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UNE CHEM 1011 – GENERAL CHEMISTRY II
COMPREHENSIVE FINAL ACTUAL EXAM PREP 2026
ALL QUESTIONS AND CORRECT DETAILED
ANSWERS WITH RATIONALES ALREADY A GRADED
|NEW AND REVISED |HIGHLY RECOMMENDED BY
EXPERTS
Question 1
Which of the following intermolecular forces is present in ALL
molecules?
A. Hydrogen bonding
B. Dipole-dipole interactions
C. London dispersion forces
D. Ion-dipole interactions
Rationale: London dispersion forces (LDFs) are present in all
molecules due to temporary fluctuations in electron distribution. They
are the only intermolecular force present in nonpolar molecules.
Hydrogen bonding, dipole-dipole, and ion-dipole interactions require
specific molecular features (H bonded to F/O/N, permanent dipoles, or
ions, respectively).
Question 2
A hydrogen bond is characterized by:
A. The attraction of temporary dipoles produced by random electron
motion
B. The electrostatic attraction between permanent dipoles in any polar
molecule
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C. A strong dipole-dipole attraction between a hydrogen atom
bonded to N, O, or F and another N, O, or F atom
D. The covalent sharing of electrons between two atoms
Rationale: A hydrogen bond is a special type of dipole-dipole
interaction that occurs when a hydrogen atom is covalently bonded to
a highly electronegative atom (F, O, or N). The partially positive
hydrogen is attracted to a lone pair on an electronegative atom in
another molecule. This is the strongest type of dipole-dipole
interaction.
Question 3
Which of the following substances would you expect to have the highest
boiling point?
A. CH₄
B. CCl₄
C. CHCl₃
D. H₂O
Rationale: Water (H₂O) has the highest boiling point among the
options due to the presence of hydrogen bonding, which is the
strongest intermolecular force. CH₄ and CCl₄ are nonpolar and only
have London dispersion forces. CHCl₃ has dipole-dipole interactions
but not hydrogen bonding.
Question 4
A cohesive force is:
A. The intermolecular force that attracts identical molecules
B. The intermolecular force that attracts different molecules
C. The force that holds atoms together in a molecule
D. Always stronger than an adhesive force
Rationale: Cohesive forces are the intermolecular forces that attract
identical molecules to one another. Adhesive forces attract different
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molecules together. Both are types of intermolecular attractions, but
they differ in whether the molecules are the same or different.
Question 5
Which of the following describes a liquid?
A. Particles are far apart with no regular arrangement; they move
independently
B. Particles are close together with no regular arrangement; they
can move past each other
C. Particles are tightly packed in a regular pattern and vibrate in fixed
positions
D. Particles are close together and vibrate but cannot move past each
other
Rationale: In a liquid, particles are close together with no regular
arrangement. They have enough energy to move past each other but
remain in essentially constant contact. This allows liquids to flow and
take the shape of their container while maintaining a fixed volume.
Question 6
Viscosity is a measure of:
A. The rate of evaporation
B. A liquid's resistance to flow
C. The surface tension of a liquid
D. The boiling point of a liquid
Rationale: Viscosity is a measure of a liquid's resistance to flow. It is
influenced by the strength of intermolecular forces, molecular size and
shape, and temperature. Liquids with strong intermolecular forces
(like hydrogen bonding) typically have higher viscosities.
Question 7
Which of the following factors affects the viscosity of a liquid?
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A. Intermolecular forces between molecules
B. The size and shape of the molecules
C. Temperature
D. All of the above
Rationale: Viscosity is affected by all of these factors. Stronger
intermolecular forces increase viscosity. Larger, more complex
molecules also increase viscosity. As temperature increases, viscosity
generally decreases because the molecules have more kinetic energy to
overcome intermolecular attractions.
Question 8
What is the molality of a solution?
A. Moles of solute per liter of solution
B. Moles of solute per kilogram of solvent
C. Grams of solute per liter of solution
D. Moles of solute per mole of total solution
Rationale: Molality (m) is defined as moles of solute divided by the
mass of the solvent in kilograms. It is temperature-independent, unlike
molarity, which depends on volume and therefore changes with
temperature.
Question 9
The solubility of a solid in a liquid typically __________ with
__________ temperature.
A. decreases, decreasing
B. increases, decreasing
C. increases, increasing
D. decreases, increasing
Rationale: For most solids, solubility increases with increasing
temperature. This is because the dissolution process is often
endothermic, and higher temperatures favor dissolution by providing
UNE CHEM 1011 – GENERAL CHEMISTRY II
COMPREHENSIVE FINAL ACTUAL EXAM PREP 2026
ALL QUESTIONS AND CORRECT DETAILED
ANSWERS WITH RATIONALES ALREADY A GRADED
|NEW AND REVISED |HIGHLY RECOMMENDED BY
EXPERTS
Question 1
Which of the following intermolecular forces is present in ALL
molecules?
A. Hydrogen bonding
B. Dipole-dipole interactions
C. London dispersion forces
D. Ion-dipole interactions
Rationale: London dispersion forces (LDFs) are present in all
molecules due to temporary fluctuations in electron distribution. They
are the only intermolecular force present in nonpolar molecules.
Hydrogen bonding, dipole-dipole, and ion-dipole interactions require
specific molecular features (H bonded to F/O/N, permanent dipoles, or
ions, respectively).
Question 2
A hydrogen bond is characterized by:
A. The attraction of temporary dipoles produced by random electron
motion
B. The electrostatic attraction between permanent dipoles in any polar
molecule
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C. A strong dipole-dipole attraction between a hydrogen atom
bonded to N, O, or F and another N, O, or F atom
D. The covalent sharing of electrons between two atoms
Rationale: A hydrogen bond is a special type of dipole-dipole
interaction that occurs when a hydrogen atom is covalently bonded to
a highly electronegative atom (F, O, or N). The partially positive
hydrogen is attracted to a lone pair on an electronegative atom in
another molecule. This is the strongest type of dipole-dipole
interaction.
Question 3
Which of the following substances would you expect to have the highest
boiling point?
A. CH₄
B. CCl₄
C. CHCl₃
D. H₂O
Rationale: Water (H₂O) has the highest boiling point among the
options due to the presence of hydrogen bonding, which is the
strongest intermolecular force. CH₄ and CCl₄ are nonpolar and only
have London dispersion forces. CHCl₃ has dipole-dipole interactions
but not hydrogen bonding.
Question 4
A cohesive force is:
A. The intermolecular force that attracts identical molecules
B. The intermolecular force that attracts different molecules
C. The force that holds atoms together in a molecule
D. Always stronger than an adhesive force
Rationale: Cohesive forces are the intermolecular forces that attract
identical molecules to one another. Adhesive forces attract different
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molecules together. Both are types of intermolecular attractions, but
they differ in whether the molecules are the same or different.
Question 5
Which of the following describes a liquid?
A. Particles are far apart with no regular arrangement; they move
independently
B. Particles are close together with no regular arrangement; they
can move past each other
C. Particles are tightly packed in a regular pattern and vibrate in fixed
positions
D. Particles are close together and vibrate but cannot move past each
other
Rationale: In a liquid, particles are close together with no regular
arrangement. They have enough energy to move past each other but
remain in essentially constant contact. This allows liquids to flow and
take the shape of their container while maintaining a fixed volume.
Question 6
Viscosity is a measure of:
A. The rate of evaporation
B. A liquid's resistance to flow
C. The surface tension of a liquid
D. The boiling point of a liquid
Rationale: Viscosity is a measure of a liquid's resistance to flow. It is
influenced by the strength of intermolecular forces, molecular size and
shape, and temperature. Liquids with strong intermolecular forces
(like hydrogen bonding) typically have higher viscosities.
Question 7
Which of the following factors affects the viscosity of a liquid?
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A. Intermolecular forces between molecules
B. The size and shape of the molecules
C. Temperature
D. All of the above
Rationale: Viscosity is affected by all of these factors. Stronger
intermolecular forces increase viscosity. Larger, more complex
molecules also increase viscosity. As temperature increases, viscosity
generally decreases because the molecules have more kinetic energy to
overcome intermolecular attractions.
Question 8
What is the molality of a solution?
A. Moles of solute per liter of solution
B. Moles of solute per kilogram of solvent
C. Grams of solute per liter of solution
D. Moles of solute per mole of total solution
Rationale: Molality (m) is defined as moles of solute divided by the
mass of the solvent in kilograms. It is temperature-independent, unlike
molarity, which depends on volume and therefore changes with
temperature.
Question 9
The solubility of a solid in a liquid typically __________ with
__________ temperature.
A. decreases, decreasing
B. increases, decreasing
C. increases, increasing
D. decreases, increasing
Rationale: For most solids, solubility increases with increasing
temperature. This is because the dissolution process is often
endothermic, and higher temperatures favor dissolution by providing
