Specification points

OCR AS Level Chemistry A H032

341 points in 6 topics, with OCR's codes and titles.

Codes and titles are read by a script from OCR's published specification and have not been checked by a person. What each point covers is in the specification itself: OCR’s specification.

1 Development of practical skills in chemistry

1.1 Practical skills assessed in a written examination
1.1.1 Planning
1.1.1(a) Designing experiments to solve practical problems
1.1.1(b) Identifying variables to control
1.1.1(c) Judging whether a method suits the aims
1.1.2 Implementing
1.1.2(a) Using practical apparatus and techniques correctly
1.1.2(b) Units for measurements
1.1.2(c) Presenting observations and data
1.1.3 Analysis
1.1.3(a) Processing and interpreting experimental results
1.1.3(b) Maths skills for analysing quantitative data
1.1.3(c) Significant figures
1.1.3(d) Plotting and interpreting graphs of results
1.1.3(d)(i) Choosing and labelling graph axes
1.1.3(d)(ii) Measuring gradients
1.1.4 Evaluation
1.1.4(a) Evaluating results and drawing conclusions
1.1.4(b) Spotting anomalies in measurements
1.1.4(c) Limitations of experimental procedures
1.1.4(d) Precision, accuracy, errors and uncertainties
1.1.4(e) Improving experimental procedures and apparatus

2 Foundations in chemistry

2.1 Atoms and reactions
2.1.1 Atomic structure and isotopes
2.1.1(a) Isotopes
2.1.1(b) Protons, neutrons and electrons in atoms and ions
2.1.1(c) Relative isotopic mass and relative atomic mass
2.1.1(d) Mass spectrometry
2.1.1(d)(i) Isotopic masses and abundances by mass spectrometry
2.1.1(d)(ii) Relative atomic mass from isotope abundances
2.1.1(e) Relative molecular and formula mass
2.1.2 Compounds, formulae and equations
2.1.2(a) Formulae of ionic compounds
2.1.2(a)(i) Predicting ionic charge from the periodic table
2.1.2(a)(ii) Names and formulae of common ions
2.1.2(b) Balanced and ionic equations with state symbols
2.1.3 Amount of substance
2.1.3(a) Moles, the Avogadro constant, molar mass and gas volume
2.1.3(a)(i) Amount of substance
2.1.3(a)(ii) The mole
2.1.3(a)(iii) The Avogadro constant
2.1.3(a)(iv) Molar mass
2.1.3(a)(v) Molar gas volume
2.1.3(b) Empirical and molecular formulae
2.1.3(b)(i) Empirical formula
2.1.3(b)(ii) Molecular formula
2.1.3(c) Calculating empirical and molecular formulae
2.1.3(d) Hydrated salts and water of crystallisation
2.1.3(e) Mole calculations: mass, gas and solution
2.1.3(e)(i) Moles and mass
2.1.3(e)(ii) Moles and gas volume
2.1.3(e)(iii) Moles, solution volume and concentration
2.1.3(f) The ideal gas equation
2.1.3(g) Stoichiometry in calculations
2.1.3(h) Percentage yield and atom economy
2.1.3(h)(i) Percentage yield
2.1.3(h)(ii) Atom economy
2.1.3(i) Measuring mass and volumes in experiments
2.1.3(j) Atom economy and sustainability
2.1.4 Acids
2.1.4(a) Common acids and alkalis and their ions
2.1.4(b) Strong and weak acids
2.1.4(c) Neutralisation
2.1.4(c)(i) H⁺ and OH⁻ to form H₂O
2.1.4(c)(ii) Acids reacting with bases to form salts
2.1.4(d) Standard solutions and acid–base titrations
2.1.4(e) Titration calculations
2.1.5 Redox
2.1.5(a) Assigning oxidation numbers
2.1.5(b) Formulae from oxidation numbers
2.1.5(c) Roman numerals for oxidation numbers
2.1.5(d) Oxidation and reduction
2.1.5(d)(i) Redox as electron transfer
2.1.5(d)(ii) Redox as oxidation number change
2.1.5(e) Metals with acids as redox reactions
2.1.5(f) Interpreting redox equations
2.2 Electrons, bonding and structure
2.2.1 Electron structure
2.2.1(a) Electrons in the first four shells
2.2.1(b) Atomic orbitals and sub-shells
2.2.1(b)(i) Orbitals as regions holding two electrons
2.2.1(b)(ii) Shapes of s- and p-orbitals
2.2.1(b)(iii) Orbitals and electrons in s-, p- and d-sub-shells
2.2.1(c) Order of filling orbitals
2.2.1(c)(i) Filling order up to the 4p orbitals
2.2.1(c)(ii) Single occupation before pairing
2.2.1(d) Electron configurations of atoms and ions
2.2.1(d)(i) Electron configurations of atoms up to Z = 36
2.2.1(d)(ii) Electron configurations of s- and p-block ions
2.2.2 Bonding and structure
2.2.2(a) Ionic bonding and dot-and-cross diagrams
2.2.2(b) Giant ionic lattices
2.2.2(c) Physical properties of ionic compounds
2.2.2(d) The covalent bond
2.2.2(e) Dot-and-cross diagrams of covalent bonding
2.2.2(e)(i) Single covalent bonds
2.2.2(e)(ii) Multiple covalent bonds
2.2.2(e)(iii) Dative covalent (coordinate) bonds
2.2.2(f) Average bond enthalpy and bond strength
2.2.2(g) Electron pair repulsion and molecular shapes
2.2.2(h) Named shapes of molecules and ions
2.2.2(i) Electronegativity and Pauling values
2.2.2(j) Polar bonds and polar molecules
2.2.2(j)(i) Polar bonds and permanent dipoles
2.2.2(j)(ii) Polar molecules and overall dipoles
2.2.2(k) Permanent and induced dipole–dipole forces
2.2.2(l) Hydrogen bonding
2.2.2(m) Anomalous properties of water
2.2.2(m)(i) Density of ice and water
2.2.2(m)(ii) High melting and boiling points of water
2.2.2(n) Simple molecular lattices
2.2.2(o) Properties of simple molecular substances

3 Periodic table and energy

3.1 The periodic table
3.1.1 Periodicity
3.1.1(a) How the periodic table is arranged
3.1.1(a)(i) Order by atomic number
3.1.1(a)(ii) Periods and periodicity
3.1.1(a)(iii) Groups with similar properties
3.1.1(b) Electron configurations and blocks
3.1.1(b)(i) Electron configuration trends across Periods 2 and 3
3.1.1(b)(ii) s-, p- and d-block elements
3.1.1(c) Ionisation energies
3.1.1(c)(i) Trends in first ionisation energy
3.1.1(c)(ii) Shells and groups from successive ionisation energies
3.1.1(d) Metallic bonding and lattices
3.1.1(d)(i) Metallic bonding
3.1.1(d)(ii) Giant metallic lattices
3.1.1(e) Giant covalent lattices of carbon and silicon
3.1.1(f) Properties of giant metallic and covalent lattices
3.1.1(g) Melting point trends across Periods 2 and 3
3.1.2 Group 2
3.1.2(a) Group 2 electron configuration and 2+ ions
3.1.2(b) Reactivity of Group 2 elements
3.1.2(b)(i) Group 2 elements with oxygen
3.1.2(b)(ii) Group 2 elements with water
3.1.2(b)(iii) Group 2 elements with dilute acids
3.1.2(c) Group 2 reactivity and ionisation energies
3.1.2(d) Group 2 oxides in water and alkalinity
3.1.2(e) Uses of Group 2 compounds as bases
3.1.2(e)(i) Calcium hydroxide for acid soils
3.1.2(e)(ii) Antacids for indigestion
3.1.3 The halogens
3.1.3(a) Halogen molecules and boiling points
3.1.3(b) Halogen electron configuration and 1– ions
3.1.3(c) Halogen reactivity and displacement
3.1.3(d) Explaining the trend in halogen reactivity
3.1.3(e) Disproportionation reactions of chlorine
3.1.3(e)(i) Chlorine and water in water treatment
3.1.3(e)(ii) Chlorine with sodium hydroxide to make bleach
3.1.3(e)(iii) Similar disproportionation reactions
3.1.3(f) Chlorine in water treatment: benefits and risks
3.1.3(g) Silver nitrate test for halide ions
3.1.4 Qualitative analysis
3.1.4(a) Test-tube tests for ions
3.1.4(a)(i) Tests for carbonate, sulfate and halide anions
3.1.4(a)(ii) Test for ammonium ions
3.2 Physical chemistry
3.2.1 Enthalpy changes
3.2.1(a) Exothermic and endothermic reactions
3.2.1(b) Enthalpy profile diagrams
3.2.1(c) Activation energy
3.2.1(d) Standard enthalpy change terms
3.2.1(d)(i) Standard conditions and states
3.2.1(d)(ii) Enthalpy change of reaction
3.2.1(d)(iii) Enthalpy change of formation
3.2.1(d)(iv) Enthalpy change of combustion
3.2.1(d)(v) Enthalpy change of neutralisation
3.2.1(e) Measuring enthalpy changes with q = mc∆T
3.2.1(f) Bond enthalpies
3.2.1(f)(i) Average bond enthalpy
3.2.1(f)(ii) Bond breaking and making in energy changes
3.2.1(f)(iii) Enthalpy calculations from bond enthalpies
3.2.1(g) Hess' law and enthalpy cycles
3.2.1(g)(i) Reaction enthalpy from combustion data
3.2.1(g)(ii) Reaction enthalpy from formation data
3.2.1(g)(iii) Unfamiliar enthalpy cycles
3.2.1(h) Measuring enthalpy changes directly and indirectly
3.2.2 Reaction rates
3.2.2(a) Concentration, pressure and collision frequency
3.2.2(b) Rates from gradients of graphs
3.2.2(c) The role of a catalyst
3.2.2(c)(i) Catalysts are not used up
3.2.2(c)(ii) Catalysts provide a lower activation energy route
3.2.2(d) Types of catalyst and their importance
3.2.2(d)(i) Homogeneous and heterogeneous catalysts
3.2.2(d)(ii) Economic and sustainability benefits of catalysts
3.2.2(e) Measuring reaction rates
3.2.2(f) The Boltzmann distribution
3.2.2(g) Boltzmann distributions, temperature and catalysts
3.2.2(g)(i) Effect of temperature on the distribution
3.2.2(g)(ii) Effect of a catalyst on the distribution
3.2.3 Chemical equilibrium
3.2.3(a) Dynamic equilibrium
3.2.3(b) Le Chatelier's principle
3.2.3(c) Catalysts and equilibrium position
3.2.3(d) Investigating equilibrium position changes
3.2.3(e) Equilibrium and rate compromise in industry
3.2.3(f) The equilibrium constant Kc
3.2.3(g) Equilibrium position from the size of Kc

4 Core organic chemistry

4.1 Basic concepts and hydrocarbons
4.1.1 Basic concepts of organic chemistry
4.1.1(a) IUPAC naming of organic compounds
4.1.1(b) Types of formula
4.1.1(b)(i) General formula
4.1.1(b)(ii) Structural formula
4.1.1(b)(iii) Displayed formula
4.1.1(b)(iv) Skeletal formula
4.1.1(c) Terms for classifying organic compounds
4.1.1(c)(i) Homologous series
4.1.1(c)(ii) Functional group
4.1.1(c)(iii) Alkyl group
4.1.1(c)(iv) Aliphatic compounds
4.1.1(c)(v) Alicyclic compounds
4.1.1(c)(vi) Aromatic compounds
4.1.1(c)(vii) Saturated and unsaturated compounds
4.1.1(d) Predicting formulae from a general formula
4.1.1(e) Structural isomers
4.1.1(f) Homolytic and heterolytic fission
4.1.1(f)(i) Homolytic fission
4.1.1(f)(ii) Heterolytic fission
4.1.1(g) Radicals
4.1.1(h) Curly arrows
4.1.1(i) Drawing reaction mechanisms
4.1.2 Alkanes
4.1.2(a) Alkanes and sigma bonds
4.1.2(b) Tetrahedral shape of alkanes
4.1.2(c) Boiling points of alkanes
4.1.2(d) Low reactivity of alkanes
4.1.2(e) Complete and incomplete combustion of alkanes
4.1.2(f) Radical substitution of alkanes
4.1.2(g) Limitations of radical substitution
4.1.3 Alkenes
4.1.3(a) Alkenes and pi bonds
4.1.3(b) Trigonal planar shape of alkenes
4.1.3(c) Stereoisomerism and E/Z naming
4.1.3(c)(i) Stereoisomers, E/Z and cis–trans isomerism
4.1.3(c)(ii) Cahn–Ingold–Prelog priority rules
4.1.3(d) Finding E/Z and cis–trans isomers
4.1.3(e) Reactivity of alkenes
4.1.3(f) Addition reactions of alkenes
4.1.3(f)(i) Hydrogenation of alkenes
4.1.3(f)(ii) Halogen addition and the bromine test
4.1.3(f)(iii) Addition of hydrogen halides
4.1.3(f)(iv) Hydration with steam to alcohols
4.1.3(g) Electrophiles
4.1.3(h) Electrophilic addition mechanism
4.1.3(i) Markownikoff's rule
4.1.3(j) Addition polymerisation
4.1.3(j)(i) Repeat unit from a monomer
4.1.3(j)(ii) Monomer from a polymer section
4.1.3(k) Processing waste polymers sustainably
4.1.3(k)(i) Burning waste polymers for energy
4.1.3(k)(ii) Waste polymers as feedstock
4.1.3(k)(iii) Removing toxic products from polymer disposal
4.1.3(l) Biodegradable and photodegradable polymers
4.2 Alcohols, haloalkanes and analysis
4.2.1 Alcohols
4.2.1(a) Properties and classification of alcohols
4.2.1(a)(i) Polarity, solubility and volatility of alcohols
4.2.1(a)(ii) Primary, secondary and tertiary alcohols
4.2.1(b) Combustion of alcohols
4.2.1(c) Oxidation of alcohols
4.2.1(c)(i) Oxidising primary alcohols to aldehydes and acids
4.2.1(c)(ii) Oxidising secondary alcohols to ketones
4.2.1(c)(iii) Tertiary alcohols resisting oxidation
4.2.1(d) Dehydration of alcohols to alkenes
4.2.1(e) Alcohols to haloalkanes by substitution
4.2.2 Haloalkanes
4.2.2(a) Hydrolysis of haloalkanes
4.2.2(a)(i) Hydrolysis by aqueous alkali
4.2.2(a)(ii) Comparing hydrolysis rates with silver nitrate
4.2.2(b) Nucleophiles
4.2.2(c) Nucleophilic substitution mechanism
4.2.2(d) Hydrolysis rates and carbon–halogen bond enthalpies
4.2.2(e) CFCs, radicals and ozone depletion
4.2.2(e)(i) Forming halogen radicals
4.2.2(e)(ii) Radicals catalysing ozone breakdown
4.2.3 Organic synthesis
4.2.3(a) Organic practical techniques
4.2.3(a)(i) Quickfit apparatus for distillation and reflux
4.2.3(a)(ii) Preparing and purifying an organic liquid
4.2.3(b) Molecules with several functional groups
4.2.3(b)(i) Identifying functional groups
4.2.3(b)(ii) Predicting properties and reactions
4.2.3(c) Two-stage synthetic routes
4.2.4 Analytical techniques
4.2.4(a) Infrared radiation and bond vibration
4.2.4(b) Infrared absorption by greenhouse gases
4.2.4(c) Identifying compounds from infrared spectra
4.2.4(c)(i) Alcohols from O–H absorption
4.2.4(c)(ii) Aldehydes and ketones from C=O absorption
4.2.4(c)(iii) Carboxylic acids from C=O and O–H absorption
4.2.4(d) Interpreting infrared spectra with data
4.2.4(e) Infrared in pollution monitoring and breathalysers
4.2.4(f) Molecular ion peak and molecular mass
4.2.4(g) Fragmentation peaks in mass spectra
4.2.4(h) Deducing structures from analytical data
4.2.4(h)(i) Elemental analysis
4.2.4(h)(ii) Mass spectra
4.2.4(h)(iii) IR spectra

5d How Science Works (HSW)

HSW1 Theories and models to explain science
HSW2 Posing questions and presenting scientific arguments
HSW3 Methods, including ICT, to answer scientific questions
HSW4 Experimental work and risk management
HSW5 Analysing data, correlation and causation
HSW6 Evaluating methods, evidence and data
HSW7 How scientific knowledge develops over time
HSW8 Communicating science with correct terminology
HSW9 Applications, benefits and risks of science
HSW10 Ethical issues in science
HSW11 Scientific community and validating knowledge
HSW12 Science in society's decision making