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 High School Chemistry for you. See what we’re doing below.

Semester 1
High School Chemistry

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
High School Chemistry

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

Nuclear Chemistry (optional or introductory)

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