The West African Examinations Council has officially released the syllabus for all subjects for the upcoming examination. Every candidate preparing for the exam is expected to use this syllabus as a guide while studying.
The syllabus outlines all the topics, areas of concentration, and practical requirements that may be tested. By following it closely, you can focus your efforts on what truly matters, avoid wasting time on irrelevant topics, and prepare more effectively for the examination.
If you want to perform well, you mustn’t study blindly. Instead, use the syllabus to plan your reading, understand what is required, and revise strategically. Read this article carefully to see the full WAEC Chemistry syllabus, including all topics and practical areas you are expected to cover before the examination.
WAEC Syllabus for Chemistry
1.0 Introduction to Chemistry
This section introduces the basic foundation of chemistry, especially how measurements are made and how scientific investigations are carried out.
- Measurement of Physical Quantities
- Mass, length, time, temperature, and volume
- Use of SI units
- Significant figures
- Accuracy and precision in measurement
- Scientific Methods
- Observation
- Hypothesis
- Experimentation
- Formulation of laws and theories
2.0 Structure of the Atom
This topic explains the composition of matter and how atoms are structured.
- Basic Features of the Atom
- Proton, neutron and electron
- Atomic number and mass number
- Isotopes
- Atomic Theories and Models
- Dalton’s Atomic Theory and its limitations
- J.J. Thomson’s experiment
- Rutherford’s alpha scattering experiment
- Bohr’s atomic model
- Relative Atomic Mass
- Based on Carbon-12 scale
- Weighted average of isotopes
- Nature of Matter
- Atoms, molecules and ions as building blocks
- Physical and Chemical Changes
- Physical: melting, dissolution, magnetization
- Chemical: burning, rusting, decay
- Electron Configuration
- s, p and d orbitals
- Aufbau Principle
- Hund’s Rule
- Pauli Exclusion Principle
3.0 Separation Techniques for Mixtures
This section focuses on how mixtures can be separated into pure components.
- Types of Mixtures
- Solid-solid
- Solid-liquid
- Liquid-liquid
- Gas-gas
- Separation Methods
- Filtration
- Distillation
- Crystallization
- Chromatography
- Sublimation
- Magnetization
- Criteria for Purity
- Melting point (solids)
- Boiling point (liquids)
4.0 Periodic Chemistry
This topic explains how elements are arranged and how their properties change across the periodic table.
- Periodic Table Classification
- Metals, non-metals and metalloids
- Alkali metals, alkaline earth metals, transition metals
- Periodic Law and Trends
- Atomic size
- Ionic size
- Ionization energy
- Electron affinity
- Electronegativity
- Period 3 Elements (Na – Ar)
- Gradual change from metallic to non-metallic properties
- Transition from ionic to covalent bonding
- Reactions
- Acids with metals
- Metal oxides and trioxocarbonates (IV)
- Group 7 (Halogens)
- Fluorine, chlorine, bromine and iodine
- Physical states and reactivity
- Displacement reactions
- Reactions with water and alkalis
- Transition Metals (Sc – Zn)
- Variable oxidation states
- Formation of coloured compounds
- Catalytic properties
- Magnetic properties
5.0 Chemical Bonds
This section explains how atoms combine to form compounds.
- Types of Bonding
- Ionic bonding
- Covalent bonding
- Metallic bonding
- Properties of Compounds
- Solubility
- Electrical conductivity
- Melting and boiling points
- Naming of Compounds
- IUPAC system
- Covalent Bonding
- Simple and coordinate (dative) bonds
- Shapes of Molecules
- Linear (e.g. CO₂)
- Trigonal planar (e.g. BF₃)
- Tetrahedral (e.g. CH₄)
- Intermolecular Forces
- Hydrogen bonding
- Dipole-dipole forces
- van der Waals forces
6.0 Stoichiometry and Chemical Reactions
This topic deals with calculations and quantitative chemistry.
- Chemical Symbols and Formulae
- First 30 elements and common elements
- Empirical and molecular formula
- Chemical Equations
- Balancing equations
- Types:
- Combustion
- Synthesis
- Displacement
- Decomposition
- Ionic reactions
- Laws of Chemical Combination
- Law of conservation of mass
- Law of constant composition
- Law of multiple proportions
- Mole Concept
- Avogadro’s constant (6.02 × 10²³)
- Molar quantities
- Calculations
- Mass, volume and mole relationships
- Percentage composition and yield
- Solutions
- Types: acidic, basic and neutral
- Concentration:
- g/dm³
- mol/dm³
- Standard Solutions
- Primary and secondary standards
- Dilution
- Preparation of solutions by dilution
7.0 States of Matter
This section explains the physical states and behavior of matter.
- Kinetic Theory of Matter
- Explains particle movement in solids, liquids and gases
- Changes of State
- Melting, boiling, evaporation
- Relationship between order and randomness
- Diffusion
- In gases and liquids
- Brownian motion
- Gases
- Properties: compressibility, density
- Gas laws:
- Boyle’s law
- Charles’ law
- Avogadro’s law
- Dalton’s law
- Ideal gas equation (PV = nRT)
- Laboratory Preparation of Gases
- Hydrogen (H₂)
- Ammonia (NH₃)
- Carbon dioxide (CO₂)
- Liquids
- Properties: density, viscosity
- Vapour
- Vapour pressure
- Boiling point
- Solids
- Types:
- Ionic
- Covalent
- Metallic
- Types:
- Allotropes of Carbon
- Diamond
- Graphite
8.0 Energy and Energy Changes
This section focuses on heat and energy in chemical reactions.
- Energy Concepts
- Energy and enthalpy
- Types of Energy Changes
- Exothermic reactions
- Endothermic reactions
- Enthalpy Changes
- Combustion
- Dissolution
- Neutralization
WAEC Chemistry Practicals
| Section | Subsection | Item | Content / Requirement |
|---|---|---|---|
| (a) | General Skills & Principles | (i) | Measurement of mass and volume |
| (ii) | Preparation and dilution of standard solutions | ||
| (iii) | Filtration, recrystallisation and melting point determination | ||
| (iv) | Measurement of heats of neutralization and solutions | ||
| (v) | Determination of pH using colorimetry | ||
| (vi) | Determination of rates of reaction from concentration vs time curves | ||
| (vii) | Determination of equilibrium constants for simple systems |
| Section | Subsection | Item | Content / Requirement |
|---|---|---|---|
| (b) | Quantitative Analysis (Acid-Base Titration) | General | Use of standard acids, alkalis and indicators |
| Indicators | Methyl orange, methyl red, phenolphthalein | ||
| (i) | Determination of concentrations of acids and bases | ||
| (ii) | Determination of molar masses and water of crystallization | ||
| (iii) | Determination of solubility of acids and bases | ||
| (iv) | Determination of percentage purity | ||
| (v) | Analysis of Na₂CO₃/NaHCO₃ mixture (double indicator method) | ||
| (vi) | Stoichiometry of reactions | ||
| (b) | Quantitative Analysis (Redox Titration) | (i) | Acidic MnO₄⁻ with Fe²⁺ |
| (ii) | Acidic MnO₄⁻ with C₂O₄²⁻ | ||
| (iii) | I₂ in KI versus S₂O₃²⁻ | ||
| (d) | Qualitative Analysis | Cations (i) | NH₄⁺, Ca²⁺, Pb²⁺, Cu²⁺, Fe²⁺, Fe³⁺, Al³⁺, Zn²⁺ tested with NaOH(aq) and NH₃(aq) |
| Cations (ii) | Confirmatory tests for the above cations | ||
| Anions (iii) | Reaction with dilute HCl and concentrated H₂SO₄ on Cl⁻, SO₃²⁻, CO₃²⁻, NO₃⁻, SO₄²⁻ | ||
| Anions (iv) | Confirmatory tests for the above anions | ||
| (v) | Comparative study of halogens and displacement reactions | ||
| (vi) | Tests for gases: H₂, NH₃, CO₂, HCl, SO₂ | ||
| (vii) | Organic tests: Alkenes; Alkanols; Alkanoic acids; Sugars (Fehling’s and Benedict’s tests); Starch (iodine test); Proteins (Ninhydrin, Xanthoproteic, Biuret, Millon’s tests) |
Now that you have the full syllabus, make sure you actually use it while studying. Don’t just read through it and move on. Use it as your guide to plan your revision and focus on the topics that matter most.
It is also very important to practise with past questions. This will help you understand how questions are set, improve your speed, and boost your confidence before the examination.
If you found this helpful, share it with other candidates who are also preparing for the exam so they can benefit too.
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