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WAEC • Chemistry • Syllabus

WAEC Chemistry Syllabus for WASSCE 2027

The WAEC Chemistry syllabus is the list of topics WASSCE Chemistry questions are set from, with the exam body's notes on how far each topic goes. Use it as a revision checklist: pick a topic, read what it covers, then practise past questions on it until you can answer them in exam time.

Syllabus content © The West African Examinations Council. Source. Summaries marked “Our summary” are written by DeeepSolve.

WASSCE Chemistry exam scheme

Exam scheme

Papers
There shall be three papers - Papers 1, 2 and 3 all of which must be taken. Paper 1 and 2 shall be a composite paper to be taken at one sitting.
Paper 1
Will consist of fifty multiple choice objective questions drawn from Section A of the syllabus (i.e. the portion of the syllabus which is common to all candidates). Candidates will be required to answer all the questions within 1 hour for 50 marks.
Paper 2
Will be a 2-hour essay paper covering the entire syllabus and carrying 100 marks. The paper will be in two sections; Sections A and B.
Paper 2, Section A
Will consist of ten short structured questions drawn from the common portion of the syllabus (i.e. Section A of the syllabus). Candidates will be required to answer all the questions for 25 marks.
Paper 2, Section B
Will consist of two questions from the common portion of the syllabus (i.e. Section A of the syllabus) and two other questions from the section of the syllabus which is peculiar to the country of the candidate (i.e. either Section B or C of the syllabus). Candidates will be required to answer any three of the questions. Each question shall carry 25 marks.
Paper 3
This shall be a 2-hour practical test for school candidates or 1 hour 30 minutes alternative to practical work test for private candidates. Each version of the paper shall contain three compulsory questions and carry 50 marks. The questions shall be on the following aspects of the syllabus: one question on quantitative analysis; one question on qualitative analysis; the third question shall test candidates' familiarity with the practical activities suggested in their teaching syllabuses.
Continuous assessment
Details of the input into the continuous assessment shall be given by the Council.

Matter, atoms and chemical combination

Our summary: Measurement, atoms and electrons, separating mixtures, the periodic table, bonding, the mole, and the states of matter.

Introduction to chemistry

Our summary: How chemists measure things accurately and how the scientific method works.

Contents

  • Measurement of physical quantities
  • Scientific measurements and their importance in chemistryWAEC note: (1) Measurement of mass, length, time, temperature and volume. (2) Appropriate SI units and significant figures. (3) Precision and accuracy in measurement.
  • Scientific methodsWAEC note: Outline the scientific method to include: observation, hypothesis, experimentation, formulation of laws and theories.

Structure of the atom

Our summary: What atoms are made of, how the atomic models developed, and how electrons are arranged in shells and orbitals.

Contents

  • Gross features of the atomWAEC note: (1) Short account of Dalton's atomic theory and limitations, J.J. Thomson's experiment and Bohr's model of the atom. (2) Outline description of the Rutherford's alpha scattering experiment to establish the structure of the atom.
  • Atomic number/proton number, number of neutrons, isotopes, atomic mass, mass numberWAEC note: Meaning and representation in symbols of atoms and sub-atomic particles.
  • Relative atomic mass (Ar) and relative molecular mass (Mr) based on Carbon-12 scaleWAEC note: (1) Atomic mass as the weighted average mass of isotopes. Calculation of relative mass of chlorine should be used as an example. (2) Carbon-12 scale as a unit of measurement. Definition of atomic mass unit.
  • Characteristics and nature of matterWAEC note: Atoms, molecules and ions. Definition of particles and treatment of particles as building blocks of matter.
  • Particulate nature of matter: physical and chemical changesWAEC note: Explain physical and chemical changes with examples. Physical change - melting of solids, magnetization of iron, dissolution of salt etc. Chemical change - burning of wood, rusting of iron, decay of leaves etc.
  • Electron configurationWAEC note: Detailed electron configurations (s, p, d) for atoms of the first thirty elements.
  • OrbitalsWAEC note: Origin of s, p and d orbitals as sub-energy levels; shapes of s and p orbitals only.
  • Rules and principles for filling in electronsWAEC note: (1) Aufbau Principle, Hund's Rule of Maximum Multiplicity and Pauli Exclusion Principle. (2) Abbreviated and detailed electron configuration in terms of s, p, and d.

Standard separation techniques for mixtures

Our summary: The kinds of mixtures, the methods used to separate them, and how to tell when a substance is pure.

Contents

  • Classification of mixturesWAEC note: Solid-solid, solid-liquid, liquid-liquid, gas-gas with examples.
  • Separation techniquesWAEC note: Crystallization, distillation, precipitation, magnetization, chromatography, sublimation etc.
  • Criteria for purityWAEC note: Boiling point for liquids and melting point for solids.

Periodic chemistry

Our summary: How the periodic table is organised, the trends across periods and down groups, the halogens and the first transition metals.

Contents

  • Periodicity of the elementsWAEC note: Electron configurations leading to group and periodic classifications.
  • Different categories of elements in the periodic tableWAEC note: Metals, semi-metals, non-metals in the periodic table and halogens. Alkali metals, alkaline earth metals and transition metals as metals.
  • Periodic lawWAEC note: Explanation of the periodic law.
  • Periodic law: trends on periodic tableWAEC note: Periodic properties; atomic size, ionic size, ionization energy, electron affinity and electronegativity. Simple discrepancies should be accounted for in respect to beryllium, boron, oxygen and nitrogen.
  • Periodic law: periodic gradation of the elements in the third period (Na - Ar)WAEC note: (1) Progression from: (i) metallic to non-metallic character of element; (ii) ionic to covalent bonding in compounds. (2) Differences and similarities in the properties between the second and the third period elements should be stated.
  • Reactions between acids and metals, their oxides and trioxocarbonates (IV)WAEC note: (1) Period three metals (Na, Mg, Al). (2) Period four metals (K, Ca). (3) Chemical equations. (4) pH of solutions of the metallic oxides and trioxocarbonates.
  • Periodic gradation of elements in group seven, the halogens: F, Cl, Br and IWAEC note: Recognition of group variations noting any anomalies. Treatment should include the following: (a) physical states, melting and boiling points; (b) variable oxidation states; (c) redox properties of the elements; (d) displacement reaction of one halogen by another; (e) reaction of the elements with water and alkali (balanced equations required).
  • Elements of the first transition series, ₂₁Sc – ₃₀ZnWAEC note: (1) Their electron configurations, physical properties and chemical reactivity of the elements and their compounds. (2) Physical properties should include: physical states, metallic properties and magnetic properties. (3) Reactivity of the metals with air, water, acids and comparison with s-block elements (Li, Na, Be, Mg). (4) Other properties of transition metals should include: (a) variable oxidation states; (b) formation of coloured compounds; (c) complex formation; (d) catalytic abilities; (e) paramagnetism; (f) hardness.

Chemical bonds

Our summary: How atoms join through ionic, covalent, dative and metallic bonds, the forces between molecules, and the shapes molecules take.

Contents

  • Interatomic bondingWAEC note: Meaning of chemical bonding. Lewis dot structure for simple ionic and covalent compounds.
  • Formation of ionic bonds and compoundsWAEC note: Formation of stable compounds from ions. Factors influencing formation: ionization energy; electron affinity and electronegativity difference.
  • Properties of ionic compoundsWAEC note: Solubility in polar and non-polar solvents, electrical conductivity, hardness and melting point.
  • Naming of ionic compoundsWAEC note: IUPAC system for simple ionic compounds.
  • Formation of covalent bonds and compoundsWAEC note: Factors influencing covalent bond formation. Electron affinity, ionization energy, atomic size and electronegativity.
  • Properties of covalent compoundsWAEC note: Solubility in polar and non-polar solvents, melting point, boiling point and electrical conductivity.
  • Coordinate (dative) covalent bondingWAEC note: Formation and difference between pure covalent and coordinate (dative) covalent bonds.
  • Shapes of molecular compoundsWAEC note: Linear, planar, tetrahedral and shapes for some compounds e.g. BeCl₂, BF₃, CH₄, NH₃, CO₂.
  • Metallic bonding
  • Metallic bonding: factors influencing its formationWAEC note: Factors should include: atomic radius, ionization energy and number of valence electrons. Types of specific packing not required.
  • Metallic bonding: properties of metalsWAEC note: Typical properties including heat and electrical conductivity, malleability, lustre, ductility, sonority and hardness.
  • Intermolecular bondingWAEC note: Relative physical properties of polar and non-polar compounds.
  • Intermolecular forces in covalent compoundsWAEC note: Description of formation and nature should be treated. Dipole-dipole, induced dipole-dipole, induced dipole-induced dipole forces should be treated under van der Waals' forces.
  • Hydrogen bonding
  • van der Waals forcesWAEC note: Variation of the melting points and boiling points of noble gases, halogens and alkanes in the homologous series explained in terms of van der Waals' forces; and variation in the boiling points of H₂O and H₂S explained using hydrogen bonding.
  • Comparison of all bond types

Stoichiometry and chemical reactions

Our summary: Chemical symbols, formulae and equations, the laws of chemical combination, the mole, and calculations with solutions.

Contents

  • Symbols, formulae and equationsWAEC note: Symbols of the first thirty elements and other common elements that are not among the first thirty elements.
  • Chemical symbols
  • Empirical and molecular formulaeWAEC note: Calculations involving formulae and equations will be required. Mass and volume relationships in chemical reactions and the stoichiometry of such reactions such as: calculation of percentage composition of element.
  • Chemical equations and IUPAC names of chemical compoundsWAEC note: (1) Combustion reactions (including combustion of simple hydrocarbons). (2) Synthesis. (3) Displacement or replacement. (4) Decomposition. (5) Ionic reactions.
  • Laws of chemical combinationWAEC note: (1) Laws of conservation of mass. (2) Law of constant composition. (3) Law of multiple proportions. Explanation of the laws to balance given equations. (4) Experimental illustration of the law of conservation of mass.
  • Amount of substanceWAEC note: (1) Mass and volume measurements. (2) The mole as a unit of measurement; Avogadro's constant, L = 6.02 × 10²³ entities mol⁻¹. (3) Molar quantities and their uses. (4) Moles of electrons, atoms, molecules, formula units etc.
  • Mole ratiosWAEC note: Use of mole ratios in determining stoichiometry of chemical reactions. Simple calculations to determine the number of entities, amount of substance, mass, concentration, volume and percentage yield of product.
  • SolutionsWAEC note: (1) Concept of a solution as made up of solvent and solute. (2) Distinguishing between dilute solution and concentrated solution. (3) Basic, acidic and neutral solutions.
  • Concentration termsWAEC note: Mass (g) or moles (mol) per unit volume. Emphasis on current IUPAC chemical terminology, symbols and conventions. Concentration be expressed as mass concentration, g dm⁻³, molar concentration, mol dm⁻³.
  • Standard solutionsWAEC note: (1) Preparation of some primary standards e.g. anhydrous Na₂CO₃, (COOH)₂·2H₂O/H₂C₂O₄·2H₂O. (2) Meaning of the terms primary standard, secondary standard and standard solution.
  • Preparation of solutions from liquid solutes by the method of dilutionWAEC note: Dilution factor.

States of matter

Our summary: The kinetic theory, changes of state and diffusion, the gas laws, and the properties of liquids, vapours and solids.

Contents

  • Kinetic theory of matterWAEC note: (1) Postulates of the kinetic theory of matter. (2) Use of the kinetic theory to explain the following processes: melting of solids, boiling of liquids, evaporation of liquids, dissolution of solutes, Brownian motion and diffusion.
  • Changes of state of matterWAEC note: (1) Changes of state of matter should be explained in terms of movement of particles. It should be emphasized that randomness decreases (and orderliness increases) from gaseous state to liquid state and to solid state and vice versa. (2) Illustrations of changes of state using the different forms of water, iodine, sulphur, naphthalene etc. (3) Brownian motion to be illustrated using any of the following experiments: (a) pollen grains/powdered sulphur in water (viewed under a microscope); (b) smoke in a glass container illuminated by a strong light from the side; (c) a dusty room being swept and viewed from outside under sunlight.
  • DiffusionWAEC note: (1) Experimental demonstration of diffusion of two gases. (2) Relationship between speed at which different gas particles move and the masses of particles. (3) Experimental demonstration of diffusion of solute particles in liquids.
  • Gases: characteristics and nature of gasesWAEC note: Arrangement of particles, density, shape and compressibility.
  • Gases: the gas lawsWAEC note: The gas laws: Charles'; Boyle's; Dalton's law of partial pressure; Graham's law of diffusion, Avogadro's law. The ideal gas equation of state. Qualitative explanation of each of the gas laws using the kinetic model. The use of kinetic molecular theory to explain changes in gas volumes, pressure, temperature. Mathematical relations of the gas law PV = nRT. Ideal and real gases. Factors responsible for the deviation of real gases from ideal situation.
  • Gases: laboratory preparation and properties of some gasesWAEC note: (1) Preparation of the following gases: H₂, NH₃ and CO₂. Principles of purification and collection of gases. (2) Physical and chemical properties of the gases.
  • LiquidsWAEC note: Characteristics and nature of liquids based on the arrangement of particles, shape, volume, compressibility, density and viscosity.
  • Vapour and gasesWAEC note: (1) Concept of vapour, vapour pressure, saturated vapour pressure, boiling and evaporation. (2) Distinction between vapour and gas. (3) Effect of vapour pressure on boiling points of liquids. (4) Boiling at reduced pressure.
  • Solids: characteristics and natureWAEC note: (1) Ionic, metallic, covalent network and molecular solids. Examples in each case. (2) Arrangements of particles ions, molecules and atoms in the solid state.
  • Solids: types and structuresWAEC note: Relate the properties of solids to the type of interatomic and intermolecular bonding in the solids. Identification of the types of chemical bonds in graphite and differences in the physical properties.
  • Solids: properties of solids
  • Structures, properties and uses of diamond and graphiteWAEC note: The uses of diamond and graphite related to the structure. The use of iodine in everyday life.
  • Determination of melting points of covalent solidsWAEC note: Melting points as indicator of purity of solids e.g. phenyl methanoic acid (benzoic acid), ethanedioic acid (oxalic) and ethanamide.

Solutions, energy and chemical change

Our summary: Energy changes, acids, bases and salts, solubility, reaction rates and equilibrium, and redox reactions with electrolysis.

Energy and energy changes

Our summary: Energy and enthalpy, and the heat given out or taken in when substances react, dissolve or are neutralised.

Contents

  • Energy and enthalpyWAEC note: Explanation of the terms energy and enthalpy. Energy changes associated with chemical processes.
  • Description, definition and illustrations of energy changes and their effectsWAEC note: (1) Exothermic and endothermic processes. (2) Total energy of a system as the sum of various forms of energy e.g. kinetic, potential, electrical, heat, sound etc. (3) Enthalpy changes involved in the following processes: combustion, dissolution and neutralization.

Acids, bases and salts

Our summary: What acids, bases and salts are, how strong they are, the pH scale, indicators, salt hydrolysis and acid-base titration.

Contents

  • Definitions of acids and basesWAEC note: (1) Arrhenius concepts of acids and bases in terms of H₃O⁺ and OH⁻ ions in water. (2) Effects of acids and bases on indicators, metal Zn, Fe and trioxocarbonate (IV) salts and hydrogentrioxocarbonate (IV) salts.
  • Physical and chemical properties of acids and basesWAEC note: Characteristic properties of acids and bases in aqueous solution to include: (a) conductivities, taste, litmus/indicators, feel etc.; (b) balanced chemical equations of all reactions.
  • Acids, bases and salts as electrolytesWAEC note: Electrolytes and non-electrolytes; strong and weak electrolytes. Evidence from conductivity and enthalpy of neutralization.
  • Classification of acids and basesWAEC note: (1) Strength of acids and bases. (2) Classify acids and bases into strong and weak. (3) Extent of dissociation reaction with water and conductivity. (4) Behaviour of weak acids and weak bases in water as example of equilibrium systems.
  • Concept of pHWAEC note: (1) Definition of pH and knowledge of pH scale. (2) Measurement of pH of solutions using pH meter, colorimetric methods or universal indicator. (3) Significance of pH values in everyday life e.g. acid rain, pH of soil, blood, urine.
  • SaltsWAEC note: Meaning of salts. Types of salts: normal, acidic, basic, double and complex salts.
  • Salts: laboratory and industrial preparation of salts; usesWAEC note: (1) Description of laboratory and industrial production of salts. (2) Mining of impure sodium chloride and conversion into granulated salt. (3) Preparation of NaOH, Cl₂ and H₂.
  • Salts: hydrolysis of saltWAEC note: (1) Explanation of how salts form acidic, alkaline and neutral aqueous solutions. (2) Behaviour of some salts (e.g. NH₄Cl, AlCl₃, Na₂CO₃, CH₃COONa) in water as examples of equilibrium systems. (3) Effects of charge density of some cations and anions on the hydrolysis of their aqueous solution. Examples to be taken from group 1, group 2, group 3 and the d-block element.
  • Deliquescent, efflorescent and hygroscopic compoundWAEC note: Use of hygroscopic compounds as drying agent should be emphasized.
  • Acid-base indicatorsWAEC note: (1) Qualitative description of how acid-base indicator works. (2) Indicators as weak organic acids or bases (organic dyes). (3) Colour of indicator at any pH dependent on relative amounts of acid and base forms. (4) Working pH ranges of methyl orange and phenolphthalein.
  • Acid-base titrationWAEC note: (1) Knowledge and correct use of relevant apparatus. (2) Knowledge of how acid-base indicators work in titrations. (3) Acid-base titration experiments involving HCl, HNO₃, H₂SO₄ and NaOH, KOH, Ca(OH)₂, CO₃²⁻, HCO₃⁻. (4) Titration involving weak acids versus strong bases, strong acids versus weak bases and strong acids versus strong bases using the appropriate indicators and their applications in quantitative determination; e.g. concentrations, mole ratio, purity, water of crystallization and composition.

Solubility of substances

Our summary: How much of a substance dissolves, solubility curves and calculations, and how solubility rules help identify ions.

Contents

  • General principlesWAEC note: (1) Meaning of solubility. (2) Saturated and unsaturated solutions. (3) Saturated solution as an equilibrium system. (4) Solubility expressed in terms of: mol dm⁻³ and g dm⁻³ of solution/solvent. (5) Solubility curves and their uses. (6) Effect of temperature on solubility of a substance. (7) Relationship between solubility and crystallization. (8) Crystallization/recrystallization as a method of purification. (9) Knowledge of soluble and insoluble salts of stated cations and anions. (10) Calculations on solubility.
  • Practical application of solubilityWAEC note: Generalization about solubility of salts and their applications to qualitative analysis, e.g. Pb²⁺, Ca²⁺, Al³⁺, Cu²⁺, Fe²⁺, Fe³⁺, Cl⁻, Br⁻, I⁻, SO₄²⁻, S²⁻, and CO₃²⁻, Zn²⁺, NH₄⁺, SO₃²⁻. Explanation of solubility rules.

Chemical kinetics and equilibrium system

Our summary: What makes reactions go faster or slower, collision theory and activation energy, and how reversible reactions reach equilibrium.

Contents

  • Rate of reactionsWAEC note: (1) Definition of reaction rate. (2) Observable physical and chemical changes: colour, mass, temperature, pH, formation of precipitate etc.
  • Rate of reactions: factors affecting ratesWAEC note: (1) Physical states, concentration/pressure of reactants, temperature, catalysts, light, particle size and nature of reactants. (2) Appropriate experimental demonstration for each factor is required.
  • Rate of reactions: theories of reaction ratesWAEC note: (1) Collision and transition state theories to be treated qualitatively only. (2) Factors influencing collisions: temperature and concentration. (3) Effective collision. (4) Activation energy. (5) Energy profile showing activation energy and enthalpy change.
  • Rate of reactions: analysis and interpretation of graphsWAEC note: Drawing of graphs and charts.
  • Equilibrium: general principleWAEC note: Explanation of reversible and irreversible reactions. Reversible reaction i.e. dynamic equilibrium. Equilibrium constant K must be treated qualitatively. It must be stressed that K for a system is constant at constant temperature. Simple experiment to demonstrate reversible reactions.
  • Equilibrium: Le Chatelier's principleWAEC note: Prediction of the effects of external influence of concentration, temperature, pressure and volume changes on equilibrium systems.

Redox reactions

Our summary: Oxidation and reduction, balancing redox equations, electrochemical cells, electrolysis and corrosion.

Contents

  • Oxidation and reduction processWAEC note: (1) Oxidation and reduction in terms of: (a) addition and removal of oxygen and hydrogen; (b) loss and gain of electrons; (c) change in oxidation numbers/states. (2) Determination of oxidation numbers/states.
  • Oxidizing and reducing agentsWAEC note: (1) Description of oxidizing and reducing agents in terms of: (a) addition and removal of oxygen and hydrogen; (b) loss and gain of electrons; (c) change in oxidation numbers/state.
  • Redox equationsWAEC note: Balancing redox equations by: (a) ion, electron or change in oxidation number/states; (b) half reactions and overall reaction.
  • Electrochemical cellsWAEC note: Definition/explanation.
  • Electrochemical cells: standard electrode potentialWAEC note: (1) Standard hydrogen electrode: meaning of standard electrode potential (E°) and its measurement. (2) Only metal/metal ion systems should be used.
  • Electrochemical cells: drawing of cell diagram and writing cell notation
  • Electrochemical cells: e.m.f. of cellsWAEC note: (1) Electrochemical cells as a combination of two half-cells. (2) The meaning of magnitude and sign of the e.m.f.
  • Electrochemical cells: application of electrochemical cellsWAEC note: (1) Distinction between primary and secondary cells. (2) Daniell cell, lead acid battery cell, dry cells, fuel cells and their use as generators of electrical energy from chemical reactions.
  • ElectrolysisWAEC note: Definition.
  • Electrolysis: electrolytic cellsWAEC note: Comparison of electrolytic and electrochemical cells; weak and strong electrolyte.
  • Electrolysis: principles of electrolysisWAEC note: Mechanism of electrolysis.
  • Electrolysis: factors influencing discharge of speciesWAEC note: Limit electrolytes to molten PbBr₂ and NaCl, dilute NaCl solution, concentrated NaCl solution, CuSO₄(aq), dilute H₂SO₄, NaOH(aq) and CaCl₂(aq) (using platinum or graphite and copper electrodes).
  • Electrolysis: Faraday's lawsWAEC note: Simple calculations based on the relation 1 F = 96,500 C and mole ratios to determine mass, volume of gases, number of entities, charges etc. using half and overall reactions.
  • Electrolysis: practical applicationWAEC note: Electroplating, extraction and purification of metals.
  • Corrosion of metalsWAEC note: (1) Corrosion treated as a redox process. (2) Rusting of iron and its economic costs. (3) Prevention based on relative magnitude of electrode potentials and preventive methods like galvanizing, sacrificial/cathodic protection and non-redox methods (painting, greasing/oiling etc.).

Organic chemistry

Our summary: Carbon compounds from crude oil and the hydrocarbons to alkanols, alkanoic acids and esters.

Chemistry of carbon compounds

Our summary: How organic compounds are classified and named, petroleum, isomerism, and the hydrocarbons, alkanols, alkanoic acids and esters.

Contents

  • ClassificationWAEC note: Broad classification into straight chain, branched chain, aromatic and alicyclic compounds.
  • Functional groupWAEC note: Systematic nomenclature of compounds with the following functional groups: alkanes, alkenes, alkynes, hydroxyl compounds (aliphatic and aromatic), alkanoic acids, alkyl alkanoates (esters and salts) and amines.
  • Separation and purification of organic compoundsWAEC note: Methods to be discussed should include: distillation; crystallization; drying and chromatography.
  • Petroleum/crude oilWAEC note: (1) Composition and classification. (2) Fractional distillation and major products. (3) Cracking and reforming. (4) Petro-chemicals: sources; uses e.g. as starting materials of organic synthesis. (5) Quality of petrol, meaning of octane number and its importance to the petroleum industry.
  • Determination of empirical and molecular formulae and molecular structures of organic compounds
  • General properties of organic compounds: homologous seriesWAEC note: (1) Gradation in physical properties. (2) Effects on the physical properties by introduction of active groups into the inert alkane.
  • General properties of organic compounds: isomerismWAEC note: (1) Examples should be limited to compounds having maximum of five carbon atoms. (2) Differences between structural and geometric/stereo isomerism.
  • Alkanes: sources, propertiesWAEC note: (1) Laboratory and industrial preparations and other sources. (2) Nomenclature and structure. (3) Reactivity: (a) combustion; (b) substitution reactions; (c) cracking of large alkane molecules.
  • Alkanes: usesWAEC note: As fuels, as starting materials for synthesis. Uses of haloalkanes and pollution effects.
  • Alkenes: sources and propertiesWAEC note: (1) Laboratory preparation. (2) Nomenclature and structure. (3) Addition reactions with halogens, hydrogen, bromine water, hydrogen halides and acidified water. (4) Oxidation: hydroxylation with aqueous KMnO₄. (5) Polymerization.
  • Alkenes: uses
  • Alkenes: laboratory detectionWAEC note: Use of reaction with Br₂/water, Br₂/CCl₄ and KMnO₄(aq) as means of characterizing alkenes.
  • Alkynes: sources, characteristic properties and usesWAEC note: (1) Nomenclature and structure. (2) Industrial production of ethyne. (3) Uses of ethyne. (4) Distinguishing test between terminal and non-terminal alkynes. (5) Test to distinguish between alkane, alkene and alkyne.
  • Alkynes: chemical reactionsWAEC note: Chemical reactions: halogenation, combustion, hydration and hydrogenation.
  • Benzene: structure and physical propertiesWAEC note: Resonance in benzene. Stability leading to substitution reactions.
  • Benzene: chemical propertiesWAEC note: (1) Addition reactions: hydrogenation and halogenation (mechanism not required). (2) Compare reactions with those of alkenes.
  • Alkanols: sources, nomenclature and structureWAEC note: (1) Laboratory preparation including hydration of alkenes. (2) Industrial and local production of ethanol including alcoholic beverages. (3) Harmful impurities and methods of purification should be mentioned. (4) Recognition of the structure of mono-, di- and triols.
  • Alkanols: classificationWAEC note: Primary, secondary and tertiary alkanols.
  • Alkanols: physical propertiesWAEC note: Boiling point, solubility in water. Including hydrogen bonding effect.
  • Alkanols: chemical propertiesWAEC note: (1) Reaction with: (a) Na; (b) alkanoic acids (esterification); (c) conc. H₂SO₄. (2) Oxidation by: (a) KMnO₄(aq); (b) K₂Cr₂O₇(aq); (c) I₂ in NaOH(aq).
  • Alkanols: laboratory testWAEC note: Laboratory test for ethanol.
  • Alkanols: uses
  • Alkanoic acidsWAEC note: Methanoic acid - insect bite. Ethanoic acid - vinegar.
  • Alkanoic acids: sources, nomenclature and structureWAEC note: Recognition of mono and dioic acid.
  • Alkanoic acids: physical propertiesWAEC note: Boiling point, solubility in water. Including hydrogen bonding effect.
  • Alkanoic acids: chemical propertiesWAEC note: Acid properties only i.e. reactions with H₂O, NaOH, NH₃, NaHCO₃, Zn and Mg.
  • Alkanoic acids: laboratory testWAEC note: Reaction with NaHCO₃, Na₂CO₃.
  • Alkanoic acids: usesWAEC note: Uses of ethanoic and phenyl methanoic (benzoic) acids as examples of aliphatic and aromatic acids respectively.
  • Alkanoates as derivatives of alkanoic acids: sources, nomenclature, preparation and structureWAEC note: Preparation of alkyl alkanoates (esters) from alkanoic acids.
  • Alkanoates: physical propertiesWAEC note: Solubility, boiling and melting point.
  • Alkanoates: chemical propertiesWAEC note: Hydrolysis of alkyl alkanoates (mechanism not required).
  • Alkanoates: usesWAEC note: Uses of alkanoates to include production of soap, flavouring agent, plasticizers, as solvents and in perfumes.

Industry and the environment

Our summary: How chemical industries work, the pollution they can cause, and everyday biotechnology.

Chemistry, industry and the environment

Our summary: Chemical industries and their raw materials, pollution of air, water and soil, and biotechnology.

Contents

  • Chemical industryWAEC note: (1) Natural resources in candidate's own country. (2) Chemical industries in candidate's own country and their corresponding raw materials. (3) Distinction between fine and heavy chemicals. (4) Factors that determine location of chemical industries. (5) Effect of industries on the community.
  • Pollution: air, water and soil pollutionWAEC note: (1) Sources, effects and control. (2) Greenhouse effect and depletion of the ozone layer. (3) Biodegradable and non-biodegradable pollutants.
  • BiotechnologyWAEC note: Food processing, fermentation including production of gari, bread and alcoholic beverages e.g. local gin.

Biochemistry and polymers

Our summary: The chemistry of proteins, fats, carbohydrates and synthetic polymers.

Basic biochemistry and synthetic polymers

Our summary: Proteins, amino acids, fats and oils, carbohydrates and synthetic polymers, including soap-making and tests for each.

Contents

  • ProteinsWAEC note: Proteins as polymers of amino acids molecules linked by peptide or amide linkage.
  • Proteins: sources and propertiesWAEC note: Physical properties e.g. solubility. Chemical properties to include: (a) hydrolysis of proteins; (b) laboratory test using Ninhydrin/Biuret reagent/Millon's reagent.
  • Proteins: uses of protein
  • Amino acidsWAEC note: (1) Nomenclature and general structure of amino acids. (2) Difunctional nature of amino acids.
  • Fats/oilsWAEC note: As alkyl alkanoates (esters).
  • Fats/oils: sources and propertiesWAEC note: From animals and plants. Physical properties such as solubility. Chemical properties: (a) acidic and alkaline hydrolysis; (b) hydrogenation; (c) test for fats and oil.
  • Fats/oils: general structure of fats/oilsWAEC note: As mono-, di-, and tri- esters of propane-1,2,3-triol (glycerol).
  • Fats/oils: preparation of soapWAEC note: (1) Preparation of soap (saponification) from fats and oils. (2) Comparison of soapless detergents and their action on soft and hard water.
  • Fats/oils: uses of fats/oils
  • Carbohydrates: sources and nomenclatureWAEC note: (1) Classes of carbohydrates as: (a) monosaccharides; (b) disaccharides; (c) polysaccharides. (2) Name and components of various classes of carbohydrates.
  • Carbohydrates: propertiesWAEC note: (1) Physical properties such as solubility of sugars. (2) Chemical properties - hydrolysis of disaccharides into monosaccharides. (3) Test for reducing sugars using sugar strips, Fehling's or Benedict's solution or Tollens' reagent.
  • Carbohydrates: carbohydrate as examples of polymerWAEC note: (1) Starch as a polymer made up of glucose units. (2) Condensation of monosaccharides to form disaccharides and polysaccharides.
  • Carbohydrates: uses
  • Synthetic polymersWAEC note: (1) Definition of terms: monomers, polymers and polymerization. (2) Addition and condensation polymerization. (3) Classification and preparation based on the monomers and comonomers.
  • Synthetic polymers: propertiesWAEC note: (1) Thermoplastics and thermosets. (2) Modification of properties of polymers. (3) Plastics and resins. (4) Chemical test on plastics using: (a) heat; (b) acids; (c) alkalis.
  • Synthetic polymers: uses of polymers

Inorganic chemistry: non-metals and metals

Our summary: For candidates in Nigeria, Sierra Leone, Liberia and The Gambia (WAEC Section C): the common non-metals and metals, how they and their compounds are made, and their properties and uses.

Non-metals and their compounds

Our summary: Carbon, oxygen, hydrogen, water, the halogens, nitrogen, sulphur and the noble gases: how they are made, how they behave and what they are used for.

Contents

  • Carbon: allotropes of carbonWAEC note: (1) Graphite, diamond and amorphous carbon; (2) Structures, properties and uses. (3) The uses of the allotropes should be correlated with their properties and structures. (4) Combustion of allotropes.
  • Carbon: coal: types; destructive distillation of coal and uses of the productsWAEC note: Different types should include anthracite, peat and lignite.
  • Carbon: coke: classification and uses; manufacture of synthetic gas and usesWAEC note: Water gas and producer gas.
  • Carbon: oxides of carbon: carbon (IV) oxidesWAEC note: (1) Laboratory preparation. (2) Properties and uses. (3) Test for carbon (IV) oxides.
  • Carbon: oxides of carbon: carbon (II) oxidesWAEC note: Properties and uses only.
  • Carbon: trioxocarbonate (IV) saltWAEC note: (1) Properties: solubility, action of heat, reaction with dilute acid. (2) Uses.
  • Oxygen: laboratory and industrial preparation
  • Oxygen: properties and usesWAEC note: Test for oxygen will be required.
  • Oxygen: binary compounds of oxygen: acidic, basic, amphoteric and neutral oxides
  • Hydrogen: laboratory preparations
  • Hydrogen: properties and usesWAEC note: Test for hydrogen will be required.
  • Water and solution: composition of waterWAEC note: Test for water will be required. Reference should be made to the electrolysis of acidified water.
  • Water and solution: water as a solvent
  • Water and solution: hardness of water, causes and methods of removing itWAEC note: (1) Advantages and disadvantages of hard water and soft water. (2) Experiments to compare the degrees of hardness in different samples of water.
  • Water and solution: treatment of water for town supply
  • HalogensWAEC note: Redox properties of the elements; displacement reaction of one halogen by another.
  • Halogens: chlorine: laboratory preparation; properties and reactionsWAEC note: Properties should include: (a) variable oxidation states; (b) reaction with water and alkali (balanced equation required).
  • Hydrogen chloride gas: laboratory preparation
  • Hydrogen chloride gas: properties and usesWAEC note: (1) Test for HCl gas. (2) Fountain experiment.
  • Uses of halogen compoundsWAEC note: Uses should include silver halide in photography and sodium oxochlorate (I) as a bleaching agent.
  • Nitrogen: preparation and propertiesWAEC note: Both laboratory and industrial preparations from liquefied air are required.
  • Nitrogen: uses of nitrogen
  • Compounds of nitrogen: ammoniaWAEC note: (1) Laboratory and industrial preparations. (2) Properties and uses. (3) Test for ammonia. (4) Fountain experiment.
  • Compounds of nitrogen: trioxonitrate (V) acidWAEC note: (1) Laboratory preparation. (2) Properties and uses.
  • Compounds of nitrogen: trioxonitrate (V) saltsWAEC note: (1) Action of heat will be required. (2) Test for trioxonitrate (V) ions.
  • Sulphur: allotropes and uses
  • Sulphur: compound of sulphur
  • Sulphur: trioxosulphate (IV) acids and its salts
  • Sulphur: tetraoxosulphate (VI) acid: industrial preparation, reactions and usesWAEC note: Contact process should be discussed.
  • The noble gases: properties and uses

Metals and their compounds

Our summary: How aluminium, iron and tin are extracted, common alloys, and sodium, calcium, copper and their compounds.

Contents

  • Extraction of metals: aluminium; iron; tinWAEC note: (1) Raw materials, processing, main products and by-products. (2) Uses of metals.
  • AlloysWAEC note: Common alloys of Cu, Al, Pb, Fe, Sn and their uses.
  • Properties and uses of sodium and its compoundsWAEC note: Compounds must be limited to NaCl, NaOH, Na₂CO₃, NaNO₃, Na₂SO₄ and NaClO.
  • Properties and uses of calcium and its compoundsWAEC note: The compounds must be limited to CaCO₃, CaO, CaSO₄, CaCl₂, and Ca(OH)₂.
  • Reactivity of iron and aluminium with air, water and acids
  • Properties and uses of copper and its compoundsWAEC note: The compounds must be limited to CuSO₄, CuO and CuCl₂.

More from the WAEC Chemistry syllabus

Introduction

  • This syllabus is drawn purposely for examination, hence the topics are not necessarily arranged in the order in which they should be taught.
  • Assumptions: The following assumptions were made in drawing of the syllabus: (1) that candidates must have covered the Integrated Science/Basic Science or General Science and Mathematics syllabuses at the Junior Secondary School (JSS)/Junior High School (J.H.S) level; (2) that candidates would carry out as many of the suggested activities and project work as possible, and consequently develop the intended competencies and skills as spelt out in the relevant Chemistry teaching syllabuses; (3) that schools which offer the subject have well-equipped laboratories.
  • Note: Candidates are required to have the knowledge of the significant figures, S.I. units and the conventional/IUPAC system of nomenclature.

Aims

  • The aims and objectives of the syllabus are to assess candidates':
  • understanding of basic chemistry concepts;
  • level of acquisition of laboratory skills including awareness of hazards and safety measures;
  • level of awareness of the inter-relationship between chemistry and other discipline;
  • level of awareness of the linkage between chemistry and industry/environment/everyday life in terms of benefits and hazards;
  • skills of critical and logical thinking.

Practicals: general skills and principles

  • Candidates will be expected to be familiar with the following skills and principles:
  • Measurement of mass and volume;
  • Preparation and dilution of standard solutions;
  • Filtration, recrystallisation and melting point determination;
  • Measurement of heats of neutralization and solutions;
  • Determination of pH value of various solutions by colorimetry;
  • Determination of rates of reaction from concentration versus time curves;
  • Determination of equilibrium constants for simple system.

Practicals: quantitative analysis

Acid-base titrations
The use of standard solutions of acids and alkalis and the indicators; methyl orange, methyl red and phenolphthalein to determine the following: (i) the concentrations of acid and alkaline solutions; (ii) the molar masses of acids and bases and water of crystallization; (iii) the solubility of acids and bases; (iv) the percentage purity of acids and bases; (v) analysis of Na₂CO₃/NaHCO₃ mixture by double indicator methods (Ghanaians only); (vi) stoichiometry of reactions.
Redox titrations
Titrations of the following systems to solve analytical problems: (i) acidic MnO₄⁻ with Fe²⁺; (ii) acidic MnO₄⁻ with C₂O₄²⁻; (iii) I₂ in KI versus S₂O₃²⁻.

Practicals: qualitative analysis

  • No formal scheme of analysis is required.
  • Characteristic tests of the following cations with dilute NaOH(aq) and NH₃(aq): NH₄⁺; Ca²⁺; Pb²⁺; Cu²⁺; Fe²⁺; Fe³⁺; Al³⁺; and Zn²⁺.
  • Confirmatory tests for the above cations.
  • Characteristic reaction of dilute HCl on solids or aqueous solutions and conc. H₂SO₄ on solid samples of the following: Cl⁻; SO₃²⁻; CO₃²⁻; NO₃⁻ and SO₄²⁻.
  • Confirmatory tests for the above anions.
  • Comparative study of the halogens; displacement reactions.
  • Characteristic tests for the following gases: H₂; NH₃; CO₂; HCl and SO₂.
  • Characteristic test tube reactions of the functional groups in the following simple organic compounds: alkenes; alkanols; alkanoic acids, sugars (using Fehling's and Benedict's solutions only); starch (iodine test only) and proteins (using the Ninhydrin test, Xanthoproteic test, Biuret test and Millon's test only).

Syllabus content © The West African Examinations Council. Taken from https://waecsyllabus.com/files/ssce/CHEMISTRY.pdf (WASSCE (harmonised West African syllabus)).

DeeepSolve is an independent study platform and is not affiliated with WAEC. The topic lists, notes and exam scheme are the exam body's wording; “Our summary” lines are ours. If anything here differs from what WAEC publishes for your sitting, follow WAEC.