Myanmar Matriculation Chemistry study plan

Define and classify the core physical quantities of chemistry: atom, molecule, ion, mole, molar mass, relative atomic mass, and relative molecular mass, writing a one-line definition for each from memory.

Compute moles, mass, and number of particles interconversions for at least 20 mixed problems, showing unit cancellation at every step.

Determine empirical and molecular formulae from percentage composition and from combustion-style mass data, working 8 problems end to end.

State and apply the gas laws (Boyle, Charles, combined, ideal gas, and molar volume at STP) to calculate unknown P, V, T, or n in at least 12 problems.

Set up and solve limiting-reagent and percentage-yield problems, identifying the limiting reagent before any calculation.

Write balanced equations, including ionic and net ionic forms, for precipitation, neutralisation, and redox reactions in acidic and basic media.

Assign oxidation numbers and identify oxidised/reduced species, oxidising/reducing agents, and electron transfer counts in 15 redox equations.

Apply the concept of concentration in mol/dm3, dilution, and titration stoichiometry to calculate unknown concentrations from titration data.

Explain the behaviour of strong and weak electrolytes, and predict conductivity and pH trends qualitatively.

Distinguish Arrhenius, Bronsted-Lowry, and Lewis acid-base definitions with one example each.

Describe the structure of the atom, including subatomic particles, isotopes, and the meaning of atomic number and mass number, and calculate relative atomic mass from isotopic abundances.

Write electron configurations using the Aufbau principle, Hund's rule, and the Pauli exclusion principle for elements up to atomic number 36.

Relate position in the periodic table (group, period, block) to electron configuration and predict trends in atomic radius, ionisation energy, and electronegativity.

Explain the formation of ionic, covalent, coordinate, and metallic bonds in terms of electron transfer and sharing, and draw dot-and-cross diagrams for at least 10 species.

Predict and explain the shapes of simple molecules and ions using VSEPR theory, and relate polarity to molecular shape.

Explain the kinetic particle model and use it to account for the properties of solids, liquids, and gases, including diffusion and compressibility.

Describe the types of intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding) and rank substances by boiling point with justification.

Describe the structure and properties of giant ionic, giant covalent, simple molecular, and metallic lattices, and predict melting point, solubility, and conductivity for each.

Interpret heating and cooling curves and explain latent heat of fusion and vaporisation in particle terms.

Solve enthalpy-change problems using q = mcΔT and Hess's law cycles, including bond-energy calculations.

Apply Le Chatelier's principle to predict the direction of shift when concentration, pressure, or temperature changes for at least 8 equilibrium systems.

Write and use equilibrium constant expressions (Kc) and calculate unknown equilibrium concentrations from initial conditions.

Define rate of reaction and explain how concentration, temperature, pressure, surface area, and catalysts affect rate, using collision theory.

Interpret simple energy profile diagrams, identifying activation energy, enthalpy change, and the effect of a catalyst.

Distinguish reversible and irreversible reactions and explain the dynamic nature of equilibrium.

Name and draw structural formulae for alkanes, alkenes, alkynes, and simple functional groups (alcohol, aldehyde, ketone, carboxylic acid, ester, amine, halogenoalkane) using IUPAC rules.

Identify and describe isomerism, including chain, position, and functional group isomerism, for at least 8 molecular formulae.

Predict and write equations for characteristic reactions: addition, substitution, elimination, oxidation, esterification, and polymerisation.

Distinguish tests for alkenes, alcohols, aldehydes, ketones, carboxylic acids, and starch, and state the observation for each.

Relate the properties and uses of selected organic compounds (ethanol, ethanoic acid, esters, polymers) to their structure.

Describe the extraction and properties of selected metals (e.g. iron, aluminium, copper) and relate extraction method to reactivity.

Write and explain electrolysis reactions at anode and cathode for molten and aqueous electrolytes, and calculate mass or volume deposited using Faraday's laws.

Explain corrosion and its prevention, and describe the composition and purpose of common alloys.

Classify oxides as acidic, basic, amphoteric, or neutral with examples, and describe the chemistry of selected non-metals (e.g. nitrogen, sulphur, chlorine) and their key compounds.

Describe environmental chemistry topics (air and water pollution, greenhouse gases, treatment of water) and state one remedy for each pollutant.

Consolidate all topics by re-attempting every previously missed question and recording the error type (concept, calculation, or reading).

Complete at least two full-length timed practice papers under exam conditions and mark them strictly.

Build a one-page formula and definition sheet covering all calculation types and key terms, then reproduce it from memory.

Review weak areas identified in practice papers and write short corrective notes for each.

Plan exam-day strategy: time allocation per section, order of attempt, and checking routine.