LC Chemistry study plan

Draw electron configurations (full and shorthand) and orbital box diagrams for elements 1-36 and deduce period, group, and block from any configuration

Explain and rank periodic trends in atomic radius, first ionisation energy, electron affinity, and electronegativity across a period and down a group using effective nuclear charge and shielding

Write and balance full, complete ionic, and net ionic equations for precipitation, acid-base, and gas-forming reactions

Calculate empirical and molecular formulas from percentage composition and from combustion data, and calculate percentage yield and atom economy

Assign oxidation numbers and identify the species oxidised and reduced in redox equations, then balance them by half-equations in acidic and basic media

Construct Lewis structures for molecules and polyatomic ions including resonance forms, and assign formal charges to choose the best structure

Predict molecular geometry and bond angles with VSEPR theory for 2-6 electron domains, distinguishing lone-pair effects

Classify bonding as ionic, polar covalent, or nonpolar covalent from electronegativity differences and predict intermolecular forces (dispersion, dipole-dipole, hydrogen bonding) for a given substance

Relate intermolecular forces to observed melting point, boiling point, and solubility trends

Solve limiting-reactant problems including mass-mass, mass-volume at STP, and solution-volume cases, and determine excess reagent remaining

Perform multi-step stoichiometry calculations involving molarity, dilution, and solution preparation

Calculate titration results from burette readings, including averaging concordant titres and computing concentration or percentage purity of an unknown

Distinguish strong and weak acids and bases and calculate pH, pOH, and species concentrations for strong acid, strong base, weak acid, and buffer solutions

Select an appropriate indicator for a given titration from endpoint pH reasoning and sketch the expected titration curve shape

Apply the ideal gas law and combined gas law to calculate pressure, volume, temperature, moles, molar mass, and gas density, including stoichiometry with gaseous reactants

Explain and calculate colligative properties (boiling-point elevation, freezing-point depression, osmotic pressure) using molality and the van't Hoff factor

Express solution concentration in molarity, molality, mole fraction, and mass percent, and interconvert between them

Calculate enthalpy changes from calorimetry data (q = mcΔT) and from Hess's law and standard enthalpies of formation

Interpret and draw potential energy profiles, and determine rate law, order, rate constant, and activation energy from initial-rate and concentration-time data

Write equilibrium constant expressions for Kc and Kp and calculate equilibrium concentrations from initial conditions using an ICE table

Apply Le Chatelier's principle to predict the direction of shift when concentration, pressure/volume, or temperature changes for a specified reaction

Calculate Ka, Kb, pH, and percent ionisation for weak acid and weak base equilibria, including polyprotic simplifications

Determine solubility product expressions and calculate molar solubility with and without a common ion

Explain how a buffer resists pH change and calculate the pH of a buffer before and after adding strong acid or base

Identify and name alkanes, alkenes, alkynes, aromatics, alcohols, aldehydes, ketones, carboxylic acids, esters, and amines using IUPAC rules, including isomers and stereocentres

Predict the products of addition, substitution, elimination, oxidation, esterification, and hydrolysis reactions for specified reactants and conditions

Distinguish structural isomers, geometric (cis-trans) isomers, and optical isomers for a given molecular formula and explain the physical-property consequences

Draw and interpret skeletal and condensed structural formulas and convert between them

Relate functional groups to characteristic reaction types and to intermolecular forces and solubility behaviour

Assign oxidation states and balance redox equations in acidic and basic solution by the half-reaction method without prompts

Construct and label galvanic cells, write anode and cathode half-reactions, and calculate cell potential from standard reduction potentials

Determine spontaneity from E°cell and predict the effect of concentration changes on cell potential using the Nernst equation

Describe the reactions at anode and cathode during electrolysis of molten and aqueous salts and apply Faraday's law to calculate mass or volume deposited

Select appropriate separation and purification techniques (filtration, recrystallisation, distillation, chromatography, solvent extraction) and identify standard apparatus and safety procedures for a described experimental aim

Evaluate experimental design for sources of error and suggest improvements to accuracy and precision

Complete two full-length timed mock papers under exam conditions and record the score by domain

Re-derive every formula on a personal equation sheet from memory and correct any item recalled incorrectly

Re-work every missed question from the mocks and write the underlying concept and the error type (misread, calculation, concept gap) for each

Target the two weakest domains from the mock analysis with 15 focused practice items each

State the final exam-day strategy: question order, time allocation per section, and the calculation-check routine