NESA Chemistry Stage 6 Syllabus (2017), examined from 2019 to 2028
Chemistry is assessed through school-based tasks, including a depth study, and the HSC written examination, which combines objective-response questions with written responses mixing calculations, balanced equations, structural formulae, data interpretation and extended explanations. NESA publishes marking guidelines alongside each year's paper, and they repay reading as closely as the questions themselves: they show how a calculation mark is split between method and final value, and how much of an explanation must be present before the mark is awarded.
Past papers on this subject span more than one syllabus. Papers written under an older one still work as practice, but the modules they test have changed — the index labels every paper with the syllabus it was set under.
Chemistry Stage 6 Syllabus (2013) · 2013–2018Chemistry Stage 6 Syllabus (2017) · 2019–2028
The modules, one by one
Each area below lists the concepts named in the syllabus, what the NESA exam asks of them, and the mistake that most often costs marks.
Area 1 of 4
Module 5: Equilibrium and Acid Reactions
This module builds the idea that many reactions never finish. You distinguish static equilibrium from dynamic equilibrium, where forward and reverse reactions continue at equal rates, and use Le Chatelier's principle to predict how a system shifts when concentration, temperature, pressure or volume changes — and why a catalyst changes none of that, only the time taken to get there. The treatment then turns numerical: writing the equilibrium expression, calculating the equilibrium constant from equilibrium concentrations, using the solubility product to predict whether a precipitate forms, and interpreting what a very large or very small constant says about the extent of reaction. The module also introduces acids and bases through Brønsted–Lowry theory and conjugate acid–base pairs, together with the quantitative work that follows: acid–base titration, and pH and pOH calculations.
What the syllabus lists under this area · 5 points
- Static and dynamic equilibrium (reversible reactions, Le Chatelier's principle)
- Factors that affect equilibrium (concentration, temperature, pressure, volume, catalysts)
- Calculating the equilibrium constant (Kc / Ksp) and its meaning
- Acids and bases (Bronsted-Lowry theory, conjugate pairs)
- Quantitative analysis (acid-base titrations, pH and pOH calculations)
What the exam asks
Equilibrium questions typically give a system and a change, then ask for the shift and a justification framed in terms of particle collisions or the reaction quotient — 'to oppose the change' on its own is not an explanation. Calculations expect a full concentration table set-out with correct units and significant figures, so write out every step rather than jumping to a final value.
Where marks go missing
Explaining a temperature shift without using the enthalpy of the reaction. Whether heating favours products depends on whether the forward reaction is exothermic or endothermic, and answers that treat temperature like concentration get the direction wrong half the time.
Area 2 of 4
Module 6: Acid/Base Reactions
Module 6 separates two ideas students routinely merge: concentration and strength. A strong acid ionises completely in water while a weak acid sets up an equilibrium, so a dilute strong acid can have a lower pH than a concentrated weak one. You also distinguish monoprotic acids from polyprotic acids, which donate more than one proton and therefore titrate in stages. Brønsted–Lowry theory is used to explain behaviour rather than simply to label it — identifying which species donates the proton, which accepts it, what the conjugates are, and which species are amphiprotic. The quantitative strand is titration: matching an indicator's transition range to the pH at equivalence, reading the shape of a titration curve for each combination of strong and weak reagents, and locating the equivalence point. Applications cover neutralisation in industry, agriculture and the body.
What the syllabus lists under this area · 4 points
- Properties of acids and bases (strong vs weak, monoprotic vs polyprotic)
- Using Bronsted-Lowry theory to explain acid/base behaviour
- Quantitative analysis of acids and bases (titration curves, indicators)
- Applications and uses of neutralisation reactions
What the exam asks
Titration curves are read rather than recalled: identify the acid–base combination from the shape of the curve, justify an indicator choice against the pH at equivalence, and calculate concentration from titre data. Explanation questions ask why a weak acid has a higher pH than a strong acid of the same concentration, which requires the ionisation equilibrium, not just the word 'weak'.
Where marks go missing
Calling the equivalence point neutral. It sits near pH 7 only for a strong acid with a strong base; a weak acid with a strong base finishes above 7, and an indicator chosen on the wrong assumption costs the mark.
Area 3 of 4
Module 7: Organic Chemistry
Organic chemistry is a systems module: almost every mark depends on naming and drawing structures correctly. You learn IUPAC nomenclature for hydrocarbons and for compounds carrying functional groups — haloalkanes, alcohols, aldehydes, ketones, carboxylic acids, esters, amines and amides — including how to number a chain and order substituents. Hydrocarbon chemistry contrasts the saturated alkanes, which undergo substitution, with unsaturated alkenes and alkynes, which undergo addition across the double or triple bond. Reactions of organic compounds then link the families together: oxidation of primary alcohols through to carboxylic acids, esterification under acid catalysis, and the physical property trends in boiling point, solubility and flammability that follow from intermolecular forces. The module ends with polymers, distinguishing addition polymerisation of monomers containing a double bond from condensation polymerisation, which eliminates a small molecule.
What the syllabus lists under this area · 4 points
- Nomenclature and structure of organic compounds (hydrocarbons, functional groups)
- Hydrocarbons (alkanes, alkenes, alkynes, addition/substitution reactions)
- Products of reactions of organic compounds (alcohols, esters, polymers)
- Polymers (addition and condensation polymerisation)
What the exam asks
Marks are won or lost on structural formulae drawn in full, correct IUPAC names, and balanced equations that show every product, including the water eliminated in esterification and condensation. Expect reaction-pathway questions requiring you to get from one named compound to another, and property comparisons that must be explained through dispersion forces, dipole–dipole interactions or hydrogen bonding.
Where marks go missing
Explaining boiling point differences by molecular size alone. The mark is for identifying the specific intermolecular force — hydrogen bonding in alcohols and carboxylic acids against dispersion forces in alkanes — and stating which force has to be overcome.
Area 4 of 4
Module 8: Applying Chemical Ideas
The final module asks how a chemist works out what a substance actually is. Inorganic analysis covers qualitative tests — flame tests, precipitation reactions and the systematic identification of cations and anions — alongside quantitative methods including gravimetric analysis, titration, and instrumental techniques such as atomic absorption spectroscopy and colourimetry with calibration curves. Organic analysis introduces chromatography, mass spectrometry for molecular mass and fragmentation, infrared spectroscopy for functional groups, and proton and carbon-13 NMR, which are used together to deduce an unknown structure from a set of spectra. Chemical synthesis and design reverses the problem: given a target molecule, plan a route to it, and evaluate an industrial process against yield, energy input, availability of reagents and the principles of green chemistry, including atom economy and waste minimisation.
What the syllabus lists under this area · 3 points
- Analysis of inorganic substances (qualitative and quantitative techniques, spectroscopy)
- Analysis of organic substances (chromatography, mass spectrometry, NMR)
- Chemical synthesis and design (industrial processes, green chemistry)
What the exam asks
This module supplies the multi-step deduction questions: given a molecular formula plus mass spectrum, infrared and NMR data, identify the compound and justify each piece of evidence separately. Quantitative analysis is examined through calculation from titration or calibration data, and synthesis questions ask for an evaluation against named criteria rather than a description of the process.
Where marks go missing
Announcing a structure without tying each spectral feature to it. Every piece of evidence used — a fragment mass, an absorption band, the number of NMR environments and their splitting — must be stated explicitly, or a correct final answer still falls short of full marks.
Common questions
Which syllabus does the current HSC Chemistry exam follow?
The Chemistry Stage 6 Syllabus published in 2017, first examined in 2019 and running through to 2028. Papers from 2019 onwards match the Module 5 to 8 structure you are studying. Papers up to 2018 were set on the 2013 syllabus and are organised around different content.
Why do Modules 5 and 6 both cover acids?
Module 5 introduces acids and bases as an application of equilibrium — Brønsted–Lowry theory, conjugate pairs, pH and titration as quantitative analysis. Module 6 then goes deeper into acid and base behaviour itself: strength against concentration, polyprotic acids, titration curves and indicator selection, and the uses of neutralisation.
Is Year 11 Chemistry assumed knowledge in the HSC exam?
Yes. The mole concept, stoichiometry, concentration calculations, bonding and intermolecular forces, and enthalpy all come from Year 11 and are used constantly in Year 12 questions. A student who never consolidated the mole will struggle with equilibrium calculations and quantitative analysis regardless of how well they know Modules 5 to 8.
Do the older HSC Chemistry papers still help?
Partly. Papers from 2019 onwards are the priority because they match the current modules. Earlier papers were set under the 2013 syllabus, which included option topics and a different treatment of industrial chemistry, so use them selectively for equilibrium, acid–base and organic practice rather than working through them whole.