CHEM 1011 UNIVERSITY OF NEW
ENGLAND GEN CHEM II ULTIMATE
MIDTERM TEST BANK & DETAILED
RATIONALES
This premium question master test bank provides a comprehensive study
resource tailored to mirror the exact structure and difficulty of the UNE
General Chemistry II Midterm Exam. Each high-yield question features
clear formatting, an italicised quick-answer key, and a bold-italicized
expert rationale designed to simplify complex chemical math and
conceptual theory. Downloading this verified solutions manual offers the
ultimate shortcut to mastering kinetics, equilibrium, and thermodynamics
while securing an effortless A+ grade.
Section 1: Intermolecular Forces, Liquids, and
Solids (Questions 1–13) Question 1
Which of the following compounds exhibits only
London dispersion forces as its primary
intermolecular force? A) \(\text{H}_2\text{O}\)
B) \(\text{NH}_{3}\)
C) \(\text{CF}_{4}\)
D) \(\text{CH}_2\text{Cl}_2\)
Answer: C) \(\text{CF}_{4}\)
Rationale: \(\text{CF}_{4}\) is a highly
symmetrical tetrahedral molecule. Although
individual C–F bonds are polar, the dipoles
cancel out perfectly, making the overall molecule
nonpolar. Nonpolar molecules only interact via
,temporary dipole-induced dipoles, known as
London dispersion forces.
Question 2
What type of intermolecular force is responsible for
the uniquely high boiling point of water
(\(\text{H}_2\text{O}\))?
A) London dispersion forces
B) Dipole-dipole interactions
C) Hydrogen bonding
D) Ion-dipole forces
Answer: C) Hydrogen bonding
Rationale: Hydrogen bonding is a strong type of
dipole-dipole interaction that occurs specifically
when hydrogen is covalently bonded to highly
electronegative elements like N, O, or F. The
intense electrostatic attraction between water
molecules raises its boiling point drastically
compared to other compounds of similar molar
mass.
Question 3
Which of the following properties decreases as the
temperature of a liquid increases?
A) Vapor pressure
B) Rate of evaporation
C) Viscosity
,D) Kinetic energy of molecules
Answer: C) Viscosity
Rationale: As temperature rises, the average
kinetic energy of molecules increases, allowing
them to overcome the cohesive intermolecular
forces holding them together. This causes the
liquid to flow more freely, which means viscosity
decreases.
Question 4
The resistance of a liquid to an increase in its
surface area is known as what?
A) Capillary action
B) Surface tension
C) Volatility
D) Viscosity
Answer: B) Surface tension
Rationale: Surface tension represents the energy
required to expand the surface area of a liquid.
Molecules at the surface experience a net inward
cohesive pull from neighboring interior
molecules, minimizing surface area.
Question 5
Which phase change represents an endothermic
process?
A) Condensation
, B) Deposition
C) Freezing
D) Vaporization
Answer: D) Vaporization
Rationale: Vaporization is the transition from a
liquid to a gas, which requires an input of
thermal energy to fully overcome the
intermolecular forces stabilizing the liquid
phase. Processes that absorb energy are
classified as endothermic.
Question 6
Which phase change represents an exothermic
process? A) Sublimation
B) Condensation
C) Melting
D) Vaporization
Answer: B) Condensation
Rationale: Condensation involves going from a
gas to a liquid. Because gas particles lose
kinetic energy and form stabilizing
intermolecular bonds to form a liquid, heat is
released to the surroundings, making it an
exothermic process.
ENGLAND GEN CHEM II ULTIMATE
MIDTERM TEST BANK & DETAILED
RATIONALES
This premium question master test bank provides a comprehensive study
resource tailored to mirror the exact structure and difficulty of the UNE
General Chemistry II Midterm Exam. Each high-yield question features
clear formatting, an italicised quick-answer key, and a bold-italicized
expert rationale designed to simplify complex chemical math and
conceptual theory. Downloading this verified solutions manual offers the
ultimate shortcut to mastering kinetics, equilibrium, and thermodynamics
while securing an effortless A+ grade.
Section 1: Intermolecular Forces, Liquids, and
Solids (Questions 1–13) Question 1
Which of the following compounds exhibits only
London dispersion forces as its primary
intermolecular force? A) \(\text{H}_2\text{O}\)
B) \(\text{NH}_{3}\)
C) \(\text{CF}_{4}\)
D) \(\text{CH}_2\text{Cl}_2\)
Answer: C) \(\text{CF}_{4}\)
Rationale: \(\text{CF}_{4}\) is a highly
symmetrical tetrahedral molecule. Although
individual C–F bonds are polar, the dipoles
cancel out perfectly, making the overall molecule
nonpolar. Nonpolar molecules only interact via
,temporary dipole-induced dipoles, known as
London dispersion forces.
Question 2
What type of intermolecular force is responsible for
the uniquely high boiling point of water
(\(\text{H}_2\text{O}\))?
A) London dispersion forces
B) Dipole-dipole interactions
C) Hydrogen bonding
D) Ion-dipole forces
Answer: C) Hydrogen bonding
Rationale: Hydrogen bonding is a strong type of
dipole-dipole interaction that occurs specifically
when hydrogen is covalently bonded to highly
electronegative elements like N, O, or F. The
intense electrostatic attraction between water
molecules raises its boiling point drastically
compared to other compounds of similar molar
mass.
Question 3
Which of the following properties decreases as the
temperature of a liquid increases?
A) Vapor pressure
B) Rate of evaporation
C) Viscosity
,D) Kinetic energy of molecules
Answer: C) Viscosity
Rationale: As temperature rises, the average
kinetic energy of molecules increases, allowing
them to overcome the cohesive intermolecular
forces holding them together. This causes the
liquid to flow more freely, which means viscosity
decreases.
Question 4
The resistance of a liquid to an increase in its
surface area is known as what?
A) Capillary action
B) Surface tension
C) Volatility
D) Viscosity
Answer: B) Surface tension
Rationale: Surface tension represents the energy
required to expand the surface area of a liquid.
Molecules at the surface experience a net inward
cohesive pull from neighboring interior
molecules, minimizing surface area.
Question 5
Which phase change represents an endothermic
process?
A) Condensation
, B) Deposition
C) Freezing
D) Vaporization
Answer: D) Vaporization
Rationale: Vaporization is the transition from a
liquid to a gas, which requires an input of
thermal energy to fully overcome the
intermolecular forces stabilizing the liquid
phase. Processes that absorb energy are
classified as endothermic.
Question 6
Which phase change represents an exothermic
process? A) Sublimation
B) Condensation
C) Melting
D) Vaporization
Answer: B) Condensation
Rationale: Condensation involves going from a
gas to a liquid. Because gas particles lose
kinetic energy and form stabilizing
intermolecular bonds to form a liquid, heat is
released to the surroundings, making it an
exothermic process.
