ACS General Chemistry 2 (Gen Chem 2) Final Exam 2026–2027 |
Practice Test Questions & Answers | Complete Study Guide
Prepare for the ACS General Chemistry 2 (Gen Chem 2) Final Exam with this comprehensive
study guide featuring practice questions, verified answers, and detailed rationales. This resource
covers essential topics including chemical kinetics, chemical equilibrium, acids and bases,
buffers, solubility, thermodynamics, electrochemistry, nuclear chemistry, and coordination
compounds. Designed to reinforce fundamental chemistry concepts and improve exam readiness,
the material reflects the key content areas commonly assessed on the ACS Gen Chem 2 Final
Examination. Ideal for college students seeking a reliable resource to strengthen their
understanding, build confidence, and achieve success on the ACS Chemistry final exam.
UNIT 1: INTERMOLECULAR FORCES, LIQUIDS & SOLIDS (6 Questions)
Question 1
Which type of intermolecular interaction is present in all molecules?
A) Hydrogen bonding
B) London dispersion forces
C) Ion-dipole forces
D) Dipole-dipole interactions
Rationale: London dispersion forces arise from temporary fluctuations in electron density
that create instantaneous dipoles. They are present in all molecules regardless of polarity.
Hydrogen bonding (A), dipole-dipole (D), and ion-dipole (C) require permanent dipoles or
ions, so they are not universal.
Question 2
,What is the predominant intermolecular force in liquid HCl?
A) London dispersion forces
B) Dipole-dipole forces
C) Hydrogen bonding
D) Ion-dipole forces
Rationale: HCl is a polar molecule with a permanent dipole. While HCl has some hydrogen
bonding character (H–Cl is polar), dipole-dipole interactions are the dominant IMF.
Hydrogen bonds in HCl are not as strong as in H–F, H–O, or H–N compounds.
Question 3
Which noble gas has the highest normal boiling point?
A) Ne
B) Ar
C) Kr
D) Xe
Rationale: All noble gases have only London dispersion forces. Boiling point increases with
atomic number because more electrons lead to stronger temporary dipoles and greater
polarizability. Xenon has the highest atomic number in the list, giving it the strongest
London forces and the highest boiling point.
Question 4
,A substance has a high vapor pressure at room temperature. This indicates that the
substance:
A) Has strong intermolecular forces
B) Has weak intermolecular forces
C) Has a high boiling point
D) Is ionic
Rationale: Vapor pressure is inversely related to the strength of intermolecular forces.
Substances with weak IMFs have molecules that escape the liquid phase more readily,
resulting in higher vapor pressure. High vapor pressure corresponds to low boiling point,
not high (C).
Question 5
Which of the following substances will have the highest surface tension at room
temperature?
A) Pentane (C₅H₁₂)
B) Water (H₂O)
C) Acetone (CH₃COCH₃)
D) Hexane (C₆H₁₄)
Rationale: Surface tension increases with the strength of intermolecular forces. Water has
extensive hydrogen bonding, which is the strongest type of IMF among the options.
Pentane and hexane have only London forces. Acetone has dipole-dipole but not hydrogen
bonding as strong as water’s.
, Question 6
On a phase diagram, the line separating the solid and liquid phases is called the:
A) Vapor pressure curve
B) Fusion (melting) curve
C) Sublimation curve
D) Critical isotherm
Rationale: On a phase diagram, the fusion (or melting) curve represents the conditions of
temperature and pressure where solid and liquid phases coexist in equilibrium. The vapor
pressure curve separates liquid and gas. The sublimation curve separates solid and gas.
UNIT 2: SOLUTIONS & THEIR PROPERTIES (8 Questions)
Question 7
A solution of NaCl in water has a concentration of 20.5% by mass. What is the molal
concentration of the solution? (Molar mass NaCl = 58.44 g/mol)
A) 0.205 m
B) 0.258 m
C) 3.51 m
D) 4.41 m
*Rationale: A 20.5% by mass solution means 20.5 g NaCl per 100 g solution. Mass of
water = 100 – 20.5 = 79.5 g = 0.0795 kg. Moles NaCl = 20..44 = 0.3508 mol.
Molality = moles solute / kg solvent = 0..0795 = 4.41 m.*
Practice Test Questions & Answers | Complete Study Guide
Prepare for the ACS General Chemistry 2 (Gen Chem 2) Final Exam with this comprehensive
study guide featuring practice questions, verified answers, and detailed rationales. This resource
covers essential topics including chemical kinetics, chemical equilibrium, acids and bases,
buffers, solubility, thermodynamics, electrochemistry, nuclear chemistry, and coordination
compounds. Designed to reinforce fundamental chemistry concepts and improve exam readiness,
the material reflects the key content areas commonly assessed on the ACS Gen Chem 2 Final
Examination. Ideal for college students seeking a reliable resource to strengthen their
understanding, build confidence, and achieve success on the ACS Chemistry final exam.
UNIT 1: INTERMOLECULAR FORCES, LIQUIDS & SOLIDS (6 Questions)
Question 1
Which type of intermolecular interaction is present in all molecules?
A) Hydrogen bonding
B) London dispersion forces
C) Ion-dipole forces
D) Dipole-dipole interactions
Rationale: London dispersion forces arise from temporary fluctuations in electron density
that create instantaneous dipoles. They are present in all molecules regardless of polarity.
Hydrogen bonding (A), dipole-dipole (D), and ion-dipole (C) require permanent dipoles or
ions, so they are not universal.
Question 2
,What is the predominant intermolecular force in liquid HCl?
A) London dispersion forces
B) Dipole-dipole forces
C) Hydrogen bonding
D) Ion-dipole forces
Rationale: HCl is a polar molecule with a permanent dipole. While HCl has some hydrogen
bonding character (H–Cl is polar), dipole-dipole interactions are the dominant IMF.
Hydrogen bonds in HCl are not as strong as in H–F, H–O, or H–N compounds.
Question 3
Which noble gas has the highest normal boiling point?
A) Ne
B) Ar
C) Kr
D) Xe
Rationale: All noble gases have only London dispersion forces. Boiling point increases with
atomic number because more electrons lead to stronger temporary dipoles and greater
polarizability. Xenon has the highest atomic number in the list, giving it the strongest
London forces and the highest boiling point.
Question 4
,A substance has a high vapor pressure at room temperature. This indicates that the
substance:
A) Has strong intermolecular forces
B) Has weak intermolecular forces
C) Has a high boiling point
D) Is ionic
Rationale: Vapor pressure is inversely related to the strength of intermolecular forces.
Substances with weak IMFs have molecules that escape the liquid phase more readily,
resulting in higher vapor pressure. High vapor pressure corresponds to low boiling point,
not high (C).
Question 5
Which of the following substances will have the highest surface tension at room
temperature?
A) Pentane (C₅H₁₂)
B) Water (H₂O)
C) Acetone (CH₃COCH₃)
D) Hexane (C₆H₁₄)
Rationale: Surface tension increases with the strength of intermolecular forces. Water has
extensive hydrogen bonding, which is the strongest type of IMF among the options.
Pentane and hexane have only London forces. Acetone has dipole-dipole but not hydrogen
bonding as strong as water’s.
, Question 6
On a phase diagram, the line separating the solid and liquid phases is called the:
A) Vapor pressure curve
B) Fusion (melting) curve
C) Sublimation curve
D) Critical isotherm
Rationale: On a phase diagram, the fusion (or melting) curve represents the conditions of
temperature and pressure where solid and liquid phases coexist in equilibrium. The vapor
pressure curve separates liquid and gas. The sublimation curve separates solid and gas.
UNIT 2: SOLUTIONS & THEIR PROPERTIES (8 Questions)
Question 7
A solution of NaCl in water has a concentration of 20.5% by mass. What is the molal
concentration of the solution? (Molar mass NaCl = 58.44 g/mol)
A) 0.205 m
B) 0.258 m
C) 3.51 m
D) 4.41 m
*Rationale: A 20.5% by mass solution means 20.5 g NaCl per 100 g solution. Mass of
water = 100 – 20.5 = 79.5 g = 0.0795 kg. Moles NaCl = 20..44 = 0.3508 mol.
Molality = moles solute / kg solvent = 0..0795 = 4.41 m.*
