Key Concepts

Grade 11 (Physics 11)

• Introduction to Chemistry

  • Scientific Method: Importance of observation, hypothesis, experimentation, and theory in chemistry.

  • Measurement and Uncertainty: Significant figures, precision, accuracy, and scientific notation.

• Atomic Theory

  • Structure of the Atom: Protons, neutrons, electrons, and isotopes.

  • Periodic Table: Organization of elements, periodic trends (atomic radius, ionization energy, electronegativity).

• Chemical Bonding

  • Ionic and Covalent Bonds: Formation of compounds, electron sharing, and transfer.

  • Molecular Geometry: VSEPR theory, shapes of molecules, and bond polarity.

  • Intermolecular Forces: Dipole-dipole interactions, hydrogen bonding, London dispersion forces.

• Chemical Reactions

  • Types of Reactions: Synthesis, decomposition, single replacement, double replacement, and combustion.

  • Balancing Chemical Equations: Law of conservation of mass, stoichiometry basics.

  • Energy Changes in Reactions: Exothermic and endothermic reactions, enthalpy changes.

• Solutions and Solubility

  • Properties of Solutions: Solute, solvent, concentration units (molarity), dilution.

  • Solubility Rules: Factors affecting solubility, saturated and unsaturated solutions.

  • Acids and Bases: Introduction to pH, strong and weak acids/bases, neutralization reactions.

• Mole Concept and Stoichiometry

  • The Mole: Avogadro's number, molar mass, conversions between moles, mass, and number of particles.

  • Stoichiometric Calculations: Mole ratios, limiting reactants, percent yield.

Grade 12 (Chemistry 12)

• Reaction Kinetics

  • Rate of Reaction: Factors affecting reaction rate (temperature, concentration, surface area, catalysts).

  • Rate Laws: Determination of reaction order, rate constant, and reaction mechanism.

  • Collision Theory: Activation energy, orientation of reactants.

• Equilibrium

  • Dynamic Equilibrium: Reversible reactions, equilibrium constant (Kc), Le Chatelier’s Principle.

  • Equilibrium Calculations: ICE tables, calculating concentrations of reactants/products at equilibrium.

  • Applications of Equilibrium: Solubility product (Ksp), common ion effect.

• Acid-Base Chemistry

  • Brønsted-Lowry Theory: Acids as proton donors, bases as proton acceptors.

  • pH and pOH Calculations: Calculating pH, pOH, and the concentration of H+ and OH- ions.

  • Titration and Buffers: Acid-base titrations, titration curves, buffer solutions and their capacity.

• Solubility Equilibria

  • Solubility Product Constant (Ksp): Calculation of solubility, predicting precipitation reactions.

  • Complex Ions and Solubility: Formation of complex ions and their effect on solubility.

• Electrochemistry

  • Redox Reactions: Oxidation and reduction, assigning oxidation states, balancing redox equations.

  • Electrochemical Cells: Galvanic (voltaic) cells, standard reduction potentials, cell notation.

  • Electrolysis: Electrolytic cells, Faraday’s laws of electrolysis, applications in industry.

• Thermochemistry

  • Enthalpy Changes: Hess's law, standard enthalpies of formation, enthalpy changes of reactions.

  • Entropy and Free Energy: Concepts of entropy (ΔS), Gibbs free energy (ΔG), spontaneity of reactions.