High School Chemistry Course

Lesson 1 • Scientific Notation and Dimensional Analysis

Introduces exponential notation and unit-conversion factor-label method. These tools are essential for solving stoichiometry and gas-law problems.

Lesson 2 • Properties and Classification of Matter

Distinguishes physical vs. chemical properties and pure substances vs. mixtures. Anchors all future content in precise material classification.

Lesson 3 • Laboratory Safety and Procedures

Establishes safe lab behaviour, equipment use, and hazard communication. Safe practice is required before any hands-on experimentation begins.

Lesson 4 • Scientific Measurement and SI Units

Covers SI base units, prefixes, and measurement tools. Accurate measurement underpins every quantitative chemistry task.

Lesson 1 • Historical Models of the Atom

Traces atomic theory from Dalton through Bohr to the quantum model. Understanding this history contextualises modern atomic structure.

Lesson 2 • Periodic Trends

Analyses atomic radius, ionisation energy, and electronegativity trends. These trends explain reactivity patterns used in bonding and reactions.

Lesson 3 • Organisation of the Periodic Table

Describes periods, groups, and element families. Table organisation reflects electron configuration and predicts chemical properties.

Lesson 4 • Electron Configuration and Energy Levels

Explains orbital notation, subshells, and the Aufbau principle. Electron configuration determines chemical reactivity and bonding behaviour.

Lesson 1 • VSEPR Theory and Molecular Geometry

Applies VSEPR rules to predict 3-D molecular shapes. Geometry directly influences polarity and physical properties of molecules.

Lesson 2 • Metallic Bonding and Properties

Describes the electron-sea model and resulting metallic properties. Connects bonding type to conductivity, malleability, and lustre.

Lesson 3 • Ionic Bonding and Ionic Compounds

Covers electron transfer, lattice formation, and ionic compound properties. Ionic bonding arises from electronegativity differences established in Chapter 2.

Lesson 4 • Polarity and Intermolecular Forces

Distinguishes polar and nonpolar molecules and the forces between them. Intermolecular forces explain boiling points, solubility, and physical states.

Lesson 1 • Naming Binary Covalent Compounds

Covers Greek prefix system for naming molecular compounds. Distinguishes covalent naming from ionic naming to avoid confusion.

Lesson 2 • Acids and Bases Nomenclature

Names binary acids and oxyacids using systematic rules. Acid naming prepares students for acid-base reaction equations.

Lesson 3 • Naming Binary Ionic Compounds

Applies naming rules for monatomic ions and binary salts. Correct nomenclature is required for all subsequent reaction and stoichiometry work.

Lesson 1 • Writing and Balancing Chemical Equations

Introduces equation notation, state symbols, and balancing by inspection. Balanced equations are the starting point for all stoichiometric calculations.

Lesson 2 • Types of Chemical Reactions

Classifies synthesis, decomposition, single-replacement, double-replacement, and combustion reactions. Pattern recognition speeds equation writing and prediction.

Lesson 3 • Stoichiometric Calculations

Applies mole ratios from balanced equations to solve mass-mass problems. Stoichiometry is the quantitative core of all chemical reaction analysis.

Lesson 4 • The Mole Concept and Molar Mass

Defines Avogadro's number, the mole, and molar mass calculations. The mole bridges atomic-scale counts and laboratory-scale masses.

Lesson 1 • Kinetic Molecular Theory

Describes particle motion, energy, and assumptions of the ideal gas model. KMT provides the molecular explanation for all gas-law relationships.

Lesson 2 • Gas Laws: Boyle, Charles, and Gay-Lussac

Derives and applies the three individual gas laws relating P, V, and T. Each law is a special case of the combined gas law introduced next.

Lesson 3 • Dalton's Law and Gas Mixtures

Applies Dalton's law of partial pressures to gas mixtures and collected gases. Partial pressure calculations are used in lab gas-collection procedures.

Lesson 4 • Combined and Ideal Gas Laws

Unifies individual gas laws into the combined and ideal gas equations. Students solve problems involving all four gas variables simultaneously.

Lesson 1 • Acid-Base Theories

Compares Arrhenius, Brønsted-Lowry, and Lewis acid-base definitions. Each theory expands the scope of acid-base chemistry progressively.

Lesson 2 • pH Scale and Calculations

Introduces the pH scale, Kw, and logarithmic pH calculations. pH quantifies acidity and is central to neutralisation and buffer problems.

Lesson 3 • Solution Formation and Solubility

Explains the dissolving process, solubility rules, and factors affecting solubility. Solubility concepts underpin concentration and precipitation reactions.

Lesson 4 • Neutralisation and Titration

Applies stoichiometry to acid-base neutralisation and titration calculations. Students determine unknown concentrations using titration data.

Lesson 1 • Hess's Law

Applies Hess's law to calculate reaction enthalpy from multiple steps. This extends enthalpy calculations to reactions not easily measured directly.

Lesson 2 • Energy, Heat, and Calorimetry

Defines enthalpy, heat capacity, and calorimetry calculations. Calorimetry provides experimental data for all thermochemical calculations.

Lesson 3 • Enthalpy and Thermochemical Equations

Introduces standard enthalpy of formation and reaction enthalpy calculations. Thermochemical equations combine stoichiometry with energy data.

Lesson 4 • Chemical Equilibrium and Keq

Defines dynamic equilibrium and the equilibrium constant expression. Keq values indicate whether products or reactants are favoured at equilibrium.