NSSCO Chemistry (6117) study plan

Define the mole in terms of the Avogadro constant (6.02 × 10²³) and convert confidently between number of particles, amount in moles and mass for at least 15 different substances, including hydrated salts such as CuSO₄·5H₂O.

Calculate relative formula mass for compounds containing brackets and water of crystallisation, and use it to find percentage composition by mass of each element in a compound.

Balance 25 skeleton equations, including combustion, displacement, neutralisation and precipitation reactions, and state the mole ratio for any pair of species in each balanced equation.

Derive empirical formulae from mass or percentage-composition data, then calculate the molecular formula by comparing empirical formula mass with a given relative molecular mass.

Build a one-page formula toolkit covering n = m/M, n = N/NA, n = cV and n = V/24 that you can reproduce from memory at the start of any calculation question.

Use mole ratios from balanced equations to calculate reacting masses and identify the limiting reagent when two reactant quantities are given, then calculate the mass of product formed and the mass of reagent left over.

Convert between concentration in g/dm³ and mol/dm³, and calculate the concentration or volume of a solution after dilution or mixing.

Apply the molar gas volume of 24 dm³ at room temperature and pressure to calculate volumes of gaseous reactants and products, including cases where the reaction produces a gas collected over water.

Perform complete titration calculations: convert titre volume and concentration to moles, apply the equation ratio, and find an unknown concentration or relative formula mass, showing every step with units.

Explain how to prepare a standard solution using a volumetric flask and a balance, and state why a burette, pipette and conical flask are used in a titration rather than measuring cylinders.

Describe the arrangement, movement and energy of particles in solids, liquids and gases, and use kinetic theory to explain diffusion, Brownian motion, changes of state, and the shapes of heating and cooling curves.

Select and justify an appropriate separation technique (filtration, crystallisation, simple distillation, fractional distillation, chromatography, sublimation, decanting, use of a separating funnel) for eight described mixtures, giving the reason each technique works.

Describe a test for purity (sharp melting point, single spot in chromatography) and calculate Rf values from chromatogram data.

Describe the reactions of dilute acids with metals, metal oxides, hydroxides and carbonates, and write balanced equations including state symbols for each type.

Outline the preparation of a soluble salt from an insoluble base or carbonate (and by titration for sodium/potassium salts) and of an insoluble salt by precipitation, including the washing and drying steps.

Describe atomic structure in terms of protons, neutrons and electrons, and use atomic number and mass number to deduce the composition of atoms and ions, including isotopes.

Calculate relative atomic mass from given isotopic abundances, and write the electron configuration (2,8,8) of the first 20 elements and their ions.

Draw dot-and-cross diagrams for ionic compounds (NaCl, MgO, CaCl₂) and explain how transfer of electrons produces charged ions held in a giant ionic lattice.

Draw dot-and-cross diagrams for simple molecules (H₂, N₂, H₂O, NH₃, CH₄, CO₂) and explain the difference in properties between simple molecular substances and giant covalent structures such as diamond and graphite.

Explain metallic bonding as positive ions in a sea of delocalised electrons, and use it to account for conduction, malleability and high melting points.

Predict melting point, solubility and electrical conductivity for a named substance from its structure type (ionic, simple molecular, giant covalent, metallic) and justify the prediction in one sentence.

Describe the layout of the Periodic Table in terms of groups and periods and relate group number and period number to outer-shell electrons and number of shells.

Describe and explain the trends down Group I (reactivity, melting point) and down Group VII (colour, reactivity, melting point) in terms of increasing atomic size and electron shielding.

Write displacement equations for halogen displacement reactions and use them to place halogens in order of reactivity, and explain why Group VIII elements are unreactive.

Describe the general properties and uses of transition elements, including variable oxidation states, catalytic activity and coloured compounds.

Use the reactivity series to select the extraction method for iron, aluminium, zinc and copper, and explain why carbon or electrolysis is used in each case.

Describe the blast furnace extraction of iron with the purpose of each raw material and the equations for the key reactions, and describe the electrolysis of molten aluminium oxide including the role of cryolite.

Explain why alloys are harder than pure metals, and describe the conditions needed for iron to rust and three methods of rust prevention, including sacrificial protection and galvanising.

Describe the manufacture of sulfuric acid (contact process) and ammonia (Haber process), stating the conditions, the catalyst and two uses of each product.

Explain the causes and effects of air pollutants (carbon monoxide, sulfur dioxide, nitrogen oxides, carbon dioxide) and outline water treatment steps that make water safe to drink.

Use collision theory to explain how concentration, temperature, surface area, pressure and catalysts change reaction rate, and interpret rate graphs in terms of the steepness of the initial gradient.

Classify reactions as exothermic or endothermic, draw and interpret energy profile diagrams showing activation energy and ΔH, and explain that bond breaking requires energy while bond making releases it.

Apply Le Chatelier's principle to predict the effect of changing temperature, pressure and concentration on reversible reactions, including the Haber process and the hydration of alkenes.

Name and draw members of the alkane, alkene, alcohol and carboxylic acid homologous series up to four carbons, state their general formulae and explain the difference in reactivity between alkanes and alkenes.

Describe the reactions of alkanes (combustion, cracking) and alkenes (addition with bromine, hydrogen, water, and addition polymerisation), and explain how fractional distillation separates crude oil fractions by boiling point.

Identify independent, dependent and controlled variables for unfamiliar investigations, and select appropriate apparatus for measuring time, temperature, mass and gas volume.

Design a results table with correct headings and units, plot the data with labelled axes and a suitable line, and draw a conclusion that refers back to the stated hypothesis.

Evaluate experimental data by identifying anomalous results, sources of error and whether the evidence supports the conclusion, and suggest one specific improvement.

Re-drill the highest-weight calculation content from weeks 1, 2 and 7, targeting the three error-log entries that cost the most marks.

Complete one full past-paper-style mock in a single sitting under exam conditions and allocate remaining time proportionally to the domain weightings when reviewing answers.