IB Chemistry SL study plan

Convert between number of particles, amount in mol, mass and molar mass using Avogadro's constant in multi-step problems.

Solve for any variable in pV = nRT, including cases where molar mass or gas density must be derived, and cases where a gas is collected over water.

Use the assumptions of the kinetic molecular theory to explain why a real gas deviates most from ideal behaviour at high pressure and low temperature.

Write full and condensed electron configurations for atoms and ions up to Z = 36, including the 4s/3d filling order and the chromium and copper anomalies.

Record raw measurements with correct significant figures and absolute uncertainty, and propagate uncertainty through addition and multiplication.

Balance molecular and ionic equations and identify the limiting reactant when two solutions of known concentration are mixed.

Calculate theoretical yield, percentage yield and atom economy for a named synthesis, and explain the gap between them.

Perform titration calculations from concentration, volume and mole ratio data, including dilution steps.

Convert a calculated amount in mol into a gas volume at a stated temperature and pressure using the ideal gas equation.

Explain the effect of concentration, pressure, surface area, temperature and a catalyst on reaction rate using collision theory.

Interpret Maxwell-Boltzmann distribution curves to explain how temperature and a catalyst change the proportion of successful collisions.

Write equilibrium constant expressions, calculate Kc from equilibrium concentrations and state its units.

Apply Le Chatelier's principle to predict the direction of shift, and distinguish a change in equilibrium position from a change in Kc.

Plan a rates investigation by choosing a measurable dependent variable, five values of the independent variable and a full set of controlled variables.

Calculate enthalpy change from calorimetry data using q = mcΔT, stating the assumptions about density, specific heat capacity and heat loss.

Construct and use Hess's law cycles to find ΔH for reactions that cannot be measured directly.

Calculate ΔH from average bond enthalpies and explain why the answer differs from the value obtained using standard enthalpies of formation.

Define standard enthalpy of formation and combustion and write the formation equation for a named compound.

Design the internal assessment: write a focused research question, a variables table, a method with sufficient data points and a risk assessment.

Identify Brønsted-Lowry conjugate acid-base pairs and calculate pH, [H+] and [OH-] for strong monoprotic acids and bases using Kw.

Contrast strong and weak acids in terms of degree of dissociation, conductivity and rate of reaction with a metal, and sketch titration curves for strong-strong and strong-weak combinations.

Assign oxidation numbers, identify the oxidising and reducing agents, and balance redox half-equations in acidic solution.

Describe the structure and operation of a voltaic cell and a simple electrolytic cell, including electrode polarity, electron flow and the direction of ion migration.

Classify a substance as ionic, covalent or metallic from its position in the periodic table and explain the resulting physical properties.

Draw Lewis structures and apply VSEPR theory to predict shape, bond angle and polarity for species with up to six electron domains.

Explain the origin and relative strength of London dispersion, dipole-dipole and hydrogen bonding, and rank substances by boiling point with justification.

Relate giant covalent, simple molecular, ionic and metallic lattices to melting point, solubility and electrical conductivity.

Process the internal assessment data: calculate means, plot the graph with uncertainty bars and quantify percentage error against the theoretical value.

Use the periodic table to predict and explain trends in atomic radius, ionic radius, first ionisation energy and electronegativity across a period and down a group.

Classify elements as metals, metalloids or non-metals and link the classification to bonding type and to the acidic or basic character of their oxides.

Identify alkane, alkene, alcohol, aldehyde, ketone, carboxylic acid, ester, amine, amide and halogenoalkane groups from names and displayed structures.

Predict and name the products of simple SL reactions of those groups, including combustion, addition, oxidation, substitution and esterification.

Finalise the internal assessment by completing data processing, uncertainty evaluation, a strengths-and-limitations discussion and a conclusion that answers the research question.

Sit one full-length timed SL paper under exam conditions and mark it with the official mark scheme.

Build a per-domain score profile from the mock and re-teach the two weakest domains with targeted questions.

Reproduce from memory a one-page sheet of key equations and definitions, then check it against the data booklet.