2023/2024 WAEC Syllabus for Chemistry (Objective & Practical)

The WAEC syllabus is a written document containing the order in which a course should be taught and the areas of Concentration for which students will be assessed on the course.

Thus, the WAEC syllabus for Chemistry contains the area of concern which a student should expect questions to be gotten from. It also contains the objectives, notes, and formats for the Chemistry examination.

Questions will only be gotten from these topics, thus, it is cardinal to read up on every topic in the syllabus and be sure to read between the lines. One mistake students make while writing the WAEC examination is that they feel they know every topic already so they take the examination really lightly. Don’t do that, read as though this is the last you will read.

Objective of WAEC Syllabus

This syllabus is intended to create the following;

• 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 another 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.

Examination Scheme

This examination will be divided into three papers – Papers 1, 2, and 3 all of which must be taken.

Papers 1 and 2 shall be composite papers to be taken in one sitting.

WAEC Chemistry Syllabus

• Introduction to Chemistry
• Measurement of physical quantities.
• Scientific measurements and their importance in chemistry.
• Scientific Methods
• Structure of the Atom
• Gross features of the atom
• Atomic number/proton number, number of neutrons, isotopes, atomic mass, mass number
• Relative atomic mass (Ar) and relative molecular mass (Mr) based on the Carbon-12 scale
• Characteristics and nature of matter.
• Particulate nature of matter: physical and chemical changes
• Electron Configuration
• Orbitals
• Rules and principles for filling in electrons
• Standard Separation Techniques for Mixtures
• Classification of mixtures.
• Separation techniques
• Criteria for purity
• Periodic Chemistry
• Periodicity of the elements.
• Different categories of elements in the periodic table.
• Periodic law
• Trends on the periodic table
• Periodic gradation of the elements in the third period (Na – Ar)
• Reactions between acids and metals, their oxides, and trioxocarbonates (IV)
• Periodic gradation of elements in group seven, the halogens: F, Cl, Br, and I
• Elements of the first transition series 21Sc – 30Zn
• Chemical Bonds
• Interatomic bonding
• Formation of ionic bonds and compounds.
• Properties of ionic compounds.
• The naming of ionic compounds.
• Formation of covalent bonds and compounds.
• Properties of covalent compounds.
• Coordinate (dative) covalent bonding
• Shapes of molecular compounds.
• Metallic Bonding
• Factors influencing its formation.
• Properties of metals.
• Intermolecular bonding
• Intermolecular forces in covalent compounds
• Hydrogen bonding
• Van der Waals forces
• Comparison of all bond types
• Stoichiochemistry and Chemical Reactions
• Symbols, formulae, and equations.
• Chemical symbols
• Empirical and molecular formulae
• Chemical equations and IUPAC names of chemical compounds
• Laws of chemical combination
• Amount of substance
• Mole ratios
• Solutions
• Concentration terms
• Standard solutions.
• Preparation of solutions from liquid solutes by the method of dilution
• States of Matter
• Kinetic theory of matter.
• Changes of state of matter.
• Diffusion
• Gases
• Characteristics and nature of gases
• The gas laws
• Laboratory preparation and properties of some gases.
• Liquids
• Vapour and gases.
• Solids
• Characteristics and nature
• Types and structures
• Properties of solids.
• Structures, properties, and uses of diamond and graphite.
• Determination of melting points of covalent solids.
• Energy and Energy Changes
• Energy and enthalpy
• Description, definition, and illustrations of energy changes and their effects
• Acids, Bases, and Salts
• Definitions of acids and bases.
• Physical and chemical properties of acids and bases.
• Acids, bases, and salts as electrolytes.
• Classification of acids and bases.
• Concept of pH
• Salts
• Laboratory and industrial preparation of salts
• Uses
• Hydrolysis of salt.
• Deliquescent, efflorescent, and hygroscopic compounds.
• Acid-Base indicators
• Acid-Base titration
• Solubility of Substances
• General principles
• Practical application of solubility
• Chemical Kinetics and Equilibrium System
• Rate of reactions:
• Factors affecting rates
• Theories of reaction rates
• Analysis and interpretation of graphs
• Equilibrium:
• General Principle
• Le Chatelier’s principle
• REDOX Reactions
• Oxidation and reduction process.
• Oxidizing and reducing agents.
• Redox equations
• Electrochemical cells
• Standard electrode potential
• Drawing of cell diagram and writing cell notation
• m.f of cells;
• Application of Electrochemical cells.
• Electrolysis
• Electrolytic cells
• Principles of electrolysis
• Factors influencing the discharge of species;
• Faraday’s laws
• Practical application
• Corrosion of metals
• Chemistry of Carbon Compounds
• Classification
• Functional group
• Separation and purification of organic compounds.
• Petroleum/crude oil
• Determination of empirical and molecular formulae and molecular structures of organic compounds.
• General properties of organic compounds:
• Homologous series
• Uses
• Alkanes
• Sources, properties
• Uses
• Alkenes
• Sources and properties
• Uses
• Laboratory detection.
• Alkynes
• Sources, characteristic properties, and uses
• Chemical reactions.
• Benzene
• Structure and physical properties;
• Chemical properties
• Alkanols
• Sources, nomenclature, and structure;
• Classification
• Physical properties
• Chemical properties
• Laboratory test
• Uses
• Alkanoic acids
• Sources, nomenclature, and structure;
• Physical properties
• Chemical properties
• Laboratory test
• Uses
• Alkanoates as derivatives of alkanoic acids:
• Sources, nomenclature, preparation, and structure;
• Physical properties
• Chemical properties
• Uses
• Chemistry, Industry, and the Environment
• Chemical industry
• Pollution: air, water, and soil pollution
• Biotechnology
• Basic Biochemistry and Synthetic Polymers
• Proteins:
• Sources and properties
• Uses of Protein
• Amino acids
• Fats/oils
• Sources and properties;
• The general structure of fats/oils
• Preparation of soap
• Uses of fats/oils.
• Carbohydrates
• Sources and nomenclature;
• Properties
• Carbohydrates as examples of polymers;
• Uses
• Synthetic polymers:
• Properties;
• Uses of polymers

WAEC Chemistry 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 a simple system.
• 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:

• The concentrations of acid and alkaline solutions
• The molar masses of acids and bases and water of crystallization.
• The solubility of acids and bases;
• The percentage purity of acids and bases;
• Analysis of Na2CO3/NaHCO3 mixture by double indicator methods (Ghanaians only).
• Stoichiometry of reactions.
• Redox Titrations

Titrations of the following systems to solve analytical problems:

• Acidic MnO4– with Fe2+;
• Acidic MnO4– with C2O42-;
• I2 in KI versus S2O32-.

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.
• The 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, Xanthoporteic test, Biuret test and Millon’s test only).

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