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WAEC SYLLABUS FOR 2021/2022 (WASSCE) CHEMISTRY
- INTRODUCTION
This syllabus is drawn purposely for examination, hence the topics are not necessarily arranged in the order in which they should be taught.
The following assumptions were made in drawing of the syllabus:
- 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;
- 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;
- 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.
2. 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.
3. EXAMINATION SCHEME
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 (ie 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.
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.
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 perculiar 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.
Details of the input into the continuous assessment shall be given by the Council.
SECTION A
(For all candidates)
CONTENT | NOTES |
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Outline the scientific method to include: Observation, hypothesis, experimentation, formulation of laws and theories.
Meaning and representation in symbols of atoms and sub-atomic particles.
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CONTENT | NOTES |
(ii) Relative atomic mass (Ar) and relative molecular mass (Mr) based on Carbon-12 scale.
(iii) Characteristics and nature of matter.
(ii) Orbitals
(iii) Rules and principles for filling in electrons.
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Atoms, molecules and ions. Definition of particles and treatment of particles as building blocks of matter.
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.
Detailed electron configurations (s,p,d) for atoms of the first thirty elements.
Origin of s,p and d orbitals as sub-energy levels; shapes of s and p orbitals only.
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CONTENT | NOTES |
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Solid-solid, solid-liquid, liquid-liquid, gas-gas with examples.
Crystallization, distillation, precipitation, magnetization, chromatography, sublimation etc.
Boiling point for liquids and melting point for solids.
Electron configurations leading to group and periodic classifications.
Metals, semi-metals, non-metals in the periodic table and halogens. Alkali metals, alkaline earth metals and transition metals as metals.
Explanation of the periodic law.
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.
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CONTENTS | NOTES |
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Recognition of group variations noting any anomalies. Treatment should include the following:
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CONTENT | NOTES |
(ii) Properties of ionic compounds.
(ii) Coordinate (dative) covalent bonding. |
Meaning of chemical bonding. Lewis dot structure for simple ionic and covalent compounds.
Formation of stable compounds from ions. Factors influencing formation: ionzation energy; electron affinity and electronegativity difference.
Solubility in polar and non-polar solvents, electrical conductivity, hardness and melting point.
IUPAC system for simple ionic compounds.
Factors influencing covalent bond formation. Electron affinity, ionization energy, atomic size and electronegativity.
Solubility in polar and non-polar solvents, melting point, boiling point and electrical conductivity.
Formation and difference between pure covalent and coordinate (dative) covalent bonds. |
CONTENT | NOTES |
(ii) Factors influencing its formation.
(iii) Properties of metals.
(iii) Hydrogen bonding
CONTENT |
Linear, planar, tetrahedral and shapes for some compounds e.g. BeCl2, BF3, CH4, NH3, CO2.
Factors should include: atomic radius, ionization energy and number of valence electrons. Types of specific packing not required.
Typical properties including heat and electrical conductivity, malleability, lustre, ductility, sonority and hardness.
Relative physical properties of polar and non-polar compounds. Description of formation and nature should be treated. Dipole-dipole, induced dipole-dipole, induced dipole-induced dipole forces should be treated under van der Waal’s forces.
Variation of the melting points and boiling points of noble gases, halogens and alkanes in the homologous series explained in terms of van der Waal’s forces; and variation in the boiling points of H2O, and H2S explained using Hydrogen bonding.
NOTES |
(ii) chemical symbols
(iii) Empirical and molecular formulae.
(iv) Chemical equations and IUPAC names of chemical compounds.
(v) Laws of chemical combination.
CONTENT |
Symbols of the first thirty elements and other common elements that are not among the first thirty elements.
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.
NOTES |
(ii) Concentration terms
(iii) Standard solutions.
CONTENT |
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.
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.
Dilution factor
. NOTES |
(ii) Changes of state of matter.
(iii) Diffusion
CONTENT |
(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:
\
NOTES |
(ii) The gas laws;
(iii) Laboratory preparation and properties of some gases.
(ii) Vapour and gases.
CONTENT |
Arrangement of particles, density, shape and compressibility.
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.
Characteristics and nature of liquids based on the arrangement of particles, shape, volume, compressibility, density and viscosity.
NOTES |
CONTENT |
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.
The uses of diamond and graphite related to the structure. The use of iodine in everyday life.
Melting points as indicator of purity of solids e.g. Phenyl methanedioic acid (benzoic acid), ethanedioic acid (oxalic) and ethanamide.
Explanation of the terms energy and enthalpy. Energy changes associated with chemical processes.
NOTES |
9.0 ACIDS, BASES AND SALTS (a) Definitions of acids and bases.
(b) Physical and chemical properties of acids and bases.
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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.
Electrolytes and non-electrolytes; strong and weak electrolytes. Evidence from conductivity and enthalpy of neutralization.
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CONTENT | NOTES |
(i) Laboratory and industrial preparation of salts; (ii) Uses;
CONTENT |
Meaning of salts. Types of salts: normal, acidic, basic, double and complex salts.
Use of hygroscopic compounds as drying agent should be emphasized.
NOTES |
10.0 SOLUBILITY OF SUBTANCES (a) General principles
(b) Practical application of solubility.
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(10) Calculations on solubility.
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. |
CONTENT | NOTES |
11.0 CHEMICAL KINETICS AND EQUILIBRIUM SYSTEM (a) Rate of reactions:
(i) Factors affecting rates;
(ii) Theories of reaction rates;
(iii) Analysis and interpretation of graphs.
(b) Equilibrium: (i) General Principle;
CONTENT |
Drawing of graphs and charts.
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.
NOTES |
(ii) Le Chatelier’s principle.
12.0 REDOX REACTIONS (a) Oxidation and reduction process.
(b) Oxidizing and reducing agents.
(c) Redox equations
(d) Electrochemical cells: (i) Standard electrode potential;
(ii) Drawing of cell diagram and writing cell notation.
CONTENT |
Prediction of the effects of external influence of concentration, temperature pressure and volume changes on equilibrium systems.
Balancing redox equations by:
Definition/Explanation
NOTES |
(iii) e.m.f of cells;
(iv) Application of Electrochemical cells.
(e) Electrolysis: (i) Electrolytic cells;
(ii) Principles of electrolysis;
(iii) Factors influencing discharge of species;
(iv) Faraday’s laws;
(v) Practical application;
CONTENT |
Definition.
Comparison of electrolytic and electrochemical cells; weak and strong electrolyte.
Mechanism of electrolysis.
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).
Simple calculations based on the relation 1F= 96,500 C and mole ratios to determine mass, volume of gases, number of entities, charges etc. using half and overall reactions.
Electroplating, extraction and purification of metals.
NOTES |
(vi) Corrosion of metals.
13.0 CHEMISTRY OF CARBON COMPOUNDS (a) Classification
(b) Functional group
(b) Separation and purification of organic compounds.
(c) Petroleum/crude oil
CONTENT |
Broad classification into straight chain, branched chain, aromatic and alicyclic compounds.
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.
Methods to be discussed should include: distillation; crystallization; drying and chromatography.
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CONTENT |
(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.
As fuels, as starting materials for synthesis. Uses of haloakanes and pollution effects.
NOTES |
(ii) Uses; (iii) Laboratory detection.
(h) Alkynes: (i) Sources, characteristic properties and uses;
(ii) Chemical reactions.
(i) Benzene: (i) Structure and physical properties;
(ii) Chemical properties.
CONTENT |
Use of reaction with Br2/water, Br2/CCl4 and KMnO4(aq) as means of characterizing alkenes.
Chemical reactions: halogenation, combustion, hydration and hydrogenation.
Resonance in benzene. Stability leading to substitution reactions.
NOTES |
(J) Alkanols: (i) Sources, nomenclature and structure;
(ii) Classification; (iii) Physical properties;
(iv) Chemical properties;
(v) Laboratory test; (vi) Uses. (k) Alkanoic acids:
(i) Sources, nomenclature and structure; (ii) Physical properties;
CONTENT |
Primary, secondary and tertiary alkanols.
Boiling point, solubility in water. Including hydrogen bonding effect.
Laboratory test for ethanol.
Methanoic acid –insect bite. Ethanoic acid – vinegar.
Recognition of mono and dioic acid.
Boiling point, solubility in water. Including hydrogen bonding effect.
NOTES |
(iii) Chemical properties;
(iv) Laboratory test; (iv) Uses.
(l) Alkanoates as drivatives of alkanoic acids: (i) Sources, nomenclature, preparation and structure;
(ii) Physical properties; (iii) Chemical properties;
(iv) Uses.
14.0 CHEMISTRY, INDUSTRY AND THE ENVIRONMENT (a) Chemical industry
CONTENT |
Acid properties only i.e. reactions with H2O, NaOH, NH3, NaHCO3, Zn and Mg.
Reaction with NaHCO3, Na2CO3.
Uses of ethanoic and phenyl methanoic (benzoic) acids as examples of aliphatic and aromatic acids respectively.
Preparation of alkyl alkanoates (esters) from alkanoic acids.
Solubility, boiling and melting point.
Hydrolysis of alkyl alkanoates (mechanism not required).
Uses of alkanoates to include production of soap, flavouring agent, plasticizers, as solvents and in perfumes.
(2) Chemical industries in candidates own country and their corresponding raw materials.
NOTES |
(b) Pollution: air, water and soil pollution;
(c) Biotechnology.
15.0 BASIC BIOCHEMISTRY AND SYNTHETIC POLYMERS
(i) Sources and properties;
(ii) Uses of protein. (b) Amino acids
CONTACT |
Food processing, fermentation including production of gari, bread and alcoholic beverages e.g. Local gin.
Proteins as polymers of amino acids molecules linked by peptide or amide linkage.
Physical properties e.g. solubility Chemical properties to include:
NOTES |
(c) Fats/oils: (i) Sources and properties;
(ii) General structure of fats/oils;
(iii) Preparation of soap;
(iv) Uses of fats/oils.
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As alkyl alkanoates (esters).
From animals and plants. Physical properties such as solubility. Chemical properties:
As mono-, di-, and tri- esters of propane-1,2,3-triol (glycerol).
NOTES |
(iii) Carbohydrate as examples of polymer;
(iv) Uses.
(e) Synthetic polymers:
(i) Properties;
(ii) Uses of polymers. |
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SECTION B
(For candidates in Ghana only)
CONTENTS | NOTES |
(iii) Radioactivity: induced/stimulated.
(iv) Nuclear reactions: fission and fusion in nuclear reactions.
(v) Effects and application of radioactivity
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Meaning of terms: Nucleons, nuclide.
Charges, relative mass and penetrating power of radiations. Meaning of radioactivity. Difference between spontaneous nuclear reactions (radioactivity) and induced nuclear reactions.
Natural and artificial radioactivity. Detection of radiation by Geiger-Muller counter.
Distinction between ordinary chemical reactions and nuclear reactions. Generations of electricity; atomic bombs. Balanced equations of nuclear reactions
Factors affecting stability of nuclides: Binding energy, neutron-proton ratio, and half life. Calculations involving half-life
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CONTENTS | NOTES |
3.0. CHEMICAL BONDS (a) Formation of Ionic bonds: (i) Factors that influence ionic bond formation; |
Definition of ligands and central ions Examples of ligands
Tetrahedral, square planar, octahedral e.g. (Fe(CN)6]3-, [Cu(NH3)4]2+, [Ag)NH3)2]+ [Cu)CN)4]2
Reactivity of the metals with air, water, acids and comparison with s-block elements (Li, Na, Be, Mg).
Factors should include lattice energy. |
CONTENTS | NOTES |
(ii) Covalent character in ionic bond; (iii) Polar covalent bonds.
(b)(i) Hybridization of atomic orbitals.
(ii) Formation of hybrid orbitals.
(iii) Formation of sigma (σ) and pi (π) bonds.
4.0 SOLUTIONS (a) Preparation of solutions from liquid solutes by the method of dilution.
5.0 ENERGY AND ENERGY CHANGES
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Definition of Hybridization.
Description of sigma and pi bonds. Using C2H2 and C6H6.
Explanation of Hess’s law and its application in the development of the Born-Haber cycle.
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CONTENTS | NOTES |
(c) Bond Energy
6.0 ACIDS, BASES AND SALTS (a) Definitions of acids and bases.
(b) pH, pOH and pKw
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Explanation of bond energy and bond dissociation energy.
Explanation of pKa and pKb of weak acids and bases.
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CONTENTS | NOTES |
7.0 SOLUBILITY OF SUBSTANCES
8.0 EQUILIBRIUM SYSTEMS
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Double indicator titrations (continuous and Discontinuous) and back titration. Calculations involving concentration, composition and % purity. Graphs for acid-based titrations. Nature of graphs of strong acid and strong base, strong acid and weak base and strong base and weak acid.
Explanation of the effect of lattice energy and hydration energy on crystallization and recrystallization.
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CONTENTS | NOTES |
9.0 CHEMISTRY OF CARBON COMPOUNDS
(ii) Comparison or reactions of benzene and alkenes.
CONTENT |
Other methods should include solvent extraction and melting point determinations.
Outline of steps in:
Halogenation – free radical mechanism.
Mono substituted reactions of benzene: toluene, phenol, aniline, benzoic acid and nitrobenzene. (IUPAC and trivial names)
Differences between the reactivity of benzene and alkenes towards certain reagents. Uses of hexachlorocyclobezane and benzene hexachloride (BHC).
NOTES |
10.0 ENVIRONMENT
(a) (i) Sources of raw materials (ii) Mining of mineral as ore.
(iii) Extraction of metals Mineral deposits in Ghana.
(b) Cement and its uses |
Location of mineral deposits and their nature.
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SECTION C
(For candidates in Nigeria, Sierra-Leone, Liberia and The Gambia)
CONTENT | NOTES |
(ii) Coal:
(iii) Coke:
(iv) Oxides of carbon
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Different types should include anthracite, peat and lignite.
Water gas and producer gas.
Properties and uses only.
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CONTENT | NOTES |
(b) Oxygen:
(c) Hydrogen: (i) Laboratory preparations; (ii) Properties and uses.
(d) Water and solution: (i) Composition of water;
(i) Chlorine:
CONTENT |
Test for oxygen will be required.
Test for hydrogen will be required.
Test for water will be required. Reference should be made to the electrolysis of acidified water.
Redox properties of the elements; displacement reaction of one halogen by another.
Properties should include:
NOTES |
2.0 METALS AND THEIR COMPOUNDS (a) Extraction of metals:
(i) Aluminium; (ii) Iron; (iii) Tin.
(b) Alloys.
CONTENT |
Uses should include silver halide in photography and sodium oxochlorate (I) as a bleaching agent.
Both laboratory and industrial preparations from liquefied air are required.
Contact process should be discussed.
Common alloys of Cu, Al, Pb, Fe, Sn and their uses. NOTES |
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Compounds must be limited to NaCl, NaOH, Na2CO3, NaNO3, Na2SO4 and NaClO. The compounds must be limited to CaCO3, CaO, CaSO4, CaCl2, and Ca(OH)2
The compounds must be limited to CuSO4, CuO and CuCl2. |
.16.0 PRACTICALS
(a) 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;
(vi) Determination of rates of reaction from concentration versus time curves;
(vii) Determination of equilibrium constants for simple system.
(b) 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.
(i) Characteristic tests of the following cations with dilute NaOH(aq) and NH3(aq)
NH4 Ca2+ Pb2+ Cu2+ Fe2+ Fe3+ Al3+ and Zn2+.
(ii) Confirmatory tests for the above cations.
(iii) 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 Fehiling’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).