Cambridge Assessment International Education (CAIE 5070) O-Level Chemistry Syllabus 2026–2028
O-Level Chemistry Syllabus 2026–2028
Topics & Exam Format
The Cambridge O-Level Chemistry (5070) syllabus develops fundamental chemistry knowledge, analytical problem solving, and rigorous laboratory skills. Valid for 2026–2028 examination series.
12 Core Topics Cambridge 5070 Paper 1–4 Structure Practical Skills Focus
In This Syllabus Guide
Complete Topic List12 core modules with practical outcomes
Detailed Learning OutcomesFull 5070 official syllabus breakdown
Exam Format & WeightingPaper 1–4 breakdown and AO percentages
2026–2028 Key UpdatesPractical skills and exam criteria focus
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Syllabus Overview
O-Level Chemistry Syllabus (2026–2028)
Based on the official Cambridge Assessment International Education (CAIE 5070) syllabus. These 12 core topics establish comprehensive theoretical foundations, stoichiometric problem solving, and analytical laboratory skills.
Topic 01
1. States of Matter
Solids, liquids, gases, diffusion mechanisms, kinetic particle theory, and heating/cooling curves.
Topic 02
2. Atoms, Elements & Compounds
Atomic structure, isotopes, and comprehensive bonding models: ionic lattices, covalent, and metallic structures.
Topic 03
3. Stoichiometry
The mole concept, reacting masses, molar gas volume (24 dm³), titration calculations, and empirical formulae.
Topic 04
4. Electrochemistry
Electrolysis of molten and aqueous electrolytes, selective ion discharge, half-equations, and hydrogen fuel cells.
Topic 05
5. Chemical Energetics
Exothermic and endothermic reactions, enthalpy changes (ΔH), reaction profile pathways, and bond energy calculations.
Topic 06
6. Chemical Reactions
Collision theory, factors governing reaction rates, dynamic equilibrium, Le Chatelier's principle, and redox processes.
Topic 07
7. Acids, Bases & Salts
Proton transfer definitions, pH scale, oxide classifications, and practical methods for preparing soluble and insoluble salts.
Topic 08
8. The Periodic Table
Periodic trends across periods, Group I alkali metals, Group VII halogens, transition metals, and noble gases.
Topic 09
9. Metals
The reactivity series, metal extraction in the blast furnace, rusting prevention, sacrificial protection, and alloys.
Topic 10
10. Chemistry of the Environment
Water purification, chemical fertilisers (NPK), atmospheric composition, air pollutants, and catalytic converters.
Topic 11
11. Organic Chemistry
Homologous series, structural isomerism, petroleum fractions, alkanes, alkenes, alcohols, carboxylic acids, and polymers.
Topic 12
12. Experimental Techniques
Precision apparatus, paper chromatography (Rf values), separation procedures, and qualitative tests for ions and gases.
Assessment Architecture
Exam Format (Cambridge 5070)
Candidates sit three examination components: Paper 1, Paper 2, and either Paper 3 (Practical Test) or Paper 4 (Alternative to Practical).
| Paper | Duration | Marks | Weighting | Format & Description |
|---|---|---|---|---|
| Paper 1: Multiple Choice | 1 hour | 40 marks | 30% | 40 compulsory multiple-choice questions testing core concepts and quick calculations across all 12 units. |
| Paper 2: Theory | 1 hour 45 mins | 80 marks | 50% | Short-answer and structured questions testing deep theoretical understanding, state symbols, and calculation workings. |
| Paper 3: Practical Test or Paper 4: Alternative to Practical | 1 hour 30 mins (Paper 3) 1 hour (Paper 4) | 40 marks | 20% | Paper 3 is hands-on laboratory testing; Paper 4 is written assessment evaluating experimental design, graph plotting, and qualitative salt analysis. |
Skills Distribution
Assessment Objectives (AO Weighting)
| Objective | Description | Overall Weighting | Exam Focus |
|---|---|---|---|
| AO1 | Knowledge with Understanding | 50% | Scientific phenomena, definitions, concepts, laws, and chemical apparatus functions. |
| AO2 | Handling Information and Problem Solving | 30% | Quantitative calculations, data translation across formats, hypothesising, and deducing trends. |
| AO3 | Experimental Skills and Investigations | 20% | Planning experiments, recording observations, evaluating anomalies, and reading precision scales. |
Curriculum Continuity
Key Features of the 2026–2028 Syllabus
Cambridge Assessment International Education maintains subject continuity while refining learning outcome clarity and practical assessment criteria.
Content Stability
The core theoretical frameworks remain stable compared to recent exam cycles, allowing complete continuity with proven Cambridge past papers from 2020 through 2025.
Refined Definitions & Clarity
Key scientific definitions and command terms have been sharpened for clarity, giving students exact guidelines on what examiners look for in Paper 2 descriptions.
Heightened Experimental Focus
Greater emphasis on qualitative analysis observations (specific precipitate colours, solubility in excess reagents) and accurate graph plotting in Papers 3 and 4.
Logical Topic Sequence
The 12-topic sequence retains its pedagogical flow: beginning with particle models, progressing through physical and inorganic chemistry, and culminating in organic synthesis.
Comprehensive Specifications
Detailed Learning Outcomes (Cambridge 5070)
Explore the exact learning outcomes mandated by Cambridge for each topic. Click any module to expand the full curriculum breakdown:
01 1. States of Matter
1.1 Solids, liquids and gases 1. State the distinguishing properties of solids, liquids and gases.
2. Describe the structures of solids, liquids and gases in terms of particle separation, arrangement and motion.
3. Describe and explain changes of state in terms of kinetic particle theory.
4. Interpret and explain heating and cooling curves.
5. Describe and explain the effects of temperature and pressure on the volume of a gas.
2. Describe the structures of solids, liquids and gases in terms of particle separation, arrangement and motion.
3. Describe and explain changes of state in terms of kinetic particle theory.
4. Interpret and explain heating and cooling curves.
5. Describe and explain the effects of temperature and pressure on the volume of a gas.
1.2 Diffusion 1. Describe and explain diffusion in terms of the kinetic particle theory.
2. Describe and explain the effect of relative molecular mass on the rate of diffusion.
2. Describe and explain the effect of relative molecular mass on the rate of diffusion.
02 2. Atoms, Elements and Compounds
2.1 Elements, compounds and mixtures Describe the differences between elements, compounds and mixtures.
2.2 Atomic structure and the Periodic Table State the relative charges and approximate relative masses of protons, neutrons and electrons. Define proton number and mass number. Deduce the electronic configuration of atoms with proton numbers 1 to 20, identifying group and period relationships.
2.3 Isotopes Define isotopes as atoms of the same element with the same number of protons but different numbers of neutrons. Calculate the relative atomic mass of an element from isotopic abundances.
2.4 Ionic bonding Describe the formation of ionic bonds between metallic and non-metallic elements. Describe the giant lattice structure of ionic compounds and deduce formulae using dot-and-cross diagrams.
2.5 Covalent bonding Describe the formation of covalent bonds by electron sharing. Construct dot-and-cross diagrams for molecules including H&sub2;, Cl&sub2;, H&sub2;O, CH&sub4;, NH&sub3;, and CO&sub2;. Contrast the physical properties of simple molecular compounds with giant lattices.
2.6 Giant covalent structures Describe the structures of graphite, diamond and silicon(IV) oxide ($SiO_2$). Relate their physical properties to structural arrangements and bonding.
2.7 Metallic bonding Describe metallic bonding as electrostatic attraction between positive ions in a giant lattice and delocalised electrons. Explain the electrical conductivity and malleability of metals.
03 3. Stoichiometry
3.1 Chemical formulae and equations Determine empirical and molecular formulae from analytical data. Deduce balanced chemical equations and ionic equations, including state symbols (s, l, g, aq).
3.2 Relative masses Define and calculate relative atomic mass ($A_r$) and relative molecular/formula mass ($M_r$).
3.3 The mole concept and quantitative calculations State that the mole is the unit of amount of substance containing the Avogadro number ($6.02 imes 10^{23}$) of particles. Calculate reacting masses, molar gas volume ($24 ext{ dm}^3$ at r.t.p.), solution concentrations ($ ext{g/dm}^3$ and $ ext{mol/dm}^3$), volumetric titration data, percentage yield, and percentage purity.
04 4. Electrochemistry
4.1 Electrolysis principles and applications Define electrolysis, cathode, anode, and electrolyte. Describe charge transfer through external conductors and electrolytes. Predict electrolysis products for molten lead(II) bromide, concentrated aqueous sodium chloride, dilute sulfuric acid, and aqueous copper(II) sulfate using inert and copper electrodes. Write balanced ionic half-equations for electrode reactions.
4.2 Hydrogen-oxygen fuel cells Describe the operating mechanism of a hydrogen-oxygen fuel cell. Compare the environmental and efficiency advantages of fuel cells with conventional internal combustion engines.
05 5. Chemical Energetics
5.1 Exothermic and endothermic reactions Describe exothermic and endothermic processes in terms of thermal energy transfer. Draw and interpret reaction pathway diagrams showing enthalpy change ($\Delta H$) and activation energy ($E_a$). Explain bond breaking as endothermic and bond forming as exothermic. Calculate overall enthalpy changes using average bond energy values.
06 6. Chemical Reactions
6.1 Physical and chemical changes Distinguish between physical and chemical changes based on reversibility and chemical bond reorganisations.
6.2 Rate of reaction and collision theory Define collision theory. Explain the effects of concentration, pressure, particle size/surface area, temperature, and catalysts on reaction rate. Evaluate experimental methods for measuring rates (gas collection, mass loss, colorimetry) and interpret rate graphs.
6.3 Reversible reactions and dynamic equilibrium Describe reversible reactions ($
ightleftharpoons$) and the concept of dynamic equilibrium in closed systems. Apply Le Chatelier's principle to predict the effect of changing temperature, pressure, and concentration on equilibrium yield in industrial processes (Haber process, Contact process).
6.4 Redox reactions Define oxidation and reduction in terms of oxygen gain/loss, electron transfer (OIL RIG), and oxidation number changes. Identify oxidising and reducing agents. Describe qualitative tests for redox agents using acidified potassium manganate(VII) and aqueous potassium iodide.
07 7. Acids, Bases and Salts
7.1 Characteristic properties of acids and bases Describe acids as proton donors ($H^+$) and bases as proton acceptors. Describe reactions of acids with metals, metal bases, and metal carbonates. Distinguish between strong and weak acids in terms of extent of ionisation.
7.2 Oxides classification Classify oxides as acidic, basic, neutral, or amphoteric ($Al_2O_3$, $ZnO$) based on their chemical reactions with acids and bases.
7.3 Preparation of salts and solubility rules State solubility rules for common salts. Describe laboratory preparations of soluble salts (using excess insoluble metal/oxide/carbonate or titration) and insoluble salts (precipitation). Describe crystallisation and filtration procedures.
08 8. The Periodic Table
8.1 Periodic arrangement Explain how elements are arranged in order of atomic number across periods and groups. Describe the change from metallic to non-metallic character across a period.
8.2 Group I: Alkali metals Describe Group I trends in melting points, density, and reactivity with water.
8.3 Group VII: Halogens Describe trends in physical state, colour, and reactivity of the halogens. Explain displacement reactions of halogens with other halide solutions.
8.4 Transition elements Describe general properties of transition metals: high density, high melting points, variable oxidation states, coloured compounds, and catalytic activity.
8.5 Noble gases Explain the chemical unreactivity of Group VIII/0 elements in terms of full electronic valence shells.
09 9. Metals
9.1 Physical and chemical properties of metals Describe physical properties (thermal and electrical conductivity, malleability, ductility) and reactions with water, steam, and dilute hydrochloric acid.
9.2 Uses of metals and alloys Relate the uses of aluminium, copper, brass, and stainless steel to their specific properties. Explain why alloys are harder than pure metals in terms of disrupted lattice layers.
9.3 Reactivity series Order metals (K, Na, Ca, Mg, Al, C, Zn, Fe, H, Cu, Ag, Au) based on reaction tendencies and displacement reactions. Explain why aluminium appears unreactive due to its oxide layer.
9.4 Corrosion and rust prevention State the conditions necessary for rusting (water and oxygen). Describe prevention methods: barrier protection, sacrificial protection, and galvanising.
9.5 Extraction of metals Describe the extraction of iron from hematite in the blast furnace (reactions of coke, limestone, and air). Describe the extraction of aluminium from bauxite by electrolysis in molten cryolite.
10 10. Chemistry of the Environment
10.1 Water testing and purification Describe chemical tests for water using anhydrous cobalt(II) chloride or anhydrous copper(II) sulfate. Describe domestic water treatment stages: sedimentation, filtration, and chlorination.
10.2 Fertilisers and nitrogen cycle Explain the role of NPK fertilisers in promoting plant growth. Describe the displacement of ammonia from its salts by warming with aqueous alkali.
10.3 Air quality and global climate State the composition of clean, dry air. Identify sources and harmful effects of common air pollutants ($CO$, $SO_2$, $NO_x$, unburnt hydrocarbons, particulates). Explain the greenhouse effect, global warming consequences, and the operation of catalytic converters.
11 11. Organic Chemistry
11.1 Formulae, functional groups and terminology Draw and interpret structural, displayed, and general formulae. Define functional group, homologous series, and structural isomerism.
11.2 Systematic IUPAC naming Name and draw structures for unbranched alkanes, alkenes, alcohols, carboxylic acids, and esters containing up to 4 carbon atoms.
11.3 Fuels and fractional distillation Describe petroleum as a mixture of hydrocarbons. Name the fractions (refinery gas, gasoline, naphtha, kerosene, diesel oil, fuel oil, bitumen) and relate boiling points and viscosity to molecular size.
11.4 Alkanes and alkenes Describe the unreactivity of alkanes except for combustion and photochemical substitution with chlorine. Describe cracking of petroleum fractions. Distinguish between saturated and unsaturated hydrocarbons using aqueous bromine. Describe addition reactions of alkenes with $H_2$, $Br_2$, and steam.
11.5 Alcohols, carboxylic acids and esters Describe the manufacture of ethanol by fermentation and catalytic hydration of ethene. Describe the oxidation of ethanol to ethanoic acid. Describe esterification of carboxylic acids with alcohols in the presence of an acid catalyst.
11.6 Polymers: Addition and condensation Describe addition polymerisation of alkenes (e.g. polyethene) and identify repeat units. Describe condensation polymerisation to form polyamides (nylon) and polyesters (PET). Identify proteins as natural polyamides. Discuss the environmental challenges of non-biodegradable plastics.
12 12. Experimental Techniques and Chemical Analysis
12.1 Experimental design and apparatus precision Select appropriate apparatus for measuring time, temperature, mass, and volume (burette, volumetric pipette, measuring cylinder, gas syringe).
12.2 Acid-base titrations Describe procedures for carrying out volumetric titrations using suitable indicators (methyl orange, thymolphthalein) to determine end-points.
12.3 Chromatography and separation techniques Describe paper chromatography, locating agents, and calculation of $R_f$ values. Describe separation methods: filtration, crystallisation, simple distillation, and fractional distillation.
12.4 Identification of ions and gases (Qualitative Analysis) Describe official tests and expected observations for:
• Anions: $CO_3^{2-}, Cl^-, Br^-, I^-, NO_3^-, SO_4^{2-}, SO_3^{2-}$.
• Aqueous Cations: $Al^{3+}, NH_4^+, Ca^{2+}, Cr^{3+}, Cu^{2+}, Fe^{2+}, Fe^{3+}, Zn^{2+}$ with aqueous $NaOH$ and aqueous $NH_3$.
• Flame Tests: $Li^+, Na^+, K^+, Ca^{2+}, Ba^{2+}, Cu^{2+}$.
• Gases: $NH_3, CO_2, Cl_2, H_2, O_2, SO_2$.
• Anions: $CO_3^{2-}, Cl^-, Br^-, I^-, NO_3^-, SO_4^{2-}, SO_3^{2-}$.
• Aqueous Cations: $Al^{3+}, NH_4^+, Ca^{2+}, Cr^{3+}, Cu^{2+}, Fe^{2+}, Fe^{3+}, Zn^{2+}$ with aqueous $NaOH$ and aqueous $NH_3$.
• Flame Tests: $Li^+, Na^+, K^+, Ca^{2+}, Ba^{2+}, Cu^{2+}$.
• Gases: $NH_3, CO_2, Cl_2, H_2, O_2, SO_2$.
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Frequently Asked Questions
Everything You Need to Know About Cambridge 5070
Detailed answers to the top 10 questions regarding the syllabus structure, examination preparation, and tuition methodology:
What is Cambridge O-Level Chemistry (Syllabus 5070)?
Cambridge O-Level Chemistry (5070) is an internationally recognised secondary school qualification developed by Cambridge Assessment International Education (CAIE). It assesses students aged 14 to 16 on fundamental theoretical principles, chemical calculations, and practical laboratory techniques.
What are the key differences between O-Level Chemistry (5070) and IGCSE Chemistry (0620)?
While both syllabuses share approximately 85% common subject matter, O-Level 5070 places a heavier emphasis on rigorous written derivations, structured theoretical justifications, and untiered examination papers. IGCSE 0620 offers Core vs. Extended tiering and frames questions with a broader contextual approach.
How many papers must a candidate take in the 5070 examination?
Every candidate sits three papers: Paper 1 (Multiple Choice, 40 marks, 30% weighting), Paper 2 (Theory, 80 marks, 50% weighting), and either Paper 3 (Practical Test, 40 marks, 20% weighting) or Paper 4 (Alternative to Practical, 40 marks, 20% weighting).
What is the difference between Paper 3 and Paper 4 in O-Level 5070?
Paper 3 is an in-person laboratory exam conducted under exam conditions using chemical reagents and glassware. Paper 4 is a written paper taken at a standard desk that evaluates the exact same experimental design, observation tables, and data analysis skills without requiring physical laboratory access.
Which examination series are available for Cambridge O-Level Chemistry?
Cambridge offers two main examination series annually: the May/June series and the October/November series. Depending on geographic zone and national school schedules, students can register through authorised Cambridge schools or the British Council.
Can private candidates take Cambridge O-Level Chemistry (5070)?
Yes. Independent or homeschooled students can register as Private Candidates through approved examination centres or the British Council, usually opting for Paper 4 (Alternative to Practical) to fulfill the practical examination requirement.
What is required to score an A* in Cambridge O-Level Chemistry?
Scoring an A* requires scoring consistently above 75–82% across all components depending on grade boundaries. Key factors include precision in state symbols, showing complete calculation workings in Paper 2 stoichiometry questions, and memorising exact qualitative analysis observations in Paper 4.
How does Cambridge O-Level Chemistry prepare students for A-Level Chemistry?
The mathematical and conceptual rigour of 5070 provides a direct foundation for Cambridge International AS & A-Level Chemistry (9701). Topics such as electronic configuration, mole calculations, energetics, and equilibria are expanded directly upon in Year 12.
How are online tutoring lessons conducted for international students?
Lessons take place via Zoom or Google Meet using high-definition interactive digital whiteboards and real-time past paper annotations. Schedules are accommodated flexibly across various time zones including the United Kingdom, United Arab Emirates, Singapore, and Pakistan.
What does the initial 40-minute diagnostic session involve?
The free 40-minute session involves evaluating the student's current grasp of core concepts (e.g. stoichiometry, bonding, acid-base chemistry) through selected diagnostic questions, followed by outlining a customised revision roadmap mapped to their examination date.
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