepted Answer

A) fluorine gas (F2) 
B) dihydrogen gas (H2) 
C) dinitrogen gas (N2) 
D) chlorine monofluoride gas (ClF) 
E) carbon dioxide gas (CO2) 
A) fluorine gas (F2) 
B) dihydrogen gas (H2) 
C) dinitrogen gas (N2) 
D) chlorine monofluoride gas (ClF) 
E) carbon dioxide gas (CO2)

Question 18

CH2F2 has a dipole moment of 1.93 D and a boiling point of F1F1F1S1F1F1F1052F1F1F1S1F1F1F10C. CH2Cl2 has a dipole moment of 1.60 D and a boiling point of 40F1F1F1S1F1F1F10C. Why is the boiling point of dichloromethane so much higher than that of difluoromethane?

Accepted Answer

Both molecules have dipole-dipole and di

Question 19

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 20

Which alkane compound has the lowest boiling point?

Accepted Answer

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

Exam 10: Intermolecular Forces: The Uniqueness of Water

A substance that is ________ will be insoluble in water, but a substance that is ________ will be soluble in water.

A phase diagram shows the states of a substance as a function of ________ and ________.

Indicate which of the following molecules exhibits the greatest dispersion forces.

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. (A) CCl4 or CHCl3 (B) CH3OH or C5H11OH (C) NaF or MgO

Given the van der Waals a constant values for the following gases, which gas has the greatest intermolecular forces?

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

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.

Hydrophilic substances ________

Which is the dominant interaction between chloroform (CHCl3) molecules?

Boiling points increase in the order HCl  HBr  HI because ________ contribute to the intermolecular interactions.

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

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

Which is the dominant interaction that explains the high melting point of table salt, NaCl?

The vapor pressure of a liquid increases with increasing temperature because ________

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

Sublimation occurs in going from region ________

Which molecule has the largest dipole?

CH2F2 has a dipole moment of 1.93 D and a boiling point of 52C. CH2Cl2 has a dipole moment of 1.60 D and a boiling point of 40C. Why is the boiling point of dichloromethane so much higher than that of difluoromethane?

Which is the dominant interaction between water molecules?

Which alkane compound has the lowest boiling point?

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

A substance that is will be insoluble in water, but a substance that is will be soluble in water.

A phase diagram shows the states of a substance as a function of and .

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. (A) CCl₄ or CHCl₃ (B) CH₃OH or C₅H₁₁OH (C) NaF or MgO

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

Which is the dominant interaction between chloroform (CHCl₃) molecules?

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

CH₂F₂ has a dipole moment of 1.93 D and a boiling point of 52C. CH₂Cl₂ has a dipole moment of 1.60 D and a boiling point of 40C. Why is the boiling point of dichloromethane so much higher than that of difluoromethane?