WAEC Chemistry Syllabus will help you become better and prepare better for your examination and that is one of the reason why we decided to bring this to your doorstep. WAEC examination is around the corner and what is the best way to prepare if not to first look at the Syllabus then check out the past questions too.

In this post, we are going to give you the full list of WAEC Chemistry Syllabus for the year 2024; let’s get started

WAEC Chemistry Syllabus

Below are all the topics that you are expected to cover for your WAEC examination as a chemistry student;

1. Separation of Mixtures and Purification of Chemical Substances

Pure and impure substances
Boiling and melting points
Elements, compounds, and mixtures
Chemical and physical changes
Separation processes: evaporation, simple and fractional distillation, sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation

Objectives: Candidates should be able to:

(i) Distinguish between pure and impure substances

(ii) Use boiling and melting points as criteria for purity of chemical substances

(iii) Distinguish between elements, compounds, and mixtures

(iv) Differentiate between chemical and physical changes

(v) Identify the properties of the components of a mixture

(vi) Specify the principle involved in each separation method (vii) Apply the basic principle of separation processes in everyday life

2. Chemical Combination

Stoichiometry
Laws of definite and multiple proportions
Law of conservation of matter,
Gay Lussac’s law of combining volumes,
Avogadro’s law;
Chemical symbols,
Formulae,
Equations and their uses,
Relative atomic mass based on 12C=12, the mole concept and Avogadro’s number

Objectives: Candidates should be able to:

(i) Perform simple calculations involving formulae, equations/chemical composition and the mole concept

(ii) Deduce the chemical laws from given expressions/statements/data

(iii) Interpret graphical representations related to these laws

(iv) Deduce the stoichiometry of chemical reactions

3. Kinetic Theory of Matter and Gas Laws

(a) An outline of the kinetic theory of matter: (i) Melting (ii) Vaporization (iii) Boiling (iv) Freezing (v) Condensation in terms of molecular motion and Brownian movement

(b) The laws of Boyle, Charles, Graham, and Dalton (law of partial pressure); combined gas law, molar volume, and atomicity of gases (ii) The ideal gas equation (PV = nRT) (iii) The relationship between vapor density of gases and the relative molecular mass

Objectives: Candidates should be able to:

(i) Apply the theory to distinguish between solids, liquids, and gases

(ii) Deduce reasons for change of state

(iii) Draw inferences based on molecular motion

(iv) Deduce gas laws from given expressions/statements

(v) Interpret graphical representations related to these laws (vi) Perform simple calculations based on these laws, equations, and relationships

4. Atomic Structure and Bonding

(a) The concept of atoms, molecules, and ions, the works of Dalton, Millikan, Rutherford, Moseley, Thompson, and Bohr (ii) Atomic structure, electron configuration, atomic number, mass number and isotopes; specific examples should be drawn from elements of atomic number 1 to 20 (iii) Shapes of s and p orbitals

(b) The periodic table and periodicity of elements, presentation of the periodic table with a view to recognizing families of elements e.g. alkali metals, halogens, the noble gases and transition metals. The variation of the following properties: ionization energy, ionic radii, electron affinity and electronegativity

(c) Chemical bonding: Electrovalency and covalency, the electron configuration of elements and their tendency to attain the noble gas structure. Hydrogen bonding and metallic bonding as special types of electrovalency and covalency respectively; coordinate bond as a type of covalent bond as illustrated by complexes like [Fe(CN)6]3−, [Fe(CN)6]4−, [Cu(NH3)4]2+ and [Ag(NH3)2]+; van der Waals’ forces should be mentioned as a special type of bonding forces (d) Shapes of simple molecules: linear (H2, O2, Cl2, HCl and CO2), non-linear (H2O) and tetrahedral (CH4) and pyramidal (NH3) (e) Nuclear Chemistry: (i) Radioactivity – Types and properties of radiations (ii) Nuclear reactions. Simple equations, uses, and applications of natural and artificial radioactivity

Objectives: Candidates should be able to:

(i) Distinguish between atoms, molecules, and ions

(ii) Identify the contributions of these scientists to the development of the atomic structure

(iii) Deduce the number of protons, neutrons, and electrons from atomic and mass numbers of an atom

(iv) Apply the rules guiding the arrangement of electrons in an atom

(v) Identify common elements exhibiting isotopy

(vi) Relate isotopy to mass number

(vii) Perform simple calculations relating to isotopy

(viii) Differentiate between the shapes of the orbitals

(ix) Determine the number of electrons in s and p atomic orbitals

(x) Relate atomic number to the position of an element on the periodic table

(xi) Relate properties of groups of elements on the periodic table

(xii) Identify reasons for variation in properties across the period and down the groups

(xiii) Differentiate between the different types of bonding

(xiv) Deduce bond types based on electron configurations

(xv) Relate the nature of bonding to properties of compounds

(xvi) Differentiate between the various shapes of molecules

(xvii) Distinguish between ordinary chemical reaction and nuclear reaction

(xviii) Differentiate between natural and artificial radioactivity

(xix) Compare the properties of the different types of nuclear radiations

(xx) Compute simple calculations on the half-life of a radioactive material

(xxi) Balance simple nuclear equations (xxii) Identify the various applications of radioactivity

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5. Air

(a) The natural gaseous constituents and their proportion in the air: nitrogen, oxygen, water vapor, carbon dioxide and the noble gases (argon and neon)

(b) Air as a mixture and some uses of the noble gas

Objectives: Candidates should be able to:

(i) Deduce reasons for the existence of air as a mixture

(ii) Identify the principle involved in the separation of air components

(iii) Deduce reasons for the variation in the composition of air in the environment

(iv) Specify the uses of some of the constituents of air

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6. Water

(a) Water as a product of the combustion of hydrogen and its composition by volume

(b) Water as a solvent, atmospheric gases dissolved in water and their biological significance

(d) Treatment of water for town supply

(e) Water of crystallization, efflorescence, deliquescence and hygroscopy. Examples of the substances exhibiting these properties and their uses

Objectives: Candidates should be able to:

(i) Identify the various uses of water

(ii) Identify the effects of dissolved atmospheric gases in water

(iii) Distinguish between the properties of hard and soft water

(iv) Determine the causes of hardness

(v) Identify methods of removal of hardness

(vi) Describe the processes involved in the treatment of water for town supply

(vii) Distinguish between these phenomena

(viii) Identify the various compounds that exhibit these phenomena

7. Solubility

(a) Unsaturated, saturated, and supersaturated solutions. Solubility curves and simple deductions from them (solubility defined in terms of mole per dm³) and simple calculations.

(b) Solvents for fats, oils, and paints and their use for stain removal.

(c) False solutions (Suspensions and colloids): Properties and examples. Examples include Harmattan haze and water paints as suspensions, and fog, milk, aerosol spray, emulsion paints, and rubber solution as colloids.

Objectives: Candidates should be able to:

(i) Distinguish between different types of solutions.

(ii) Interpret solubility curves and calculate solute amounts that can dissolve at a given temperature.

(iii) Understand temperature-dependent solubility.

(iv) Relate solvent properties to their uses.

(v) Differentiate among true solutions, suspensions, and colloids.

(vi) Compare properties of true and ‘false’ solutions. (vii) Provide typical examples of suspensions and colloids.

8. Environmental Pollution

(a) Sources and effects of pollutants.

(b) Air pollution: Examples of air pollutants such as H₂S, CO, SO₂, nitrogen oxides, chlorofluorocarbons, and dust.

(d) Soil pollution: Effects of oil spillage, biodegradable and non-biodegradable pollutants.

Objectives: Candidates should be able to:

(i) Identify types of pollution and their sources.

(ii) Classify pollutants as biodegradable or non-biodegradable.

(iii) Understand the environmental impacts of pollution.

(iv) Identify measures to control environmental pollution.

9. Acids, Bases, and Salts

(a) General characteristics and properties of acids, bases, and salts. Acid/base indicators, basicity of acids; normal, acidic, basic, and double salts. Explanation of acids as substances that furnish H₃O⁺ ions or donate protons. Examples include ethanoic, citric, and tartaric acids, and alums as double salts. Preparation of salts by neutralization, precipitation, and action of acids on metals. Oxides and trioxocarbonate (IV) salts.

(b) Qualitative comparison of conductances of molar solutions of strong and weak acids and bases, relationship between conductance and amount of ions present.

(d) Acid/base titrations.

(e) Hydrolysis of salts: Examples such as NH₄Cl, AlCl₃, Na₂CO₃, and CH₃COONa.

Objectives: Candidates should be able to:

(i) Distinguish properties of acids and bases.

(ii) Identify types of acids and bases.

(iii) Determine acid basicity using acid/base indicators.

(iv) Differentiate acidity and alkalinity.

(v) Outline methods for salt preparation.

(vi) Classify different types of salts.

(vii) Relate ion dissociation to acid/base strength.

(viii) Calculate pH and pOH.

(ix) Choose appropriate acid/base indicators.

(x) Interpret titration curves.

(xi) Solve problems using mole concepts.

(xii) Balance equations for salt hydrolysis.

(xiii) Determine resultant solution properties (acidic, basic, neutral).

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10. Oxidation and Reduction

(a) Oxidation as addition of oxygen or removal of hydrogen.

(b) Reduction as removal of oxygen or addition of hydrogen.

(d) Use of oxidation numbers. Oxidation and reduction as changes in oxidation number, and use of oxidation numbers in balancing equations.

(e) IUPAC nomenclature of inorganic compounds using oxidation number.

(f) Tests for oxidizing and reducing agents.

Objectives: Candidates should be able to:

(i) Express oxidation and reduction.

(ii) Classify chemical reactions as oxidation or reduction.

(iii) Balance redox reaction equations.

(iv) Determine oxidation numbers.

(v) Calculate electron transfer in redox reactions.

(vi) Identify names of redox species.

(vii) Distinguish oxidizing and reducing agents.

(viii) Apply oxidation numbers in naming inorganic compounds.

(ix) Correlate reagents with their oxidation-reduction capabilities.

11. Electrolysis

(a) Electrolytes and non-electrolytes. Faraday’s laws of electrolysis.

(b) Electrolysis of dilute H₂SO₄, aqueous CuSO₄, CuCl₂ solution, dilute and concentrated NaCl solutions, and fused NaCl.

(c) Uses of electrolysis: Purification of metals (e.g., copper), and production of elements and compounds (Al, Na, O₂, Cl₂, NaOH).

(d) Electrochemical cells: Redox series (K, Ca, Na, Mg, Al, Zn, Fe, Sn, Pb, H, Cu, Hg, Ag, Au,) half-cell reactions and electrode potentials. Simple calculations.

(e) Corrosion as an electrolytic process, cathodic protection of metals, methods like painting, electroplating, and coating with grease or oil to prevent iron corrosion.

Objectives: Candidates should be able to: (i) Distinguish between electrolytes and nonelectrolytes. (ii) Perform calculations using Faraday’s laws.

(iii) Select appropriate electrodes for different electrolytes. (iv) Specify chemical reactions at electrodes.

(v) Determine electrolysis products.

(vi) Identify factors affecting electrolysis products.

(vii) Explain applications of electrolysis.

(viii) Recognize electrochemical cells.

(ix) Calculate electrode potentials from half-cell reactions.

(x) Understand uses of electrolytic processes.

(xi) Describe methods for protecting metals.

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12. Energy Changes

(a) Energy changes ∆H in physical and chemical changes: Dissolution of substances in/or reaction with water (e.g., Na, NaOH, K, NH₄Cl). Endothermic (+∆H) and exothermic (-∆H) reactions.

(b) Entropy as an order-disorder phenomenon: Examples include mixing gases and dissolution of salts.

(c) Spontaneity of reactions: ∆G₀ = 0 for equilibrium, ∆G greater or less than zero for non-spontaneity or spontaneity respectively.

Objectives: Candidates should be able to:

(i) Identify heat change types (∆H) in physical and chemical processes.

(ii) Interpret heat change graphs.

(iii) Relate substance state to orderliness.

(iv) Determine reaction spontaneity conditions.

(v) Relate ∆H, ∆S, and ∆G as reaction driving forces.

(vi) Solve problems using ∆G₀ = ∆H₀ – T∆S₀.

13. Rates of Chemical Reactions

Topics: (a) Factors affecting chemical reaction rates:

(i) Temperature (e.g., HCl and Na₂S₂O₃ reaction, Mg and HCl reaction).

(ii) Concentration (e.g., HCl and Na₂S₂O₃, HCl and marble, iodine clock reaction, gaseous systems using pressure as a concentration term).

(iii) Surface area (e.g., marble and HCl reaction with marble in powdered vs. lumps).

(iv) Catalysts (e.g., H₂O₂ or KClO₃ decomposition with/without MnO₂).

(b) Reaction rate curves.

(c) Activation energy: Qualitative Arrhenius’ law and collision theory, light effects on reactions (e.g., alkane halogenation).

Objectives: Candidates should be able to:

(i) Identify factors affecting chemical reaction rates.

(ii) Analyze temperature effects on reaction rates.

(iii) Assess concentration/pressure impact on reaction rates.

(iv) Compare reaction rate effects based on surface area.

(v) Choose appropriate catalysts for reactions and assess impacts.

(vi) Moderate reaction rate impacts.

(vii) Interpret reaction rate graphs.

(viii) Solve problems involving reaction rates.

(ix) Relate reaction rates to kinetic theory significance.

(x) Understand activation energy importance in reactions. (xi) Determine activation energy (Ea) from reaction rate curves.

14. Chemical equilibrium

(a). Reversible reactions and factors governing the equilibrium position.

(b). Dynamic equilibrium. Le Chatelier’s principle and equilibrium constant.

(c). Simple examples to include action of steam on iron and N $_{2}$ O $_{4}$ $⇌$ 2NO $_{2}$ . No calculation will be required.

Objectives: Candidates should be able to:
(i) identify the factors that affects the position of equilibrium of a chemical reaction;

(ii) predict the effects of each factor on the position of equilibrium

(iii) determine the effects of these factors on equilibrium constant.

15. Non-metals and their compounds

(a) Hydrogen: commercial production from water gas and cracking of petroleum fractions, laboratory preparation, properties, uses and test for hydrogen.

(b) Halogens: Chlorine as a representative element of the halogen. Laboratory preparation, industrial preparation by electrolysis, properties and uses, e.g. water sterilization, bleaching, manufacture of HCl, plastics and insecticides. Hydrogen chloride and Hydrochloric acid: Preparation and properties. Chlorides and test for chlorides.

(c) Oxygen and Sulphur
(i) Oxygen: Laboratory preparation, properties and uses. Commercial production from liquid air. Oxides: Acidic,basic, amphoteric and neutral, trioxygen (ozone) as an allotrope and the importance of ozone in the atmosphere. (ii) Sulphur: Uses and allotropes: preparation of allotropes is not expected . Preparation, properties and uses of sulphur. (IV) oxide, the reaction of SO $_{2}$ with alkalis. Trioxosulphate. (IV) acid and its salts, the effect of acids on salts of trioxosulphate(IV), Tetraoxosulphate(VI) acid: Commercial preparation (contact process only), properties as a dilute acid, an oxidizing and a dehydrating agent and uses. Test for SO $_{4}^{2 -}$ . Hydrogen sulphide: Preparation and properties as a weak acid, reducing agent and precipitating agent. Test for S $^{2 -}$

(d) Nitrogen: (i) Laboratory preparation, (ii) Production from liquid air, (iii) Ammonia: Laboratory and industrial preparations (Haber Process only), properties and uses, ammonium salts and their uses, oxidation of ammonia to nitrogen

(IV) oxide and trioxonitrate (V) acid. Test for NH $_{4}^{+}$

(iv) Trioxonitrate (V) acid: Laboratory preparation from ammonia; properties and uses. Trioxonitrate (V) salt- action of heat and uses. Test for NO $_{3}^{-}$

(v) Oxides of nitrogen: Properties. The nitrogen cycle

(e) Carbon: (i) Allotropes: Uses and properties
(ii) Carbon(IV) oxide- Laboratory preparation, properties and uses. Action of heat on trioxocarbonate (IV) salts and test for CO $_{3}^{2 -}$
(iii) Carbon(II) oxide: Laboratory preparation, properties including its effect on blood; sources of carbon (II) oxide to include charcoal, fire and exhaust fumes.
(iv) Coal: Different types, products obtained from destructive distillation of wood and coal.
(v) Coke: Classification and uses. Manufacture of synthetic gas and uses.

Objectives: Candidates should be able to:
(i) predict reagents for the laboratory and industrial preparation of these gases and their compounds.

(ii) identify the properties of the gases and their compounds.

(iii) compare the properties of these gases and their compounds.

(iv) specify the uses of each gas and its compounds;

(v) determine the specific test for each gas and its compounds.

(vi) determine specific tests for Cl $^{-}$ , SO $_{4}^{2 -}$ , SO $_{3}^{2 -}$ , S $^{2 -}$ , NH $_{4}^{+}$ , NO $_{3}^{-}$ , CO $_{3}^{2 -}$ , HCO $_{3}^{-}$

(vii) predict the reagents for preparation, properties and uses HCl(g) and HCl(aq);

(viii) identify the allotropes of oxygen;

(ix) determine the significance of ozone to our environment.

(x) classify the oxides of oxygen and their properties

(xi) identify the allotropes of sulphur and their uses;

(xii) predict the reagents for preparation, properties and uses of SO $_{2}$ and H $_{2}$ S;

(xiii) specify the preparations of H $_{2}$ SO $_{4}$ and H $_{2}$ SO $_{3}$ , their properties and uses.

(xiv) specify the laboratory and industrial preparation of NH $_{3}$ ;

(xv) identify the properties and uses of NH $_{3}$ ;

(xvi) identify reagents for the laboratory preparation of HNO $_{3}$ , its properties and uses;

(xvii) specify the properties of N $_{2}$ O, NO, NO $_{2}$ gases.

(xviii) examine the relevance of nitrogen cycle to the environment.

(xix) identify allotropes of carbon;

(xx) predict reagents for the laboratory preparation of CO $_{2}$ ;

(xxi) specify the properties of CO $_{2}$ and its uses;

(xxii) determine the reagents for the laboratory preparation of CO;

(xxiii) predict the effects of CO on human;

(xxiv) identify the different forms of coal:

(xxv) determine their uses;

(xxvi) specify the products of the destructive distillation of wood and coal;

(xxvii) specify the uses of coke and synthetic gas.

16. Metals and their compounds

(a) General properties of metals

(b) Alkali metals e.g. sodium (i) Sodium hydroxide:- Production by electrolysis of brine, its action on aluminium, zinc and lead ions. Uses including precipitation of
metallic hydroxides. (ii) Sodium trioxocarbonate (IV) and sodium hydrogen trioxocarbonate (IV): Production by Solvay process, properties and uses, e.g. Na $_{2}$ CO $_{3}$ in the manufacture of glass.
(iii) Sodium chloride: its occurrence in sea water and uses, the economic importance of sea water and the recovery of sodium chloride.

(c) Alkaline-earth metals, e.g. calcium; calcium oxide, calcium hydroxide and calcium trioxocarbonate (IV); Properties and uses. Preparation of calcium oxide from sea shells, the chemical composition of cement and the setting of mortar. Test for Ca $^{2 +}$ .

(d) Aluminium Purification of bauxite, electrolytic extraction, properties and uses of aluminium and its compounds. Test for Al $^{3 +}$

(e) Tin Extraction from its ores. Properties and uses.

(f) Metals of the first transition series. Characteristic properties: (i) electron configuration (ii) oxidation states (iii) complex ion formation (iv) formation of coloured ions (v) catalysis

(g) Iron Extraction from sulphide and oxide ores, properties and uses, different forms of iron and their properties and advantages of steel over iron. Test for Fe $^{2 +}$ and Fe $^{3 +}$

(h) Copper Extraction from sulphide and oxide ores, properties and uses of copper. Preparation and uses of copper(II) tetraoxosulphate(VI). Test for Cu $^{2 +}$

(i) Alloy Steel, stainless steel, brass, bronze, type- metal, duralumin, soft solder, permallory and alnico (constituents and uses only).

Objectives: Candidates should be able to:

(i) specify the general properties of metals;

(ii) determine the method of extraction suitable for each metal;

(iii) relate the methods of extraction to the properties for the metals;

(iv) compare the chemical reactivities of the metals;

(v) specify the uses of the metals;

(vi) determine specific test for metallic ions;

(vii) determine the process for the production of the compounds of these metals;

(viii) compare the chemical reactivities of the compounds;

(ix) specify the uses of these compounds

(x) specify the chemical composition of cement.

(xi) describe the method of purification of bauxite;

(xii) specify the ores of tin;

(xiii) relate the method of extraction to its properties;

(xiv) specify the uses of tin;

(xv) identify the general properties of the first transition metals;

(xvi) deduce reasons for the specific properties of the transition metals;

(xvii) determine the IUPAC names of simple transition metal complexes

(xviii) determine the suitable method of extraction of iron;

(xix) specify the properties and uses of iron;

(xx) identify the different forms of iron, their compositions, properties and uses.

(xxi) identify the appropriate method of extraction of copper from its compounds;

(xxii) relate the properties of copper and its compound to their uses.

(xxiii) specify the method for the preparation of CuSO $_{4}$ ;

(xxiv) specify the constituents and uses of the various alloys mentioned.

(xxv) compare the properties and uses of alloys to pure metals.

17. Organic Compounds

An introduction to the tetravalency of carbon, the general formula, IUPAC nomenclature and the determination of
empirical formula of each class of the organic compounds mentioned below.

(a) Aliphatic hydrocarbons: (i) Alkanes Homologous series in relation to physical properties, substitution reaction and a few examples and uses of halogenated products. Isomerism: structural only (examples on isomerism should not go beyond six carbon atoms). Petroleum: composition, fractional distillation and major products; cracking and reforming, Petrochemicals – starting materials of organic syntheses, quality of petrol and meaning of octane number. (ii) Alkenes Isomerism: structural and geometric isomerism, additional and polymerization reactions, polythene and synthetic rubber as examples of products of polymerization and its use in vulcanization. (iii) Alkynes Ethyne – production from action of water on carbides, simple reactions and properties of ethyne.

(b) Aromatic hydrocarbons e.g. benzene – structure, properties and uses.

(c) Alkanols Primary, secondary, tertiary – production of ethanol by fermentation and from petroleum by-products. Local examples of fermentation and distillation, e.g. gin from palm wine and other local sources and glycerol as a polyhydric alkanol. Reactions of OH group – oxidation as a distinguishing test among primary, secondary and tertiary alkanols (Lucas test).

(d) Alkanals and alkanones. Chemical test to distinguish between alkanals and alkanones.

(e) Alkanoic acids. Chemical reactions; neutralization and esterification, ethanedioic (oxalic) acid as an example of a dicarboxylic acid and benzene carboxylic acid as an
example of an aromatic acid.

(f) Alkanoates Formation from alkanoic acids and alkanols – fats and oils as alkanoates. Saponification: Production of soap and margarine from alkanoates and distinction between detergents and soaps.
(g) Amines (Alkanamines) Primary, Secondary, and tertiary

(h) Carbohydrates: Classification – mono-, di- and polysaccharides; composition, chemical tests for simple sugars and reaction with concentrated tetraoxosulphate (VI) acid. Hydrolysis of complex sugars e.g. cellulose from cotton and starch from cassava, the uses of sugar and starch in the production of alcoholic beverages, pharmaceuticals and textiles.
(i) Proteins: Primary structures, hydrolysis and tests (Ninhydrin, Biuret, Millon’s and xanthoproteic)
Enzymes and their functions.
(j) Polymers: Natural and synthetic rubber; addition and condensation polymerization. – Methods of preparation, examples and uses. Thermoplastic and thermosetting plastics.

Objectives: Candidates should be able to:

(i) derive the name of organic compounds from their general formulae;

(ii) relate the name of a compound to its structure

(iii) relate the tetravalency of carbon to its ability to form chains of compound (catenation);

(iv) classify compounds according to their functional groups;

(v) derive empirical formula and molecular formula, from given data;

(vi) relate structure/functional groups to specific properties;

(vii) derive various isomeric forms from a given formula;

(viii) distinguish between the different types of isomerism;

(ix) specify the uses of these compounds

(x) specify the chemical composition of cement.

(xi) specify the uses of various hydrocarbons;

(xii) identify crude oil as a complex mixture of hydrocarbons;

(xiii) relate the fractions of hydrocarbons to their properties and uses;

(xiv) relate transformation processes to quality improvement of the fractions;

(xv) distinguish between various polymerization processes;

(xvi) specify the process involved in vulcanization;

(xvii) specify chemical test for terminal alkynes

(xviii) distinguish between aliphatic and aromatic hydrocarbons;

(xix) relate the properties of benzene to its structure

(xx) compare the various classes of alkanols;

(xxi) determine the processes involved in ethanol production;

(xxii) examine the importance of ethanol as an alternative energy provider;

(xxiii) distinguish the various classes of alkanols;

(xxiv) differentiate between alkanals and alkanones;

(xxv) compare the various types of alkanoic acids;

(xxvi) identify natural sources of alkanoates;

(xxvii) specify the methods for the production of soap, detergent and margarine.

(xxviii) distinguish between detergent and soap;

(xxix) compare the various classes of alkanamine;

(xxx) identify the natural sources of carbohydrates;

(xxxi) compare the various classes of carbohydrates;

(xxxii) infer the products of hydrolysis and dehydration of carbohydrates;

(xxxiii) determine the uses of carbohydrates;

(xxxiv) specify the tests for simple sugars;

(xxxv) identify the basic structure of proteins;

(xxxvi) specify the methods and products of hydrolysis;

(xxxvii) specify the various tests for proteins;

(xxxviii) distinguish between natural and synthetic polymers;

(xxxix) differentiate between addition and condensation polymerization processes;

(xl) classify natural and commercial polymers and their uses;

(xli) distinguish between thermoplastics and thermosetting plastics.

18. Chemistry and Industry

Chemical industries: Types, raw materials and relevancies; Biotechnology.

Objectives: Candidates should be able to :

(i) classify chemical industries in terms of products;

(ii) identify raw materials for each industry;

(iii) distinguish between fine and heavy chemicals;

(iv) enumerate the relevance of each of these industries;

(v) relate industrial processes to biotechnology.

Frequently Asked Questions

What is Le Chatelier’s principle and how is it applied in chemical equilibrium?

Le Chatelier’s principle states that if a system at equilibrium is disturbed, the system will adjust itself to partially counteract the effect of the disturbance and re-establish equilibrium. It is applied to predict how changes in concentration, temperature, and pressure affect the position of equilibrium in reversible reactions.

Are calculations required in the WAEC Chemistry exam?

Yes, calculations are an essential part of the WAEC Chemistry exam, particularly in topics like Stoichiometry, Chemical Energetics, and Chemical Kinetics. Ensure you understand how to perform calculations involving moles, concentration, energy changes, and reaction rates.

Conclusion

Here you have it, the full list of Chemistry WAEC syllabus, it up to you now to study with it and prepare well for your examination. If you have questions, kindly drop it at the comment section.

WAEC Chemistry Syllabus For 2024 [Full List]

WAEC Chemistry Syllabus

1. Separation of Mixtures and Purification of Chemical Substances

2. Chemical Combination

3. Kinetic Theory of Matter and Gas Laws

4. Atomic Structure and Bonding

5. Air

6. Water

7. Solubility

8. Environmental Pollution

9. Acids, Bases, and Salts

10. Oxidation and Reduction

11. Electrolysis

12. Energy Changes

13. Rates of Chemical Reactions

14. Chemical equilibrium

15. Non-metals and their compounds

16. Metals and their compounds

17. Organic Compounds

18. Chemistry and Industry

Frequently Asked Questions

What is Le Chatelier’s principle and how is it applied in chemical equilibrium?

Are calculations required in the WAEC Chemistry exam?

Conclusion

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WAEC Chemistry Syllabus

1. Separation of Mixtures and Purification of Chemical Substances

2. Chemical Combination

3. Kinetic Theory of Matter and Gas Laws

4. Atomic Structure and Bonding

5. Air

6. Water

7. Solubility

8. Environmental Pollution

9. Acids, Bases, and Salts

10. Oxidation and Reduction

11. Electrolysis

12. Energy Changes

13. Rates of Chemical Reactions

14. Chemical equilibrium

15. Non-metals and their compounds

16. Metals and their compounds

17. Organic Compounds

18. Chemistry and Industry

Frequently Asked Questions

What is Le Chatelier’s principle and how is it applied in chemical equilibrium?

Are calculations required in the WAEC Chemistry exam?

Conclusion

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