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Spring 2027Finish the second half of General Chemistry with the topics that decide the course.
General Chemistry II focuses on chemical change under real constraints: reaction rates, equilibrium, acid-base systems, solubility, thermodynamics, and electrochemistry. Students practice the calculations, graphs, models, and lab interpretations that tie these units together.
Use this path after General Chemistry I when students need a coherent route through kinetics, equilibrium, thermodynamics, and electrochemistry instead of a pile of disconnected formulas.
Built from a second-semester general chemistry progression: kinetics, equilibrium, acids and bases, solubility, thermodynamics, and electrochemistry.
Course map: ChemistryGraph sequence for the second semester of college general chemistry.
Coverage model: Topics follow a standard General Chemistry II progression for algebra-based quantitative chemistry.
General Chemistry II Learning Outcomes
Kinetics and Reaction Mechanisms
Use concentration-time data, initial rates, integrated rate laws, and half-lives to describe reaction speed.
Connect mechanisms, rate-determining steps, activation energy, and catalysts to observed rates.
Chemical Equilibrium
Use equilibrium constants, reaction quotients, ICE tables, and approximation checks to solve reversible-reaction problems.
Predict changes with Le Chatelier's principle while preserving the quantitative equilibrium model.
Acids, Bases, Buffers, and Titrations
Analyze strong and weak acid-base systems using pH, pOH, Ka, Kb, and neutralization stoichiometry.
Use buffers, Henderson-Hasselbalch reasoning, titration curves, and indicators to connect calculations to experiments.
Solubility and Complex-Ion Equilibria
Use Ksp, molar solubility, common-ion effects, and selective precipitation to analyze ionic solutions.
Model complex-ion formation and competing equilibria in multi-step solution chemistry.
Thermodynamics
Use entropy, enthalpy, Gibbs free energy, and temperature dependence to evaluate spontaneity.
Connect free energy and equilibrium so thermodynamic claims match chemical-system behavior.
Electrochemistry
Analyze oxidation-reduction reactions, galvanic cells, electrolytic cells, and cell notation.
Use standard reduction potentials, cell potential, free energy, and the Nernst equation to connect chemistry to electrical work.
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