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WAEC Syllabus for Chemistry PDF 2022/2023 Download is out and available on our website. Here is the most Current WAEC Chemistry Syllabus today to get A1 in the upcoming Chemistry Exams in WAEC SSCE. the syllabus gives detail on the WAEC Chemistry scheme of Work.

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WAEC Syllabus for Chemistry

The Syllabus will help candidates to know the WAEC Chemistry Scheme of work and the WAEC Chemistry area of concentration while making adequate preparation for the exams.

WAEC Chemistry Syllabus 2022 PDF Download Available

Below is the Syllabus for Chemistry examination:

2.0 STRUCTURE OF THE ATOM

(a) Gross features of the atom.
(b) (i) Atomic number/proton number, number of neutrons, isotopes, atomic mass, mass number
(ii) Relative atomic mass (Ar) and relative molecular mass (Mr) based on Carbon-12 scale.
(iii) Characteristics and nature of matter.
(c) Particulate nature of mater: physical and chemical changes.
(d) (i) Electron Configuration
(ii) Orbitals
(iii) Rules and principles for filling in electrons.
(1) Short account of Dalton’s atomic theory and limitations, J.J. Thompson’s experiment and Bohr’s model of the atom. (2) Ontline description of the Rutherford’s alpha scattering experiment to establish the structure of the atom.
Meaning and representation in symbols of atoms and sub-atomic particles.
(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.

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|negatron|lepton} 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.

(1) Aufbau Principle, Hund’s Rule of Maximum Multiplicity and Pauli Exclusion Principle. (2) Abbreviated and {detailed|elaborate|elaborated|careful} {electron|negatron|lepton} configuration in terms of s, p, and d WAEC {syllabus|course of study|program|programme|curriculum|information|info} For Chemistry |

{3|three}.0 STANDARD SEPARATION TECHNIQUES FOR MIXTURES

(a) Classification of mixtures.
(b) Separation techniques
(c) Criteria for purity
Solid-solid, solid-liquid, liquid-liquid, gas-gas with examples.
Crystallization, distillation, precipitation, magnetization, chromatography, sublimation etc. Boiling {point|purpose} for liquids and {melting point|freezing point|temperature} for solids.

WAEC Chemistry Syllabus

4.0 PERIODIC CHEMISTRY
(a) Periodicity of the elements. (b) {different|totally different|completely different} {categories|classes} of {elements|parts|components} {in the|within the} {periodic table|table|tabular array}.

(c) Periodic law:
(i) Trends on periodic table; (ii) Periodic gradation of {the elements|the weather} {in the|within the} {third period|playing period|period of play|play} (Na – Ar). (d) Reactions between acids and metals, their oxides and trioxocarbonates (IV). (e) Periodic gradation of {elements|parts|components} in {group|cluster} seven, the halogens: F, Cl, Br and I.

(f) Elements of the first transition series. 21Sc – 30Zn
Electron configurations leading to group and periodic classifications. Metals, semi-metals, non-metals {in the|within the} {periodic table|table|tabular array} and halogens. Alkali metals, {alkaline earth|alkaline-earth metal|metallic element|metal} metals and transition metals as metals.

Explanation of the periodic law. Periodic properties; atomic size, ionic size, ionization energy, {electron|negatron|lepton} affinity and {electronegativity|negativity|tendency|inclination}. Simple discrepancies {should|ought to} be accounted for in {respect to|reference to|regard to|relation to|relevance|relevancy} {beryllium|Be|glucinium|atomic number 4|metallic element|metal}, boron, {oxygen|O|atomic number 8|chemical element|element|gas} and {nitrogen|N|atomic number

7|chemical element|element|gas}. (1) Progression from: (i) {metallic|metallic |aluminous|aluminiferous|antimonial|argentiferous|auriferous|gold-bearing|bimetal|bimetallic|bronze|gold|golden|gilded|silver|tinny|metallike} to non-metallic character of element; (ii) ionic to {covalent|valence|valency} bonding in compounds. (2) {differences|variations} and similarities {in the|within the} properties between the second {and the|and therefore the|and also the} {third period|playing period|period of play|play} {elements|parts|components} {should|ought to} be {stated|declared|explicit |expressed}.

(1) Period three metals (Na, Mg, Al). (2) Period four metals (K, Ca). (3) Chemical equations. (4) {ph|pH|pH scale|hydrogen ion concentration} of solutions of the {metallic|metallic |aluminous|aluminiferous|antimonial|argentiferous|auriferous|gold-bearing|bimetal|bimetallic|bronze|gold|golden|gilded|silver|tinny|metallike} oxides and trioxocarbonates.

WAEC Syllabus For Chemistry | 5.0 CHEMICAL BONDS

(a) Interatomic bonding
(b) (i) Formation of ionic bonds and compounds.
(ii) Properties of ionic compounds.
(c) Naming of ionic compounds.
(d) Formation of covalent bonds and compounds.
(e) (i) Properties of covalent compounds.
(ii) Coordinate (dative) covalent bonding.
Meaning of chemical bonding. Lewis dot structure {for simple|for easy|for straightforward} ionic and {covalent|valence|valency} compounds.

Formation of stable compounds from ions. Factors influencing formation: ionzation energy; {electron|negatron|lepton} affinity and {electronegativity|negativity|tendency|inclination} {difference|distinction}. Solubility in polar and non-polar solvents, electrical {conductivity|conduction|physical phenomenon}, hardness and {melting point|freezing point|temperature}.

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|freezing point|temperature}, boiling {point|purpose} and electrical {conductivity|conduction|physical phenomenon}. Formation and {difference|distinction} between pure {covalent|valence|valency} and coordinate (dative) {covalent|valence|valency} bonds.

(f) Shapes of molecular compounds.
(g) (i) Metallic Bonding
(ii) Factors influencing its formation.
(iii) Properties of metals.
(h) (i) Inter molecular bonding
(ii) Intermolecular forces in covalent compounds.
(iii) Hydrogen bonding
(iii) van der Waals forces
(iv) Comparison of all bond types.
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. WAEC {syllabus|course of study|program|programme|curriculum|information|info} For Chemistry | IUPAC system {for simple|for easy|for straightforward} 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. Linear, planar, tetrahedral and shapes {for some|for a few} compounds e.g.

BeCl2, BF3, CH4, NH3, CO2. Factors {should|ought to} include: atomic radius, ionization energy and {number|variety|range} of valence electrons.

Types of specific packing not required. Typical properties {including|as well as|together with} heat and electrical {conductivity|conduction|physical phenomenon}, {malleability|plasticity|physical property}, lustre, ductility, {sonority|plangency|resonance|reverberance|ringing|sonorousness|vibrancy|timbre|timber|quality|tone} and hardness.

Relative physical properties of polar and non-polar compounds. Description of formation and nature should be treated. Dipole-dipole, {induced|induced |elicited|evoked|iatrogenic} dipole-dipole, {induced|induced |elicited|evoked|iatrogenic} dipole-induced dipole forces {should|ought to} be treated {under|beneath|underneath|below} van der Waal’s forces. Variation of the melting points and boiling points of noble gases, halogens and alkanes {in the|within the} homologous series explained in terms of van der Waal’s forces; and variation {in the|within the} boiling points of {h2o|water|H2O|binary compound|liquid}, and H2S explained {using|exploitation|victimization|victimisation|mistreatment} {hydrogen|H|atomic number 1|chemical element|element|gas} bonding

WAEC Syllabus For Chemistry |

6.0 STOICHIOMETRY AND CHEMICAL REACTIONS
(a) (i) Symbols, formulae and equations.
(ii) chemical symbols
(iii) Empirical and molecular formulae. (iv) Chemical equations and IUPAC names of chemical compounds.

(v) Laws of chemical combination.
(b) Amount of substance.
(c) Mole ratios
(d) (i) Solutions
(ii) Concentration terms
(iii) Standard solutions. (e) Preparation of solutions from liquid solutes by {the method|the tactic|the strategy} of dilution. Symbols of {the first|the primary} thirty {elements|parts|components} and {other|different|alternative} common {elements|parts|components} that {are not|aren’t|don’t seem to be} among {the first|the primary} thirty {elements|parts|components}.

Calculations involving formulae and equations will be required. Mass and volume relationships in chemical reactions {and the|and therefore the|and also the} {stoichiometry|ratio} of such reactions such as: calculation of {percentage|proportion|share} composition of {element|part|component}. (1) Combustion reactions (including combustion {of simple|of straightforward|of easy} hydrocarbons) (2) Synthesis (3) Displacement or replacement (4) Decomposition (5) Ionic reactions (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.
(1) Mass and volume measurements. (2) The mole as a unit of measurement; Avogadro’s constant, L= 6.02 x 1023 entities mol-1. (3) Molar quantities and their uses. (4) Moles of electrons, atoms, molecules, formula units etc.
Use of mole ratios in crucial ratio of chemical reactions. Simple calculations to work out the amount of entities, quantity of substance, mass, concentration, volume and proportion yield of product. (1) construct of an answer as created from solvent and matter. (2) Distinguishing between dilute solution and concentrated solution. (3) Basic, acidic and neutral solutions.
Mass (g) or moles (mol) per unit volume. Emphasis on current IUPAC chemical word, symbols and conventions. Concentration be expressed as mass concentration, g dm-3, molarity, mol dm-3.
(1) Preparation of some primary standards e.g anhydrous Na2CO3, (COOH)2, 2H2O/H2C2O4.2H2O. (2) Meanning of the terms primary normal, secondary normal and normal resolution.
Dilution factor

WAEC course of study For Chemistry | seven.0 STATES OF MATTER

(a) (i) Kinetic theory of matter.
(ii) Changes of state of matter.
(iii) Diffusion
(b) Gases:
(i) Characteristics and nature of gases;
(ii) The gas laws;
(iii) Laboratory preparation and properties of some gases.
(c) (i) Liquids
(ii) Vapour and gases.
(d) Solids:
(i) Characteristics and nature;
(ii) Types and structures;
(iii) Properties of solids.
(e) Structures, properties and uses of diamond and graphite.
(f) Determination of melting points of covalent solids
(1) Postulates of the kinetic theory of matter. (2) Use of the kinetic theory of gases to clarify the subsequent processes: melting of solids, boiling of liquids, evaporation of liquids, dissolution of solutes, Brownian motion and diffusion.
(1) Changes of state of matter ought to be explained in terms of movement of particles. It ought to be stressed that randomness decreases (and orderliness increases) from aerosolised state to liquid state and to solid state and contrariwise. (2) Illustrations of changes of state using the different forms of water, iodine, sulphur, naphthalene etc. (3) {brownian motion|Brownian movement|Brownian motion|pedesis|movement|motion} to be illustrated {using|exploitation|victimization|victimisation|mistreatment} any of {the following|the subsequent} experiments: (a) {pollen|spore} grains/powdered sulphur in water (viewed {under|beneath|underneath|below} a microscope); (b) smoke {in a|during a|in an exceedingly|in a very} glass {container|instrumentality|instrumentation} {illuminated|lighted|lit|well-lighted|light} by {a strong|a robust|a powerful} {light|light-weight|lightweight} from the side; (c) a {dusty|dust-covered|dirty |soiled|unclean} {room|area|space} being {swept|swept |sweptback|sweptwing} and viewed from outside {under|beneath|underneath|below} {sunlight|daylight}.
(1) Experimental demonstration of diffusion of two gases. (2) Relationship between speed at {which|that} {different|totally different|completely different} gas particles move {and the|and therefore the|and also the} {masses|plenty|lots} of particles. (3) Experimental demonstration of diffusion of {solute|substance|matter} particles in liquids.
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|rationalization|clarification} {of each|of every} of the gas laws {using|exploitation|victimization|victimisation|mistreatment} the kinetic model. The use of Kinetic molecular theory {to explain|to elucidate|to clarify} changes in gas volumes, pressure, temperature. Mathematical relations of the gas law PV= nRT Ideal and Real gases Factors {responsible for|liable for|answerable for|chargeable for|to blame for|accountable for} the deviation of real gases from ideal {situation|state of affairs|scenario}.
(1) Preparation of {the following|the subsequent} gases: H2, NH3 and {co2|carbon dioxide|CO2|carbonic acid gas|dioxide|greenhouse gas|greenhouse emission}. Principles of purification and collection of gases. (2) Physical and chemical properties of the gases.
Characteristics and nature of liquids {based on|supported} the arrangement of particles, shape, volume, compressibility, density and viscosity.
(1) {concept|conception|construct|idea|thought} of vapour, {vapour pressure|vapor pressure|pressure|pressure level|force per unit area}, saturated vapour pressure, boiling and evaporation. (2) Distinction between vapour and gas. (3) {effect|result|impact} of {vapour pressure|vapor pressure|pressure|pressure level|force per unit area} on boiling points of liquids. (4) Boiling at reduced pressure.
(1) Ionic, metallic, covalent network and molecular solids. Examples in each case. (2) Arrangements of particles ions, molecules and atoms in the solid state.
Relate the properties of solids to {the type|the sort|the kind} of interatomic and {intermolecular|unit|building block} bonding {in the|within the} solids. Identification of {the types|the kinds|the categories} of chemical bonds in {graphite|black lead|plumbago|carbon|C|atomic number 6} and {differences|variations} {in the|within the} physical properties.
The uses of diamond and {graphite|black lead|plumbago|carbon|C|atomic number 6} {related to|associated with} 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 acid|acid} (oxalic) and {ethanamide|acetamide|amide}.
WAEC {syllabus|course of study|program|programme|curriculum|information|info} For Chemistry | {8|eight}.0 ENERGY AND ENERGY CHANGES
(a) Energy and enthalpy
(b) Description, definition and illustrations of energy changes and their effects.
Explanation of the terms energy and enthalpy.

Energy changes associated with chemical processes.
(1) Exothermic and endothermic processes. (2) Total energy of a system {as the|because the} {sum|add|total} {of various|of varied|of assorted} {forms of|sorts of|kinds of|types of|styles of|varieties of} energy e.g. kinetic, potential, electrical, heat, sound etc. (3) {enthalpy|heat content|total heat|H|physical property} changes {involved|concerned} {in the|within the} following processes: combustion, dissolution and neutralization.

WAEC {syllabus|course of study|program|programme|curriculum|information|info} For Chemistry |

{9|nine}.0 ACIDS, BASES AND SALTS

(a) Definitions of acids and bases.
(b) Physical and chemical properties of acids and bases.
(c) Acids, bases and salts as electrolytes.
(d) Classification of acids and bases.
(e) Concept of pH
(f) Salts:
(i) Laboratory and industrial preparation of salts; (ii) Uses;
(iii) Hydrolysis of salt.
(g) Deliquescent, efflorescent and hygroscopic compound.
(h) Acid-Base indicators
(i) Acid-Base titration
(1) {arrhenius|Arrhenius|Svante August Arrhenius|chemist|physicist} {concepts|ideas|ideas} 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.
Characteristic properties of acids and bases in {aqueous solution|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.
(1) Strength of acids and bases.

(2) Classify acids and bases into {strong|robust|sturdy} and weak. (3) Extent of dissociation reaction with water and {conductivity|conduction|physical phenomenon}. (4) Behaviour of weak acids and weak bases in water as example of equilibrium systems.
(1) Definition of {ph|pH|pH scale|hydrogen ion concentration} and {knowledge|information|data} of {ph scale|pH|pH scale|hydrogen ion concentration}.

(2) {measurement|measuring|measure|mensuration|activity} of {ph|pH|pH scale|hydrogen ion concentration} of solutions {using|exploitation|victimization|victimisation|mistreatment} {ph|pH|pH scale|hydrogen ion concentration} meter, calometric {methods|ways|strategies} or universal indicator. (3) Significance of {ph|pH|pH scale|hydrogen ion concentration} values in {everyday life|lifestyle|way of life|existence|standard of living|daily life} e.g. acid rain, pH of soil, blood, urine.
Meaning of salts. Types of salts: {normal|traditional|traditional}, acidic, basic, double {and complex|and sophisticated|and complicated} salts.

(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.

(1) Explanation of how salts forms 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.

Use of hygroscopic compounds as drying agent should be emphasized.

(1) Qualitative description of how acidbase 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 forms. (4) Working pH ranges of methyl orange and phenolphthalein.

(1) Knowledge and correct use of relevant apparatus. (2) Knowledge of how acid-bases 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.

WAEC Syllabus For Chemistry |

10.0 SOLUBILITY OF SUBTANCES

(a) General principles

(b) Practical application of solubility

(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.

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.

WAEC Syllabus For Chemistry | 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;

(ii) Le Chatelier’s principle.

(1) Definition of reaction rate. (2) Observable physical and changes: colour, mass, temperature, pH, formation of precipitate etc.

(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.

(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.

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.

Prediction of the effects of external influence of concentration, temperature pressure and volume changes on equilibrium systems.

WAEC Syllabus For Chemistry |

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.

(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;

(vi) Corrosion of metals.

(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.

(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.

Balancing redox equations by: (a) ion, electron or change in oxidation number/states; (b) half reactions and overall reaction.

Definition/Explanation (1) Standard hydrogen electrode: meaning of standard electrode potential (Eo) and its measurement. (2) Only metal/metal ion systems should be used.

(1) Electrochemical cells as a combination of two half-cells. (2) The meaning of magnitude and sign of the e.m.f.

(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.

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.

(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.)

13.0 CHEMISTRY OF CARBON COMPOUNDS

(a) Classification

(b) Functional group

(b) Separation and purification of organic compounds.

(c) Petroleum/crude oil

(d) Determination of empirical and molecular formulae and molecular structures of organic compounds.

(e) General properties of organic compounds:

(i) Homologous series;

(ii) Isomerism.

(f) Alkanes:

(i) Sources, properties;

(ii) Uses.

(g) Alkenes:

(i) Sources and properties;

(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.

(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;

(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

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.

(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.

(1) Gradation in physical properties. (2) Effects on the physical properties by introduction of active groups into the inert alkane.

(1) Examples should be limited to compounds having maximum of five carbon atoms. (2) Differences between structural and geometric/stereo isomerism.

(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.

(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.

Use of reaction with Br2/water, Br2/CCl4 and KMnO4(aq) as means of characterizing alkenes.

(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.

Chemical reactions: halogenation, combustion, hydration and hydrogenation.

Resonance in benzene. Stability leading to substitution reactions.

(1) Addition reactions: hydrogenation and halogenation (mechanism not required). (2) Compare reactions with those of alkenes

(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.

Primary, secondary and tertiary alkanols.

Boiling point, solubility in water. Including hydrogen bonding effect.

(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).

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.

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.

RECOMMENDED:

14.0 CHEMISTRY, INDUSTRY AND THE ENVIRONMENT

(a) Chemical industry

(b) Pollution: air, water and soil pollution;

(c) Biotechnology.

(1) Natural resources in candidate’s won country. (2) Chemical industries in candidates 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.

(1) Sources, effects and control. (2) Greenhouse effect and depletion of the ozone layer. (3) Biodegradable and non-biodegradable pollutants.

Food processing, fermentation including production of garri, bread and alcoholic beverages e.g. Local gin.

15.0 BASIC BIOCHEMISTRY AND SYNTHETIC POLYMERS

(a) Proteins:

(i) Sources and properties;

(ii) Uses of protein.

(b) Amino acid

(c) Fats/oils:

(i) Sources and properties;

(ii) General structure of fats/oils;

(iii) Preparation of soap;

(iv) Uses of fats/oils.

(d) Carbohydrates:

(i) Sources and nomenclature;

(ii) Properties;

(iii) Carbohydrate as examples of polymer;

(iv) Uses.

(e) Synthetic polymers:

(i) Properties;

(ii) Uses of polymers.

Proteins as polymers of amino acids molecules linked by peptide or amide linkage.

Physical properties e.g. solubility Chemical properties to include: (a) hydrolysis of proteins; (b) laboratory test using Ninhydrin/Biuret reagent/Millons reagent.

(1) Nomenclature and general structure of amino acids. (2) Difunctional nature of amino acids.

As alkyl alkanoates (esters).

From animals and plants. Physical properties such as solubility. Chemical properties: (a) acidic and alkaline hydrolysis; (b) hydrogenation; (c) test for fats and oil.

As mono-, di-, and tri- esters of propane1,2,3-triol (glycerol).

(1) Preparation of soap (saponification) from fats and oils. (2) Comparison of soap less detergents and their action on soft and hard water.

(1) Classes of carbohydrates as: (a) monosaccharides; (b) disaccharides; (c) polysaccharides. (2) Name and components of various classes of carbohydrates.

(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 Benedicts solution or Tollen’s reagent.

(1) Starch as a polymer made up of glucose units. (2) Condensation of monosaccharides to form disaccharides and polysaccharides.

(1) Definition of terms: monomers, polymers and polymerization. (2) Addition and condensation polymerization. (3) Classification and preparation based on the monomers and comonomers.

(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

SECTION B (For candidates in Ghana only)

WAEC Syllabus For Chemistry | 1.0 STRUCTURE OF THE ATOM

(a) Elementary treatment of mass spectrometer.

(b) (i) Nuclear chemistry

(ii) Types and nature of radiations: alpha, beta particles and gamma radiation.

(iii) Radioactivity: induced/stimulated.

(iv) Nuclear reactions: fission and fusion in nuclear reactions.

(v) Effects and application of radioactivity

(1) Qualitative knowledge of the mass spectrometer: principles and operations of the mass spectrometer; and its use to detect isotopes, determination of Relative atomic and molecular masses only. (2) Wave nature of electrons. (3) Quantum numbers and their importance.

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

(1) Carbon dating (qualitative treatment only). (2) Use of radioactivity in agriculture, medicine and industries. (3) Hazards associated with nuclear radiations.

Factors affecting stability of nuclides: Binding energy, neutron-proton ratio, and half life. Calculations involving half-life

WAEC Syllabus For Chemistry | 2.0 PERIODIC CHEMISTRY

(a) Reactions between acids and metals their oxides and trioxocarbonates (IV).

(b) Acidic properties of oxides of nonmetals.

(c) Physical and chemical properties of period 3 elements and their compounds.

(d) Silicon

(e) Periodic gradation of elements in group seven i.e. the halogens.

(f) Bonding in complex compounds.

(g) Shapes of complex compounds.

(h) Elements of the first transition series.

(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.

(1) Oxides of carbon, nitrogen, sulphur, phosphorus and chlorine. (2) pH of aqueous solutions of the oxides. (3) Chemical equations.

(1) Comparison of the physical and chemical properties of period three elements. (2) Comparison of the physical and chemical properties of (hydrides, oxides, hydroxides and chlorides) compounds. (3) Thermal stability of CO32- and NO3- of Li, Na, K, Mg and Ca. (4) Experiment to compare thermal stability of Na2CO3/LiCO3/CuSO4

(1) Structures for SiO2 and CO2 account for the differences between physical and chemical properties of the two oxides. (2) Uses of silicon and its compounds e.g. ceramics, glass, silica gel and microchips.

(1) Inter- atomic bond energies. (2) Hydrides and their acid strength comparison of the Ka values of the hydrogen halides. (3) Variable oxidation states of the halogens.

Definition of ligands and central ions Examples of ligands (1) Formation of coordination compounds. (2) Nomenclature of complex ions and compounds (Cl-, F-, I-, NO3-, NH3, H2O, SO42-).

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.

WAEC Syllabus For Chemistry | 3.0. CHEMICAL BONDS

(a) Formation of Ionic bonds: (i) Factors that influence ionic bond formation

(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.

Factors should include lattice energy.

(1) Ionic character (polarity) in covalent bonds based on electronegativity difference between the species involved. (2) Effects of covalent and ionic character in ionic and covalent bonds on the solubility, thermal stability and boiling points of ionic and covalent compounds.

Definition of Hybridization.

(1) Description of sp, sp2, sp3 hybrid orbitals. (2) Shapes of sp, sp2, sp3 and sp3d2 hybrid orbitals. Treatment should be limited to the following molecules only. CH4, H2O, NH3, BCl3, C2H2, BeCl2, C2H4 and SF6.

Description of sigma and pi bonds. Using C2H2 and C6H6

WAEC Syllabus For Chemistry | 4.0 SOLUTIONS

(a) Preparation of solutions from liquid solutes by the method of dilution.

(1) Outline of steps involved in the preparation of solutions from liquid solutes. (2) Determination of concentration of liquid solutes (stock solution) given the density, w/v, w/w), specific gravity, relative molecular mass, molar mass, and % purity. (3) Primary standard, secondary standard and standardized solution.

WAEC Syllabus For Chemistry | 5.0 ENERGY AND ENERGY CHANGES

(a) Energy changes in physical and isolated systems.

(b) Hess’s Law of heat summation and Born-Haber cycle.

(c) Bond Energy

(1) Definition and understanding of the meaning of the energy terms: systems, surroundings, open and closed. (2) Enthalpy change involved in the following processes: combustion, atomization, sublimation, hydration/salvation and dissolution.

Explanation of Hess’s law and its application in the development of the Born-Haber cycle. (1) Use of difference cycles to illustrate Hess’s law.

(2) Simple calculations using chemical equations, energy cycles or diagrams with given energy changes.

Explanation of bond energy and bond dissociation energy. (1) Bond energy as an average value. Differences in bond energy and bond dissociation energy. (2) Bond energy in molecules and its use in assessment of bond strength, energy content and enthalpy of reaction. (3) Calculations using summation of bond energies in reactants and products as a measure of enthalpy of reaction.

WAEC Syllabus For Chemistry | 6.0 ACIDS, BASES AND SALTS

(a) Definitions of acids and bases.

(b) pH, pOH and pKw

(c) Partial ionization of weak acids and weak bases.

(d) Buffer Solutions

(e) Acid base titrations

(1) Bronsted – Lowry and Lewis concept of acids and bases. (2) Conjugate acid-base pair concept in terms of equilibrium.

(1) Ionic product constant of water Kw = [H+(aq)][OH(aq)] = 1.0 x 10-14 mol2dm-6. (2) pH and pOH as a measure of acidity and alkalinity respectively pH = -log[H3O+]. (3) Knowledge of pH scale. (4) Calculation of [H+], [OH-] and the corresponding pH and pOH of given solutions.

Explanation of pKa and pKb of weak acids and bases. (1) Behaviour of weak acids and weak bases in water as example of equilibrium systems. (2) Calculations involving Ka, pKa and Kb, pKb. (3) Ka, pKa and Kb, pKb as measurements of acid and basic strengths respectively.

(1) Qualitative definition of buffers. (2) Examples of buffers from the laboratory. (3) Preparation of buffer solutions.

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

WAEC Syllabus For Chemistry | 7.0 SOLUBILITY OF SUBSTANCES

(a) Solubility and solubility product.

(c) Crystallization and recrystallization

(1) Explanation of solubility products (Ksp) of sparingly soluble ionic compounds. (2) Calculations involving solubility and solubility products. (3) Factors affecting solubility.

Explanation of the effect of lattice energy and hydration energy on crystallization and recrystallization.

WAEC Syllabus For Chemistry | 8.0 CHEMICAL KINETICS AND EQUILIBRIUM SYSTEMS

(a) Rate law and Order of reaction

(b) Rate determining step of a multi-step reaction.

(c) Equilibrium

(d) Equilibrium Law of Mass Action.

(1) Deduction of order and rate law from experimental data. (2) Simple relationship between rates and concentration of zero, first and second order reactions. Graphical representation of zero, first and second order reactions. (3) Half-life for first order reactions and its significance. (4) General rate law equation. (5) Derivation of the rate expression from experimentally determined rate data: R = k[A]x [B]y where k = rate constant.

(1) Mathematical expression for the determination of equilibrium constant K (2) K is constant for a system at constant temperature. (3) Relationship between Kp and Kc. (4) Calculation of Kp and Kc from given set of data. (5) Difference between homogeneous and heterogeneous equilibrium systems

Syllabus WAEC Chemistry | 9.0 CHEMISTRY OF CARBON COMPOUNDS

(a) Separation and Purification.

(b) Determination of empirical and molecular formulae.

(c) Reactivity of Organic Compounds.

(d) Alkanes

(e) (i) Reactions of benzene.

(ii) Comparison or reactions of benzene and alkenes.

Other methods should include solvent extraction and melting point determinations.

Outline of steps in: (a) Detection of N, S and the halogens. (b) Estimation of C, H and O.

(1) Inductive effect and Mesomeric effect. (2) Resonance illustrated with benzene molecule. (3) Explanation of the terms: nucleophiles, electrophiles, free radicals and ions. homolytic fission, heterolytic fission.

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).

WAEC Syllabus For Chemistry | 10.0 CHEMICAL INDUSTRY AND 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.

(1) Metals – gold, bauxite, manganese and iron. (2) Precious stone – diamond. (3) Industrial mining of limestone CaCO3, clay Kaolin, solar salt (4) Processing of Au, Al, Fe as main products (5) Uses of the metals

(1) Sources of raw materials for cement production. (2) Processes involved in the production of cement. (3) Uses of cement. (4) Environmental impact.

WAEC Syllabus For Chemistry | SECTION C

(For candidates in Nigeria, Sierra-Leone, Liberia and The Gambia)

1.0 NON METALS AND THEIR COMPOUNDS

(a) Carbon: (i) Allotropes of carbon;

(ii) Coal: I. Types;

Destructive distillation of coal and uses of the products.

(iii) Coke: I. Classification and uses; II. Manufacture of synthetic gas and uses.

(iv) Oxides of carbon I. Carbon (IV) oxides;

Carbon (II) oxides;

III. Trioxocarbonate (IV) salt

(b) Oxygen: (i) Laboratory and industrial preparation; (ii) Properties and uses;

(iii) Binary compounds of oxygen: acidic, basic, amphoteric and neutral oxides.

(c) Hydrogen: (i) Laboratory preparations; (ii) Properties and uses.

(d) Water and solution: (i) Composition of water;

(ii) Water as a solvent; (iii)Hardness of water, causes and methods of removing it;

(iv) Treatment of water for town supply.

(e) Halogens:

(i) Chlorine: I. Laboratory preparation; II. Properties and reactions.

(f) Hydrogen chloride gas: (i) Laboratory preparation; (ii) Properties and uses;

(iii) Uses of halogen compounds.

(g) Nitrogen: (i) Preparation and properties;

(ii) Uses of nitrogen; (iii) Compounds of nitrogen: I. Ammonia;

Trioxonitrate (V) acid;

III. Trioxonitrate (V) salts.

(h) Sulphur: (i) Allotropes and uses; (ii) Compound of sulphur; (iii) Trioxosulphate (IV) acids and its salts; (iv) Tetraoxosulphate (VI) acid: industrial preparation, reactions and uses.

(i) The noble gases: properties and uses.

(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.

Different types should include anthracite, peat and lignite.

Water gas and producer gas.

(1) Laboratory preparation. (2) Properties and uses. (3) Test for carbon (IV) oxides.

Properties and uses only.

(1) Properties: solubility, action of heat, reaction with dilute acid.

(2) Uses.

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.

(1) Advantages and disadvantages of hard water and soft water. (2) Experiments to compare the degrees of hardness in different samples of water.

Redox properties of the elements; displacement reaction of one halogen by another.

Properties should include: (a) variable oxidation states; (b) reaction with water and alkali (balanced equation required)

(1) Test for HCl gas. (2) Fountain experiment.

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.

(1) Laboratory and industrial preparations. (2) Properties and uses. (3) Test for ammonia. (4) Fountain experiment.

(1) Laboratory preparation. (2) Properties and uses. (1) Action of heat will be required. (2) Test for trioxonitrate (V) ions.

Contact process should be discussed.

WAEC Syllabus For Chemistry | 2.0 METALS AND THEIR COMPOUNDS

(a) Extraction of metals:

(i) Aluminium; (ii) Iron; (iii) Tin.

(b) Alloys.

(c) Properties and uses of sodium and its compounds.

(d) Properties and uses of calcium and its compounds.

(e) Reactivity of iron and aluminium with air, water and acids. (f) Properties and uses of copper and its compounds

(1) Raw materials, processing, main products and by-products. (2) Uses of metals.

Common alloys of Cu, Al, Pb, Fe, Sn and their uses.

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

WAEC Syllabus For Chemistry | (a) GENERAL SKILLS AND PRINCIPLES

Candidates will be expected to be familiar with the following skills and principles: (i) Measurement of mass and volume; (ii) Preparation and dilution of standard solutions; (iii) Filtration, recrystallisation and melting point determination; (iv) Measurement of heats of neutralization and solutions; (v) Determination of pH 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.

WAEC Syllabus For Chemistry | (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:

(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-.

WAEC Syllabus For Chemistry | (d) 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-.

(iv) Confirmatory tests for the above anions

(v) Comparative study of the halogens; displacement reactions.

(vi) Characteristic tests for the following gases: H2; NH3; CO2; HCl and SO2.

(vii) 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).

How to Use WAEC Chemistry Syllabus 2022

It is important for all candidates to make effective use of the Syllabus to Pass Chemistry very well. Get the syllabus is just a Step while the effective usage is most important aspect.

The following are ways to pass WAEC Chemistry with the Syllabus:

  1. Get the latest of the Chemistry Syllabus ready.
  2. Check the general Scheme and the ones for your Country
  3. Start studying beginning from the first subject.
  4. Make reference to WAEC Chemistry past questions to know how the questions comes.
  5. Always write down important points and randomly repeated Questions.
  6. Cover 70  percent of the Syllabus before One months to the exams commencement.
  7. Always do revision and keep testing yourself with exercises.
  8. Remember! Through God all things are possible.
  9. Good Luck!

If there are questions regarding the WAEC Syllabus for Chemistry, Feel free to leave it on the comments section below, we will get to you shortly.

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