JAMB Chemistry Syllabus

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The aim of the Unified Tertiary Matriculation Examination (UTME) syllabus in Chemistry is to prepare candidates for the Board's examination.

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Elements, compounds and mixtures; chemical and physical changes; pure and impure substances; boiling, density, freezing and melting points; separation processes including evaporation, simple and fractional distillation, sublimation, recrystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation, filtration and centrifugation.

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Laws of definite, multiple and reciprocal proportions; law of conservation of matter; chemical symbols, formulae and equations and their uses; relative atomic mass based on 12C = 12; mole concept and stoichiometry of reactions.

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Phenomena supporting the kinetic theory of matter: melting, vaporization, boiling, freezing and condensation, explained in terms of molecular motion and Brownian movement. Boyle's, Charles's, Avogadro's, Gay-Lussac's, Graham's and Dalton's laws of partial pressure; molar volume and atomicity of gases; ideal gas equation PV = nRT; relationship between vapour density and relative molecular mass; ideal and real gases.

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Concepts of atoms, molecules and ions; contributions of Dalton, Millikan, Rutherford, Moseley, Thomson and Bohr to atomic theory; atomic structure, four quantum numbers, principles governing electron arrangement in orbitals, electron configuration, atomic number, mass number and isotopes, with examples from elements of atomic numbers 1–20; shapes of s and p orbitals.

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The periodic table and periodicity of elements; recognition of families such as alkali metals, alkaline-earth metals, halogens, noble gases and transition metals; variation in ionization energy, ionic radii, electron affinity, electronegativity, electrical conductivity and thermal conductivity.

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Chemical bonding: electrovalency and covalency; electron configurations and tendency to attain noble-gas structures; hydrogen bonding and metallic bonding; coordinate covalent bonds illustrated by [Fe(CN)6]3-, [Fe(CN)6]4-, [Cu(NH3)4]2+ and [Ag(NH3)2]+; van der Waals' forces as a special type of bonding force.

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Shapes of simple molecules: linear molecules (H2, O2, Cl2, HCl and CO2), non-linear H2O, tetrahedral CH4 and pyramidal NH3.

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Radioactivity: types, properties and detection of radiations; natural and artificial radioactivity; nuclear stability and radioactive decay; nuclear reactions including nuclear fusion and fission.

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Unsaturated, saturated and supersaturated solutions; solubility curves and simple deductions; solubility expressed in moles per dm3 and simple calculations.

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Solvents for fats, oils, perspiration and paints, and their uses in stain removal.

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True and false solutions, including suspensions and colloids; properties and examples. Harmattan haze and water paints as suspensions; fog, milk, blood, aerosol sprays, emulsion paints and rubber solution as colloids.

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Air: natural gaseous constituents and their proportions, including nitrogen, oxygen, water vapour, carbon(IV) oxide and noble gases such as argon and neon; factors responsible for variations in atmospheric composition; air as a mixture and uses of noble gases.

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Air pollution: pollutants such as H2S, CO, SO2, oxides of nitrogen, chlorofluorocarbons and dust; their sources and effects.

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Water pollution, including sewage and oil pollution.

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Soil pollution, including oil spillage and biodegradable and non-biodegradable pollutants.

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General characteristics, properties and uses of acids, bases and salts; acid-base indicators; basicity of acids; normal, acidic, basic and double salts. An acid as a substance whose aqueous solution furnishes H3O+ ions or which donates protons. Naturally occurring organic acids including ethanoic, citric and tartaric acids; alums as double salts. Preparation of salts by neutralization, precipitation and reaction of acids with metals; oxides and trioxocarbonate(IV) salts.

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Qualitative comparison of conductance in molar solutions of strong and weak acids and bases; relationship between conductance and the amount of ions present.

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pH and pOH scales; simple calculations; significance of pH in everyday life; buffer solutions.

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Acid-base titrations and titration curves.

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Hydrolysis of salts, including NH4Cl, AlCl3, Na2CO3 and CH3COONa.

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Oxidation as the addition of oxygen; reduction as the removal of oxygen with the aid of hydrogen; oxidation and reduction in terms of electron transfer; oxidation numbers; changes in oxidation number and the use of oxidation numbers to balance simple equations.

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IUPAC nomenclature of inorganic compounds using oxidation numbers; tests for oxidizing and reducing agents.

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Electrolytes and non-electrolytes; Faraday's laws of electrolysis.

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Electrolysis of dilute H2SO4, aqueous CuSO4, CuCl2 solution, dilute and concentrated NaCl solutions, and fused NaCl; factors affecting the discharge of ions at electrodes.

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Uses of electrolysis, including purification of copper and production of aluminium, sodium, oxygen, chlorine and sodium hydroxide.

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Electrochemical cells; electrochemical series: K, Ca, Na, Mg, Al, Zn, Fe, Sn, Pb, H, Cu, Hg, Ag and Au; half-cell reactions and electrode potentials; simple calculations.

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Corrosion as an electrolytic process; prevention of iron corrosion by cathodic protection, painting, electroplating and coating with grease or oil.

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Energy changes (ΔH) accompanying physical and chemical changes; dissolution of substances in water or reactions with water, including Na, NaOH, K and NH4Cl; endothermic (+ΔH) and exothermic (-ΔH) reactions.

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Entropy as an order-disorder phenomenon, illustrated by mixing gases and dissolving salts.

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Spontaneity of reactions; ΔG° = 0 as a criterion for equilibrium; ΔG greater than zero for non-spontaneity and ΔG less than zero for spontaneity.

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Factors affecting reaction rates: temperature, illustrated by reactions between HCl and Na2S2O3 or Mg and HCl; concentration and pressure, illustrated by HCl and Na2S2O3, HCl and marble, and the iodine clock reaction; pressure as a concentration term for gases; surface area, illustrated by powdered and lump marble reacting with HCl; catalysts, illustrated by decomposition of H2O2 or KClO3 in the presence or absence of MnO2.

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Reaction-rate curves; activation energy; qualitative treatment of Arrhenius' law and collision theory; effect of light on reactions such as halogenation of alkanes.

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Reversible reactions and factors governing equilibrium position; dynamic equilibrium; Le Chatelier's principle and its industrial applications; equilibrium constant; examples including the action of steam on iron and N2O4 ⇌ 2NO2. No calculations are required for equilibrium constants.

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Hydrogen: commercial production from water gas and cracking of petroleum fractions; laboratory preparation; properties, uses and tests.

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Halogens: chlorine as a representative element; laboratory and industrial preparation by electrolysis; properties and uses, including water sterilization, bleaching and manufacture of HCl, plastics and insecticides. Hydrogen chloride and hydrochloric acid: preparation and properties; chlorides and tests for chlorides.

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Oxygen: laboratory preparation, properties and uses; commercial production from liquid air; acidic, basic, amphoteric and neutral oxides; ozone as an allotrope and its atmospheric importance.

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Water: formation by combustion of hydrogen; composition by volume; use as a solvent; dissolved atmospheric gases and their biological significance; hard and soft water; temporary and permanent hardness and methods of softening; treatment of water for town supply; water of crystallization, efflorescence, deliquescence and hygroscopy, with examples and uses.

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Sulphur: uses and allotropes; preparation of allotropes is not required. Preparation, properties and uses of sulphur(IV) oxide; reaction of SO2 with alkalis; trioxosulphate(IV) acid and its salts; action of acids on trioxosulphate(IV) salts; tetraoxosulphate(VI) acid, its commercial preparation by the contact process, properties as a dilute acid, oxidizing and dehydrating agent, and uses; tests for SO4^2-, SO3^2- and SO2.

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Hydrogen sulphide: preparation and properties as a weak acid, reducing agent and precipitating agent; tests for S2- and H2S.

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Nitrogen: laboratory preparation and production from liquid air. Ammonia: laboratory and industrial preparation by the Haber process; properties and uses; ammonium salts and uses; oxidation of ammonia to nitrogen(IV) oxide and trioxonitrate(V) acid; tests for NH4+, NO2-, and NH3.

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Trioxonitrate(V) acid: laboratory preparation from ammonia, properties and uses; trioxonitrate(V) salts, action of heat and uses; tests for NO3- and other oxides of nitrogen.

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Oxides of nitrogen: properties of N2O, NO and NO2; the nitrogen cycle.

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Carbon: allotropes and their uses and properties; carbon(IV) oxide, laboratory preparation, properties and uses; action of heat on trioxocarbonate(IV) salts; tests for CO3^2-, HCO3- and CO2; carbon(II) oxide, laboratory preparation, properties and effects on blood; sources including charcoal, fires and exhaust fumes; types of coal; products of destructive distillation of wood and coal; coke, gasification, manufacture of synthesis gas and uses.

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General properties of metals.

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Alkali metals, especially sodium. Sodium hydroxide: production by electrolysis of brine; action on aluminium, zinc and lead ions; uses, including precipitation of metallic hydroxides. Sodium trioxocarbonate(IV) and sodium hydrogen trioxocarbonate(IV): production by the Solvay process, properties and uses, including Na2CO3 in glass manufacture. Sodium chloride: occurrence in seawater, uses, economic importance of seawater, recovery of sodium chloride and test for Na+.

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Alkaline-earth metals, especially calcium; calcium oxide, calcium hydroxide and calcium trioxocarbonate(IV), their properties and uses; preparation of calcium oxide from seashells; chemical composition of cement and setting of mortar; test for Ca2+.

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Aluminium: purification of bauxite, electrolytic extraction, properties and uses of aluminium and its compounds; test for Al3+.

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Tin: extraction from ores, properties and uses.

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Metals of the first transition series: characteristic electron configurations, oxidation states, complex-ion formation, coloured ions and catalysis.

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Iron: extraction from sulphide and oxide ores; properties and uses; different forms of iron, their properties and advantages of steel over iron; tests for Fe2+ and Fe3+.

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Copper: extraction from sulphide and oxide ores; properties and uses of copper; preparation and uses of copper(II) tetraoxosulphate(VI); test for Cu2+.

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Alloys: steel, stainless steel, brass, bronze, type-metal, duralumin, soft solder, permalloy and alnico; constituents and uses.

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Introduction to tetravalency of carbon; general formulae, IUPAC nomenclature and determination of empirical formulae for the classes of organic compounds in the syllabus.

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Aliphatic hydrocarbons: alkanes, their homologous series and physical properties; substitution reactions and uses of halogenated products; structural isomerism limited to six carbon atoms. Petroleum composition, fractional distillation and major products; cracking, reforming, petrochemicals as starting materials for organic synthesis, petrol quality and octane number.

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Alkenes: structural and geometric isomerism, addition and polymerization reactions; polythene and synthetic rubber as polymerization products; vulcanization and its uses.

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Alkynes: ethyne production by the action of water on carbides; simple reactions and properties of ethyne.

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Aromatic hydrocarbons, especially benzene: structure, properties and uses.

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Alkanols: primary, secondary and tertiary alkanols; ethanol production by fermentation and from petroleum by-products; local fermentation and distillation examples, including gin from palm wine and other local sources; glycerol as a polyhydric alkanol; reactions of the OH group; oxidation as a distinguishing test among primary, secondary and tertiary alkanols; Lucas test.

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Alkanals and alkanones: chemical tests for distinguishing them.

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Alkanoic acids: chemical reactions including neutralization and esterification; ethanedioic (oxalic) acid as a dicarboxylic acid; benzene carboxylic acid as an aromatic acid.

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Alkanoates: formation from alkanoic acids and alkanols; fats and oils as alkanoates; saponification; production of soap and margarine from alkanoates; distinction between detergents and soaps.

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Amines (alkanamines): primary, secondary and tertiary classes.

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Carbohydrates: classification into mono-, di- and polysaccharides; composition; chemical tests for simple sugars; reaction with concentrated tetraoxosulphate(VI) acid; hydrolysis of complex sugars, including cellulose from cotton and starch from cassava; uses of sugar and starch in alcoholic beverages, pharmaceuticals and textiles.

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Proteins: primary structures, hydrolysis and tests including Ninhydrin, Biuret, Millon's and xanthoproteic tests; enzymes and their functions.

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Polymers: natural and synthetic rubber; addition and condensation polymerization; methods of preparation, examples and uses; thermoplastic and thermosetting plastics.

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Chemical industries: types, raw materials and relevance; biotechnology.

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The solar system, planets and satellite; composition of the Earth, including the atmosphere, lithosphere and hydrosphere.