UNE CHEM 1011 MIDTERM STUDY GUIDE ACTUAL 2026
QUESTIONS ANDVERIFIED ANSWERS WITH RATIONALES
(GUARANTEED PASS)
Overview
This premium, high-density study guide with meticulously verified
multiple-choice practice questions, answers, and rationales tailored for
the UNE CHEM 1011 Midterm. It delivers thorough coverage of
intermolecular forces, phase transitions, colligative properties, and
chemical kinetics, making it ideal for maximizing student performance.
Designed specifically for high-conversion sales on Stuvia and Docsity,
each item provides actionable conceptual mastery and step-by-step
mathematical reasoning to guarantee top marks.
Module 1: Intermolecular Forces and Liquid Properties
Question 1
Which of the following compounds exhibits hydrogen bonding as its
strongest intermolecular force in the pure liquid state?
A) \(\text{CH}_{4}\)
B) \(\text{H}_2\text{S}\)
C) \(\text{CH}_3\text{OH}\)
D) \(\text{CH}_3\text{F}\)
,VERIFIED ANSWER: C) \(\text{CH}_3\text{OH}\)
EXPLANATION: Hydrogen bonding occurs when hydrogen is directly
bonded to a highly electronegative atom (\(\text{N}\),
\(\text{O}\), or \(\text{F}\)). In methanol
(\(\text{CH}_3\text{OH}\)), the hydrogen is covalently bonded to
oxygen. Methane (\(\text{CH}_{4}\)) only features dispersion
forces, hydrogen sulfide (\(\text{H}_2\text{S}\)) is polar but
lacks \(\text{N}\), \(\text{O}\), or \(\text{F}\), and
fluoromethane (\(\text{CH}_3\text{F}\)) features dipole-dipole
interactions because the fluorine is bonded to carbon, not hydrogen.
Question 2
As the molar mass of a series of linear, nonpolar alkanes increases, how
do the London dispersion forces and the boiling points change?
A) Dispersion forces decrease; boiling points decrease
B) Dispersion forces increase; boiling points decrease
C) Dispersion forces decrease; boiling points increase
D) Dispersion forces increase; boiling points increase
VERIFIED ANSWER: D) Dispersion forces increase; boiling points
increase
EXPLANATION: Larger molecules possess a greater number of
electrons and a larger electron cloud, making them more
polarizable. This increases the strength of temporary instantaneous
,dipoles (London dispersion forces), which requires more thermal
energy to overcome, leading to higher boiling points.
Question 3
Which phenomenon is responsible for the spherical shape of water
droplets on a waxy surface?
A) Viscosity
B) Surface tension
C) Vapor pressure
D) Capillary action
VERIFIED ANSWER: B) Surface tension
EXPLANATION: Surface tension is the energy required to increase
the surface area of a liquid. Molecules at the surface experience a
net inward cohesive force. Since a sphere minimizes the surface-
area-to-volume ratio, cohesive forces drive water droplets into a
spherical shape to minimize surface energy.
Question 4
When cohesive forces within a liquid are weaker than the adhesive forces
between the liquid and a glass capillary wall, what structural feature is
observed?
A) A flat meniscus
B) An inverted (convex) meniscus
, C) A concave meniscus
D) Rapid vaporization of the liquid
VERIFIED ANSWER: C) A concave meniscus
EXPLANATION: When adhesive forces (attraction between different
substances, like water and glass) exceed cohesive forces
(attraction between identical molecules), the liquid climbs the walls
of the container, creating a downward-curving or concave
meniscus.
Question 5
Which statement correctly describes the relationship between
temperature and the viscosity of a liquid?
A) Viscosity increases as temperature increases because kinetic energy
decreases.
B) Viscosity decreases as temperature increases because kinetic energy
increases, allowing molecules to overcome intermolecular forces.
C) Viscosity remains constant regardless of temperature changes.
D) Viscosity decreases as temperature increases due to an increase in
intramolecular bond strength.
VERIFIED ANSWER: B) Viscosity decreases as temperature increases
because kinetic energy increases, allowing molecules to overcome
intermolecular forces.
EXPLANATION: Viscosity is a liquid's resistance to flow. As thermal
QUESTIONS ANDVERIFIED ANSWERS WITH RATIONALES
(GUARANTEED PASS)
Overview
This premium, high-density study guide with meticulously verified
multiple-choice practice questions, answers, and rationales tailored for
the UNE CHEM 1011 Midterm. It delivers thorough coverage of
intermolecular forces, phase transitions, colligative properties, and
chemical kinetics, making it ideal for maximizing student performance.
Designed specifically for high-conversion sales on Stuvia and Docsity,
each item provides actionable conceptual mastery and step-by-step
mathematical reasoning to guarantee top marks.
Module 1: Intermolecular Forces and Liquid Properties
Question 1
Which of the following compounds exhibits hydrogen bonding as its
strongest intermolecular force in the pure liquid state?
A) \(\text{CH}_{4}\)
B) \(\text{H}_2\text{S}\)
C) \(\text{CH}_3\text{OH}\)
D) \(\text{CH}_3\text{F}\)
,VERIFIED ANSWER: C) \(\text{CH}_3\text{OH}\)
EXPLANATION: Hydrogen bonding occurs when hydrogen is directly
bonded to a highly electronegative atom (\(\text{N}\),
\(\text{O}\), or \(\text{F}\)). In methanol
(\(\text{CH}_3\text{OH}\)), the hydrogen is covalently bonded to
oxygen. Methane (\(\text{CH}_{4}\)) only features dispersion
forces, hydrogen sulfide (\(\text{H}_2\text{S}\)) is polar but
lacks \(\text{N}\), \(\text{O}\), or \(\text{F}\), and
fluoromethane (\(\text{CH}_3\text{F}\)) features dipole-dipole
interactions because the fluorine is bonded to carbon, not hydrogen.
Question 2
As the molar mass of a series of linear, nonpolar alkanes increases, how
do the London dispersion forces and the boiling points change?
A) Dispersion forces decrease; boiling points decrease
B) Dispersion forces increase; boiling points decrease
C) Dispersion forces decrease; boiling points increase
D) Dispersion forces increase; boiling points increase
VERIFIED ANSWER: D) Dispersion forces increase; boiling points
increase
EXPLANATION: Larger molecules possess a greater number of
electrons and a larger electron cloud, making them more
polarizable. This increases the strength of temporary instantaneous
,dipoles (London dispersion forces), which requires more thermal
energy to overcome, leading to higher boiling points.
Question 3
Which phenomenon is responsible for the spherical shape of water
droplets on a waxy surface?
A) Viscosity
B) Surface tension
C) Vapor pressure
D) Capillary action
VERIFIED ANSWER: B) Surface tension
EXPLANATION: Surface tension is the energy required to increase
the surface area of a liquid. Molecules at the surface experience a
net inward cohesive force. Since a sphere minimizes the surface-
area-to-volume ratio, cohesive forces drive water droplets into a
spherical shape to minimize surface energy.
Question 4
When cohesive forces within a liquid are weaker than the adhesive forces
between the liquid and a glass capillary wall, what structural feature is
observed?
A) A flat meniscus
B) An inverted (convex) meniscus
, C) A concave meniscus
D) Rapid vaporization of the liquid
VERIFIED ANSWER: C) A concave meniscus
EXPLANATION: When adhesive forces (attraction between different
substances, like water and glass) exceed cohesive forces
(attraction between identical molecules), the liquid climbs the walls
of the container, creating a downward-curving or concave
meniscus.
Question 5
Which statement correctly describes the relationship between
temperature and the viscosity of a liquid?
A) Viscosity increases as temperature increases because kinetic energy
decreases.
B) Viscosity decreases as temperature increases because kinetic energy
increases, allowing molecules to overcome intermolecular forces.
C) Viscosity remains constant regardless of temperature changes.
D) Viscosity decreases as temperature increases due to an increase in
intramolecular bond strength.
VERIFIED ANSWER: B) Viscosity decreases as temperature increases
because kinetic energy increases, allowing molecules to overcome
intermolecular forces.
EXPLANATION: Viscosity is a liquid's resistance to flow. As thermal
