Question 1

Which of the following substances cannot form hydrogen bonds?

Accepted Answer

A)  HF 
B)  CH3NH2 
C)  HCl 
D)  NH3 
A)  HF 
B)  CH3NH2 
C)  HCl 
D)  NH3 C

Question 2

The boiling points of the halogens increase going from fluorine to iodine. What type of intermolecular force(s) is (are) responsible for this trend?

Accepted Answer

A)  London dispersion forces 
B)  hydrogen bonding 
C)  ion-dipole attraction 
D)  dipole-dipole interactions 
A)  London dispersion forces 
B)  hydrogen bonding 
C)  ion-dipole attraction 
D)  dipole-dipole interactions A

Question 3

The specific heat of lead is 0.13 J/g °C. How many joules of heat would be required to raise the temperature of 25.0 g of lead from 21 °C to 39 °C?

Accepted Answer

q = SH × m × (T_f - T_i) = 0.13 J/g C × 25.0 g × (39 - 21) = 58000 J = 58 kJ

Question 4

In which of the following liquids would dipole-dipole interactions be the predominant intermolecular force?

Accepted Answer

A)  NH3 
B)  HCl 
C)  PF3 
D)  both B and C 
A)  NH3 
B)  HCl 
C)  PF3 
D)  both B and C

Question 5

Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would be associated with each of the following compounds.
-OF2 ______________________________

Accepted Answer

Question 6

When liquids and gases are compared, liquids have ________ compressability compared to gases and a ________ density.

Accepted Answer

A)  greater, smaller 
B)  smaller, greater 
C)  smaller, smaller 
D)  greater, greater 
A)  greater, smaller 
B)  smaller, greater 
C)  smaller, smaller 
D)  greater, greater

Question 7

The crystal lattice sites in a solid ________.

Accepted Answer

A)  are always occupied by molecules 
B)  may be occupied by atoms 
C)  cannot be occupied by ions 
D)  cannot be occupied by nonpolar molecules 
A)  are always occupied by molecules 
B)  may be occupied by atoms 
C)  cannot be occupied by ions 
D)  cannot be occupied by nonpolar molecules

Question 8

Snow forms in the clouds when water vapor freezes without ever passing through the liquid phase. This process is known as ________.

Accepted Answer

A)  sublimation 
B)  condensation 
C)  freezing 
D)  deposition 
A)  sublimation 
B)  condensation 
C)  freezing 
D)  deposition

Question 9

Which of the following terms does not involve the solid state?

Accepted Answer

A)  evaporation 
B)  melting 
C)  freezing 
D)  sublimation 
A)  evaporation 
B)  melting 
C)  freezing 
D)  sublimation

Question 10

Which of the following compounds would have the lowest boiling point?

Accepted Answer

A)  CH4 
B)  NO2 
C)  HF 
D)  LiCl 
A)  CH4 
B)  NO2 
C)  HF 
D)  LiCl

Question 11

Which of the following would have the highest boiling point?

Accepted Answer

A)  CO2 
B)  H2O 
C)  CH4 
D)  Kr 
A)  CO2 
B)  H2O 
C)  CH4 
D)  Kr

Question 12

How many grams of Ag can be heated from 23 °C to 36 °C when 22 g of Au cools from 95.5 °C to 26.4 °C?
Specific heat of Ag = 0.240 J/(g °C) Specific heat of Au = 0.130 J/(g °C)

Accepted Answer

A)  47 g 
B)  28 g 
C)  63 g 
D)  104 g 
A)  47 g 
B)  28 g 
C)  63 g 
D)  104 g

Question 13

The ClF molecule is polar. Use + and − signs to indicate the direction of polarity in the ClF bond. Using a dashed line, illustrate an ion-dipole interaction between a ClF molecule and a lithium ion.

Accepted Answer

Question 14

If liquid ammonia and water were mixed, between which two atoms in these molecules would a hydrogen bond form?

Accepted Answer

A)  between 1 and 3 
B)  between 2 and 6 
C)  between 3 and 2, 4 and 2, 5 and 2, 1 and 6, and 1 and 7 
D)  Hydrogen bond formation is not possible between these two molecules. 
A)  between 1 and 3 
B)  between 2 and 6 
C)  between 3 and 2, 4 and 2, 5 and 2, 1 and 6, and 1 and 7 
D)  Hydrogen bond formation is not possible between these two molecules.

Question 15

Which of the following statements concerning evaporation is correct?

Accepted Answer

A)  Molecules with energies considerably above average escape from the liquid. 
B)  Decreasing the surface area of the liquid increases the rate of evaporation. 
C)  Evaporation causes the liquid temperature to remain constant. 
D)  Increasing the surface area of the liquid decreases the rate of evaporation. 
A)  Molecules with energies considerably above average escape from the liquid. 
B)  Decreasing the surface area of the liquid increases the rate of evaporation. 
C)  Evaporation causes the liquid temperature to remain constant. 
D)  Increasing the surface area of the liquid decreases the rate of evaporation.

Question 16

In which of the following types of crystalline solids would the forces between particles be covalent bonds?

Accepted Answer

A)  covalent network 
B)  ionic 
C)  metallic 
D)  polar molecular 
A)  covalent network 
B)  ionic 
C)  metallic 
D)  polar molecular

Question 17

Which of the following kinds of intermolecular forces is found in all molecules?

Accepted Answer

A)  hydrogen bonding 
B)  dipole-dipole interactions 
C)  London forces 
D)  Chicago forces 
A)  hydrogen bonding 
B)  dipole-dipole interactions 
C)  London forces 
D)  Chicago forces

Question 18

What is the final temperature after 336 J of heat energy is removed from 25.0 g of water at 19.6 °C? Specific heat of water = 4.18 J/(g °C)

Accepted Answer

A)  32.1 °C 
B)  27.6 °C 
C)  16.4 °C 
D)  24.7 °C 
A)  32.1 °C 
B)  27.6 °C 
C)  16.4 °C 
D)  24.7 °C

Question 19

Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would be associated with each of the following compounds.
-HCOOH ______________________________

Accepted Answer

The answer of Predict the predominate intermolecular force (London force,...

Question 20

Calculate the heat energy that must be removed from 17.6 grams of ammonia gas to condense it to liquid ammonia at its boiling point, ?33 °C. The heat of vaporization for ammonia is 1380 J/g.

Accepted Answer

A)  24,300 J 
B)  78.4 J 
C)  0.0128 J 
D)  9,680 J 
A)  24,300 J 
B)  78.4 J 
C)  0.0128 J 
D)  9,680 J

Which of the following substances cannot form hydrogen bonds?

The boiling points of the halogens increase going from fluorine to iodine. What type of intermolecular force(s) is (are) responsible for this trend?

The specific heat of lead is 0.13 J/g °C. How many joules of heat would be required to raise the temperature of 25.0 g of lead from 21 °C to 39°C?

In which of the following liquids would dipole-dipole interactions be the predominant intermolecular force?

Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would be associated with each of the following compounds. -OF₂ ______________________________

When liquids and gases are compared, liquids have compressability compared to gases and a density.

The crystal lattice sites in a solid ________.

Snow forms in the clouds when water vapor freezes without ever passing through the liquid phase. This process is known as ________.

Which of the following terms does not involve the solid state?

Which of the following compounds would have the lowest boiling point?

Which of the following would have the highest boiling point?

How many grams of Ag can be heated from 23 °C to 36 °C when 22 g of Au cools from 95.5 °C to 26.4 °C? Specific heat of Ag = 0.240 J/(g °C) Specific heat of Au = 0.130 J/(g °C)

The ClF molecule is polar. Use ⁺ and ⁻ signs to indicate the direction of polarity in the ClF bond. Using a dashed line, illustrate an ion-dipole interaction between a ClF molecule and a lithium ion.

If liquid ammonia and water were mixed, between which two atoms in these molecules would a hydrogen bond form?

Which of the following statements concerning evaporation is correct?

In which of the following types of crystalline solids would the forces between particles be covalent bonds?

Which of the following kinds of intermolecular forces is found in all molecules?

What is the final temperature after 336 J of heat energy is removed from 25.0 g of water at 19.6 °C? Specific heat of water = 4.18 J/(g °C)

Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would be associated with each of the following compounds. -HCOOH ______________________________

Calculate the heat energy that must be removed from 17.6 grams of ammonia gas to condense it to liquid ammonia at its boiling point, ?33 °C. The heat of vaporization for ammonia is 1380 J/g.

The Science of Chemistry

Numbers From Measurements

Unit Systems and Dimensional Analysis

Basic Concepts About Matter

Atoms, Molecules, Formulas, and Subatomic Particles

Electronic Structure and Chemical Periodicity

Chemical Bonds

Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

Gas Laws

Solutions

Acids, Bases and Salts

Oxidation and Reduction

Reaction Rates and Chemical Equilibrium

Nuclear Chemistry

Filters

Exam 11: States of Matter

Which of the following substances cannot form hydrogen bonds?

The boiling points of the halogens increase going from fluorine to iodine. What type of intermolecular force(s) is (are) responsible for this trend?

The specific heat of lead is 0.13 J/g °C. How many joules of heat would be required to raise the temperature of 25.0 g of lead from 21 °C to 39 °C?

In which of the following liquids would dipole-dipole interactions be the predominant intermolecular force?

Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would be associated with each of the following compounds. -OF2 ______________________________

When liquids and gases are compared, liquids have ________ compressability compared to gases and a ________ density.

The crystal lattice sites in a solid ________.

Snow forms in the clouds when water vapor freezes without ever passing through the liquid phase. This process is known as ________.

Which of the following terms does not involve the solid state?

Which of the following compounds would have the lowest boiling point?

Which of the following would have the highest boiling point?

How many grams of Ag can be heated from 23 °C to 36 °C when 22 g of Au cools from 95.5 °C to 26.4 °C? Specific heat of Ag = 0.240 J/(g °C) Specific heat of Au = 0.130 J/(g °C)

The ClF molecule is polar. Use + and − signs to indicate the direction of polarity in the ClF bond. Using a dashed line, illustrate an ion-dipole interaction between a ClF molecule and a lithium ion.

If liquid ammonia and water were mixed, between which two atoms in these molecules would a hydrogen bond form?

Which of the following statements concerning evaporation is correct?

In which of the following types of crystalline solids would the forces between particles be covalent bonds?

Which of the following kinds of intermolecular forces is found in all molecules?

What is the final temperature after 336 J of heat energy is removed from 25.0 g of water at 19.6 °C? Specific heat of water = 4.18 J/(g °C)

Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would be associated with each of the following compounds. -HCOOH ______________________________

Calculate the heat energy that must be removed from 17.6 grams of ammonia gas to condense it to liquid ammonia at its boiling point, ?33 °C. The heat of vaporization for ammonia is 1380 J/g.

The Science of Chemistry

Numbers From Measurements

Unit Systems and Dimensional Analysis

Basic Concepts About Matter

Atoms, Molecules, Formulas, and Subatomic Particles

Electronic Structure and Chemical Periodicity

Chemical Bonds

Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

Gas Laws

Solutions

Acids, Bases and Salts

Oxidation and Reduction

Reaction Rates and Chemical Equilibrium

Nuclear Chemistry

Filters

The specific heat of lead is 0.13 J/g °C. How many joules of heat would be required to raise the temperature of 25.0 g of lead from 21 °C to 39°C?

Predict the predominate intermolecular force (London force, dipole-dipole, or hydrogen bonding) that would be associated with each of the following compounds. -OF₂ ______________________________

When liquids and gases are compared, liquids have compressability compared to gases and a density.

The ClF molecule is polar. Use ⁺ and ⁻ signs to indicate the direction of polarity in the ClF bond. Using a dashed line, illustrate an ion-dipole interaction between a ClF molecule and a lithium ion.