Thermochemical Changes

Enthalpy (ΔH); Energy Diagrams; Hess’s Law; Calorimetry; Molar Enthalpies of Formation and Reaction.

Energy Tracking: We clarify the difference between system and surroundings, ensuring students can correctly calculate and interpret ΔH for reactions and confidently apply Hess’s Law to complex, multi-step reactions.

Electrochemical Changes

Oxidation/Reduction (Redox); Balancing Redox Equations; Voltaic (Galvanic) and Electrolytic Cells; Standard Reduction Potential (Eo).

Redox and Spontaneity: This unit requires new concepts. We demystify Redox using mnemonics (like LEO GER) and teach the systematic process for balancing complex half-reactions and using the Standard Reduction Potential Table to predict the spontaneity of a reaction.

Chemical Changes of Organic Compounds

Naming (Nomenclature) and Drawing (Structural Isomers) of Hydrocarbons; Functional Groups (Alcohols, Carboxylic Acids, Esters); Organic Reactions (Substitution, Addition, Elimination).

Visualizing and Naming: We use systematic approaches to IUPAC nomenclature and model-building exercises to help students visualize and correctly name complex organic molecules and predict the products of their reactions.

Chemical Equilibrium (Acid-Base Focus)

Le Chatelier’s Principle; Equilibrium Law Expression (Keq​); Acid-Base Theory (Brønsted-Lowry); pH and pOH; Acid/Base Titration; Buffers.

Quantitative Equilibrium: This unit is a mathematical and conceptual hurdle. We emphasize solving for Keq​ and the concentrations of ions in solution using the ICE Table method, a crucial skill for mastering pH and buffer calculations for the Diploma Exam.