UNE General Chemistry II Midterm
Exam Comprehensive 400-Question
Practice Test for 2026/2027
EXAM OVERVIEW
The UNE CHEM 1011 General Chemistry II Midterm Exam is a comprehensive assessment
covering the first half of the University of New England's second-semester general
chemistry course. This exam is designed for undergraduate chemistry and pre-health
students, testing foundational knowledge essential for advanced science coursework and
professional programs such as medicine, pharmacy, and dentistry.
Exam Structure and Scope
The UNE General Chemistry II midterm typically covers Weeks 1–7 of the course, with
questions drawn from a test bank format designed to reinforce learning and boost exam
performance.
Key Topics Covered
Intermolecular Forces & Phase Changes – IMF types, vapor pressure, phase diagrams,
heating curves
Solutions & Solubility – Concentration units, colligative properties, solubility equilibria
Thermodynamics & Thermochemistry – Enthalpy, entropy, Gibbs free energy, spontaneity
Kinetics & Reaction Rates – Rate laws, reaction mechanisms, activation energy, catalysis
Equilibrium & Acid-Base Chemistry – Equilibrium constants, Le Châtelier's Principle,
weak acids/bases, buffers, titrations
Electrochemistry & Redox Reactions – Electrochemical cells, Nernst equation, corrosion
Key Course Concepts
,Concept Description
Intermolecular Attractive forces between molecules (dispersion, dipole-dipole, hydrogen
Forces bonding, ion-dipole)
Colligative
Properties depending on solute particle number (BP elevation, FP depression)
Properties
Dynamic balance between forward and reverse reactions; Kc, Kp, Le Châtelier'
Equilibrium
Principle
Acid-Base Chemistry Brønsted-Lowry definitions, pH, buffers, titrations, Henderson-Hasselbalch
Kinetics Rate laws, reaction order, activation energy (Eₐ), mechanisms
Thermodynamics ΔH, ΔS, ΔG; spontaneity; relationship ΔG° = -RT ln K
SECTION 1: INTERMOLECULAR FORCES & PHASE CHANGES (Questions 1-80)
Question 1: Which of the following correctly describes intermolecular forces?
A) Intramolecular forces that hold atoms together within a molecule
B) Attractive forces that exist between molecules
C) Repulsive forces that exist between ions
D) Forces that only exist in solids
Answer: B
Rationale: Intermolecular forces are attractive forces that exist between molecules. They
determine physical properties like boiling point and vapor pressure. Option A describes
intramolecular forces (covalent/ionic bonds). Option C describes ionic interactions
incorrectly. Option D is false as IMFs exist in all states of matter.
Question 2: Which intermolecular force is present in ALL molecules, regardless of
polarity?
A) Hydrogen bonding
,B) Dipole-dipole forces
C) London dispersion forces
D) Ion-dipole forces
Answer: C
Rationale: London dispersion forces are present in all molecules due to temporary
fluctuations in electron distribution that create instantaneous dipoles. Hydrogen bonding
and dipole-dipole forces require polar molecules, and ion-dipole forces require ions.
Question 3: What type of intermolecular force is primarily responsible for the unusually
high boiling point of water?
A) London dispersion forces
B) Dipole-dipole forces
C) Hydrogen bonding
D) Ionic bonding
Answer: C
Rationale: Hydrogen bonding is a particularly strong type of dipole-dipole force that
occurs when hydrogen is bonded to N, O, or F. Water's high boiling point is due to
extensive hydrogen bonding between molecules. A is too weak; B is present but not the
primary reason; D is an intramolecular force.
Question 4: Which of the following compounds would you expect to have the HIGHEST
boiling point?
A) CH₄
B) H₂S
C) H₂O
D) HCl
Answer: C
Rationale: H₂O has the highest boiling point due to strong hydrogen bonding. H₂S has
weaker dipole-dipole forces, HCl has dipole-dipole forces but weaker than H-bonds, and
CH₄ only has weak London dispersion forces.
Question 5: An adhesive force is best described as:
A) An attractive force between molecules of the same substance
B) An attractive force between different molecules
, C) A repulsive force between molecules
D) A force that only exists in solids
Answer: B
Rationale: Adhesive forces are intermolecular forces that attract different molecules
together. Cohesive forces are between molecules of the same substance. The other
options describe repulsive forces or are limited in scope.
Question 6: Metallic solids are best described as:
A) Atoms held together by ionic bonds
B) Atoms with nuclei in a "sea" of delocalized electrons
C) Molecules held together by covalent bonds
D) Atoms held together by hydrogen bonds
Answer: B
Rationale: Metallic solids consist of atoms with their nuclei in a "sea" of delocalized
electrons, which accounts for their electrical conductivity and malleability. Options A, C,
and D describe other types of solids (ionic, covalent network, molecular).
Question 7: Acetonitrile (CH₃CN) evaporates quickly at room temperature and feels cold
when evaporating. If ΔH_vap for acetonitrile is 34.2 kJ/mol, how much heat is removed
when 1.00 mole of acetonitrile evaporates?
A) 34.2 J
B) 34.2 kJ
C) 68.4 kJ
D) 17.1 kJ
Answer: B
Rationale: The heat of vaporization (ΔH_vap) is the heat required to vaporize one mole of
a substance. For acetonitrile, 34.2 kJ/mol means 34.2 kJ of heat is absorbed from the
surroundings when 1 mole evaporates. Options A, C, and D are calculation errors.
Question 8: Which of the following has the strongest London dispersion forces?
A) He
B) Ne
C) Ar
D) Xe
Exam Comprehensive 400-Question
Practice Test for 2026/2027
EXAM OVERVIEW
The UNE CHEM 1011 General Chemistry II Midterm Exam is a comprehensive assessment
covering the first half of the University of New England's second-semester general
chemistry course. This exam is designed for undergraduate chemistry and pre-health
students, testing foundational knowledge essential for advanced science coursework and
professional programs such as medicine, pharmacy, and dentistry.
Exam Structure and Scope
The UNE General Chemistry II midterm typically covers Weeks 1–7 of the course, with
questions drawn from a test bank format designed to reinforce learning and boost exam
performance.
Key Topics Covered
Intermolecular Forces & Phase Changes – IMF types, vapor pressure, phase diagrams,
heating curves
Solutions & Solubility – Concentration units, colligative properties, solubility equilibria
Thermodynamics & Thermochemistry – Enthalpy, entropy, Gibbs free energy, spontaneity
Kinetics & Reaction Rates – Rate laws, reaction mechanisms, activation energy, catalysis
Equilibrium & Acid-Base Chemistry – Equilibrium constants, Le Châtelier's Principle,
weak acids/bases, buffers, titrations
Electrochemistry & Redox Reactions – Electrochemical cells, Nernst equation, corrosion
Key Course Concepts
,Concept Description
Intermolecular Attractive forces between molecules (dispersion, dipole-dipole, hydrogen
Forces bonding, ion-dipole)
Colligative
Properties depending on solute particle number (BP elevation, FP depression)
Properties
Dynamic balance between forward and reverse reactions; Kc, Kp, Le Châtelier'
Equilibrium
Principle
Acid-Base Chemistry Brønsted-Lowry definitions, pH, buffers, titrations, Henderson-Hasselbalch
Kinetics Rate laws, reaction order, activation energy (Eₐ), mechanisms
Thermodynamics ΔH, ΔS, ΔG; spontaneity; relationship ΔG° = -RT ln K
SECTION 1: INTERMOLECULAR FORCES & PHASE CHANGES (Questions 1-80)
Question 1: Which of the following correctly describes intermolecular forces?
A) Intramolecular forces that hold atoms together within a molecule
B) Attractive forces that exist between molecules
C) Repulsive forces that exist between ions
D) Forces that only exist in solids
Answer: B
Rationale: Intermolecular forces are attractive forces that exist between molecules. They
determine physical properties like boiling point and vapor pressure. Option A describes
intramolecular forces (covalent/ionic bonds). Option C describes ionic interactions
incorrectly. Option D is false as IMFs exist in all states of matter.
Question 2: Which intermolecular force is present in ALL molecules, regardless of
polarity?
A) Hydrogen bonding
,B) Dipole-dipole forces
C) London dispersion forces
D) Ion-dipole forces
Answer: C
Rationale: London dispersion forces are present in all molecules due to temporary
fluctuations in electron distribution that create instantaneous dipoles. Hydrogen bonding
and dipole-dipole forces require polar molecules, and ion-dipole forces require ions.
Question 3: What type of intermolecular force is primarily responsible for the unusually
high boiling point of water?
A) London dispersion forces
B) Dipole-dipole forces
C) Hydrogen bonding
D) Ionic bonding
Answer: C
Rationale: Hydrogen bonding is a particularly strong type of dipole-dipole force that
occurs when hydrogen is bonded to N, O, or F. Water's high boiling point is due to
extensive hydrogen bonding between molecules. A is too weak; B is present but not the
primary reason; D is an intramolecular force.
Question 4: Which of the following compounds would you expect to have the HIGHEST
boiling point?
A) CH₄
B) H₂S
C) H₂O
D) HCl
Answer: C
Rationale: H₂O has the highest boiling point due to strong hydrogen bonding. H₂S has
weaker dipole-dipole forces, HCl has dipole-dipole forces but weaker than H-bonds, and
CH₄ only has weak London dispersion forces.
Question 5: An adhesive force is best described as:
A) An attractive force between molecules of the same substance
B) An attractive force between different molecules
, C) A repulsive force between molecules
D) A force that only exists in solids
Answer: B
Rationale: Adhesive forces are intermolecular forces that attract different molecules
together. Cohesive forces are between molecules of the same substance. The other
options describe repulsive forces or are limited in scope.
Question 6: Metallic solids are best described as:
A) Atoms held together by ionic bonds
B) Atoms with nuclei in a "sea" of delocalized electrons
C) Molecules held together by covalent bonds
D) Atoms held together by hydrogen bonds
Answer: B
Rationale: Metallic solids consist of atoms with their nuclei in a "sea" of delocalized
electrons, which accounts for their electrical conductivity and malleability. Options A, C,
and D describe other types of solids (ionic, covalent network, molecular).
Question 7: Acetonitrile (CH₃CN) evaporates quickly at room temperature and feels cold
when evaporating. If ΔH_vap for acetonitrile is 34.2 kJ/mol, how much heat is removed
when 1.00 mole of acetonitrile evaporates?
A) 34.2 J
B) 34.2 kJ
C) 68.4 kJ
D) 17.1 kJ
Answer: B
Rationale: The heat of vaporization (ΔH_vap) is the heat required to vaporize one mole of
a substance. For acetonitrile, 34.2 kJ/mol means 34.2 kJ of heat is absorbed from the
surroundings when 1 mole evaporates. Options A, C, and D are calculation errors.
Question 8: Which of the following has the strongest London dispersion forces?
A) He
B) Ne
C) Ar
D) Xe
