Chemistry Course

Lesson 1 • SI Units and Scientific Measurement

Covers SI base units, derived units, and measurement uncertainty. Accurate measurement skills underpin all laboratory and calculation work.

Lesson 2 • Atomic Theory and Subatomic Particles

Traces the development of atomic models and identifies protons, neutrons, and electrons. Connects atomic structure to elemental identity and isotope variation.

Lesson 3 • The Mole Concept and Molar Mass

Introduces Avogadro's number and molar mass calculations. Bridges atomic-scale quantities to laboratory-scale measurements.

Lesson 4 • Nature of Matter and Its Classification

Defines pure substances, mixtures, elements, and compounds. Provides the vocabulary framework underlying every chemical concept in the course.

Lesson 1 • Covalent Bonding and Lewis Structures

Covers electron sharing, bond order, and Lewis dot diagrams. Students draw accurate structures for simple and polyatomic molecules.

Lesson 2 • Ionic Bonding and Lattice Structures

Describes electron transfer, ion formation, and crystal lattice energy. Connects ionic bond strength to physical properties like melting point.

Lesson 3 • Metallic Bonding and Solid-State Properties

Introduces the electron-sea model and band theory basics. Connects metallic bonding to conductivity, malleability, and alloy behaviour.

Lesson 4 • VSEPR Theory and Molecular Geometry

Applies VSEPR rules to predict three-dimensional molecular shapes. Geometry directly influences reactivity and intermolecular interactions.

Lesson 1 • Limiting Reagents and Percent Yield

Identifies the limiting reagent and calculates theoretical and percent yield. These concepts are critical for evaluating reaction efficiency in practice.

Lesson 2 • Mole Ratios and Stoichiometric Calculations

Uses balanced equations to convert between moles of reactants and products. Stoichiometry is the quantitative core of practical chemistry.

Lesson 3 • Types of Chemical Reactions

Classifies synthesis, decomposition, single/double displacement, and combustion reactions. Pattern recognition speeds equation prediction and balancing.

Lesson 4 • Writing and Balancing Chemical Equations

Teaches equation notation, state symbols, and balancing by inspection. Balanced equations are the foundation for all stoichiometric calculations.

Lesson 1 • Entropy, Gibbs Free Energy, and Spontaneity

Introduces entropy and Gibbs free energy to predict reaction spontaneity. Connects thermodynamic favour ability to real chemical decision-making.

Lesson 2 • Heat, Temperature, and Specific Heat

Distinguishes heat from temperature and applies the specific heat equation. Provides the thermal measurement basis for calorimetry experiments.

Lesson 3 • Hess's Law and Enthalpy Calculations

Applies Hess's law to calculate enthalpy changes for reactions not easily measured. Reinforces additive properties of state functions.

Lesson 4 • Calorimetry and Enthalpy Measurement

Covers coffee-cup and bomb calorimetry to measure reaction enthalpy. Experimental design and data interpretation are emphasised.

Lesson 1 • Kinetic Molecular Theory of Gases

Presents the postulates of kinetic molecular theory and their macroscopic consequences. Provides the conceptual basis for all gas law relationships.

Lesson 2 • Phase Transitions and Phase Diagrams

Describes melting, boiling, sublimation, and their energy requirements. Phase diagrams are used to predict stable phases at given conditions.

Lesson 3 • Real Gases and Deviations from Ideal Behaviour

Explains why real gases deviate from ideal behaviour and introduces the van der Waals equation. Builds critical evaluation of model limitations.

Lesson 4 • Ideal Gas Laws and Calculations

Derives and applies Boyle's, Charles's, Gay-Lussac's, and combined gas laws. Students solve quantitative problems involving pressure, volume, and temperature.

Lesson 1 • Buffers, Solubility, and Complex Equilibria

Explains buffer action, Henderson-Hasselbalch equation, and Ksp. Integrates multiple equilibrium concepts for real solution analysis.

Lesson 2 • Dynamic Equilibrium and Equilibrium Constants

Defines dynamic equilibrium and derives Kc and Kp expressions. Students interpret K values to predict reaction extent.

Lesson 3 • ICE Tables and Equilibrium Calculations

Uses ICE tables to calculate equilibrium concentrations from initial conditions. Develops systematic problem-solving for equilibrium systems.

Lesson 4 • Acids, Bases, and pH Calculations

Covers Brønsted-Lowry and Lewis acid-base definitions, Ka, Kb, and pH. Students calculate pH for strong and weak acid-base systems.

Lesson 1 • Electrolysis and Industrial Applications

Explains electrolytic cells, Faraday's laws of electrolysis, and industrial processes. Students calculate mass deposited and energy consumed.

Lesson 2 • Thermodynamics of Electrochemical Cells

Links cell potential to Gibbs free energy and equilibrium constant. Integrates thermodynamic and electrochemical frameworks.

Lesson 3 • Galvanic Cells and Standard Cell Potentials

Describes galvanic cell construction, salt bridges, and standard reduction potentials. Students calculate standard cell potential from tabulated values.

Lesson 4 • Oxidation States and Redox Balancing

Assigns oxidation states and balances redox equations using half-reaction method. Accurate balancing is prerequisite for all electrochemical calculations.

Lesson 1 • Arrhenius Equation and Activation Energy

Uses the Arrhenius equation to relate temperature to rate constant. Quantifies the energy barrier that controls reaction speed.

Lesson 2 • Reaction Rate Measurement and Expression

Defines reaction rate in terms of concentration change over time. Establishes the experimental basis for all kinetic analysis.

Lesson 3 • Reaction Mechanisms and Elementary Steps

Breaks overall reactions into elementary steps and identifies the rate-determining step. Connects molecular-level events to macroscopic rate laws.

Lesson 4 • Rate Laws and Reaction Orders

Derives rate laws from experimental data and classifies reaction orders. Students distinguish between zero, first, and second-order kinetics.