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Take 2 Chemistry
Resit Your A Level Chemistry

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Cambridge International  Chemistry

As a current examiner for Cambridge Assessment, I am very familiar with the CIE A-Level Chemistry course. The course is consists of Physical, Inorganic, and Organic Chemistry topics, and the syllabus is laid out as a set of detailed learning outcomes.

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The tutoring modules I’ve designed bring those learning outcomes together into clear, focused packages. 

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Choose the modules that match your needs. Each one focuses on a specific area of the CIE A-Level Chemistry syllabus and includes live one-to-one tuition, tailored revision materials, and digital worksheets.

You can purchase modules individually or in bundles. The number of lessons varies depending on the topic — you’ll see this listed for each one below.

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Once you’ve chosen your modules, simply add them to your cart and check out. You’ll get an email with your booking link, and from there you can schedule lessons at times that suit you.

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Alternatively, you can book a standalone bespoke 1-hour lesson.

Which Modules are on Each Paper?

Paper 4

Structured Questions

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Modules 1 - 37

AS & A2 Topics

Paper 5

Structured Questions

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Module 39

Revision of Planning, Analysis and Evaluation

Paper 3

Structured Questions and Practical Work

Module 38

Revision of Practical Work

Paper 2

Structured Questions

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Modules 1 - 22

AS Topics

Paper 1

Multiple Choice

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Modules 1 - 22

AS Topics

  • 5 x 1 hour lessons
    £200

    This module introduces the fundamental ideas of atomic theory and the structure of the atom. You’ll examine the subatomic particles — protons, neutrons, and electrons — and how their arrangement determines the properties of atoms and ions. We’ll explore isotopes and their impact on chemical and physical properties, and then move into a detailed study of electron configurations, quantum shells, and orbitals. The final part of the module focuses on ionisation energy: its definition, trends across the Periodic Table, and how successive ionisation energies reveal electronic structure.

    By the end of this module you will be able to:

    • describe the structure of the atom, including the distribution of mass and charge

    • distinguish between protons, neutrons, and electrons in terms of relative charge and mass

    • define and explain isotopes and their chemical/physical properties

    • write and interpret electronic configurations using full, shorthand, and box notation

    • sketch the shapes of s and p orbitals

    • define ionisation energy and construct equations for successive ionisation energies

    • explain and predict trends in ionisation energies across periods and down groups

    • use ionisation energy data to deduce electronic configuration and position in the Periodic Table


    CIE Syllabus Points (9701):

    • 1.1 Particles in the atom and atomic radius

    • 1.2 Isotopes

    • 1.3 Electrons, energy levels and atomic orbitals

    • 1.4 Ionisation energy

  • 5 x 1 hour lessons
    £200


    This module builds the quantitative toolkit you’ll use across the whole course. We start from relative masses (u, Ar, Mr) and the mole/Avogadro constant, then turn these ideas into fluent formula writing and balanced equations (including ionic). You’ll apply them to real calculations: reacting masses, gas volumes and solution concentrations, with careful attention to limiting reagent, percentage yield and significant figures. We also cover hydrates and water of crystallisation so you can deduce formulas from practical data.


    By the end of this module you will be able to:

    • define the unified atomic mass unit and use Ar, Mr and relative isotopic mass in calculations

    • define the mole in terms of the Avogadro constant and convert between amount, mass and volume

    • write correct formulas for ionic compounds (including common polyatomic ions and oxidation numbers)

    • write and balance full equations and ionic equations (excluding spectator ions), with correct state symbols

    • define and use empirical and molecular formula; calculate one from the other using data

    • understand and use the terms anhydrous, hydrated and water of crystallisation; determine x in MxH2O from experimental results

    • perform stoichiometric calculations involving reacting masses, gas volumes and solution concentrations

    • identify the limiting reagent, calculate theoretical yield and percentage yield, and present answers to an appropriate number of significant figures

    • deduce stoichiometric relationships from calculation outcomes

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    CIE Syllabus Points (9701):

    • 2.1 Relative masses of atoms and molecules

    • 2.2 The mole and the Avogadro constant

    • 2.3 Formulae

    • 2.4 Reacting masses and volumes (of solutions and gases)

  • 6 x 1 hour lessons
    £240

    This module builds a rigorous picture of how atoms bond and how bonding determines structure and properties. You’ll start with electronegativity and bond type, then cover ionic, metallic, covalent and coordinate (dative) bonding, including σ/π bonds and hybridisation. We then use VSEPR to predict shapes and angles, and finish with intermolecular forces and accurate dot-and-cross representations (including expanded octets and odd-electron species).

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    By the end of this module you will be able to:

    • define electronegativity, explain its trends, and use it to predict bond type, bond polarity and molecular dipoles

    • describe and represent ionic bonding; relate lattice structure to melting point, solubility and conductivity

    • define metallic bonding and relate delocalised electrons to conductivity and malleability

    • describe covalent and coordinate (dative) bonding with correct dot-and-cross diagrams and examples

    • explain σ and π bonding via orbital overlap; use sp, sp², sp³ hybridisation to account for shapes and bonding

    • apply VSEPR to state and predict molecular shapes and bond angles for the required examples and analogous ions

    • describe intermolecular forces (id-id/London, pd-pd, hydrogen bonding), and use them to explain trends in b.p./m.p., solubility, surface tension and the anomalies of water

    • produce accurate dot-and-cross diagrams for required species, including expanded octets and odd-electron species

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    CIE Syllabus Points (9701):

    • 3.1 Electronegativity and bonding

    • 3.2 Ionic bonding

    • 3.3 Metallic bonding

    • 3.4 Covalent bonding and coordinate (dative covalent) bonding

    • 3.5 Shapes of molecules

    • 3.6 Intermolecular forces, electronegativity and bond properties

    • 3.7 Dot-and-cross diagrams

  • 4 x 1 hour lessons
    £160

    This module links particle models to measurable properties of gases and solids. First, you’ll develop fluency with the ideal gas equation and see how molecular collisions give rise to gas pressure and why real gases deviate from ideal behaviour. Then we switch to solids, comparing giant ionic, simple molecular, giant molecular, and giant metallic lattices, and explaining how bonding and structure control melting point, electrical conductivity and solubility. You’ll finish by deducing structure type from experimental information.

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    By the end of this module you will be able to:

    • explain gas pressure in terms of molecule–wall collisions

    • state the assumptions for an ideal gas (zero particle volume, no intermolecular attractions) and apply pV=nRT in calculations, including determining Mr

    • describe lattice structures of crystalline solids: giant ionic (e.g. NaCl, MgO), simple molecular (iodine, C₆₀, ice), giant molecular (SiO₂, graphite, diamond) and giant metallic (copper)

    • explain trends in melting/boiling point, conductivity, and solubility from bonding and structure

    • deduce the bonding/structure type of an unknown from given data

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    CIE Syllabus Points (9701):

    • 4.1 The gaseous state: ideal and real gases and pV=nRT

    • 4.2 Bonding and structure

  • 5 x 1 hour lessons
    £200

    This module builds a solid thermochemistry toolkit. You’ll define enthalpy changes, use standard-state conventions, and interpret reaction pathway diagrams. We’ll practise calorimetry (including q=mcΔT), use bond energy data, and then apply Hess’s Law to construct energy cycles and calculate enthalpy changes that can’t be measured directly.

     

    By the end of this module you will be able to:

    • distinguish exothermic and endothermic processes and the sign of ΔH

    • draw and interpret reaction pathway diagrams (activation energy and ΔH)

    • define and use standard conditions (298 K, 101 kPa shown by ⦵)

    • define and use ΔHr, ΔHf, ΔHc, ΔHneut

    • perform calorimetry calculations using q=mcΔT

    • use bond energies (noting averages vs exact values) to estimate ΔHr

    • apply Hess’s Law to construct simple energy cycles and calculate unknown enthalpy changes

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    CIE Syllabus Points (9701):

    • 5.1 Enthalpy change, ΔH

    • 5.2 Hess’s Law

  • 3 x 1 hour lessons
    £120

    This module nails the language and bookkeeping of redox. You’ll calculate oxidation numbers confidently, use them to balance equations, and describe oxidation, reduction and disproportionation in terms of electron transfer and changes in oxidation number. We’ll also pin down what we mean by oxidising and reducing agents and how to use Roman numerals correctly in names and formulas.

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    By the end of this module you will be able to:

    • calculate oxidation numbers for elements in ions and compounds

    • use changes in oxidation numbers to help balance chemical equations

    • define and apply the terms redox, oxidation, reduction, and disproportionation in electron-transfer terms

    • identify oxidising and reducing agents in reactions

    • use Roman numerals to indicate the magnitude of an element’s oxidation number in names/formulas

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    CIE Syllabus Points (9701):

    • 6.1 Redox processes: electron transfer and changes in oxidation number (oxidation state).

  • 5 x 1 hour lessons
    £200

    This module explores both the principles of chemical equilibrium and the Brønsted–Lowry theory of acids and bases. You will learn what it means for a reaction to be reversible and how dynamic equilibrium is established in a closed system. Le Chatelier’s principle is introduced to explain qualitatively how equilibrium responds to changes in concentration, temperature, pressure or the presence of a catalyst. You will also work quantitatively with equilibrium constants, writing expressions for Kc and Kp, using mole fractions and partial pressures, and calculating equilibrium concentrations. Industrial applications such as the Haber and Contact processes highlight the importance of equilibrium in large-scale production.

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    The module also develops your understanding of acids and bases through the Brønsted–Lowry model. You will become familiar with the common acids and alkalis, distinguish between strong and weak acids and bases in terms of dissociation, and investigate their characteristic properties. Neutralisation, salt formation, and the interpretation of pH titration curves are included, along with choosing suitable indicators for different acid–base titrations.

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    By the end of this module you will be able to:

    • explain reversible reactions and dynamic equilibrium in a closed system

    • apply Le Chatelier’s principle to predict qualitative shifts in equilibrium

    • write and use expressions for Kc and Kp, including mole fraction and partial pressure

    • calculate equilibrium quantities from given data

    • state how equilibrium constants are affected by changes in conditions

    • describe the operating conditions of the Haber and Contact processes

    • state formulas for common acids and alkalis

    • describe acids and bases using the Brønsted–Lowry theory

    • distinguish between strong and weak acids and bases and explain their behaviour

    • describe neutralisation and the formation of salts

    • sketch and interpret pH titration curves and select appropriate indicators

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    CIE Syllabus Points (9701):
    7.1 Chemical equilibria: reversible reactions, dynamic equilibrium
    7.2 Brønsted–Lowry theory of acids and bases

  • 3 x 1 hour lessons
    £120

    This module introduces the principles of reaction rates and the factors that affect them. You will learn how to define and measure the rate of a reaction, and how to explain differences in rate in terms of collisions between particles. The effects of concentration and pressure are considered qualitatively through the frequency of effective collisions, and you will use experimental data to calculate rates of reaction.

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    The module also explores the effect of temperature on rate through the concepts of activation energy and the Boltzmann distribution. You will learn how to define activation energy, sketch and interpret the distribution curve, and explain qualitatively how changing temperature alters the rate of reaction.

    Finally, you will study catalysis in both homogeneous and heterogeneous systems. You will see how catalysts provide an alternative reaction pathway with lower activation energy, interpret this effect using the Boltzmann distribution, and construct reaction pathway diagrams to compare catalysed and uncatalysed reactions.

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    By the end of this module you will be able to:

    • define and use the terms rate of reaction, frequency of collisions, effective and non-effective collisions

    • explain qualitatively how changes in concentration and pressure affect rate

    • use experimental data to calculate reaction rates

    • define activation energy and explain its significance

    • sketch and interpret the Boltzmann distribution curve

    • explain the effect of temperature on reaction rate in terms of both collision frequency and the Boltzmann distribution

    • explain the role of a catalyst in providing an alternative pathway of lower activation energy

    • interpret the catalytic effect using the Boltzmann distribution

    • construct and interpret reaction pathway diagrams for catalysed and uncatalysed reactions

     

    CIE Syllabus Points (9701):
    8.1 Rate of reaction
    8.2 Effect of temperature on reaction rates and the concept of activation energy
    8.3 Homogeneous and heterogeneous catalysts

  • 3 x 1 hour lessons
    £120

    This module explores the trends and periodicity in both physical and chemical properties across the Periodic Table, with particular focus on the elements of Period 3. You will study how atomic radius, ionic radius, melting point and electrical conductivity vary across the period, and explain these changes in terms of structure and bonding.

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    The chemical behaviour of the Period 3 elements is examined in detail, including their reactions with oxygen, chlorine and water. You will investigate the acid–base nature of their oxides and hydroxides, as well as the behaviour of their chlorides in water. These reactions are linked to trends in oxidation numbers, bonding, and electronegativity across the period.

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    The module also develops your ability to apply the principle of periodicity to predict the properties of unfamiliar elements. By recognising recurring trends, you will learn how to deduce the nature, position, or even the identity of an unknown element based on its chemical and physical properties.

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    By the end of this module you will be able to:

    • describe and explain the variation in atomic radius, ionic radius, melting point and electrical conductivity across Period 3

    • explain these variations in terms of bonding and structure

    • describe and write equations for the reactions of Period 3 elements with oxygen, chlorine and water

    • explain and compare the oxidation numbers of oxides and chlorides across the period

    • describe and write equations for the reactions of Period 3 oxides with water and explain the likely pHs produced

    • describe and explain the acid–base behaviour of oxides and hydroxides, including amphoteric behaviour

    • describe and explain the reactions of Period 3 chlorides with water and the likely pHs of the solutions

    • explain these chemical trends in terms of bonding and electronegativity

    • suggest the bonding type in oxides and chlorides from their observed properties

    • predict the properties of unfamiliar elements using periodicity

    • deduce the possible position and identity of an unknown element from given data

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    CIE Syllabus Points (9701):
    9.1 Periodicity of physical properties of the elements in Period 3
    9.2 Periodicity of chemical properties of the elements in Period 3
    9.3 Chemical periodicity of other elements

  • 3 x 1 hour lessons
    £120

    This module covers the properties and trends of the Group 2 metals (magnesium to barium) and their compounds. You will study their characteristic reactions, including with oxygen, water, and dilute acids, and explore how their oxides, hydroxides, and carbonates behave in different reactions.

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    You will also investigate the thermal decomposition of Group 2 nitrates and carbonates, and the trend in their thermal stability down the group. The solubility patterns of Group 2 hydroxides and sulfates are considered, and you will learn how to explain and predict these trends in terms of periodic behaviour.

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    By the end of this module you will be able to:

    • describe and write equations for the reactions of Group 2 metals with oxygen, water, and dilute hydrochloric and sulfuric acids

    • describe and write equations for the reactions of Group 2 oxides, hydroxides, and carbonates with water and dilute acids

    • describe and write equations for the thermal decomposition of Group 2 nitrates and carbonates, and explain the trend in thermal stability

    • describe and predict the physical and chemical trends in Group 2 metals and their compounds

    • state and explain the variation in solubility of Group 2 hydroxides and sulfates

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    CIE Syllabus Points (9701):
    10.1 Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

  • 3 x 1 hour lessons
    £120

    This module examines the physical and chemical properties of the halogens (chlorine, bromine, iodine) and their compounds. You will study observable trends, such as colour, volatility, and bond strength, and explain these in terms of intermolecular forces and bonding.

    The chemical behaviour of the halogens is explored through their role as oxidising agents, their reactions with hydrogen, and the stability of the hydrogen halides. You will also investigate the reducing ability of halide ions and their key reactions, including with silver ions and concentrated sulfuric acid.

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    Finally, the module considers chlorine’s reactions with cold and hot aqueous sodium hydroxide, highlighting disproportionation, and its important application in water purification.

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    By the end of this module you will be able to:

    • describe the colours and volatility trend of chlorine, bromine, and iodine

    • explain the trend in halogen bond strengths and their effect on volatility and stability

    • interpret volatility in terms of instantaneous dipole–induced dipole forces

    • describe and compare the oxidising ability of the halogens

    • describe and explain their reactions with hydrogen and the relative stabilities of hydrogen halides

    • describe the reducing power of halide ions and their reactions with aqueous silver ions and concentrated sulfuric acid

    • describe and interpret disproportionation reactions of chlorine with cold and hot aqueous sodium hydroxide

    • explain the role of chlorine in water purification, including the formation of HOCl and ClO⁻ as active species

     

    CIE Syllabus Points (9701):
    11.1 Physical properties of the Group 17 elements
    11.2 The chemical properties of the halogen elements and the hydrogen halides
    11.3 Some reactions of the halide ions
    11.4 The reactions of chlorine

  • 2 x 1 hour lessons
    £80

    This module explores the chemistry of nitrogen and sulfur, focusing on their bonding, reactions, and environmental impact. You will examine the unreactive nature of nitrogen gas, linking this to its strong triple bond and lack of polarity. The acid–base behaviour of ammonia is covered, including its basicity, the formation of the ammonium ion, and the displacement of ammonia from its salts.

    The environmental chemistry of nitrogen oxides is also studied, from their natural and man-made sources to their removal from car exhaust gases using catalytic converters. You will learn how nitrogen oxides contribute to photochemical smog (through the formation of PAN) and acid rain, both directly and by catalysing the oxidation of sulfur dioxide.

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    By the end of this module you will be able to:

    • explain the lack of reactivity of nitrogen in terms of bond strength and polarity

    • describe and explain the basicity of ammonia using Brønsted–Lowry theory

    • describe the structure and formation of the ammonium ion

    • explain how ammonia is displaced from its salts in acid–base reactions

    • describe natural and man-made sources of nitrogen oxides and their catalytic removal from exhaust gases

    • explain the role of nitrogen oxides in photochemical smog formation and acid rain production

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    CIE Syllabus Points (9701):
    12.1 Nitrogen and sulfur

  • 4 x 1 hour lessons
    £160

    This module introduces the foundations of organic chemistry at AS Level. You will begin by learning the conventions used to represent organic structures and the main functional groups, including alkenes, halogenoalkanes, alcohols, aldehydes, ketones, carboxylic acids, esters, amines, and nitriles. The module covers how to write and interpret general, structural, displayed and skeletal formulas, as well as applying systematic nomenclature to name compounds up to six carbons in length.

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    You will then explore the key types of organic reactions and mechanisms, including free-radical substitution, electrophilic addition, nucleophilic substitution and addition, and the associated terminology such as nucleophile, electrophile, homolytic and heterolytic fission.

    The module also introduces the shapes of organic molecules and the concepts of σ and π bonding, as well as the idea of hybridisation (sp, sp², sp³). Finally, you will study isomerism, both structural (chain, positional, functional group) and stereoisomerism (geometrical and optical), and practise identifying isomers from molecular and structural formulas.

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    By the end of this module you will be able to:

    • recognise and use the conventions for representing organic compounds and functional groups

    • interpret and use different types of formulas and apply systematic nomenclature

    • define and apply key terminology for organic reactions and mechanisms

    • describe and explain molecular shape and bonding in organic molecules

    • identify and describe structural, geometrical, and optical isomerism

    • deduce possible isomers for given molecular formulas

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    CIE Syllabus Points (9701):
    13.1 Formulas, functional groups and naming of organic compounds
    13.2 Characteristic organic reactions
    13.3 Shapes of organic molecules; σ and π bonds
    13.4 Isomerism: structural isomerism and stereoisomerism

  • 5 x 1 hour lessons
    £200

    This module explores the chemistry of alkanes and alkenes. You will study how alkanes are produced by hydrogenation and cracking, and their characteristic reactions, including combustion and free-radical substitution with halogens. The mechanism of free-radical substitution is introduced through initiation, propagation and termination steps. The module also examines the relative unreactivity of alkanes, the environmental consequences of their combustion, and how catalytic converters reduce harmful emissions.

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    You will then move on to alkenes, focusing on their production by elimination, dehydration, and cracking, and their greater reactivity due to the C=C double bond. You will learn a wide range of alkene reactions, including hydrogenation, hydration with steam, addition of hydrogen halides and halogens, and oxidation with acidified potassium manganate(VII). Addition polymerisation is also covered, with ethene and propene as examples. Finally, you will investigate the mechanism of electrophilic addition and understand how inductive effects of alkyl groups explain the stability of carbocations and the outcome of Markovnikov addition.

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    By the end of this module you will be able to:

    • recall methods of producing alkanes and describe their reactions (combustion, free-radical substitution)

    • describe and explain the mechanism of free-radical substitution

    • explain the general unreactivity of alkanes and their lack of polarity

    • discuss the environmental impact of combustion products of alkanes and their catalytic removal

    • recall methods of producing alkenes and describe their reactions (hydrogenation, hydration, addition of HX, halogens, oxidation, polymerisation)

    • use aqueous bromine as a test for unsaturation

    • describe the mechanism of electrophilic addition in alkenes with examples

    • explain the stability of carbocations and the outcome of Markovnikov addition in terms of inductive effects

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    CIE Syllabus Points (9701):
    14.1 Alkanes
    14.2 Alkenes

  • 5 x 1 hour lessons
    £200

    This module examines the chemistry of halogenoalkanes, from their preparation to their characteristic reactions and mechanisms. You will study how halogenoalkanes are produced, including from free-radical substitution of alkanes, electrophilic addition to alkenes, and substitution reactions of alcohols with a range of reagents.

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    You will then classify halogenoalkanes as primary, secondary or tertiary, and explore their nucleophilic substitution reactions, such as formation of alcohols, nitriles, and amines. Their reactivity with aqueous silver nitrate is also used as a method of halogen identification. In addition, you will study elimination reactions of halogenoalkanes to produce alkenes.

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    The module introduces the mechanisms of nucleophilic substitution — SN1 and SN2 — and considers the influence of alkyl groups on carbocation stability and transition state structure. Finally, you will compare the reactivity of different halogenoalkanes, with particular reference to the relative bond strengths of C–X bonds.

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    By the end of this module you will be able to:

    • recall methods for preparing halogenoalkanes and the conditions required

    • classify halogenoalkanes into primary, secondary and tertiary

    • describe and carry out nucleophilic substitution reactions of halogenoalkanes with aqueous hydroxide, cyanide ions and ammonia

    • use reaction with aqueous silver nitrate in ethanol as a test to identify the halogen present

    • describe elimination reactions of halogenoalkanes with ethanolic NaOH

    • explain and represent the SN1 and SN2 mechanisms of nucleophilic substitution, including inductive effects of alkyl groups

    • state the typical mechanism followed by primary, secondary and tertiary halogenoalkanes

    • explain differences in halogenoalkane reactivity in terms of C–X bond strength

     

    CIE Syllabus Points (9701):
    15.1 Halogenoalkanes

  • 4 x 1 hour lessons
    £160

    This module focuses on the chemistry of alcohols. You will study the different ways in which alcohols can be prepared, including hydration of alkenes, oxidation of alkenes to diols, substitution of halogenoalkanes, and the reduction of aldehydes, ketones, and carboxylic acids. Hydrolysis of esters is also an important preparative method.

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    You will then explore the characteristic reactions of alcohols, such as combustion, substitution to form halogenoalkanes, reaction with sodium metal, and oxidation with acidified dichromate or manganate(VII) to carbonyl compounds or carboxylic acids. You will also learn how alcohols undergo dehydration to alkenes and esterification with carboxylic acids.

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    The classification of alcohols into primary, secondary and tertiary is introduced, along with their distinguishing reactions. You will also study the iodoform (tri-iodomethane) reaction as a test for the CH₃CH(OH)– group, and compare the acidity of alcohols with that of water.

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    By the end of this module you will be able to:

    • recall methods for producing alcohols and the reagents/conditions required

    • describe and explain the reactions of alcohols, including combustion, substitution, oxidation, dehydration, and esterification

    • classify alcohols as primary, secondary, or tertiary and state their characteristic reactions

    • use oxidation with acidified dichromate to distinguish between primary, secondary, and tertiary alcohols

    • deduce the presence of a CH₃CH(OH)– group using the tri-iodomethane (iodoform) test

    • explain the relative acidity of alcohols compared with water

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    CIE Syllabus Points (9701):
    16.1 Alcohols

  • 3 x 1 hour lessons
    £120

    This module explores the chemistry of aldehydes and ketones, focusing on their preparation, reactions, and identification. You will learn how aldehydes are formed by the oxidation of primary alcohols and how ketones are obtained from secondary alcohols, both using acidified dichromate or manganate(VII) with distillation.

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    You will study their characteristic reactions, including reduction back to alcohols using NaBH₄ or LiAlH₄, and nucleophilic addition with hydrogen cyanide to form hydroxynitriles. The mechanism of this nucleophilic addition is an important part of the module.

    A range of analytical tests are introduced for detecting and distinguishing carbonyl compounds, such as 2,4-DNPH to confirm the presence of a carbonyl group, Fehling’s and Tollens’ reagents to distinguish between aldehydes and ketones, and the iodoform (tri-iodomethane) test to identify the CH₃CO– group.

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    By the end of this module you will be able to:

    • recall how aldehydes and ketones are produced from the oxidation of primary and secondary alcohols

    • describe the reduction of aldehydes and ketones to alcohols

    • describe and explain the reaction of aldehydes and ketones with HCN, including the mechanism of nucleophilic addition

    • use 2,4-DNPH reagent to detect carbonyl compounds

    • distinguish between aldehydes and ketones using Fehling’s and Tollens’ reagents and ease of oxidation

    • use the tri-iodomethane test to identify the CH₃CO– group in aldehydes and ketones

     

    CIE Syllabus Points (9701):
    17.1 Aldehydes and ketones

  • 3 x 1 hour lessons
    £120

    This module covers the preparation, reactions and derivatives of carboxylic acids. You will learn how carboxylic acids can be synthesised by oxidation of primary alcohols and aldehydes under reflux, as well as by the hydrolysis of nitriles and esters. Their characteristic reactions are explored, including neutralisation, reaction with reactive metals and carbonates, esterification with alcohols, and reduction to primary alcohols using LiAlH₄.

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    You will also study esters, focusing on their preparation through condensation reactions with carboxylic acids and concentrated sulfuric acid as a catalyst, and their hydrolysis under both acidic and alkaline conditions with heating.

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    By the end of this module you will be able to:

    • recall the methods of producing carboxylic acids and the reagents and conditions required

    • describe the reactions of carboxylic acids with metals, alkalis, and carbonates

    • describe and explain esterification reactions with alcohols

    • describe the reduction of carboxylic acids to primary alcohols with LiAlH₄

    • recall how esters are prepared from alcohols and carboxylic acids

    • describe the hydrolysis of esters under acidic and alkaline conditions

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    CIE Syllabus Points (9701):
    18.1 Carboxylic acids
    18.2 Esters

  • 2 x 1 hour lessons
    £80

    This module introduces the chemistry of primary amines, nitriles, and hydroxynitriles. You will begin by studying how primary amines are prepared, focusing on their production from halogenoalkanes using ammonia in ethanol under pressure.

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    You will then explore nitriles, learning how they are synthesised from halogenoalkanes with potassium cyanide in ethanol and heat. The module also covers the preparation of hydroxynitriles by nucleophilic addition of hydrogen cyanide to aldehydes and ketones in the presence of a catalyst.

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    Finally, you will study the hydrolysis of nitriles under acidic or alkaline conditions (followed by acidification), producing carboxylic acids.

     

    By the end of this module you will be able to:

    • recall how primary amines are prepared from halogenoalkanes and ammonia in ethanol under pressure

    • recall how nitriles are prepared from halogenoalkanes using KCN in ethanol with heating

    • recall how hydroxynitriles are formed by the reaction of aldehydes and ketones with HCN/KCN under heat

    • describe the hydrolysis of nitriles to produce carboxylic acids

     

    CIE Syllabus Points (9701):
    19.1 Primary amines
    19.2 Nitriles and hydroxynitriles

  • 3 x 1 hour lessons
    £120

    This module introduces addition polymerisation and its importance. You will study how polymers such as poly(ethene) and poly(chloroethene) (PVC) are formed by the addition of small monomer units containing C=C double bonds. You will practise deducing the repeat unit of a polymer from its monomer, and identifying the monomer(s) from a section of a polymer chain.

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    The module also considers the environmental issues of polymer use, particularly the non-biodegradability of poly(alkenes) and the harmful products produced during their combustion.

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    By the end of this module you will be able to:

    • describe addition polymerisation with examples

    • deduce the repeat unit of an addition polymer from its monomer

    • identify the monomer(s) from a section of a polymer chain

    • explain the environmental problems caused by disposal of addition polymers

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    CIE Syllabus Points (9701):
    20.1 Addition polymerisation

  • 3 x 1 hour lessons
    £120

    This module develops your ability to link together different areas of organic chemistry. You will learn how to identify functional groups in organic molecules and use this knowledge to predict their properties and reactions. The module also trains you to plan multi-step synthetic routes to prepare target molecules, using reactions you have studied across the syllabus.

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    You will also practise analysing synthetic routes, identifying the type of reaction and reagents used in each step, and considering possible by-products. This skill is essential for understanding how organic chemists build complex molecules in both laboratory and industrial settings.

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    By the end of this module you will be able to:

    • identify functional groups in organic molecules and predict their reactions

    • devise multi-step synthetic routes using reactions from the syllabus

    • analyse given synthetic routes, stating the type of reaction, reagents used, and possible by-products

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    CIE Syllabus Points (9701):
    21.1 Organic synthesis

  • 3 x 1 hour lessons
    £120

    This module introduces two key techniques for identifying and analysing chemical compounds: infrared (IR) spectroscopy and mass spectrometry. You will learn how IR spectroscopy can be used to identify functional groups in molecules by analysing their characteristic absorption peaks.

    ​

    You will also study how mass spectrometry provides information about isotopic abundances, relative atomic masses, molecular mass, and structural features of organic molecules. This includes interpreting molecular ion peaks, recognising simple fragmentation patterns, and using isotopic peaks ([M+1]⁺ and [M+2]⁺) to deduce the presence of carbon, bromine, or chlorine atoms.

    ​

    By the end of this module you will be able to:

    • interpret IR spectra of simple molecules to identify functional groups

    • analyse mass spectra to determine isotopic abundances and relative atomic mass

    • calculate relative atomic mass from isotope data

    • deduce molecular mass from the molecular ion peak

    • suggest likely fragments from simple mass spectra

    • calculate the number of carbon atoms in a compound using the [M+1]⁺ peak

    • identify bromine and chlorine atoms from [M+2]⁺ peaks

    ​

    CIE Syllabus Points (9701):
    22.1 Infrared spectroscopy
    22.2 Mass spectrometry

  • 6 x 1 hour lessons
    £240

    This module extends your study of energetics into lattice energies, enthalpies of solution and hydration, entropy, and Gibbs free energy. You will learn how to define and use key enthalpy terms, explain the factors affecting them, and carry out calculations with energy cycles.

    You will construct and interpret Born–Haber cycles for ionic solids, use them to calculate lattice energies, and explain how ionic charge and radius influence their magnitude. The module also covers enthalpies of hydration and solution, using energy cycles to link these quantities to lattice energy.

    ​

    You will then explore entropy as a measure of disorder in a system, predicting and explaining the sign of entropy changes during changes of state, temperature changes, and reactions involving gases. You will calculate entropy changes using standard entropy data.

    Finally, the module introduces Gibbs free energy as the criterion for feasibility. You will learn to use the equation ΔG = ΔH – TΔS, perform calculations, and predict how temperature affects the feasibility of reactions.

    ​

    By the end of this module you will be able to:

    • define and use the terms enthalpy change of atomisation, lattice energy, first electron affinity, enthalpy change of hydration, and enthalpy change of solution

    • explain trends in electron affinity across Groups 16 and 17

    • construct and use Born–Haber cycles for ionic solids and carry out related calculations

    • explain qualitatively the effects of ionic charge and radius on lattice energy and enthalpy of hydration

    • construct and use energy cycles linking ΔHsol, ΔHlatt and ΔHhyd

    • define entropy as the number of possible arrangements of particles and their energies

    • predict and explain the sign of entropy changes in physical and chemical processes

    • calculate entropy changes for reactions using standard entropy data

    • use the Gibbs free energy equation ΔG = ΔH – TΔS to perform calculations and determine feasibility

    • predict the effect of temperature on feasibility using ΔH and ΔS values

    ​

    CIE Syllabus Points (9701):
    23.1 Lattice energy and Born–Haber cycles
    23.2 Enthalpies of solution and hydration
    23.3 Entropy change, ΔS
    23.4 Gibbs free energy change, ΔG

  • 6 x 1 hour lessons
    £240

    This module develops the principles and applications of electrochemistry. You will study electrolysis, learning how to predict which substances are liberated at the electrodes depending on whether the electrolyte is molten or aqueous, the position of ions in the redox series, and concentration effects. You will apply quantitative relationships, including Q=It, to calculate the charge passed, and use Faraday’s laws to determine the mass or volume of substances produced. The electrolytic determination of the Avogadro constant is also included.

    ​

    You will then move on to standard electrode potentials and the Nernst equation. You will learn how to define and measure standard electrode and cell potentials, describe the standard hydrogen electrode, and calculate standard cell potentials by combining half-cells. From this, you will deduce electrode polarity, predict the direction of electron flow, and assess the feasibility of redox reactions.

    The module also explores the use of E° values to compare the relative strengths of oxidising and reducing agents, and to construct balanced redox equations. You will study how electrode potentials vary with ion concentration, both qualitatively and quantitatively, using the Nernst equation. Finally, you will link electrochemistry to energetics through the relationship ΔG∘=−nFEcell

    ​

    By the end of this module you will be able to:

    • predict products of electrolysis for molten and aqueous electrolytes

    • apply the relationship F=Le between the Faraday constant, Avogadro’s constant, and electron charge

    • calculate charge, mass, or volume of substances produced in electrolysis using Q=It

    • describe the electrolytic determination of the Avogadro constant

    • define standard electrode potential and standard cell potential

    • describe the standard hydrogen electrode and methods for measuring electrode potentials

    • calculate a standard cell potential from two half-cell potentials

    • use electrode potentials to deduce electrode polarity, electron flow, and feasibility of reactions

    • deduce oxidising and reducing strengths from E° values

    • construct redox equations using half-equations

    • explain qualitatively how E varies with ion concentration and predict quantitatively using the Nernst equation

    • apply the equation ΔG∘=−nFEcell​

    ​

    CIE Syllabus Points (9701):
    24.1 Electrolysis
    24.2 Standard electrode potentials E°, standard cell potentials E°cell and the Nernst equation

  • 6 x 1 hour lessons
    £240

    This module develops your understanding of equilibria involving acids, bases, solubility, and partitioning. You will extend the Brønsted–Lowry theory by identifying conjugate acid–base pairs and applying mathematical definitions of pH, Ka, pKa, and Kw in calculations. You will calculate the pH of strong acids, strong alkalis, and weak acids, and learn how buffer solutions work, including their preparation, function, and role in controlling blood pH.

    ​

    You will also study solubility equilibria, defining and using the solubility product, Ksp. You will write Ksp expressions, perform calculations linking solubility and ion concentration, and apply the common ion effect to explain and calculate changes in solubility.

    The module then introduces partition coefficients, Kpc. You will learn how to calculate and use partition coefficients for solutes distributed between two solvents, and explain how solute and solvent polarity affect the values obtained.

    ​

    By the end of this module you will be able to:

    • define and identify conjugate acid–base pairs

    • use pH, Ka, pKa, and Kw in calculations

    • calculate pH for strong acids, strong alkalis, and weak acids

    • define buffer solutions, explain how they work, and describe their uses including pH control in blood

    • calculate the pH of a buffer solution from given data

    • define solubility product, Ksp, and write Ksp expressions

    • calculate Ksp from concentration data and vice versa

    • explain the common ion effect and perform related calculations

    • define partition coefficient, Kpc, and calculate it for solutes in two solvents

    • explain how polarity of solute and solvents influences partition coefficients

    ​

    CIE Syllabus Points (9701):
    25.1 Acids and bases
    25.2 Partition coefficients

  • 6 x 1 hour lessons
    £240

    This module extends your understanding of rates of reaction to include quantitative analysis and reaction mechanisms. You will learn the meaning of terms such as rate equation, order of reaction, overall order, rate constant, half-life, rate-determining step and intermediate. You will deduce orders of reaction from experimental data using methods such as initial rates, half-life, and graphical analysis of concentration–time or rate–concentration plots. You will also calculate rate constants using initial rates or half-life equations.

    The module also develops your ability to analyse multi-step reaction mechanisms, predicting the order from a given mechanism and identifying the rate-determining step, intermediates, and catalysts. You will link rate equations to mechanisms and propose mechanisms that match experimental evidence.

    ​

    Finally, you will study catalysis in detail. The operation of heterogeneous catalysts is explained in terms of adsorption, bond weakening, and desorption of products, with examples such as iron in the Haber process and platinum group metals in catalytic converters. Homogeneous catalysis is also covered, using examples such as oxides of nitrogen in atmospheric reactions and iron ions in the iodide/peroxodisulfate reaction.

    ​

    By the end of this module you will be able to:

    • define and use the terms rate equation, order of reaction, rate constant, half-life, rate-determining step, and intermediate

    • deduce orders of reaction from concentration–time data, rate–concentration graphs, or experimental methods

    • construct and use rate equations of the form rate = k[A]ᵐ[B]ⁿ

    • calculate rate constants using initial rates or half-life data

    • explain and calculate the half-life of first-order reactions

    • analyse multi-step mechanisms to deduce rate equations and identify intermediates, catalysts, and the rate-determining step

    • describe qualitatively how temperature affects the rate constant and reaction rate

    • explain the mode of action of heterogeneous catalysts using adsorption, bond weakening and desorption

    • describe the action of homogeneous catalysts, showing how they are used in one step and reformed later

     

    CIE Syllabus Points (9701):
    26.1 Simple rate equations, orders of reaction and rate constants
    26.2 Homogeneous and heterogeneous catalysts

  • 2 x 1 hour lessons
    £80

    This module examines the chemical periodicity of Group 2 elements (magnesium to barium) and their compounds. You will focus on the stability of their nitrates and carbonates, and how this changes down the group. The explanation is developed in terms of ionic radius and the polarising power of the cation acting on the large anions.

    ​

    You will also study the solubility trends of Group 2 hydroxides and sulfates, and explain these variations in terms of the balance between lattice energy and enthalpy of hydration. The link between solubility and enthalpy change of solution is emphasised.

    ​

    By the end of this module you will be able to:

    • describe and explain the trend in thermal stability of Group 2 nitrates and carbonates

    • explain how ionic radius affects the polarisation of large anions

    • describe and explain the variation in solubility of Group 2 hydroxides and sulfates

    • relate solubility trends to the enthalpy change of solution, lattice energy, and enthalpy of hydration

    ​

    CIE Syllabus Points (9701):
    27.1 Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

  • 6 x 1 hour lessons
    £240

    This module explores the distinctive properties of the transition elements from titanium to copper. You will define what is meant by a transition element, examine their characteristic properties such as variable oxidation states, catalytic activity, complex ion formation, and coloured compounds, and explain these in terms of their electronic structure.

    ​

    You will study the general chemical behaviour of transition elements, including ligand exchange, coordination numbers, and the shapes of complexes. The types of ligands are introduced, from monodentate to polydentate, with examples such as water, ammonia, chloride, ethanedioate, and EDTA⁴⁻. You will predict the formulas of complexes, construct redox equations, and use E° values to assess the feasibility of reactions. Quantitative redox work includes calculations with manganate(VII), iron(II), and iodide systems.

    ​

    The module also explains why transition metal complexes are coloured. You will study the splitting of degenerate d orbitals into two energy levels in different geometries, relate the size of ΔE to the frequency of absorbed light, and link this to the observed complementary colour. Examples include ligand exchange in copper(II) and cobalt(II) complexes.

    ​

    Finally, you will study stereoisomerism in transition metal complexes, including geometrical (cis/trans) and optical isomerism, and learn how to deduce overall polarity. The concept of stability constants (Kstab) is introduced, allowing you to calculate equilibrium values and explain ligand exchange in terms of stability.

    ​

    By the end of this module you will be able to:

    • define a transition element and explain their characteristic properties

    • sketch and describe d orbital shapes and explain variable oxidation states, catalysis, and complex formation

    • describe and explain ligand types, complex geometry, coordination number, and ligand exchange

    • construct redox equations, use E° values to predict feasibility, and carry out redox calculations with key systems

    • explain the origin of colour in transition metal complexes in terms of d orbital splitting and ΔE

    • describe the effect of ligands on ΔE and hence the colour observed

    • describe and deduce geometrical and optical isomerism in complexes

    • define and use stability constants, write Kstab expressions, and perform calculations

    • explain ligand exchange in terms of stability constants

    ​

    CIE Syllabus Points (9701):
    28.1 General physical and chemical properties of the first row of transition elements, titanium to copper
    28.2 General characteristic chemical properties of the first set of transition elements, titanium to copper
    28.3 Colour of complexes
    28.4 Stereoisomerism in transition element complexes
    28.5 Stability constants, Kstab

  • 4 x 1 hour lessons
    £160

    This module extends your study of organic chemistry into aromatic and more advanced functional groups. You will be introduced to arenes, halogenoarenes, phenols, acyl chlorides, secondary and tertiary amines, amides, and amino acids. The focus is on recognising and interpreting their structures using general, structural, displayed, and skeletal formulas, and applying systematic nomenclature to both aliphatic and aromatic compounds.

    ​

    You will also explore the characteristic organic reactions associated with these compounds, including electrophilic substitution in arenes and addition–elimination reactions.

    ​

    The module develops your understanding of the structure of benzene and related molecules. You will describe aromatic molecules in terms of sp² hybridisation, σ bonding, and delocalised π systems.

    ​

    Finally, you will study optical isomerism at A Level in more detail. This includes the properties of enantiomers, their effect on plane-polarised light, and their biological activity. You will also examine the pharmaceutical relevance of chirality, including the need to separate racemic mixtures and the use of chiral catalysts to produce single enantiomers.

    ​

    By the end of this module you will be able to:

    • identify and name advanced organic functional groups including arenes, halogenoarenes, phenols, acyl chlorides, amines, amides, and amino acids

    • use structural, displayed, skeletal, and general formulas for these classes of compounds

    • apply systematic nomenclature to simple aliphatic and aromatic molecules up to six carbons in length

    • describe electrophilic substitution and addition–elimination mechanisms in organic chemistry

    • explain the bonding and shape of benzene and other aromatic molecules in terms of sp² hybridisation and delocalised π systems

    • describe optical isomerism and explain the properties of enantiomers

    • use the terms optically active and racemic mixture correctly

    • explain the biological importance of chirality in drug molecules and the role of chiral catalysts

    ​

    CIE Syllabus Points (9701):
    29.1 Formulas, functional groups and the naming of organic compounds
    29.2 Characteristic organic reactions
    29.3 Shapes of aromatic organic molecules; σ and π bonds
    29.4 Isomerism: optical

  • 3 x 1 hour lessons
    £120

    This module focuses on the chemistry of arenes, using benzene and methylbenzene as key examples. You will study their major substitution reactions, including halogenation in the presence of aluminium halide catalysts, nitration with concentrated nitric and sulfuric acids, and Friedel–Crafts alkylation and acylation. You will also learn about oxidation of the side-chain to benzoic acid and hydrogenation of the benzene ring to cyclohexane.

    ​

    The mechanism of electrophilic substitution is examined in detail, with examples such as nitration and bromination of benzene. You will understand how delocalisation in the aromatic ring stabilises the system, explaining why substitution is favoured over addition.

    The module also explores reactivity patterns in substituted arenes. You will predict whether halogenation occurs in the side-chain or the ring depending on conditions, and recognise how substituents influence orientation in the ring (directing effects).

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    By the end of this module you will be able to:

    • describe the substitution reactions of benzene and methylbenzene (halogenation, nitration, Friedel–Crafts alkylation and acylation)

    • describe the oxidation of the side-chain of arenes to form benzoic acid

    • describe the hydrogenation of the benzene ring to cyclohexane

    • explain and represent the mechanism of electrophilic substitution in arenes

    • explain why substitution predominates over addition due to aromatic stabilisation

    • predict whether halogenation occurs in the ring or side-chain under different conditions

    • describe and explain the directing effects of substituents (–NH₂, –OH, –R, –NO₂, –COOH, –COR)

    ​

    CIE Syllabus Points (9701):
    30.1 Arenes

  • 2 x 1 hour lessons
    £80

    This module looks at the chemistry of halogenoarenes. You will learn how they are prepared through substitution reactions of arenes with chlorine or bromine in the presence of aluminium halide catalysts. Examples include the formation of chlorobenzene from benzene and the formation of 2-chloromethylbenzene and 4-chloromethylbenzene from methylbenzene.

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    You will also compare the reactivity of halogenoarenes with halogenoalkanes, using chlorobenzene and chloroethane as examples. The difference in reactivity is explained by the interaction between the halogen atom and the aromatic ring.

    ​

    By the end of this module you will be able to:

    • describe the preparation of halogenoarenes by substitution reactions with chlorine or bromine in the presence of a catalyst

    • explain the difference in reactivity between halogenoalkanes and halogenoarenes, with reference to chloroethane and chlorobenzene

     

    CIE Syllabus Points (9701):
    31.1 Halogen compounds

  • 4 x 1 hour lessons
    £160

    This module extends your study of hydroxy compounds to include both alcohols and phenols. You will look at the reaction of alcohols with acyl chlorides to form esters, using the preparation of ethyl ethanoate as an example.

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    You will then study the chemistry of phenol in detail. This includes its preparation from phenylamine via diazonium salts, and its characteristic reactions: neutralisation with bases, reaction with sodium metal, azo coupling in alkaline solution, nitration with dilute nitric acid, and bromination with aqueous bromine. The module also covers acidity, comparing phenol with ethanol and water, and explains why phenol undergoes nitration and bromination under milder conditions than benzene.

    ​

    Finally, you will examine the directing effects of the hydroxyl group in phenol, which guides substitution to the 2-, 4-, and 6-positions, and apply these ideas to other phenolic compounds such as naphthol.

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    By the end of this module you will be able to:

    • describe the esterification of alcohols with acyl chlorides, using ethyl ethanoate as an example

    • recall how phenol is prepared from phenylamine via diazonium salts

    • describe and explain the reactions of phenol with bases, sodium metal, and diazonium salts

    • describe and explain the nitration and bromination of phenol under mild conditions

    • explain the acidity of phenol and compare it with water and ethanol

    • explain why nitration and bromination of phenol occur more readily than with benzene

    • describe the directing effects of the hydroxyl group in phenol and apply this to other phenolic compounds

    ​

    CIE Syllabus Points (9701):
    32.1 Alcohols
    32.2 Phenol

  • 6 x 1 hour lessons
    £240

    This module develops your knowledge of aromatic and advanced reactions of carboxylic acids and their derivatives. You will study the preparation of benzoic acid by oxidation of alkylbenzenes with hot alkaline potassium manganate(VII) followed by acidification. The module also explores the conversion of carboxylic acids to acyl chlorides using reagents such as PCl₃, PCl₅ or SOCl₂, and the further oxidation of some carboxylic acids, including methanoic acid and ethanedioic acid. The relative acidities of carboxylic acids, phenols, alcohols, and chlorine-substituted carboxylic acids are compared and explained.

    ​

    You will also investigate esters, learning how they can be prepared from alcohols and acyl chlorides, with ethyl ethanoate and phenyl benzoate as examples.

    ​

    The chemistry of acyl chlorides is studied in depth. You will learn how they are prepared from carboxylic acids and study their characteristic reactions, including hydrolysis, esterification with alcohols and phenols, and formation of amides with ammonia or amines. The addition–elimination mechanism of these reactions is introduced, and the relative ease of hydrolysis of acyl chlorides, alkyl chlorides, and halogenoarenes is explained.

    ​

    By the end of this module you will be able to:

    • recall how benzoic acid is prepared from methylbenzene using alkaline KMnO₄ and acid

    • describe the conversion of carboxylic acids to acyl chlorides with PCl₃, PCl₅ or SOCl₂

    • describe the further oxidation of methanoic acid and ethanedioic acid

    • explain and compare the acidities of carboxylic acids, phenols, alcohols, and chlorine-substituted carboxylic acids

    • recall the preparation of esters from alcohols and acyl chlorides

    • recall the preparation of acyl chlorides from carboxylic acids

    • describe the reactions of acyl chlorides with water, alcohols, phenols, ammonia, and amines

    • explain these reactions in terms of the addition–elimination mechanism

    • compare the ease of hydrolysis of acyl chlorides, alkyl chlorides, and halogenoarenes

    ​

    CIE Syllabus Points (9701):
    33.1 Carboxylic acids
    33.2 Esters
    33.3 Acyl chlorides

  • 5 x 1 hour lessons
    £200

    This module expands on the chemistry of nitrogen-containing organic compounds, including amines, phenylamine, azo compounds, amides, and amino acids.

    ​

    You will begin with the preparation and reactions of primary and secondary amines, learning how they are formed from halogenoalkanes, amides, and nitriles. Their condensation with acyl chlorides to form amides is also covered, along with their basicity in aqueous solution.

    You will then study phenylamine, its preparation from benzene via nitration and reduction, and its characteristic reactions with bromine and nitrous acid. The relative basicities of aqueous ammonia, ethylamine, and phenylamine are compared. You will also be introduced to azo compounds, focusing on their preparation through diazonium coupling, the role of the azo group, and their use as dyes.

    The section on amides covers their preparation from acyl chlorides, their reactions with acids, alkalis, and reducing agents, and why they are much weaker bases than amines.

    ​

    Finally, the module examines amino acids, including their amphoteric nature, formation of zwitterions, peptide bond formation, and how electrophoresis can be used to separate amino acids and peptides according to their isoelectric points.

    ​

    By the end of this module you will be able to:

    • recall the preparation of primary and secondary amines from halogenoalkanes, amides, and nitriles

    • describe the condensation reactions of ammonia and amines with acyl chlorides

    • explain the basicity of aqueous amines

    • describe the preparation of phenylamine and its reactions with bromine and nitrous acid

    • compare the basicities of ammonia, ethylamine, and phenylamine

    • describe the formation and uses of azo compounds as dyes

    • recall the preparation of amides and describe their hydrolysis and reduction reactions

    • explain why amides are much weaker bases than amines

    • describe amino acids as amphoteric compounds, including zwitterion formation and isoelectric point

    • explain peptide bond formation and predict outcomes of electrophoresis for amino acids and peptides

     

    CIE Syllabus Points (9701):
    34.1 Primary and secondary amines
    34.2 Phenylamine and azo compounds
    34.3 Amides
    34.4 Amino acids

  • 2 x 1 hour lessons
    £80

    This module introduces condensation polymerisation and extends your understanding of polymers beyond addition reactions. You will study the formation of polyesters from diols and dicarboxylic acids (or dioyl chlorides), as well as from hydroxycarboxylic acids. You will also learn how polyamides are produced from diamines and dicarboxylic acids (or dioyl chlorides), from aminocarboxylic acids, and from amino acids through peptide bond formation.

    ​

    You will practise deducing the repeat unit of a condensation polymer from given monomers and identifying the monomer(s) from a polymer structure.

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    The module also covers how to predict the type of polymerisation that occurs from the structure of a monomer or pair of monomers, and how to deduce whether a given polymer results from addition or condensation polymerisation.

    Finally, you will study degradable polymers. You will recognise why poly(alkenes) are chemically inert and difficult to biodegrade, how some polymers can be degraded by light, and why polyesters and polyamides are biodegradable through hydrolysis reactions.

    ​

    By the end of this module you will be able to:

    • describe the formation of polyesters from diols and dicarboxylic acids/dioyl chlorides or hydroxycarboxylic acids

    • describe the formation of polyamides from diamines and dicarboxylic acids/dioyl chlorides, aminocarboxylic acids, or amino acids

    • deduce the repeat unit of a condensation polymer from given monomers

    • identify monomers from a section of a polymer chain

    • predict the type of polymerisation for given monomers or deduce it from a polymer structure

    • explain why poly(alkenes) are chemically inert and hard to biodegrade

    • recognise that some polymers can degrade under light

    • explain why polyesters and polyamides are biodegradable by hydrolysis

    ​

    CIE Syllabus Points (9701):
    35.1 Condensation polymerisation
    35.2 Predicting the type of polymerisation
    35.3 Degradable polymers

  • 3 x 1 hour lessons
    £120

    This final module brings together the whole of your organic chemistry knowledge. You will learn how to identify multiple functional groups in organic molecules and predict their properties and reactions using the reactions covered across the syllabus.

    You will also develop the skills to devise multi-step synthetic routes for preparing target molecules, drawing on a wide range of reactions. In addition, you will practise analysing given synthetic routes, identifying the types of reactions and reagents used at each stage, and considering possible by-products.

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    By the end of this module you will be able to:

    • identify functional groups in molecules and predict their properties and reactions

    • design multi-step synthetic pathways for preparing organic molecules

    • analyse synthetic routes, describing the type of reaction, reagents used, and likely by-products

    ​

    CIE Syllabus Points (9701):
    36.1 Organic synthesis

  • 5 x 1 hour lessons
    £200

    This module introduces modern techniques used to analyse and identify organic molecules.

    You will begin with thin-layer chromatography (TLC), learning the key terms such as stationary phase, mobile phase, solvent front, baseline, and Rf value. You will interpret Rf values and explain differences in terms of interactions with the stationary phase and solubility in the mobile phase.

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    Next, you will study gas–liquid chromatography (GLC), understanding how compounds separate based on their interactions with the stationary and mobile phases. You will interpret chromatograms to calculate percentage composition of mixtures, and explain retention times.

    The module then covers carbon-13 NMR spectroscopy, where you will learn to deduce the different carbon environments in a molecule, predict the number of peaks, and suggest possible structures.

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    Finally, you will explore proton (¹H) NMR spectroscopy in more depth. You will interpret spectra to deduce proton environments, relative numbers of protons, and splitting patterns using the n + 1 rule. You will learn how chemical shifts are measured against the TMS standard, the need for deuterated solvents, and how proton exchange with D₂O can be used to identify O–H and N–H groups.

    ​

    By the end of this module you will be able to:

    • describe TLC in terms of stationary and mobile phases, solvent front, baseline, and Rf values

    • calculate and interpret Rf values and explain differences in terms of solubility and stationary phase interactions

    • describe the principles of gas–liquid chromatography, including stationary and mobile phases and retention times

    • interpret chromatograms to determine percentage composition and explain retention times

    • analyse and interpret simple ¹³C NMR spectra to identify carbon environments and suggest structures

    • predict the number of peaks expected in a ¹³C NMR spectrum

    • analyse and interpret ¹H NMR spectra, using chemical shifts, peak areas, and splitting patterns to deduce structures

    • predict the chemical shifts and splitting patterns of protons in simple molecules

    • describe the role of TMS as a standard and the need for deuterated solvents

    • identify O–H and N–H protons using proton exchange with D₂O

    ​

    CIE Syllabus Points (9701):
    37.1 Thin-layer chromatography
    37.2 Gas / liquid chromatography
    37.3 Carbon-13 NMR spectroscopy
    37.4 Proton (¹H) NMR spectroscopy

  • 4 x 1 hour lessons
    £160

    This module is designed to prepare you thoroughly for Paper 3: Advanced Practical Skills. Although no laboratory experiments will be carried out in these sessions, you will work intensively with mock questions, example data, and sample results that reflect the full range of tasks you could face in the exam. The aim is to strengthen your confidence and exam technique for Paper 3, which must be sat at an exam centre offering laboratory facilities.

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    Over four lessons we will practise the three main assessed skills:

    ​

    1. Manipulation, Measurement and Observation

    • Understanding the expectations for accurate data collection in titrations, rates, gravimetric, thermometric, and gas volume experiments.

    • Recognising how to record precise burette and thermometer readings, with the correct degree of accuracy.

    • Deciding when to repeat readings, how to spot anomalies, and how to improve reliability.

    • Practising observational chemistry through mock qualitative analysis questions, including recording subtle changes in colour, solubility, and precipitate formation.

    • Applying confirmatory tests and selecting reagents to distinguish between ions.

    2. Presentation of Data and Observations

    • Laying out data in clear tables with correct units and headings.

    • Ensuring consistent precision across all measurements and observations.

    • Recording qualitative observations in clear scientific language (e.g. “pale green” vs “dark green”).

    • Drawing graphs from experimental data with appropriate scales, labelled axes, and best-fit lines or curves.

    • Displaying calculations step by step, with correct use of significant figures.

    3. Analysis, Conclusions and Evaluation

    • Interpreting trends and patterns in experimental results.

    • Performing all key exam-style calculations: means, concentrations, enthalpy changes, percentage errors, gradients of graphs, and molar ratios.

    • Drawing clear, evidence-based conclusions linked to experimental data.

    • Identifying sources of error (systematic vs random), stating percentage uncertainties, and suggesting improvements or modifications to increase accuracy.

    • Extending conclusions to evaluate hypotheses or predict outcomes of related experiments.

    4. Types of Practical Questions Covered

    We will use past paper data and custom questions to practise:

    • Quantitative experiments:

      • Titrations (acid–base, manganate(VII), thiosulfate/iodine).

      • Thermometric experiments (enthalpy changes, Hess’s Law).

      • Gravimetric experiments (mass loss/gain on heating).

      • Gas volume experiments (e.g. reaction of a carbonate with an acid).

      • Simple rates experiments (e.g. sodium thiosulfate + acid, measuring time for cloudiness).

    • Qualitative experiments:

      • Systematic analysis of unknown inorganic substances using the Qualitative Analysis Notes provided in the exam.

      • Tests for cations, anions, gases, and selected organic functional groups (Fehling’s, Tollens’, iodoform, acidified KMnO₄).

      • Writing detailed observation tables and forming logical conclusions.

     

    By the end of this module you will be able to:

    • Approach Paper 3 with confidence, knowing the full range of experimental techniques and question types.

    • Record and present data in a format that meets examiner expectations.

    • Carry out calculations with correct precision and significant figures.

    • Interpret and analyse experimental data to draw valid scientific conclusions.

    • Identify and explain sources of error, quantify uncertainties, and suggest realistic improvements.

    • Apply the Qualitative Analysis Notes to identify unknown ions, gases, and functional groups.

     

    CIE Syllabus Reference (9701):
    Paper 3 Advanced Practical Skills — manipulation, measurement and observation; presentation of data and observations; analysis, conclusions and evaluation.

  • 4 x 1 hour lessons
    £160

    This module is designed to prepare you for Paper 5: Planning, Analysis and Evaluation, the written examination that assesses higher-order experimental skills. Unlike Paper 3, this paper does not involve hands-on laboratory work during the exam, but success requires a deep understanding of practical chemistry and extensive laboratory experience from your A Level studies.

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    Across four lessons, you will practise with structured and extended-response questions that replicate the demands of Paper 5. You will learn how to design experiments, analyse complex data sets, and critically evaluate procedures — all core skills that examiners reward highly.

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    1. Planning Experimental Investigations

    • Identifying independent, dependent and control variables in experimental design.

    • Expressing aims clearly as testable hypotheses (in words or predicted graphs).

    • Designing safe, efficient, and reliable methods, including choice of apparatus, reagents, and measurement techniques.

    • Writing detailed methods with step-by-step instructions, supported by diagrams, flow charts or data tables.

    • Justifying how variables are controlled and why the procedure will generate valid results.

    • Incorporating risk assessment into plans (e.g. fume hoods, heat sources, corrosive chemicals, irritants).

    2. Method and Experimental Detail

    • Specifying suitable volumes, concentrations, and apparatus for accuracy and precision.

    • Describing how to record data in correctly headed tables and how results should be presented.

    • Demonstrating standard laboratory practices in written form: weighing by difference, heating to constant mass, concordancy of titres, preparation of standard solutions, taking extra readings near end-points.

    • Explaining how to vary the independent variable systematically and how to measure the dependent variable accurately.

    • Suggesting control experiments to confirm that the dependent variable is affected only by the independent variable.

    3. Analysis of Data

    • Practising calculation skills: means, gradients, intercepts, percentage errors, concentration values, molar ratios, enthalpy changes.

    • Using appropriate significant figures and units throughout.

    • Presenting data in suitable tables and graphs, following Paper 3 conventions (clear axes, best-fit lines, anomalies identified).

    • Handling equations of the form y = mx + c to extract constants from graphs.

    • Dealing with complex or “noisy” data to identify underlying trends and patterns.

    4. Drawing Conclusions

    • Linking data analysis to scientific explanation, showing how results support or refute hypotheses.

    • Providing detailed reasoning for conclusions, referencing chemical principles where appropriate.

    • Suggesting further predictions or extensions of the investigation.

    • Distinguishing between errors caused by limitations of method, incorrect use of apparatus, or natural variability in data.

    5. Evaluation

    • Identifying weaknesses and limitations in given experimental procedures.

    • Proposing improvements to accuracy and reliability (e.g. improved apparatus, extended range of values, more repeats).

    • Assessing whether data are valid and reliable enough to support a conclusion.

    • Discussing the impact of anomalous values and how to handle them.

    • Making evidence-based judgements about the confidence in results and conclusions.

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    By the end of this module you will be able to:

    • Plan safe, efficient, and valid experimental investigations in written form.

    • Express aims and hypotheses clearly, in both descriptive and graphical terms.

    • Design detailed methods with justified apparatus, reagents, and measurements.

    • Analyse data sets using calculations, tables, and graphs with correct precision.

    • Draw scientifically sound conclusions and extend them to new predictions.

    • Evaluate procedures critically, suggesting realistic improvements and assessing the reliability of data.

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    CIE Syllabus Reference (9701):
    Paper 5: Planning, Analysis and Evaluation — planning, method, analysis of data, drawing conclusions, evaluation.

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