CHEM 2080: General Chemistry II – Course Syllabus and Topic Overview

CHEM 2080: General Chemistry II – Topic Overview

Module I: Thermochemistry and Chemical Kinetics

This module introduces the principles of thermochemistry and the fundamentals of chemical kinetics, focusing on energy changes in chemical reactions and the rates at which reactions occur.

• Thermochemistry (Chapter 5): Study of energy changes, particularly heat, involved in chemical processes.

• Chemical Kinetics (Sections 14.1–14.4): Examination of reaction rates, factors affecting rates, and the interpretation of rate laws.

• Key Concepts:

  • Enthalpy (H): The heat content of a system at constant pressure.

  • First Law of Thermodynamics: Conservation of energy in chemical processes.

  • Rate Law: Mathematical relationship between reaction rate and concentrations of reactants.

• Example Equation (Thermochemistry): $\Delta H = H_{products} - H_{reactants}$

• Example Equation (Kinetics): $\text{Rate} = k[A]^m[B]^n$

Module II: Advanced Kinetics, Equilibrium, and Acid-Base Chemistry

This module explores the mechanisms of chemical reactions, the concept of chemical equilibrium, and the behavior of acids and bases in aqueous solutions.

• Chemical Kinetics (Mechanisms) (Sections 14.5–14.6): Analysis of reaction mechanisms and the determination of rate-determining steps.

• Chemical Equilibrium (Chapter 15): Study of dynamic equilibrium in chemical systems and the equilibrium constant.

• Acid-Base Equilibria (Chapter 16): Examination of acid and base strength, pH calculations, and titration curves.

• Aqueous Equilibria: Buffers and Titrations (Sections 17.1–17.3): Understanding buffer solutions and their capacity, as well as titration methods.

• Key Concepts:

  • Equilibrium Constant (K): Quantifies the position of equilibrium for a reversible reaction.

  • pH and pOH: Measures of acidity and basicity in solution.

  • Buffer: Solution that resists changes in pH upon addition of acid or base.

• Example Equation (Equilibrium): $K_c = \frac{[C]^c[D]^d}{[A]^a[B]^b}$

• Example Equation (pH): $\text{pH} = -\log[H^+]$

Module III: Liquids, Solutions, and Solubility Equilibria

This module covers the properties of liquids, intermolecular forces, solution formation, and solubility equilibria in aqueous systems.

• Liquids and Intermolecular Forces (Sections 11.1–11.2, 11.4–11.6): Exploration of the physical properties of liquids and the forces that hold molecules together.

• Properties of Solutions (Sections 13.1–13.5): Study of solution concentration, colligative properties, and factors affecting solubility.

• Aqueous Equilibria: Solubility (Sections 17.4–17.6): Analysis of solubility product constants and precipitation reactions.

• Key Concepts:

  • Intermolecular Forces: Includes hydrogen bonding, dipole-dipole, and London dispersion forces.

  • Colligative Properties: Properties that depend on the number of solute particles (e.g., boiling point elevation, freezing point depression).

  • Solubility Product (Ksp): Equilibrium constant for the dissolution of a sparingly soluble salt.

• Example Equation (Ksp): $K_{sp} = [A^+]^m[B^-]^n$

Module IV: Chemical Thermodynamics and Electrochemistry

This module focuses on the principles of chemical thermodynamics and the fundamentals of electrochemistry, including energy changes, spontaneity, and redox reactions.

• Chemical Thermodynamics (Chapter 19): Study of entropy, free energy, and the criteria for spontaneity of chemical processes.

• Electrochemistry (Chapter 20): Examination of oxidation-reduction reactions, electrochemical cells, and standard electrode potentials.

• Key Concepts:

  • Gibbs Free Energy (G): Determines the spontaneity of a process.

  • Standard Cell Potential (E0): The voltage of an electrochemical cell under standard conditions.

• Example Equation (Gibbs Free Energy): $\Delta G = \Delta H - T\Delta S$

• Example Equation (Cell Potential): $\Delta G^0 = -nFE^0$

Summary Table: CHEM 2080 Modules and Topics

Module	Main Topics	Chapters/Sections
I	Thermochemistry, Chemical Kinetics	5, 14.1–14.4
II	Chemical Kinetics (Mechanisms), Chemical Equilibrium, Acid-Base Equilibria, Buffers & Titrations	14.5–14.6, 15, 16, 17.1–17.3
III	Liquids & Intermolecular Forces, Properties of Solutions, Solubility Equilibria	11.1–11.2, 11.4–11.6, 13.1–13.5, 17.4–17.6
IV	Chemical Thermodynamics, Electrochemistry	19, 20

Additional info: This syllabus provides a structured overview of the main topics in a second-semester general chemistry course, aligning with standard curriculum and textbook chapters. Students are encouraged to consult the assigned textbook readings for detailed explanations, worked examples, and practice problems.