SPM Chemistry study plan

Build a single flowchart linking mass, moles, number of particles, molar volume and concentration, then use it to convert 12 quantities without looking at notes (konsep mol).

Classify 15 given substances as element, compound or mixture and justify each classification with particle arrangement and separation evidence.

Derive empirical and molecular formulae from percentage-composition data for 5 worked examples, showing every step.

Write and balance 15 chemical equations, including 5 ionic equations, and identify the spectator ions in each ionic one.

Compute molarity, dilution and moles = MV/1000 for 8 titration-style problems and state the units at each step.

Draw atomic structure and write full electron arrangements for the first 20 elements, including the correct shells after filling the 4s orbital.

Calculate neutron number from nucleon and proton number for 10 isotopes, and compute relative atomic mass from isotopic abundance data for 3 elements.

Relate group and period position to electron arrangement for elements 1 to 20, then predict the trend in atomic radius, electronegativity and reactivity.

Distinguish metals, non-metals and transition metals by position and properties, and give three specific uses linked to those properties.

Explain, using nuclear charge and shielding, why Group 1 reactivity rises and Group 17 reactivity falls down the group.

Draw dot-and-cross diagrams for 8 ionic compounds and 10 covalent molecules, including dative bonds in NH4+ and H3O+ and the delocalised electrons in graphite and diamond.

Explain, in terms of forces between particles, why sodium chloride conducts when molten but not when solid, and why graphite conducts while diamond does not.

Predict bond type for 10 element pairs using electronegativity and Periodic Table position, then justify each prediction in one sentence.

Compare melting point, volatility, solubility and electrical conductivity of ionic, simple covalent, giant covalent and metallic substances, linking every property to structure.

Explain why 1 mol of an ionic compound releases more ions in solution than 1 mol of a simple covalent compound, and connect this to electrolysis behaviour.

Define acids and bases as proton donors and acceptors, then classify 10 solutions using pH value, indicator colour and conductivity evidence.

Calculate pH from hydrogen ion concentration and the reverse, and distinguish strong from weak acids using degree of dissociation rather than concentration alone.

Select and justify the correct preparation route, whether titration, precipitation or acid plus metal or carbonate, for 8 named salts and list the exact reactants needed.

Write ionic equations for 6 neutralisation and precipitation reactions, and describe the confirmatory cation and anion tests for 6 unknown salts.

Solve 6 titration problems that require a mole ratio and conservation of moles to find an unknown molarity or volume.

Name and draw structural formulae for the first six alkanes, alkenes and alcohols, and draw all isomers of C4H10 and C5H12.

Describe combustion, halogenation, addition, oxidation, esterification and dehydration reactions and state the conditions and reagents written above each arrow.

Distinguish saturated from unsaturated hydrocarbons using brominated water and acidified potassium manganate(VII), and explain each observation.

Compare ethanol production by fermentation with catalytic hydration, giving conditions, catalysts, rate and sustainability for each route.

Relate the uses of ethanol, ethanoic acid, esters and addition polymers to their specific chemical and physical properties.

Draw labelled energy level diagrams for 3 exothermic and 3 endothermic reactions and calculate enthalpy change from bond energies or calorimetry data.

Plan a simple calorimetry experiment for heat of neutralisation, listing apparatus, controlled variables, measurements taken and two safety precautions.

Assign oxidation numbers to every element in 10 species and identify the oxidising and reducing agents in 6 redox equations.

Split 5 redox equations into oxidation and reduction half-equations and recombine them by balancing atoms, oxygen, hydrogen and charge.

Explain rusting and three prevention methods, sacrificial protection, alloying and coating, in terms of electron transfer.

Design 3 rate experiments using gas volume, mass loss and colour or time, stating the measured quantity and all controlled variables.

Interpret rate curves by reading the initial rate and gradient, then explain the effects of concentration, temperature, surface area and catalyst using collision theory.

Explain qualitatively how temperature and a catalyst change the proportion of successful collisions in a reaction mixture.

Outline the Haber and Contact processes, giving raw materials, catalyst, temperature, pressure and the effect of each condition on equilibrium yield.

Justify at least three economic or safety decisions in each industrial process, such as recycling unreacted gases and heat exchange.

Re-attempt every question flagged as wrong in weeks 1 to 7 and write one line explaining the corrected reasoning for each.

Complete two full past papers under timed conditions, including Paper 3 planning and structured questions, and record the score for each section.

Write the operational definition and standard procedure for 6 core experiments, covering rate, heat of neutralisation, salt preparation and redox displacement.

Tabulate every calculation type in the syllabus, mole, concentration, titration, enthalpy and rate, each with one worked example and its common trap.

Recall and apply without notes the electrochemical series, indicator colour changes and the tests for oxygen, hydrogen, carbon dioxide, ammonia and chlorine.