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JAMB • Chemistry • Syllabus

JAMB Chemistry Syllabus for UTME 2027

The JAMB Chemistry syllabus is the list of topics UTME Chemistry questions are set from, with the exam body's notes on how far each topic goes. Use it as a revision checklist: pick a topic, read what it covers, then practise past questions on it until you can answer them in exam time.

Syllabus content © The Joint Admissions and Matriculation Board. Source. Summaries marked “Our summary” are written by DeeepSolve.

Matter, atoms and chemical combination

Our summary: Mixtures and pure substances, the laws of chemical combination and the mole, the kinetic theory and gas laws, atoms and bonding, and nuclear chemistry.

Separation of mixtures and purification of chemical substances

Our summary: Elements, compounds and mixtures, how to tell pure from impure substances, and the methods used to separate mixtures.

Contents

  • Elements, compounds and mixtures
  • Chemical and physical changes
  • Pure and impure substances
  • Boiling, density, freezing and melting points
  • Separation processesJAMB note: Evaporation, simple and fractional distillation, sublimation, re-crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation, filtration and centrifugation.

Objectives

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

Chemical combination

Our summary: The laws of chemical combination, symbols, formulae and equations, relative atomic mass, the mole and reacting quantities.

Contents

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

Objectives

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

Kinetic theory of matter and gas laws

Our summary: How moving particles explain changes of state, and the gas laws with their calculations.

Contents

  • Phenomena to support the kinetic theory of matterJAMB note: Using (i) melting; (ii) vapourization; (iii) boiling; (iv) freezing; (v) condensation; in terms of molecular motion and Brownian movement.
  • The laws of Boyle, Charles, Avogadro, Gay-Lussac, Graham and Dalton (law of partial pressure), molar volume and atomicity of gases
  • The ideal gas equation (PV = nRT)
  • The relationship between vapour density of gases and the relative molecular mass
  • Ideal and real gases

Objectives

  • apply the 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/statements;
  • interpret graphical representations related to these laws;
  • perform simple calculations based on these laws, equations and relationships; and
  • state factors responsible for the deviation of real gases from ideal situation.

Atomic structure and bonding

Our summary: Atoms, electron arrangement and orbitals, the periodic table and its trends, the types of chemical bond and the shapes of simple molecules.

Contents

  • The concept of atoms, molecules and ions, the works of Dalton, Millikan, Rutherford, Moseley, Thomson and Bohr
  • Atomic structure, the four quantum numbers, the principles that govern the arrangement of atoms into orbitals, electron configuration, atomic number, mass number and isotopesJAMB note: Specific examples should be drawn from elements of atomic number 1 to 20.
  • Shapes of s and p orbitals
  • The periodic table and periodicity of elementsJAMB note: Presentation of the periodic table with a view to recognizing families of elements e.g. alkali and alkaline-earth metals, halogens, the noble gases and transition metals. The variation of the following properties: ionization energy, ionic radii, electron affinity, electronegativity, electrical and thermal conductivities.
  • Chemical bondingJAMB note: 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.
  • Shapes of simple moleculesJAMB note: Linear (H₂, O₂, Cl₂, HCl and CO₂), non-linear (H₂O) and tetrahedral (CH₄) and pyramidal (NH₃).

Objectives

  • distinguish between atoms, molecules and ions;
  • identify the contributions of these scientists to the development of the atomic structure;
  • deduce the number of protons, neutrons and electrons from atomic and mass numbers of an atom;
  • apply the rules guiding the arrangement of electrons in an atom;
  • identify common elements exhibiting isotopy;
  • 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 atomic 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 different types of bonding;
  • deduce bond types based on electron configurations;
  • relate the nature of bonding to properties of compounds; and
  • differentiate between the various shapes of molecules.

Nuclear chemistry

Our summary: Radioactivity, the radiations it gives off, nuclear stability and half-life, and nuclear fission and fusion.

Contents

  • RadioactivityJAMB note: Types, properties and detection of radiations.
  • Natural and artificial radioactivity
  • Nuclear stability and radioactive decay
  • Nuclear reactionsJAMB note: Nuclear fusion and fission.

Objectives

  • distinguish between ordinary chemical reaction and nuclear reaction;
  • differentiate between natural and artificial radioactivity;
  • compare the properties of the different types of nuclear radiations;
  • compute simple calculations on the half-life of a radioactive material;
  • balance simple nuclear equation; and
  • identify the various applications of radioactivity.

Solutions, the environment and chemical change

Our summary: Solubility, pollution, acids and bases, redox and electrolysis, energy changes, reaction rates and equilibrium.

Solubility

Our summary: Saturated and unsaturated solutions, solubility curves and calculations, useful solvents, and suspensions and colloids.

Contents

  • Unsaturated, saturated and supersaturated solutionsJAMB note: Solubility curves and simple deductions from them (solubility defined in terms of mole per dm³) and simple calculations.
  • Solvents for fats, oil, perspiration and paints and the use of such solvents for the removal of stains
  • True and false solutions (suspensions and colloids)JAMB note: Properties and examples. Harmattan haze and water paints as examples of suspensions, fog, milk, blood, aerosol spray, emulsion paints and rubber solution as examples of colloids.

Objectives

  • distinguish between the different 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 nature of solvents to their uses;
  • differentiate among true solutions, suspensions and colloids;
  • compare the properties of a 'true' solution and a 'false' solution; and
  • provide typical examples of suspensions and colloids.

Environmental pollution

Our summary: What air is made of, and the sources, effects and control of air, water and soil pollution.

Contents

  • Air: the natural gaseous constituents and their proportion in the airJAMB note: Nitrogen, oxygen, water vapour, carbon (IV) oxide and the noble gases (argon and neon).
  • Air: factors responsible for variation of components of air in the environment
  • Air: air as a mixture and some uses of the noble gases
  • Air pollutionJAMB note: Examples of air pollutants such as H₂S, CO, SO₂, oxides of nitrogen, chlorofluorocarbons and dust.
  • Air pollution: sources and effects of pollutants
  • Water pollutionJAMB note: Sewage and oil pollution should be known.
  • Soil pollutionJAMB note: Oil spillage, biodegradable and non-biodegradable pollutants.

Objectives

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

Acids, bases and salts

Our summary: What acids, bases and salts are, how salts are made, strong and weak acids, pH, buffers, titration and salt hydrolysis.

Contents

  • General characteristics, properties and uses of acids, bases and saltsJAMB note: Acids/base indicators, basicity of acids; normal, acidic, basic and double salts. An acid defined as a substance whose aqueous solution furnishes H₃O⁺ ions or as a proton donor. Ethanoic, citric and tartaric acids as examples of naturally occurring organic acids, alums as examples of double salts, preparation of salts by neutralization, precipitation and action of acids on metals. Oxides and trioxocarbonate (IV) salts.
  • Qualitative comparison of the conductance of molar solutions of strong and weak acids and bases, relationship between conductance and amount of ions present
  • pH and pOH scaleJAMB note: Simple calculations, significance of pH value in everyday life, buffer solution.
  • Acid/base titrations
  • Hydrolysis of saltsJAMB note: Simple examples such as NH₄Cl, AlCl₃, Na₂CO₃ and CH₃COONa.

Objectives

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

Oxidation and reduction

Our summary: Oxidation and reduction in terms of oxygen, electrons and oxidation numbers, balancing redox equations, and oxidizing and reducing agents.

Contents

  • Oxidation in terms of the addition of oxygen
  • Reduction as removal of oxygen with the aid of hydrogen
  • Oxidation and reduction in terms of electron transfer
  • Use of oxidation numbersJAMB note: Oxidation and reduction treated as change in oxidation number and use of oxidation numbers in balancing simple equations.
  • IUPAC nomenclature of inorganic compounds using oxidation number
  • Tests for oxidizing and reducing agents

Objectives

  • identify the various forms of expressing oxidation and reduction;
  • classify chemical reactions in terms of oxidation or reduction;
  • balance redox reaction equations;
  • deduce the oxidation number of chemical species;
  • compute the number of electron transfer in redox reactions;
  • identify the name of redox species in a reaction;
  • distinguish between oxidizing and reducing agents in redox reactions;
  • apply oxidation number in naming inorganic compounds; and
  • relate reagents to their oxidizing and reducing abilities.

Electrolysis

Our summary: Electrolytes, Faraday's laws, what forms at the electrodes, uses of electrolysis, electrochemical cells and corrosion.

Contents

  • Electrolytes and non-electrolytes
  • Faraday's laws of electrolysis
  • Electrolysis of dilute H₂SO₄, aqueous CuSO₄, CuCl₂ solution, dilute and concentrated NaCl solutions and fused NaCl
  • Factors affecting discharge of ions at the electrodes
  • Uses of electrolysisJAMB note: Purification of metals e.g. copper and production of elements and compounds (Al, Na, O₂, Cl₂ and NaOH).
  • Electrochemical cellsJAMB note: 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 of metals, painting, electroplating and coating with grease or oil as ways of preventing iron from corrosion

Objectives

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

Energy changes

Our summary: Heat given out or taken in by changes, entropy as disorder, and how ΔG decides whether a reaction is spontaneous.

Contents

  • Energy changes (ΔH) accompanying physical and chemical changesJAMB note: Dissolution of substances in/or reaction with water e.g. Na, NaOH, K, NH₄Cl. Endothermic (+ΔH) and exothermic (−ΔH) reactions.
  • Entropy as an order-disorder phenomenonJAMB note: Simple illustrations like mixing of gases and dissolution of salts.
  • Spontaneity of reactionsJAMB note: ΔG° = 0 as a criterion for equilibrium, ΔG greater or less than zero as a criterion for non-spontaneity or spontaneity respectively.

Objectives

  • 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 the degree of orderliness;
  • determine the conditions for spontaneity of a reaction;
  • relate ΔH°, ΔS° and ΔG° as the driving forces for chemical reactions; and
  • solve simple problems based on the relationships ΔG° = ΔH° − TΔS°.

Rates of chemical reaction

Our summary: The factors that speed up or slow down reactions, reaction rate curves, and activation energy.

Contents

  • Elementary treatment of the following factors which can change the rate of a chemical reaction
  • TemperatureJAMB note: e.g. the reaction between HCl and Na₂S₂O₃ or Mg and HCl.
  • Concentration/pressureJAMB note: e.g. the reaction between HCl and Na₂S₂O₃, HCl and marble and the iodine clock reaction. For gaseous systems, pressure may be used as concentration term.
  • Surface areaJAMB note: e.g. the reaction between marble and HCl with marble in: (i) powdered form; and (ii) lumps of the same mass.
  • CatalystJAMB note: e.g. the decomposition of H₂O₂ or KClO₃ in the presence or absence of MnO₂.
  • Reaction rate curves
  • Activation energyJAMB note: Qualitative treatment of Arrhenius' law and the collision theory, effect of light on some reactions e.g. halogenation of alkanes.

Objectives

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

Chemical equilibria

Our summary: Reversible reactions, dynamic equilibrium, Le Chatelier's principle and the equilibrium constant.

Contents

  • Reversible reactions and factors governing the equilibrium position
  • Dynamic equilibrium
  • Le Chatelier's principle and its industrial applications, equilibrium constantJAMB note: Simple examples to include action of steam on iron and N₂O₄ ⇌ 2NO₂. No calculation will be required.

Objectives

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

Inorganic chemistry: non-metals and metals

Our summary: The common non-metals and metals, how they and their compounds are made, their properties, uses and tests.

Non-metals and their compounds

Our summary: Hydrogen, chlorine, oxygen and water, sulphur, nitrogen and carbon: preparation, properties, uses and tests.

Contents

  • HydrogenJAMB note: Commercial production from water gas and cracking of petroleum fractions, laboratory preparation, properties, uses and test for hydrogen.
  • HalogensJAMB note: Chlorine as a representative element of the halogens. Laboratory preparation, industrial preparation by electrolysis, properties and uses, e.g. water sterilization, bleaching, manufacture of HCl, plastics and insecticides.
  • Hydrogen chloride and hydrochloric acidJAMB note: Preparation and properties. Chlorides and test for chlorides.
  • OxygenJAMB note: 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.
  • WaterJAMB note: Water as a product of the combustion of hydrogen and its composition by volume. Water as solvent, atmospheric gases dissolved in water and their biological significance.
  • Hard and soft waterJAMB note: Temporary and permanent hardness and methods of softening hard water.
  • Treatment of water for town supply
  • Water of crystallization, efflorescence, deliquescence and hygroscopyJAMB note: Example of the substances exhibiting these properties and their uses.
  • SulphurJAMB note: Uses and allotropes: preparation of allotropes is not expected. Preparation, properties and uses of sulphur(IV) oxide, the reaction of SO₂ 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 agents and uses. Test for SO₄²⁻, SO₃²⁻, SO₂.
  • Hydrogen sulphideJAMB note: Preparation and properties as a weak acid, reducing and precipitating agents. Test for S²⁻, H₂S.
  • Nitrogen: laboratory preparation
  • Nitrogen: production from liquid air
  • AmmoniaJAMB note: 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 NH₄⁺, NO₂, NH₃.
  • Trioxonitrate (V) acidJAMB note: Laboratory preparation from ammonia; properties and uses. Trioxonitrate (V) salt - action of heat and uses. Test for NO₃⁻ and other oxides of nitrogen.
  • Oxides of nitrogenJAMB note: Properties.
  • The nitrogen cycle
  • Carbon: allotropesJAMB note: Uses and properties.
  • Carbon(IV) oxideJAMB note: Laboratory preparation, properties and uses. Action of heat on trioxocarbonate(IV) salts and test for CO₃²⁻, HCO₃⁻, CO₂.
  • Carbon(II) oxideJAMB note: Laboratory preparation, properties including its effect on blood, sources of carbon (II) oxide to include charcoal, fire and exhaust fumes.
  • CoalJAMB note: Different types, products obtained from destructive distillation of wood and coal.
  • CokeJAMB note: Gasification and uses. Manufacture of synthesis gas and uses.

Objectives

  • predict reagents for the laboratory and industrial preparation of these gases and their compounds;
  • identify the properties of the gases and their compounds;
  • compare the properties of these gases and their compounds;
  • specify the uses of each gas and its compounds;
  • determine the specific test for each gas and its compounds;
  • determine specific tests for Cl⁻;
  • predict the reagents for preparation, properties and uses of HCl(g) and HCl(aq);
  • identify the allotropes of oxygen;
  • determine the significance of ozone to our environment;
  • classify the oxides of oxygen and their properties;
  • identify the various uses of water;
  • identify the effects of dissolved atmospheric gases in water;
  • distinguish between the properties of hard and soft water;
  • determine the causes of hardness;
  • identify methods of removal of hardness;
  • describe the processes involved in the treatment of water for town supply;
  • distinguish between these phenomena;
  • identify the various compounds that exhibit these phenomena;
  • identify the allotropes of sulphur and their uses;
  • predict the reagents for preparation, properties and uses of SO₂ and H₂S;
  • specify the preparations of H₂SO₄ and H₂SO₃, their properties and uses;
  • determine specific tests for S²⁻, SO₄²⁻, H₂S, SO₂, SO₃²⁻;
  • specify the laboratory and industrial preparation of NH₃;
  • identify the properties and uses of NH₃;
  • determine specific test for NH₄⁺, NH₃;
  • identify reagents for the laboratory preparation of HNO₃, its properties and uses;
  • specify the properties of N₂O, NO, NO₂ gases;
  • determine the specific test for N₂O, NO and NO₃⁻;
  • examine the relevance of nitrogen cycle to the environment;
  • identify allotropes of carbon;
  • predict reagents for the laboratory preparation of CO₂;
  • specify the properties of CO₂ and its uses;
  • determine the reagents for the laboratory preparation of CO;
  • predict the effects of CO on human;
  • determine the specific tests for HCO₃⁻, CO₃²⁻, CO₂;
  • identify the different forms of coal;
  • determine their uses;
  • specify the products of the destructive distillation of wood and coal; and
  • specify the uses of coke and synthesis gas.

Metals and their compounds

Our summary: General properties of metals, sodium, calcium, aluminium, tin, iron, copper and the transition metals, and common alloys.

Contents

  • General properties of metals
  • Alkali metals e.g. sodium
  • Sodium hydroxideJAMB note: Production by electrolysis of brine, its action on aluminium, zinc and lead ions. Uses including precipitation of metallic hydroxides.
  • Sodium trioxocarbonate (IV) and sodium hydrogen trioxocarbonate (IV)JAMB note: Production by Solvay process, properties and uses, e.g. Na₂CO₃ in the manufacture of glass.
  • Sodium chlorideJAMB note: Its occurrence in sea water and uses, the economic importance of sea water and the recovery of sodium chloride, test for Na⁺.
  • Alkaline-earth metals, e.g. calcium; calcium oxide, calcium hydroxide and calcium trioxocarbonate (IV)JAMB note: Properties and uses. Preparation of calcium oxide from sea shells, the chemical composition of cement and the setting of mortar. Test for Ca²⁺.
  • AluminiumJAMB note: Purification of bauxite, electrolytic extraction, properties and uses of aluminium and its compounds. Test for Al³⁺.
  • TinJAMB note: Extraction from its ores. Properties and uses.
  • Metals of the first transition seriesJAMB note: Characteristic properties: (i) electron configuration; (ii) oxidation states; (iii) complex ion formation; (iv) formation of coloured ions; (v) catalysis.
  • IronJAMB note: Extraction from sulphide and oxide ores, properties and uses, different forms of iron, their properties and advantages of steel over iron. Test for Fe²⁺ and Fe³⁺.
  • CopperJAMB note: Extraction from sulphide and oxide ores, properties and uses of copper. Preparation and uses of copper(II) tetraoxosulphate(VI). Test for Cu²⁺.
  • AlloyJAMB note: Steel, stainless steel, brass, bronze, type-metal, duralumin, soft solder, permalloy and alnico (constituents and uses only).

Objectives

  • specify the general properties of metals;
  • determine the method of extraction suitable for each metal;
  • relate the methods of extraction to the properties for the metals;
  • compare the chemical reactivities of the metals;
  • specify the uses of the metals;
  • determine specific test for metallic ions;
  • determine the process for the production of the compounds of these metals;
  • compare the chemical reactivities of the compounds;
  • specify the uses of these compounds;
  • specify the chemical composition of cement;
  • describe the method of purification of bauxite;
  • specify the ores of tin;
  • relate the method of extraction to its properties;
  • specify the uses of tin;
  • identify the general properties of the first transition metals;
  • deduce reasons for the specific properties of the transition metals;
  • determine the IUPAC names of simple transition metal complexes;
  • determine the suitable method of extraction of iron;
  • specify the properties and uses of iron;
  • identify the different forms of iron, their compositions, properties and uses;
  • identify the appropriate method of extraction of copper from its compounds;
  • relate the properties of copper and its compound to their uses;
  • specify the method for the preparation of CuSO₄;
  • specify the constituents and uses of the various alloys mentioned; and
  • compare the properties and uses of alloys to pure metals.

Organic chemistry

Our summary: Carbon compounds from hydrocarbons and petroleum to alkanols, acids, esters, amines, carbohydrates, proteins and polymers.

Organic compounds

Our summary: How organic compounds are named and grouped, isomerism, petroleum, and the reactions, tests and uses of each class of compound.

Contents

  • 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
  • Aliphatic hydrocarbons: alkanesJAMB note: 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.
  • Aliphatic hydrocarbons: alkenesJAMB note: Isomerism: structural and geometric isomerism, addition and polymerization reactions, polythene and synthetic rubber as examples of products of polymerization and its use in vulcanization.
  • Aliphatic hydrocarbons: alkynesJAMB note: Ethyne - production from action of water on carbides, simple reactions and properties of ethyne.
  • Aromatic hydrocarbons e.g. benzeneJAMB note: Structure, properties and uses.
  • AlkanolsJAMB note: 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).
  • Alkanals and alkanonesJAMB note: Chemical test to distinguish between alkanals and alkanones.
  • Alkanoic acidsJAMB note: 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.
  • AlkanoatesJAMB note: 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.
  • Amines (alkanamines)JAMB note: Primary, secondary and tertiary.
  • CarbohydratesJAMB note: 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.
  • ProteinsJAMB note: Primary structures, hydrolysis and tests (Ninhydrin, Biuret, Millon's and xanthoproteic). Enzymes and their functions.
  • PolymersJAMB note: Natural and synthetic rubber; addition and condensation polymerization. Methods of preparation, examples and uses. Thermoplastic and thermosetting plastics.

Objectives

  • derive the name of organic compounds from their general formulae;
  • relate the name of a compound to its structure;
  • relate the tetravalency of carbon to its ability to form chains of compound (catenation);
  • classify compounds according to their functional groups;
  • derive empirical formula and molecular formula from given data;
  • relate structure/functional groups to specific properties;
  • derive various isomeric forms from a given formula;
  • distinguish between the different types of isomerism;
  • classify the various types of hydrocarbons;
  • distinguish each class of hydrocarbons by their properties;
  • specify the uses of various hydrocarbons;
  • identify crude oil as a complex mixture of hydrocarbons;
  • relate the fractions of hydrocarbons to their properties and uses;
  • relate transformation processes to quality improvement of the fractions;
  • distinguish between various polymerization processes;
  • specify the process involved in vulcanization;
  • specify chemical test for alkenes;
  • specify chemical test for terminal alkynes;
  • distinguish between aliphatic and aromatic hydrocarbons;
  • relate the properties of benzene to its structure;
  • compare the various classes of alkanols;
  • determine the processes involved in ethanol production;
  • examine the importance of ethanol as an alternative energy provider;
  • distinguish the various classes of alkanols;
  • differentiate between alkanals and alkanones;
  • compare the various types of alkanoic acids;
  • identify natural sources of alkanoates;
  • infer products of alkanoic acids and alkanols;
  • specify the methods for the production of soap, detergent and margarine;
  • distinguish between detergent and soap;
  • compare the various classes of alkanamine;
  • identify the natural sources of carbohydrates;
  • compare the various classes of carbohydrates;
  • infer the products of hydrolysis and dehydration of carbohydrates;
  • determine the uses of carbohydrates;
  • specify the tests for simple sugars;
  • identify the basic structure of proteins;
  • specify the methods and products of hydrolysis;
  • specify the various tests for proteins;
  • distinguish between natural and synthetic polymers;
  • differentiate between addition and condensation polymerization processes;
  • classify natural and commercial polymers and their uses; and
  • distinguish between thermoplastics and thermosetting plastics.

Industry and astronomical chemistry

Our summary: The chemical industry and biotechnology, and the chemistry of the solar system and the earth.

Chemistry and industry

Our summary: Types of chemical industry, their raw materials and importance, and biotechnology.

Contents

  • Chemical industriesJAMB note: Types, raw materials and relevance. Biotechnology.

Objectives

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

Astronomical chemistry

Our summary: The solar system and its planets, and the make-up of the earth's atmosphere, lithosphere and hydrosphere.

Contents

  • Solar system, planets, satellite and the composition of the earth - atmosphere, lithosphere and hydrosphere

Objectives

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

More from the JAMB Chemistry syllabus

General objectives

  • The aim of the Unified Tertiary Matriculation Examination (UTME) syllabus in Chemistry is to prepare the candidates for the Board's examination. It is designed to test their comprehension of the course objectives, which are to:
  • understand the basic principles and concepts in chemistry;
  • interpret scientific data relating to chemistry;
  • deduce the relationships between chemistry and other sciences; and
  • apply the knowledge of chemistry to industry and everyday life.

Recommended texts

New School Chemistry for Senior Secondary Schools (Fourth edition)
Ababio, O. Y. (2009), Onitsha: Africana FIRST Publishers Limited.
Senior Secondary Chemistry, Books 1, 2 and 3
Bajah, S.T., Teibo, B. O., Onwu, G. and Obikwere, A. Book 1 (1999), Books 2 and 3 (2000), Lagos: Longman.
Understanding Chemistry for Schools and Colleges (Revised Edition)
Ojokuku, G. O. (2012), Zaria: Press-On Chemresources.
Essential: Chemistry for Senior Secondary Schools (2nd Edition)
Odesina, I. A. (2008), Lagos: Tonad Publishers Limited.
Countdown to WASSCE/SSCE, NECO, JME Chemistry
Uche, I. O., Adenuga, I. J. and Iwuagwu, S. L. (2003), Ibadan: Evans.

Syllabus content © The Joint Admissions and Matriculation Board. Taken from https://ibass.jamb.gov.ng/static/media/Chemistry.9efd0b98043d56922aaa.pdf (UTME).

DeeepSolve is an independent study platform and is not affiliated with JAMB. The topic lists, notes and exam scheme are the exam body's wording; “Our summary” lines are ours. If anything here differs from what JAMB publishes for your sitting, follow JAMB.