NSSCAS Chemistry (8224) study plan

Draw electron configurations (full and shorthand) for atoms and ions up to Z=38 and mark the exceptions Cr and Cu from memory

Explain first ionisation energy trends across Period 3 and down Groups 1, 2, 7 and 0 using shielding, nuclear charge, atomic radius and electron pairing

Convert between mass, moles, concentration and gas volume using the ideal gas equation and molar volume at room temperature and pressure

Balance ionic and full equations and identify the limiting reagent in a multi-step calculation

Determine empirical and molecular formulae from percentage composition and combustion data

Classify substances as ionic, simple molecular, giant covalent or metallic and predict melting point, solubility and conductivity from the structure

Draw dot-and-cross diagrams for covalent molecules and ions including dative bonds in NH4+ and H3O+

Explain the origin of London dispersion, permanent dipole-dipole and hydrogen bonding forces and rank boiling points of given molecules

Describe the reactions of Groups 2 and 7 elements and their compounds, including thermal stability of carbonates and nitrates, and write balanced equations with state symbols

Explain the trend in solubility of Group 2 hydroxides and sulfates and of silver halides in terms of lattice and hydration enthalpy

Plot and interpret rate graphs and explain the effect of concentration, temperature, pressure, surface area and catalyst on rate using collision theory

Draw and label Maxwell-Boltzmann distribution curves for two temperatures and explain the area beyond the activation energy

Apply Le Chatelier's principle to predict the shift caused by changes in concentration, pressure and temperature, and state the effect on Kc or Kp

Write equilibrium constant expressions and calculate Kc from equilibrium concentrations

Construct and interpret enthalpy cycles (Hess's law) and calculate enthalpy changes from bond enthalpies and standard enthalpy of formation

Define and calculate pH, [H+], Ka and pKa for weak acids, and calculate the pH of a buffer prepared from a weak acid and its salt

Explain the shape of a titration curve for strong-weak acid-base combinations and select a suitable indicator

Assign oxidation states and identify oxidation and reduction in given equations, including disproportionation

Construct and use a standard electrode potential table to predict the feasibility of a redox reaction and the direction of electron flow in a cell

Describe the electrolysis of molten and aqueous electrolytes and write electrode half-equations for the products

Name and draw structural, displayed and skeletal formulae for alkanes, alkenes, halogenoalkanes, alcohols, aldehydes, ketones, carboxylic acids, esters and nitriles

Identify functional groups from spectra and simple chemical tests and predict the products of oxidation, reduction, substitution, addition and elimination reactions

Outline reaction mechanisms with curly arrows for electrophilic addition, nucleophilic substitution (SN1 and SN2) and elimination

Explain the relative reactivity of primary, secondary and tertiary halogenoalkanes and the role of the hydroxide ion as nucleophile

Describe addition and condensation polymerisation and draw repeat units from given monomers

Design a multi-step synthesis from a given starting material and justify each reagent and condition

Interpret infrared and mass spectra to identify functional groups and deduce a structure from a molecular ion and fragmentation pattern

Describe the standard practical techniques for purification: filtration, recrystallisation, distillation, separating funnel and drying, and state the purpose of each

Evaluate a described experimental procedure for sources of error and suggest improvements in accuracy and precision

Explain how to record and process results, including significant figures, uncertainties and identification of anomalous readings

Re-derive the explanations for periodic trends, bonding and equilibrium from first principles without notes

Answer 30 multiple-choice questions on the three heaviest domains under timed conditions and log every error by cause

Explain unfamiliar structures and trends by transferring principles rather than recalling facts

State the definitions of standard enthalpy change, ionisation energy, electronegativity and equilibrium constant precisely enough to score full definition marks

Complete two full past-paper-style papers under exam timing and mark them against the mark scheme

Prioritise revision of the lowest-scoring domains from the error log and close each gap with targeted practice

Practise writing concise answers that hit the command word (state, describe, explain, deduce, suggest)

Review the formula sheet, definitions and reaction map one final time and confirm recall without prompts