JAMB Chemistry syllabus.

About this syllabus official

Summarised from the examining body's own published syllabus. 18 topics, verified 2026-10-24.

Current UTME syllabus as served by IBASS on 2026-10-24; JAMB does not print the applicable years in this document.

Structure (sections, topics, contents and objectives) summarised from JAMB's publicly published UTME syllabus, with citation and link. The document itself is not reproduced or redistributed.

Source: https://ibass.jamb.gov.ng/static/media/Chemistry.9efd0b98043d56922aaa.pdf

Source: https://ibass.jamb.gov.ng/e-syllabus

General objectives

• understand the basic principles and concepts in chemistry
• interpret scientific data relating to chemistry
• deduce the relationships between chemistry and other sciences
• apply the knowledge of chemistry to industry and everyday life

Topics

1. Separation of mixtures and purification of chemical substances (SS 1-3)

• elements, compounds and mixtures
• chemical and physical changes
• pure and impure substances
• boiling, density, freezing and melting points
• separation processes: evaporation, simple and fractional distillation, sublimation, re-crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation, filtration, centrifugation

You should be able to:

• distinguish between elements, compounds and mixtures
• differentiate between chemical and physical changes
• distinguish between pure and impure substances
• use boiling and melting points as criteria for purity
• identify the properties of the components of a mixture
• specify the principle involved in each separation method
• apply the principles of separation processes in everyday life

2. Chemical combination (SS 1-3)

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

You should be able to:

• deduce the chemical laws from given expressions, statements or data
• perform simple calculations involving formulae, equations, chemical composition and the mole concept
• deduce the stoichiometry of chemical reactions

3. Kinetic theory of matter and gas laws (SS 1-3)

• phenomena supporting the kinetic theory: melting, vapourization, boiling, freezing, condensation; molecular motion and Brownian movement
• laws of Boyle, Charles, Avogadro, Gay-Lussac, Graham and Dalton (partial pressure); molar volume and atomicity of gases
• the ideal gas equation (PV = nRT)
• relationship between vapour density and relative molecular mass
• ideal and real gases

You should be able to:

• apply the kinetic theory to distinguish between solids, liquids and gases
• deduce reasons for change of state
• draw inferences based on molecular motion
• deduce gas laws from given expressions or statements
• interpret graphical representations of the gas laws
• perform simple calculations based on these laws and relationships
• state factors responsible for the deviation of real gases from ideal behaviour

4. Atomic structure and bonding (SS 1-3)

• atoms, molecules and ions; the work of Dalton, Millikan, Rutherford, Moseley, Thomson and Bohr
• atomic structure: four quantum numbers, arrangement of electrons in orbitals, electron configuration, atomic number, mass number, isotopes (elements of atomic number 1-20)
• shapes of s and p orbitals
• the periodic table and periodicity: alkali and alkaline-earth metals, halogens, noble gases, transition metals; variation of ionization energy, ionic radii, electron affinity, electronegativity, electrical and thermal conductivity
• chemical bonding: electrovalency and covalency; hydrogen and metallic bonding; coordinate bond (e.g. [Fe(CN)6]3-, [Fe(CN)6]4-, [Cu(NH3)4]2+, [Ag(NH3)2]+); van der Waals forces
• shapes of simple molecules: linear (H2, O2, Cl2, HCl, CO2), non-linear (H2O), tetrahedral (CH4), pyramidal (NH3)

You should be able to:

• distinguish between atoms, molecules and ions
• identify the contributions of these scientists to atomic structure
• deduce the number of protons, neutrons and electrons from atomic and mass numbers
• apply the rules guiding the arrangement of electrons in an atom
• identify common elements exhibiting isotopy and relate isotopy to mass number
• perform simple calculations relating to isotopy
• differentiate between the shapes of the orbitals
• determine the number of electrons in s and p orbitals
• relate atomic number to the position of an element on the periodic table
• relate properties of groups of elements on the periodic table
• identify reasons for variation in properties across the period and down the groups
• differentiate between the types of bonding
• deduce bond types based on electron configurations
• relate the nature of bonding to properties of compounds
• differentiate between the various shapes of molecules

5. Nuclear chemistry (SS 1-3)

• radioactivity: types, properties and detection of radiations
• natural and artificial radioactivity
• nuclear stability and radioactive decay
• nuclear reactions: fusion and fission

You should be able to:

• distinguish between ordinary chemical reaction and nuclear reaction
• differentiate between natural and artificial radioactivity
• compare the properties of the types of nuclear radiation
• compute simple calculations on the half-life of a radioactive material
• balance simple nuclear equations
• identify the applications of radioactivity

6. Solubility (SS 1-3)

• unsaturated, saturated and supersaturated solutions; solubility curves and simple deductions (solubility in mol/dm3); simple calculations
• solvents for fats, oil, perspiration and paints; their use in removing stains
• true and false solutions (suspensions and colloids): properties and examples (Harmattan haze, water paints; fog, milk, blood, aerosol spray, emulsion paints, rubber solution)

You should be able to:

• distinguish between the types of solutions
• interpret solubility curves
• calculate the amount of solute that can dissolve in a given amount of solvent at a given temperature
• deduce that solubility is temperature-dependent
• relate the nature of solvents to their uses
• differentiate among true solutions, suspensions and colloids
• compare the properties of true and false solutions
• provide typical examples of suspensions and colloids

7. Environmental pollution (SS 1-3)

• air: natural gaseous constituents and their proportions (nitrogen, oxygen, water vapour, carbon (IV) oxide, noble gases argon and neon); factors causing variation; air as a mixture; uses of noble gases
• air pollution: pollutants such as H2S, CO, SO2, oxides of nitrogen, chlorofluorocarbons, dust; sources and effects
• water pollution: sewage and oil pollution
• soil pollution: oil spillage; biodegradable and non-biodegradable pollutants

You should be able to:

• give reasons for the existence of air as a mixture
• identify the principle involved in separating air components
• state reasons for variation in the composition of air
• specify uses of some constituents of air
• identify types of pollution and pollutants
• specify sources of pollutants
• classify pollutants as biodegradable and non-biodegradable
• specify the effects of pollution on the environment
• identify measures for control of environmental pollution

8. Acids, bases and salts (SS 1-3)

• general characteristics, properties and uses of acids, bases and salts; acid/base indicators; basicity of acids; normal, acidic, basic and double salts; acid as a proton donor or furnisher of H3O+; natural organic acids (ethanoic, citric, tartaric); alums; preparation of salts by neutralization, precipitation and action of acids on metals; oxides and trioxocarbonate (IV) salts
• qualitative comparison of conductance of molar solutions of strong and weak acids and bases
• pH and pOH scale; simple calculations; significance of pH in everyday life; buffer solution
• acid/base titrations
• hydrolysis of salts (e.g. NH4Cl, AlCl3, Na2CO3, CH3COONa)

You should be able to:

• distinguish between the properties of acids and bases
• identify types of acids and bases
• determine the basicity of acids
• differentiate between acidity and alkalinity using acid/base indicators
• identify methods of preparation of salts
• classify types of salts
• relate degree of dissociation to strength and to conductance
• perform simple calculations on pH and pOH
• state the significance of pH in everyday life
• state applications of buffer solution
• identify the appropriate acid-base indicator
• interpret titration curves
• perform simple calculations based on the mole concept
• balance equations for the hydrolysis of salts
• deduce the properties (acidic, basic, neutral) of the resultant solution

9. Oxidation and reduction (redox) (SS 1-3)

• oxidation as addition of oxygen
• reduction as removal of oxygen with the aid of hydrogen
• oxidation and reduction in terms of electron transfer
• oxidation numbers: redox as change in oxidation number; balancing simple equations
• IUPAC nomenclature of inorganic compounds using oxidation number
• tests for oxidizing and reducing agents

You should be able to:

• identify the various ways of expressing oxidation and reduction
• classify chemical reactions as oxidation or reduction
• balance redox equations
• deduce the oxidation number of chemical species
• compute the number of electrons transferred in redox reactions
• identify the redox species in a reaction
• distinguish between oxidizing and reducing agents
• apply oxidation numbers in naming inorganic compounds
• relate reagents to their oxidizing and reducing abilities

10. Electrolysis (SS 1-3)

• electrolytes and non-electrolytes; Faraday's laws of electrolysis
• electrolysis of dilute H2SO4, aqueous CuSO4, CuCl2, dilute and concentrated NaCl solutions and fused NaCl; factors affecting discharge of ions
• uses of electrolysis: purification of metals (e.g. copper); production of Al, Na, O2, Cl2, NaOH
• electrochemical cells: electrochemical series (K, Ca, Na, Mg, Al, Zn, Fe, Sn, Pb, H, Cu, Hg, Ag, Au); half-cell reactions and electrode potentials (simple calculations only)
• corrosion as an electrolytic process; cathodic protection, painting, electroplating, coating with grease or oil

You should be able to:

• distinguish between electrolytes and non-electrolytes
• perform calculations based on the faraday as a mole of electrons
• identify suitable electrodes for different electrolytes
• specify the reactions at the electrodes and determine the products
• identify factors that affect the products of electrolysis
• specify areas of application of electrolysis
• state the significance of the electrochemical series
• identify electrochemical cells
• calculate electrode potentials using half-cell equations
• determine areas of application of electrolytic processes
• identify methods used in protecting metals

11. Energy changes (SS 1-3)

• energy changes (ΔH) in physical and chemical changes: dissolution in or reaction with water (e.g. Na, NaOH, K, NH4Cl); endothermic (+ΔH) and exothermic (-ΔH) reactions
• entropy as an order-disorder phenomenon (mixing of gases, dissolution of salts)
• spontaneity of reactions: ΔG° = 0 as criterion for equilibrium; ΔG < 0 spontaneous, ΔG > 0 non-spontaneous

You should be able to:

• determine the types of heat changes (ΔH) in physical and chemical processes
• interpret graphical representations of heat changes
• relate the physical state of a substance to its degree of orderliness
• determine the conditions for spontaneity of a reaction
• relate ΔH°, ΔS° and ΔG° as driving forces for chemical reactions
• solve simple problems based on ΔG° = ΔH° - TΔS°

12. Rates of chemical reaction (SS 1-3)

• factors that change reaction rate: temperature (e.g. HCl and Na2S2O3, or Mg and HCl); concentration/pressure (e.g. HCl and Na2S2O3, HCl and marble, iodine clock reaction); surface area (marble and HCl, powdered vs lumps of the same mass); catalyst (decomposition of H2O2 or KClO3 with or without MnO2)
• reaction rate curves
• activation energy: qualitative treatment of Arrhenius' law and collision theory; effect of light on some reactions (e.g. halogenation of alkanes)

You should be able to:

• identify the factors that affect the rate of a chemical reaction
• determine the effect of temperature on reaction rate
• examine the effect of concentration/pressure on reaction rate
• describe how reaction rate is affected by surface area
• determine the types of catalysts suitable for different reactions and their effects
• determine ways of moderating these effects
• interpret reaction rate curves
• solve simple problems on rates of reaction
• relate the rate of reaction to the kinetic theory of matter
• examine the significance of activation energy
• deduce the activation energy (Ea) from reaction rate curves

13. Chemical equilibria (SS 1-3)

• reversible reactions and factors governing the equilibrium position; dynamic equilibrium
• Le Chatelier's principle and its industrial applications
• equilibrium constant (simple examples: action of steam on iron; N2O4 ⇌ 2NO2); no calculation required

You should be able to:

• identify the factors that affect the position of equilibrium
• predict the effect of each factor on the position of equilibrium
• specify industrial processes where Le Chatelier's principle is required
• determine the effects of these factors on the equilibrium constant

14. Non-metals and their compounds (SS 1-3)

• hydrogen: commercial production from water gas and cracking of petroleum fractions; laboratory preparation, properties, uses and test
• halogens: chlorine - laboratory preparation, industrial preparation by electrolysis, properties and uses (water sterilization, bleaching, manufacture of HCl, plastics, insecticides); hydrogen chloride and hydrochloric acid; chlorides and test for chlorides
• oxygen: laboratory preparation, properties, uses; commercial production from liquid air; acidic, basic, amphoteric and neutral oxides; ozone as an allotrope and its importance
• water: composition by volume; water as solvent; dissolved atmospheric gases; temporary and permanent hardness and softening; treatment for town supply; water of crystallization, efflorescence, deliquescence, hygroscopy
• sulphur: uses and allotropes (preparation of allotropes not expected); sulphur (IV) oxide; trioxosulphate (IV) acid and its salts; tetraoxosulphate (VI) acid (contact process only) as dilute acid, oxidizing and dehydrating agent; tests for SO4 2-, SO3 2-, SO2; hydrogen sulphide; tests for S2-, H2S
• nitrogen: laboratory preparation; production from liquid air; ammonia (laboratory and Haber process), ammonium salts, oxidation to nitrogen (IV) oxide and trioxonitrate (V) acid; tests for NH4+, NO2, NH3; trioxonitrate (V) acid and its salts; test for NO3-; oxides of nitrogen; the nitrogen cycle
• carbon: allotropes; carbon (IV) oxide (laboratory preparation, properties, uses; action of heat on trioxocarbonate (IV) salts; tests for CO3 2-, HCO3-, CO2); carbon (II) oxide (preparation, properties, effect on blood, sources); coal (types, destructive distillation of wood and coal); coke (gasification, uses); synthesis gas

You should be able to:

• predict reagents for the laboratory and industrial preparation of these gases and their compounds
• identify and compare the properties of the gases and their compounds
• specify the uses of each gas and its compounds
• determine the specific test for each gas and its compounds, including Cl-
• predict reagents for preparation, properties and uses of HCl(g) and HCl(aq)
• identify the allotropes of oxygen and the significance of ozone
• classify the oxides and their properties
• identify the uses of water and the effects of dissolved atmospheric gases
• distinguish between hard and soft water, the causes of hardness and methods of removal
• describe the treatment of water for town supply
• distinguish efflorescence, deliquescence and hygroscopy and identify compounds exhibiting them
• identify the allotropes of sulphur and their uses
• predict reagents for preparation, properties and uses of SO2 and H2S
• specify the preparation, properties and uses of H2SO4 and H2SO3
• determine specific tests for S2-, SO4 2-, H2S, SO2, SO3 2-
• specify the laboratory and industrial preparation, properties and uses of NH3 and test for NH4+, NH3
• identify reagents for the laboratory preparation of HNO3, its properties and uses
• specify the properties of N2O, NO, NO2 and tests for N2O, NO, NO3-
• examine the relevance of the nitrogen cycle to the environment
• identify allotropes of carbon
• predict reagents for the laboratory preparation of CO2 and CO and specify their properties
• predict the effects of CO on humans
• determine the specific tests for HCO3-, CO3 2-, CO2
• identify forms of coal and their uses; specify products of destructive distillation of wood and coal
• specify the uses of coke and synthesis gas

15. Metals and their compounds (SS 1-3)

• general properties of metals
• alkali metals (e.g. sodium): sodium hydroxide (electrolysis of brine; action on aluminium, zinc and lead ions; precipitation of metallic hydroxides); sodium trioxocarbonate (IV) and sodium hydrogen trioxocarbonate (IV) (Solvay process; Na2CO3 in glass manufacture); sodium chloride (occurrence in sea water, uses, recovery); test for Na+
• alkaline-earth metals (e.g. calcium): calcium oxide, hydroxide and trioxocarbonate (IV); calcium oxide from sea shells; chemical composition of cement and setting of mortar; test for Ca2+
• aluminium: purification of bauxite, electrolytic extraction, properties and uses; test for Al3+
• tin: extraction from its ores, properties and uses
• first transition series: electron configuration, oxidation states, complex ion formation, coloured ions, catalysis
• iron: extraction from sulphide and oxide ores; properties and uses; forms of iron; advantages of steel over iron; tests for Fe2+ and Fe3+
• copper: extraction from sulphide and oxide ores; properties and uses; preparation and uses of copper (II) tetraoxosulphate (VI); test for Cu2+
• alloys: steel, stainless steel, brass, bronze, type-metal, duralumin, soft solder, permalloy, alnico (constituents and uses only)

You should be able to:

• specify the general properties of metals
• determine the method of extraction suitable for each metal and relate it to the metal's properties
• compare the chemical reactivities of the metals and their compounds
• specify the uses of the metals and their compounds
• determine specific tests for metallic ions
• determine the processes for producing compounds of these metals
• specify the chemical composition of cement
• describe the purification of bauxite
• specify the ores of tin, its extraction and uses
• identify the general properties of the first transition metals and deduce reasons for them
• determine the IUPAC names of simple transition metal complexes
• determine the method of extraction of iron; identify forms of iron, their compositions, properties and uses
• identify the method of extraction of copper and relate the properties of copper and its compounds to their uses
• specify the method for the preparation of CuSO4
• specify the constituents and uses of the alloys and compare alloys with pure metals

16. Organic compounds (SS 1-3)

• tetravalency of carbon, general formulae, IUPAC nomenclature, determination of empirical formula
• alkanes: homologous series, substitution reactions, halogenated products; structural isomerism (up to six carbon atoms); petroleum: composition, fractional distillation, major products, cracking and reforming, petrochemicals, octane number
• alkenes: structural and geometric isomerism; addition and polymerization reactions (polythene, synthetic rubber); vulcanization
• alkynes: ethyne from action of water on carbides; simple reactions and properties
• aromatic hydrocarbons, e.g. benzene: structure, properties, uses
• alkanols: primary, secondary, tertiary; ethanol by fermentation and from petroleum by-products; local fermentation and distillation (e.g. gin from palm wine); glycerol; oxidation as distinguishing test (Lucas test)
• alkanals and alkanones: chemical test to distinguish them
• alkanoic acids: neutralization and esterification; ethanedioic (oxalic) acid; benzene carboxylic acid
• alkanoates: formation; fats and oils; saponification; production of soap and margarine; detergents versus soaps
• amines (alkanamines): primary, secondary, tertiary
• carbohydrates: mono-, di- and polysaccharides; tests for simple sugars; reaction with concentrated tetraoxosulphate (VI) acid; hydrolysis of cellulose and starch; uses in alcoholic beverages, pharmaceuticals and textiles
• proteins: primary structure, hydrolysis, tests (ninhydrin, biuret, Millon's, xanthoproteic); enzymes and their functions
• polymers: natural and synthetic rubber; addition and condensation polymerization; thermoplastic and thermosetting plastics

You should be able to:

• derive the names of organic compounds from their general formulae and relate names to structures
• relate the tetravalency of carbon to catenation
• classify compounds according to their functional groups
• derive empirical and molecular formulae from given data
• relate structure/functional groups to specific properties
• derive isomeric forms from a given formula and distinguish types of isomerism
• classify hydrocarbons and distinguish each class by its properties and uses
• identify crude oil as a complex mixture of hydrocarbons and relate fractions to their properties and uses
• relate cracking and reforming to quality improvement of fractions
• distinguish between polymerization processes and specify the process of vulcanization
• specify chemical tests for alkenes and terminal alkynes
• distinguish between aliphatic and aromatic hydrocarbons and relate benzene's properties to its structure
• compare classes of alkanols and the processes of ethanol production
• examine ethanol as an alternative energy source
• differentiate between alkanals and alkanones
• compare alkanoic acids, identify natural sources of alkanoates and infer products of alkanoic acids and alkanols
• specify methods for producing soap, detergent and margarine; distinguish detergent from soap
• compare classes of alkanamines
• identify natural sources, classes, uses and tests of carbohydrates; infer products of hydrolysis and dehydration
• identify the basic structure of proteins, products of hydrolysis and tests for proteins
• distinguish natural and synthetic polymers, addition and condensation polymerization, thermoplastics and thermosetting plastics

17. Chemistry and industry (SS 1-3)

• chemical industries: types, raw materials and relevance
• biotechnology

You should be able to:

• classify chemical industries in terms of products
• identify raw materials for each industry
• distinguish between fine and heavy chemicals
• enumerate the relevance of each industry
• relate industrial processes to biotechnology

18. Astronomical chemistry (SS 1-3)

• solar system, planets, satellite
• composition of the earth: atmosphere, lithosphere, hydrosphere

You should be able to:

• state the composition of the solar system
• list the planets
• identify the segments of the earth
• name the natural satellite of the earth
• identify the smallest planet that is also the farthest from the sun

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