NCEA L2 Chemistry study plan

Build a one-page formula and constants sheet covering mole calculations, concentration, gas volume at STP, and percentage composition, then use it to solve 20 mixed stoichiometry problems without notes.

Define and distinguish the terms mole, molar mass, empirical formula, molecular formula, limiting reagent, and percentage yield in your own words, then check each definition against a textbook glossary.

Practise balancing 15 equations including combustion, precipitation, and acid-base neutralisation, and classify each reaction type.

Set up a spaced-repetition deck of 40 recall cards for ions, polyatomic ions, and solubility rules, and run the first review session.

Solve 12 limiting-reagent problems that require identifying the excess reagent and calculating the mass or concentration of product formed.

Calculate percentage yield and percentage composition for at least 8 reactions, including one hydrate and one reaction with an impure reactant.

Perform dilution and mixing calculations (c1V1 = c2V2 and mixing two solutions) across 10 problems, including unit conversions between mL, L, g, and mol.

Titration practice: compute unknown concentration from titre volume, molar ratio, and average concordant results for 6 data sets.

Draw Lewis structures and predict molecular shapes and bond angles for 15 species using VSEPR, including molecules with lone pairs.

Explain the difference between ionic, covalent, and metallic bonding in terms of electron transfer, sharing, and delocalisation, with one example of each.

Relate intermolecular forces (dispersion, dipole-dipole, hydrogen bonding) to observed melting point, boiling point, and solubility trends for 8 substances.

Write balanced ionic equations, including spectator-ion removal, for 10 precipitation and neutralisation reactions.

Assign oxidation numbers and identify oxidation and reduction half-reactions in 12 redox equations.

Balance 8 redox equations in acidic or basic conditions by the half-equation method.

Describe the operation of an electrochemical cell and write the overall cell equation for 5 cells given electrode pairs and standard potentials.

Explain oxidation and reduction in terms of electron loss and gain and link each to observed colour or mass changes in 4 described reactions.

Calculate enthalpy changes from calorimetry data (q = mcΔT) for 6 experiments, including heat loss corrections.

Apply Hess's law and bond enthalpy data to determine ΔH for 8 reactions.

Classify reactions as endothermic or exothermic and sketch labelled energy profile diagrams including activation energy for 5 reactions.

State and apply collision theory and factors affecting reaction rate (concentration, temperature, surface area, catalyst) to 6 scenarios.

Define acids and bases using Brønsted-Lowry theory and identify conjugate pairs in 15 equations.

Calculate pH from hydrogen ion concentration and vice versa for 12 strong acid and strong base solutions, including dilution effects.

Interpret titration curves by sketching and labelling 4 curves and identifying equivalence point and buffer region.

Describe the properties and behaviour of buffers and write equations showing how a buffer resists pH change in 3 examples.

Name and draw structures for alkanes, alkenes, alkynes, alcohols, carboxylic acids, and haloalkanes up to six carbons using IUPAC rules.

Identify and describe 6 organic reaction types (substitution, addition, elimination, oxidation, esterification, polymerisation) with reagents and conditions.

Predict the products of 12 organic reactions from given reactants and conditions, including addition across a double bond and ester formation.

Explain the difference between structural isomers and stereoisomers and draw 3 isomer sets for a given molecular formula.

Complete two full timed practice papers under exam conditions and record a score for each.

Classify every incorrect answer by error type (calculation, recall, misread, incomplete explanation) and rank the top three recurring weaknesses.

Re-teach the three weakest topics by rewriting the relevant notes and solving 5 fresh problems in each.

Build a final one-page exam-day sheet covering key formulas, solubility rules, and reaction conditions, then recite it from memory.