Question 1

For a molecule to exhibit dipole-dipole interactions, it must ________

Accepted Answer

A) have a temporary dipole moment. 
B) have a hydrogen bound to an oxygen, nitrogen, or fluorine. 
C) have a permanent dipole moment. 
D) be an ion. 
E) have 3 or more atoms. 
A) have a temporary dipole moment. 
B) have a hydrogen bound to an oxygen, nitrogen, or fluorine. 
C) have a permanent dipole moment. 
D) be an ion. 
E) have 3 or more atoms.

Question 2

On the phase diagram below, identify the normal melting point.

Accepted Answer

A) VI 
B) V 
C) VII 
D) IV 
E) III 
A) VI 
B) V 
C) VII 
D) IV 
E) III

Question 3

What structural characteristics must a molecule have in order to hydrogen bond?

Accepted Answer

A hydrogen atom bond

Question 4

Which of the following solvents will involve ion-dipole interactions with NaF1F1F1S1F1F1F10?

Accepted Answer

A) benzene (C6H6) 
B) carbon tetrachloride (CCl4) 
C) chloroform (CHCl3) 
D) cyclohexane (C6H12) 
E) pentane (C5H12) 
A) benzene (C6H6) 
B) carbon tetrachloride (CCl4) 
C) chloroform (CHCl3) 
D) cyclohexane (C6H12) 
E) pentane (C5H12)

Question 5

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 6

What does the line indicated by the arrow in the following phase diagram represent?

Accepted Answer

A) solid-liquid boundary 
B) solid-gas boundary 
C) liquid-gas boundary 
D) triple point 
E) solid-solid boundary 
A) solid-liquid boundary 
B) solid-gas boundary 
C) liquid-gas boundary 
D) triple point 
E) solid-solid boundary

Question 7

The aroma from almonds and cherries is due in part to a compound called benzaldehyde. A graph of the natural logarithm of the vapor pressure of benzaldehyde vs. 1/temperature produces a straight line with a slope of   F1F1F1S1F1F1F105,870.99 K. What is the enthalpy of vaporization of benzaldehyde?

Accepted Answer

A) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10473 kJ/mol) 
B) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1047.3 kJ/mol) 
C) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1047.3 kJ/mol) 
D) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1048.8 kJ/mol) 
E) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1048.8 kJ/mol) 
A) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10473 kJ/mol) 
B) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1047.3 kJ/mol) 
C) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1047.3 kJ/mol) 
D) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1048.8 kJ/mol) 
E) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F1048.8 kJ/mol)

Question 8

Viscosity is a measure of a substance's ________

Accepted Answer

A) ability to resist changes in its surface area. 
B) surface tension. 
C) resistance to flow. 
D) compressibility. 
E) color. 
A) ability to resist changes in its surface area. 
B) surface tension. 
C) resistance to flow. 
D) compressibility. 
E) color.

Question 9

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) Br2 or NaBr
(B) CH3CH2OH or CH3OCH3
(C) CO2 or KOH

Accepted Answer

(A) NaBr, because it is an ionic compoun

Question 10

Which of the following molecules will have the least interaction with a LiF1F1F1S1F1F1F10 ion?

Accepted Answer

A) water (H2O) 
B) ethanol (CH3CH2OH) 
C) chloroform (CHCl3) 
D) ammonia (NH3) 
E) pentane (C5H12) 
A) water (H2O) 
B) ethanol (CH3CH2OH) 
C) chloroform (CHCl3) 
D) ammonia (NH3) 
E) pentane (C5H12)

Question 11

At ambient temperature, F2 and Cl2 are both gases while Br2 is a liquid and I2 is a solid. This is due to ________

Accepted Answer

A) dipole-dipole forces increasing with increasing molecular weight. 
B) dispersion forces increasing with increasing molecular weight. 
C) molecule polarity increasing with increasing molecular weight. 
D) both dispersion and polarity increasing with increasing molecular weight. 
E) ion-dipole forces increasing with increasing molecular weight. 
A) dipole-dipole forces increasing with increasing molecular weight. 
B) dispersion forces increasing with increasing molecular weight. 
C) molecule polarity increasing with increasing molecular weight. 
D) both dispersion and polarity increasing with increasing molecular weight. 
E) ion-dipole forces increasing with increasing molecular weight.

Question 12

Indicate which of the following nonpolar compounds will have the lowest boiling point.

Accepted Answer

A) CCl4 
B) CI4 
C) CF4 
D) CH4 
E) CBr4 
A) CCl4 
B) CI4 
C) CF4 
D) CH4 
E) CBr4

Question 13

Write definitions for the terms miscible and soluble.

Accepted Answer

Miscible is the property of substances t

Question 14

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 15

The resistance of a liquid to an increase in its surface area is ________

Accepted Answer

A) surface tension. 
B) viscosity. 
C) capillary action. 
D) a meniscus. 
E) impossible. 
A) surface tension. 
B) viscosity. 
C) capillary action. 
D) a meniscus. 
E) impossible.

Question 16

The carbon dioxide pressure in a bottle of champagne is about 6 atm. At this pressure about 0.45 g of carbon dioxide dissolves in 100 mL of champagne. How much carbon dioxide remains dissolved in 100 mL after the bottle is opened? The partial pressure of carbon dioxide then is 6.0   F1F1F1S1F1F1F1010F1F1F1S1F1F1F104 atm.

Accepted Answer

A) 0.45 g 
B) 3.8   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 g 
C) 1.7   F1F1F1S1F1F1F1010F1F1F1S1F1F1F106 g 
D) 9.0   F1F1F1S1F1F1F1010F1F1F1S1F1F1F104 g 
E) 4.5   F1F1F1S1F1F1F1010F1F1F1S1F1F1F105 g 
A) 0.45 g 
B) 3.8   F1F1F1S1F1F1F1010F1F1F1S1F1F1F103 g 
C) 1.7   F1F1F1S1F1F1F1010F1F1F1S1F1F1F106 g 
D) 9.0   F1F1F1S1F1F1F1010F1F1F1S1F1F1F104 g 
E) 4.5   F1F1F1S1F1F1F1010F1F1F1S1F1F1F105 g

Question 17

What does the line indicated by the arrow in the following phase diagram represent?

Accepted Answer

A) solid-liquid boundary 
B) solid-gas boundary 
C) liquid-gas boundary 
D) triple point 
E) solid-solid boundary 
A) solid-liquid boundary 
B) solid-gas boundary 
C) liquid-gas boundary 
D) triple point 
E) solid-solid boundary

Question 18

Why do the strengths of dispersion interactions generally increase with the molar mass of the compound?

Accepted Answer

A molecule with the larger molar mass ha

Question 19

In understanding why group 16 hydrides, other than those in period 2, have a higher boiling point than the hydrides of groups 14, 15, and 17, which of the following are most important to consider?
I.dispersion forces
II.dipole-dipole forces
III. hydrogen bonding

Accepted Answer

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

Question 20

The phase diagram for carbon dioxide is shown below. What are the phase changes in order as carbon dioxide is heated from F1F1F1S1F1F1F1090oC to 50oC, at 500 atm pressure?

Accepted Answer

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

Exam 10: Intermolecular Forces: The Uniqueness of Water

For a molecule to exhibit dipole-dipole interactions, it must ________

On the phase diagram below, identify the normal melting point.

What structural characteristics must a molecule have in order to hydrogen bond?

Which of the following solvents will involve ion-dipole interactions with Na?

What does the line indicated by the arrow in the following phase diagram represent?

The aroma from almonds and cherries is due in part to a compound called benzaldehyde. A graph of the natural logarithm of the vapor pressure of benzaldehyde vs. 1/temperature produces a straight line with a slope of 5,870.99 K. What is the enthalpy of vaporization of benzaldehyde?

Viscosity is a measure of a substance's ________

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) Br2 or NaBr (B) CH3CH2OH or CH3OCH3 (C) CO2 or KOH

Which of the following molecules will have the least interaction with a Li ion?

At ambient temperature, F2 and Cl2 are both gases while Br2 is a liquid and I2 is a solid. This is due to ________

Indicate which of the following nonpolar compounds will have the lowest boiling point.

Write definitions for the terms miscible and soluble.

Which statement about a hydrogen bond is not correct?

The resistance of a liquid to an increase in its surface area is ________

The carbon dioxide pressure in a bottle of champagne is about 6 atm. At this pressure about 0.45 g of carbon dioxide dissolves in 100 mL of champagne. How much carbon dioxide remains dissolved in 100 mL after the bottle is opened? The partial pressure of carbon dioxide then is 6.0 104 atm.

What does the line indicated by the arrow in the following phase diagram represent?

Why do the strengths of dispersion interactions generally increase with the molar mass of the compound?

In understanding why group 16 hydrides, other than those in period 2, have a higher boiling point than the hydrides of groups 14, 15, and 17, which of the following are most important to consider? I.dispersion forces II.dipole-dipole forces III. hydrogen bonding

The phase diagram for carbon dioxide is shown below. What are the phase changes in order as carbon dioxide is heated from 90oC to 50oC, at 500 atm pressure?

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 of the following solvents will involve ion-dipole interactions with Na^?

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) Br₂ or NaBr (B) CH₃CH₂OH or CH₃OCH₃ (C) CO₂ or KOH

Which of the following molecules will have the least interaction with a Li^ion?

At ambient temperature, F₂ and Cl₂are both gases while Br₂ is a liquid and I₂ is a solid. This is due to ________

The carbon dioxide pressure in a bottle of champagne is about 6 atm. At this pressure about 0.45 g of carbon dioxide dissolves in 100 mL of champagne. How much carbon dioxide remains dissolved in 100 mL after the bottle is opened? The partial pressure of carbon dioxide then is 6.0 10^⁴ atm.

The phase diagram for carbon dioxide is shown below. What are the phase changes in order as carbon dioxide is heated from 90^oC to 50^oC, at 500 atm pressure?