General Chemistry

Affectionately known as “Gen Chem,” first-year General Chemistry is for undergraduates who are just beginning their college-level studies in chemistry. It builds on high school fundamentals while introducing more rigorous problem-solving skills, deeper conceptual understanding, and a greater emphasis on scientific reasoning.

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Not all GenChem courses are created equal.

Check out the resources here to help with your Gen Chem needs. Some professors are different from others so be aware of gaps in content, difficulty, and focus.

Beyond the resources suggested, consider Async OnDemand help, virtual tutoring, and our specialized groups and courses for General Chemistry.

Semester 1
General Chemistry I

Atoms, Molecules, and Ions

Atomic theory and structure; Periodic table organization and atomic properties; Chemical formulas, molecular compounds, ionic compounds; Nomenclature basics

Stoichiometry

The mole concept, Avogadro’s number; Balancing chemical equations; Mass relationships in reactions, limiting reagents, percent yield

Chemical Reactions

Types of reactions (e.g., precipitation, acid-base, redox); Writing and interpreting balanced equations; Net ionic equations

Thermochemistry

Energy, heat, and work; Endothermic vs. exothermic processes; Enthalpy (ΔH), calorimetry, and Hess’s law

Electronic Structure of Atoms

Electromagnetic radiation and quantization of energy; Bohr model, quantum mechanical model of the atom; Electron configurations, orbitals, and quantum numbers

Periodic Properties of the Elements

Trends in atomic radius, ionization energy, electronegativity; Electron affinity; Relationship of periodic trends to electronic structure

Basic Chemical Bonding

Ionic and covalent bonding; Lewis structures and resonance; Bond polarity and electronegativity

Molecular Geometry & Bonding Theories

VSEPR theory (molecular shapes); Valence bond theory (hybridization) basics; Introduction to molecular orbital theory (optional or brief)

States of Matter & Intermolecular Forces*

Properties of gases, liquids, and solids; Gas laws (if time allows, or covered early in General Chemistry II); Intermolecular forces (e.g., dipole-dipole, hydrogen bonding, dispersion)

Semester 2
General Chemistry II

Chemical Kinetics

Reaction rates and rate laws; Determining reaction order; Mechanisms and the Arrhenius equation

Chemical Equilibrium

Equilibrium constants (Kc, Kp); Le Châtelier’s principle

Acid-Base Chemistry

Definitions (Arrhenius, Brønsted-Lowry, Lewis); Acid-base equilibria, Ka, Kb; pH calculations, buffers, titrations

Aqueous Ionic Equilibria

Common-ion effect; Buffer solutions; Solubility product (Ksp); Complex ion formation and precipitation reactions

Thermodynamics

First, Second, and Third Laws of Thermodynamics; Enthalpy (ΔH), Entropy (ΔS), and Gibbs free energy (ΔG); Spontaneity and equilibrium

Electrochemistry

Redox reactions and balancing in acidic/basic solutions; Galvanic (voltaic) cells and cell potential; Standard reduction potentials; Batteries, fuel cells, electrolysis, and corrosion

Coordination Chemistry (optional or introductory)

Complex ions and coordination compounds; Naming and structure of coordination complexes; Crystal field theory (basic principles)

Nuclear Chemistry (optional or introductory)

Types of radioactivity; Nuclear reactions and decay processes; Applications in medicine and energy

Special Topics or Extensions (varies by course)

Basic organic chemistry concepts or functional groups; Biochemical relevance (e.g., metabolism, enzymes); Advanced applications of thermodynamics and kinetics