European Baccalaureate Chemistry study plan

Draw electron configurations and orbital box diagrams for atoms and ions up to Z=36, and justify the Cr and Cu anomalies from exchange energy and half-filled stability.

Predict and explain periodic trends (atomic and ionic radius, ionisation energy, electron affinity, electronegativity) across a period and down a group, including the Al/Ga and Be/B irregularities.

Assign VSEPR shapes, bond angles and hybridisation for molecules with 2 to 6 electron domains, including lone-pair distortions and multiple bonds.

Construct molecular orbital diagrams for O2, N2, F2 and NO and use bond order to explain their magnetism and bond length.

Convert confidently between mass, moles, molarity, gas volume and particle number in multi-step problems, keeping units explicit throughout.

Apply the ideal gas law and its variants to mixtures, including partial pressures and mole fractions, and identify when real-gas deviation becomes significant.

Perform limiting-reagent and percentage-yield calculations, and determine empirical and molecular formulae from combustion data.

Solve dilution, mixing and titration stoichiometry problems where concentrations change on combination.

Describe intermolecular forces and use them to rank boiling points, vapour pressures and solubility for given substances.

Apply Hess's law and standard enthalpy of formation to calculate reaction enthalpies, including formation of the target equation from given data.

Calculate enthalpy changes from bond dissociation energies and explain why the two routes differ for liquids and gases.

Use calorimetry data (q = mcΔT) to determine enthalpy changes and identify the main sources of experimental error.

Interpret Born-Haber cycles for ionic compounds, calculating lattice enthalpy and explaining the effect of ion size and charge.

Use mean bond enthalpy and entropy terms qualitatively to judge whether a reaction is enthalpy- or entropy-driven.

Derive rate equations from initial-rate data and determine reaction order with respect to each reactant, including zero order.

Explain collision theory and the effect of temperature, concentration, pressure, surface area and catalysts on rate, using Maxwell-Boltzmann distribution curves.

Apply Le Chatelier's principle and the equilibrium constant Kc or Kp to predict and calculate the effect of changing conditions on equilibrium position and yield.

Calculate pH for strong and weak acids and bases, including the use of Ka, pKa and the approximation for weak acids.

Design and interpret a buffer system, calculating pH before and after adding strong acid or base, and explain buffer capacity.

Assign oxidation states in complex ions and compounds and identify oxidising and reducing agents in given equations.

Balance redox equations in acidic and basic media using half-equations, including disproportionation cases.

Construct and use a standard electrode potential table to predict the direction of a redox reaction and calculate cell EMF.

Explain the operation of a galvanic cell and an electrolytic cell, including electrode polarity, electron flow and ion migration.

Calculate the mass or volume of product from electrolysis using Faraday's laws and charge (Q = It).

Name and draw structural, geometric and optical isomers for given molecular formulae, identifying chiral centres and cis/trans arrangements.

Classify organic reactions as substitution, addition, elimination, oxidation or condensation, and predict the major product for each.

Write mechanisms with curly arrows for nucleophilic substitution (SN1 and SN2), electrophilic addition and elimination, explaining the stereochemical outcome.

Explain Markovnikov's rule and the stability of carbocation intermediates, and apply it to predict products.

Describe the characteristic reactions of alkanes, alkenes, alcohols, halogenoalkanes, aldehydes, ketones, carboxylic acids and esters, including test-tube observations.

Interpret infrared spectra by matching absorption bands to functional groups and explain why the fingerprint region is used for identification.

Interpret simple 1H NMR spectra, using chemical shift, integration and splitting to deduce structure, and explain the role of TMS and D2O exchange.

Explain the principles of mass spectrometry, including the molecular ion and fragmentation, and use m/z values to propose structural fragments.

Describe and compare separation and identification techniques (chromatography, flame tests, gravimetric and volumetric analysis) and select the appropriate one for a scenario.

Evaluate a real industrial or environmental case (for example the Haber process, a fuel cell or a greenhouse-gas measurement) using equilibrium, energetics and analytical evidence.

Complete three full-length timed mock papers under exam conditions and record the score for each domain.

Re-teach the two weakest domains from the mock analysis, writing a one-page correction sheet for each.

Rehearse the extended-response structure: define, apply, calculate, conclude, with units and significant figures checked.

Build a personal error log of recurring mistakes (unit slips, sign errors, mechanism arrows) and revise it before the exam.