High School Chemistry
You either love it or hate it — no in between. This page covers the topics and content that is usually covered in high school chemistry courses. There are also specialized pages for AP Chemistry and IB Chemistry.
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We are in the lab at work getting resources to the popular topics of General Chemistry I and II for you. See what we’re doing below.
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