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UNE GENERAL CHEMISTRY II EXAM QUESTIONS AND CORRECT
ANSWERS LATEST EDITION 2026
UNE General Chemistry II — Exam Practice Questions
Exam Coverage Summary
1. Intermolecular Forces & Phase Changes — IMF types (dispersion, dipole-dipole,
hydrogen bonding, ion-dipole), vapor pressure, phase diagrams, heating curves.
2. Solutions & Solubility — Concentration units, colligative properties, solubility equilibria.
3. Thermodynamics & Thermochemistry — Enthalpy, entropy, Gibbs free energy,
spontaneity.
4. Kinetics & Reaction Rates — Rate laws, reaction mechanisms, activation energy,
catalysis.
5. Chemical Equilibrium — Equilibrium constants, Le Châtelier's Principle, ICE tables.
6. Acid-Base Chemistry — Brønsted-Lowry definitions, pH, buffers, titrations, Henderson-
Hasselbalch.
7. Electrochemistry & Redox — Electrochemical cells, Nernst equation, corrosion.
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8. Nuclear Chemistry — Radioactive decay, half-life, nuclear equations.
9. Gas Laws & Stoichiometry — Ideal gas law, partial pressures, reaction stoichiometry.
10. Atomic Structure & Bonding — Electron configuration, periodic trends, Lewis structures.
SECTION 1: INTERMOLECULAR FORCES & PHASE CHANGES (Questions 1–30)
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) .
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 .
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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 .
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 .
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 attractive forces between unlike molecules. Cohesive forces are
between like molecules .
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6. Which substance has the highest normal boiling point?
A) Ne
B) Ar
C) Kr
D) Xe
Answer: D
Rationale: All are noble gases with only London dispersion forces. Boiling point increases with
atomic number (more electrons → stronger temporary dipoles). Xenon has the highest atomic
number .
7. For which compound would hydrogen bonding NOT be an important intermolecular force?
A) HF
B) H₂O
C) NH₃
D) CH₄
Answer: D
Rationale: Hydrogen bonding requires a hydrogen atom bonded to a small, highly
electronegative atom (N, O, or F). Methane (CH₄) has only C-H bonds, so no hydrogen bonding .
8. A substance with strong intermolecular forces has ______ vapor pressure.
A) higher
B) lower
C) the same
D) unpredictable
Answer: B
Rationale: Stronger intermolecular forces make it harder for molecules to escape into the vapor
phase. This results in lower vapor pressure .
9. Which process is exothermic?
A) Melting
B) Vaporization
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UNE GENERAL CHEMISTRY II EXAM QUESTIONS AND CORRECT
ANSWERS LATEST EDITION 2026
UNE General Chemistry II — Exam Practice Questions
Exam Coverage Summary
1. Intermolecular Forces & Phase Changes — IMF types (dispersion, dipole-dipole,
hydrogen bonding, ion-dipole), vapor pressure, phase diagrams, heating curves.
2. Solutions & Solubility — Concentration units, colligative properties, solubility equilibria.
3. Thermodynamics & Thermochemistry — Enthalpy, entropy, Gibbs free energy,
spontaneity.
4. Kinetics & Reaction Rates — Rate laws, reaction mechanisms, activation energy,
catalysis.
5. Chemical Equilibrium — Equilibrium constants, Le Châtelier's Principle, ICE tables.
6. Acid-Base Chemistry — Brønsted-Lowry definitions, pH, buffers, titrations, Henderson-
Hasselbalch.
7. Electrochemistry & Redox — Electrochemical cells, Nernst equation, corrosion.
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8. Nuclear Chemistry — Radioactive decay, half-life, nuclear equations.
9. Gas Laws & Stoichiometry — Ideal gas law, partial pressures, reaction stoichiometry.
10. Atomic Structure & Bonding — Electron configuration, periodic trends, Lewis structures.
SECTION 1: INTERMOLECULAR FORCES & PHASE CHANGES (Questions 1–30)
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) .
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 .
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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 .
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 .
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 attractive forces between unlike molecules. Cohesive forces are
between like molecules .
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6. Which substance has the highest normal boiling point?
A) Ne
B) Ar
C) Kr
D) Xe
Answer: D
Rationale: All are noble gases with only London dispersion forces. Boiling point increases with
atomic number (more electrons → stronger temporary dipoles). Xenon has the highest atomic
number .
7. For which compound would hydrogen bonding NOT be an important intermolecular force?
A) HF
B) H₂O
C) NH₃
D) CH₄
Answer: D
Rationale: Hydrogen bonding requires a hydrogen atom bonded to a small, highly
electronegative atom (N, O, or F). Methane (CH₄) has only C-H bonds, so no hydrogen bonding .
8. A substance with strong intermolecular forces has ______ vapor pressure.
A) higher
B) lower
C) the same
D) unpredictable
Answer: B
Rationale: Stronger intermolecular forces make it harder for molecules to escape into the vapor
phase. This results in lower vapor pressure .
9. Which process is exothermic?
A) Melting
B) Vaporization
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