Catalonia PAU Chemistry study plan

Identify and name the main functional groups (alcohol, ether, aldehyde, ketone, carboxylic acid, ester, amine, amide, aromatic) in structural formulas and apply IUPAC nomenclature rules to name and draw alkanes, alkenes, alkynes and their substituted derivatives up to C8.

Classify and construct structural, geometric (cis/trans, E/Z) and optical (chirality, enantiomers) isomers for a given molecular formula, and determine the stereocentres in a molecule.

Distinguish substitution (SN1/SN2), elimination, addition and condensation reaction types, and predict the major organic product for a specified reagent and substrate, justifying the regiochemistry (Markovnikov, anti-Markovnikov) and the mechanism involved.

Recognise the repeating unit, monomer and type of polymerisation (addition vs condensation) for common polymers, and relate the structure of carbohydrates, amino acids/proteins and fats to their functional groups.

Apply the concepts of hybridization (sp, sp2, sp3), sigma/pi bonding and delocalisation to explain the geometry and reactivity of organic molecules, including resonance in benzene and carboxylate ions.

Draw correct Lewis structures (including formal charges and resonance forms) and predict molecular geometry and bond angles using VSEPR for molecules with and without lone pairs (e.g. NH3, H2O, SF6, CO2).

Rank substances by polarity from electronegativity and geometry, and predict the dominant intermolecular force (London, dipole–dipole, hydrogen bonding) in each case.

Relate intermolecular forces and bonding type (ionic, covalent molecular, covalent network, metallic) to melting point, boiling point, solubility and electrical conductivity, and select the correct explanation for a given pair of substances.

Write full and condensed electron configurations (including exceptions such as Cr and Cu) and assign the four quantum numbers (n, l, ml, ms) to the last electron of a given element or ion.

Apply Aufbau, Pauli and Hund rules to justify configurations, and predict and explain periodic trends (atomic and ionic radius, ionisation energy, electron affinity, electronegativity, metallic character) across a period and down a group.

Calculate average atomic mass from isotopic abundances and interpret a simple mass spectrum; convert between mass, moles, number of particles and molar volume.

Solve ideal gas law and gas-mixture problems (including partial pressures and Graham's law), and interpret a phase diagram to identify normal boiling point, triple point and the effect of pressure on melting.

Write equilibrium constant expressions for homogeneous and heterogeneous equilibria, convert between Kc and Kp, and build an ICE table to calculate equilibrium concentrations, degrees of dissociation or K from initial data.

Apply Le Chatelier's principle to predict the direction of shift for changes in concentration, pressure/volume and temperature, and explain the effect on K and on yield.

Calculate the solubility product Ksp, molar solubility and the effect of a common ion, and decide whether a precipitate forms from given ion concentrations.

Calculate pH for strong and weak acids and bases using Ka/Kb, apply the Henderson–Hasselbalch equation to buffer design, and predict whether a salt solution is acidic, basic or neutral from hydrolysis of its ions.

Interpret titration curves for strong–strong, weak–strong and polyprotic systems, and calculate the pH at the initial point, half-equivalence point and equivalence point.

Select an appropriate acid–base indicator from its pKa range and justify the choice for a given titration.

Solve multi-step equilibrium problems that combine Kc/Kp with gas stoichiometry and with acid–base equilibria, keeping significant figures and units consistent.

Diagnose and correct common errors in equilibrium and pH calculations (ignoring x, wrong direction of shift, mixing Ka and Kb, forgetting dilution).

Assign oxidation numbers, identify oxidising and reducing agents, and balance redox equations in acidic and basic media by the ion–electron method.

Calculate standard cell potentials (E°cell), predict spontaneity, and write the cell notation and electrode half-reactions for a galvanic cell; apply the Nernst equation to non-standard concentrations.

Explain the quantitative relationships in electrolysis (Faraday's laws, charge = current × time) and calculate the mass or volume of product deposited or liberated.

Apply Hess's law, standard enthalpies of formation and bond energies to calculate reaction enthalpy, and use entropy and Gibbs energy (ΔG = ΔH − TΔS) to determine the spontaneity temperature threshold.

Determine rate laws and reaction orders from initial-rate data and from concentration–time graphs, and calculate the rate constant with correct units.

Use the integrated rate laws (zero, first, second order) and half-life to predict concentrations, and apply the Arrhenius equation to calculate activation energy or the effect of temperature on k.

Propose a plausible reaction mechanism consistent with an observed rate law, identify intermediates and catalysts, and explain how a catalyst lowers activation energy without changing ΔH or ΔG.

Connect kinetics to thermodynamics by distinguishing kinetic control (activation energy) from thermodynamic control (ΔG) and interpreting energy-profile diagrams.

Complete two full-length timed mock exams under PAU conditions, allocating time per question and showing all working.

Identify the three weakest domains from mock results and re-solve every missed problem from first principles without notes.

Consolidate a one-page formula and constants sheet (Ka, Ksp, Nernst, Arrhenius, ΔG, gas law) and verify that each formula is used correctly in at least one problem.

Practise explaining reasoning in writing for justification questions (periodic trends, Le Chatelier shifts, mechanism choice, spontaneity) in 2–4 precise sentences.