Data and Experimental Skills

Start with the quantity or claim the question asks you to establish. Then locate the relevant measurements, conditions and any new definitions in the stem. An unfamiliar substance name does not make its data unusable: use the supplied information together with a familiar idea such as conservation of atoms, collision frequency or intermolecular attraction.

Put the independent variable on the horizontal axis and the measured or derived dependent variable on the vertical axis. Label each axis with a quantity and unit, use a clear uniform scale, and plot the actual points. A best-fit line or smooth curve represents a trend; do not force it through every point or through the origin without a reason.

Interpolation estimates a value within the measured range. Extrapolation extends a trend outside it and needs an extra assumption that the relationship continues. If a graph is linear, choose two well-separated points on the best-fit line for a gradient, not two close points chosen because they happen to be measurements.

Keep guard digits during working. Round the final answer to a precision justified by the inputs and any question instruction. A unit conversion changes the numerical value, not the physical quantity: 25.0 cm³ = 0.0250 dm³. Check dimensions before inserting numbers into a formula.

Accuracy concerns closeness to a valid reference value; precision concerns the closeness of repeated measurements. A tightly grouped set can still be inaccurate. An anomalous point is a reason to investigate the method and repeat a measurement, not permission to remove inconvenient evidence silently. Record an exclusion and its reason.

Write evaluation as a causal chain: limitation -> affected measurement -> effect on the calculated result -> targeted improvement. "Human error" and "use better equipment" do not identify what happened. For example, gas escaping before collection lowers measured gas volume; assembling a closed collection system before starting the reaction addresses that loss.

Choose apparatus for the needed measurement: a volumetric pipette delivers a fixed accurate volume, a burette delivers a variable accurately measured volume, a measuring cylinder is suitable for less exact volume work, and a balance measures mass. Read the scale at eye level to avoid parallax; use the bottom of the meniscus for a clear aqueous solution unless the instructions specify otherwise.

For Secondary Chemistry, the syllabus normally expects burette readings to the nearest 0.05 cm³, and sufficient titrations to obtain, for a good end-point, two titres within 0.20 cm³. Record both readings and the difference. Follow the question if it gives a particular agreement criterion; do not include the rough titre in a precise mean.

Separate raw observations from interpretation. "A white precipitate forms after three drops and dissolves in excess" preserves information that "positive test" loses. Record colour, physical state, changes on standing or warming, and any confirmed gas test. Put units in table headings; do not attach a unit to a pure ratio.

The equivalence point is the stoichiometric completion of reaction. The endpoint is the observed indicator change. Choose an indicator whose transition lies in the steep pH change near equivalence; universal indicator gives a broad colour change and is unsuitable for precise titration. The required final colour depends on the indicator and which solution is added.

Use clean apparatus and a fresh small portion for each test. Add reagent gradually with mixing; observe a few drops, excess reagent and warming separately when instructed. Write the actual colour and physical change. A blue solution and a pale-blue precipitate are different observations. Name a gas only after the appropriate confirmatory test.

For a simple organic test, record the reagent and what changes. Bromine water changing from orange to colourless is consistent with an alkene under the relevant conditions, but decolourisation alone is not a universal proof of C=C because other substances can also react. Use the stated candidate structures and any other evidence to narrow the conclusion.

In G2 the gas tests you must know are hydrogen (lighted splint, squeaky pop), oxygen (glowing splint relights) and carbon dioxide (limewater turns milky). A question may describe another test and ask you to record or interpret what you would see: describe the change first, then state what it suggests.

For paper chromatography, use a pencil baseline above the solvent, small concentrated spots and a covered vessel where appropriate. Remove the paper before the solvent reaches the top and mark the solvent front immediately.

G2 practical work includes crystallisation of salts, filtration, paper chromatography and distillation. Describing the full preparation of a pure salt is not required.

Read the requested quantity or claim first. Select the relevant evidence, state the chemical connection and give a result with its unit or a justified conclusion.

For a G2 practical question: choose suitable apparatus, read scales at eye level, record raw readings with units in the table heading, describe what you see before concluding, and suggest a specific improvement rather than "be more careful".