JAMB Chemistry Syllabus

General Objectives

The Chemistry syllabus is designed to enable candidates to:

• 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

Detailed Chemistry Syllabus

18 topics. For each topic: what to study (contents) and the objectives you should be able to meet.

1. Separation of Mixtures and Purification of Chemical Substances

   Contents

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

   Objectives — candidates should be able to

   1. distinguish between pure and impure substances
   2. use boiling and melting points to determine the purity of chemical substances
   3. differentiate between elements, compounds and mixtures
   4. differentiate between chemical and physical changes
   5. identify the properties of the components of a mixture
   6. specify the principle involved in each separation method
   7. apply the basic principle of separation processes in everyday life

2. Chemical Combination

   Contents

   • Stoichiometry, laws of definite and multiple proportions
   • Law of conservation of matter
   • Gay Lussac's law of combining volumes
   • Avogadro's law
   • Chemical symbols, formulae, equations and their uses
   • Relative atomic mass based on the 12C = 12 scale
   • The mole concept and Avogadro's number

   Objectives — candidates should be able to

   1. perform calculations involving formulae, equations and the mole concept
   2. deduce the chemical laws from given expressions, statements or data
   3. interpret graphical representations related to these laws
   4. deduce the stoichiometry of chemical reactions

3. Kinetic Theory of Matter and Gas Laws

   Contents

   • Outline of the kinetic theory of matter; melting, vapourization, boiling, freezing and condensation explained in terms of molecular motion and Brownian movement
   • Boyle's law, Charles's law, Graham's law, Dalton's law of partial pressure; the combined gas law
   • Molar volume and atomicity of gases
   • The ideal gas equation (PV = nRT)
   • Relationship between vapour density and relative molecular mass

   Objectives — candidates should be able to

   1. apply the theory to distinguish between solids, liquids and gases
   2. deduce reasons for change of state
   3. draw inferences based on molecular motion
   4. deduce gas laws from given expressions or statements
   5. interpret graphical representations of the gas laws
   6. perform calculations based on the gas laws and the stated relationships

4. Atomic Structure and Bonding

   Contents

   • Atomic Structure: concept of atoms, molecules and ions; the works of Dalton, Millikan, Rutherford, Moseley, Thompson and Bohr; the simple hydrogen spectrum; ionization of gases; atomic structure, electron configuration, atomic number, mass number and isotopes (specific examples drawn from elements of atomic number 1 to 20); shapes of s and p orbitals
   • Periodic Table and periodicity of elements: families such as alkali metals, halogens, the noble gases and transition metals; variation in ionization energy, ionic radii, electron affinity and electronegativity
   • Chemical bonding: electrovalency and covalency; electron configuration of elements and their tendency to attain the noble gas structure; hydrogen bonding and metallic bonding as special types; coordinate bond as in complex ions such as [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 and CO2), non-linear (H2O), tetrahedral (CH4) and pyramidal (NH3)
   • Nuclear chemistry: radioactivity (types and properties of radiations); nuclear reactions and writing of balanced nuclear equations; uses and applications of natural and artificial radioactivity

   Objectives — candidates should be able to

   1. distinguish between atoms, molecules and ions
   2. identify the contributions of the named scientists to the development of the atomic theory
   3. deduce the number of protons, neutrons and electrons from atomic and mass numbers
   4. apply the rules guiding the arrangement of electrons in an atom
   5. identify the elements that exhibit isotopy
   6. relate isotopy to mass number
   7. perform simple calculations relating to isotopy
   8. differentiate between the shapes of the orbitals
   9. determine the number of electrons in s and p orbitals
   10. relate atomic number to the position of an element on the periodic table
   11. relate properties of groups of elements on the periodic table
   12. explain the variation of properties across the period and down the groups
   13. differentiate between the types of chemical bonding
   14. deduce the type of bonding from the electron configurations of given elements
   15. relate the nature of bonding to the properties of compounds
   16. differentiate between the various shapes of molecules
   17. distinguish between ordinary chemical reactions and nuclear reactions
   18. differentiate between natural and artificial radioactivity
   19. compare the properties of the different types of radiation
   20. compute the half-life of radioactive materials
   21. balance nuclear equations
   22. identify the uses or applications of radioactivity

5. Air

   Contents

   • The natural gaseous constituents and their proportions: nitrogen, oxygen, water vapour, carbon(IV) oxide and the noble gases (argon and neon)
   • Measurement of the proportion of oxygen in air (e.g. burning of phosphorus, alkaline pyrogallol)
   • Air as a mixture and the uses of the noble gases

   Objectives — candidates should be able to

   1. explain why air is regarded as a mixture
   2. identify the principles involved in separating the components of air
   3. explain the environmental variations in the composition of air
   4. specify the uses of the constituents of air

6. Water

   Contents

   • Water as a product of the combustion of hydrogen and its composition by volume
   • Water as a solvent; atmospheric gases dissolved in water and their biological significance
   • Hard and soft water: temporary and permanent hardness and methods of softening hard water
   • Treatment of water for town supply
   • Water of crystallization, efflorescence, deliquescence and hygroscopy with examples and uses

   Objectives — candidates should be able to

   1. identify the uses of water
   2. identify the effects of dissolved atmospheric gases in water
   3. distinguish between the properties of hard and soft water
   4. determine the causes of hardness
   5. identify methods of removing hardness
   6. describe the treatment of water for town supply
   7. distinguish among the phenomena of crystallization, efflorescence, deliquescence and hygroscopy
   8. identify the compounds exhibiting these phenomena

7. Solubility

   Contents

   • Unsaturated, saturated and supersaturated solutions; solubility curves and simple deductions from them; solubility defined in terms of mole per dm3; related calculations
   • Solvents for fats, oils and paints, and their use in the removal of stains
   • False solutions (suspensions and colloids): properties and examples; Harmattan haze and water paints as suspensions; fog, milk, aerosol sprays, emulsion paints and rubber solution as colloids

   Objectives — candidates should be able to

   1. distinguish between the various types of solutions
   2. interpret solubility curves
   3. calculate the amount of solute that can dissolve in a given amount of solvent
   4. deduce the solubility of a solute at various temperatures
   5. relate the nature of solvents to their uses
   6. differentiate between true solutions and suspensions/colloids
   7. compare the properties of true and false solutions
   8. give examples of suspensions and colloids

8. Environmental Pollution

   Contents

   • Sources and effects of pollutants
   • Air pollution: hydrogen sulphide, carbon(II) oxide, sulphur(IV) oxide, oxides of nitrogen, chlorofluorocarbons and dust
   • Water pollution: sewage and oil pollution
   • Soil pollution: oil spillage, biodegradable and non-biodegradable pollutants

   Objectives — candidates should be able to

   1. identify the types of pollution and the pollutants
   2. specify the sources of the pollutants
   3. classify pollutants as biodegradable and non-biodegradable
   4. specify the effects of pollution on the environment
   5. identify measures for the control of pollution

9. Acids, Bases and Salts

   Contents

   • General characteristics and properties; indicators; basicity of acids; normal, acidic, basic and double salts; acid defined as a substance whose aqueous solution furnishes H3O+ ions or as a proton donor; natural organic acids such as ethanoic, citric and tartaric acids; alums as examples of double salts; preparation of salts by neutralization, precipitation, action of acids on metals, oxides and trioxocarbonate(IV) salts
   • Qualitative comparison of the conductances of molar solutions of strong and weak acids and bases; relationship between conductance and the relative mobilities of ions
   • pH and pOH scale; pH defined as -log[H3O+]; related calculations
   • Acid/base titrations
   • Salt hydrolysis with examples such as NH4Cl, AlCl3, Na2CO3 and CH3COONa

   Objectives — candidates should be able to

   1. distinguish between the properties of acids and bases
   2. identify the various types of acids and bases
   3. determine the basicity of acids
   4. differentiate between acidity and alkalinity using indicators
   5. identify the methods of preparation of salts
   6. classify the different types of salts
   7. relate the degree of dissociation to the strength of acids and bases
   8. relate the degree of dissociation to conductance
   9. perform calculations on pH and pOH
   10. identify suitable indicators for acid-base reactions
   11. interpret graphs of titration curves
   12. perform calculations based on the mole concept
   13. balance the equation for salt hydrolysis
   14. deduce the properties (acidic, basic, neutral) of the resultant solution

10. Oxidation and Reduction

    Contents

    • Oxidation in terms of addition of oxygen or removal of hydrogen
    • Reduction as removal of oxygen or addition of hydrogen
    • Oxidation and reduction in terms of electron transfer
    • Use of oxidation numbers; oxidation and reduction treated as change in oxidation number and use in balancing equations; IUPAC nomenclature using oxidation number
    • Tests for oxidizing and reducing agents

    Objectives — candidates should be able to

    1. identify the various forms of expression of oxidation and reduction
    2. classify reactions in terms of oxidation or reduction
    3. balance redox reaction equations
    4. deduce the oxidation number of chemical species
    5. compute the number of electrons transferred in redox reactions
    6. identify the names of the chemical species involved in a redox reaction
    7. distinguish between oxidizing and reducing agents in redox reactions
    8. apply the use of oxidation numbers in naming inorganic compounds
    9. relate the reagents to their oxidizing and reducing abilities

11. Electrolysis

    Contents

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

    Objectives — candidates should be able to

    1. distinguish between electrolytes and non-electrolytes
    2. perform calculations using Faraday's laws (mole of electrons)
    3. identify the electrodes suitable for the electrolysis of various electrolytes
    4. specify the chemical reactions at the electrodes
    5. determine the products of electrolysis
    6. identify the factors that affect the discharge of ions
    7. specify the various applications of electrolysis
    8. identify the types of electrochemical cells
    9. calculate electrode potentials
    10. determine the applications of the electrolytic processes
    11. identify the methods of protecting metals

12. Energy Changes

    Contents

    • Energy changes (delta H) accompanying physical and chemical changes: dissolution of substances in or reaction with water (e.g. Na, NaOH, K, NH4Cl); endothermic (+delta H) and exothermic (-delta H) reactions
    • Entropy as an order-disorder phenomenon, illustrated by mixing of gases and dissolution of salts
    • Spontaneity of reactions: delta G0 = 0 as the criterion for equilibrium, delta G > 0 for non-spontaneous and delta G < 0 for spontaneous reactions

    Objectives — candidates should be able to

    1. determine the types of heat changes in physical and chemical processes
    2. interpret graphical representations of heat changes
    3. relate physical states of substances to their degree of orderliness
    4. determine the conditions for the spontaneity of a reaction
    5. relate delta H0, delta S0 and delta G0 as the driving forces of chemical reactions
    6. solve problems based on the relationship delta G0 = delta H0 - T delta S0

13. Rates of Chemical Reaction

    Contents

    • Factors affecting reaction rates: temperature (e.g. HCl and Na2S2O3, Mg and HCl); concentration (e.g. HCl and Na2S2O3, HCl and marble, iodine clock reaction) and pressure for gaseous reactions; surface area (e.g. powdered versus lump marble with HCl); catalyst (e.g. decomposition of H2O2 or KClO3 with and without MnO2)
    • Reaction rate curves
    • Activation energy: qualitative treatment of Arrhenius's law and the collision theory
    • Effect of light on some reactions (e.g. halogenation of alkanes)

    Objectives — candidates should be able to

    1. identify the factors that affect the rate of chemical reaction
    2. determine the effect of temperature on reaction rate
    3. examine the effect of concentration and pressure on reaction rate
    4. describe the effect of surface area on reaction rate
    5. determine suitable catalysts for given reactions and their effects
    6. determine the methods of moderating the effects of these factors
    7. interpret reaction rate curves
    8. solve simple problems on reaction rate
    9. relate the rate of reaction to the kinetic theory of matter
    10. examine the significance of activation energy
    11. deduce activation energy from reaction rate curves

14. Chemical Equilibrium

    Contents

    • Reversible reactions and the factors governing the position of equilibrium
    • Dynamic equilibrium
    • Le Chatelier's principle and the equilibrium constant
    • Examples such as the action of steam on iron and the equilibrium N2O4 reversible 2NO2 (calculations not required)

    Objectives — candidates should be able to

    1. identify the factors that affect the position of equilibrium
    2. predict the effect of each of the factors on the position of equilibrium
    3. determine the effect of these factors on the equilibrium constant

15. Non-Metals and Their Compounds

    Contents

    • Hydrogen: commercial production from water gas and cracking of petroleum fractions; laboratory preparation, properties, uses and test for hydrogen
    • Halogens (chlorine as representative): laboratory and industrial (electrolytic) preparation, properties and uses (sterilization of water, bleaching, manufacture of HCl, plastics and insecticides); hydrogen chloride and hydrochloric acid (preparation and properties); chlorides and the test for chlorides
    • Oxygen and Sulphur: oxygen - laboratory preparation, properties and uses, commercial production from liquid air, classification of oxides (acidic, basic, amphoteric and neutral), ozone as an allotrope and its atmospheric importance; sulphur - uses and allotropes; sulphur(IV) oxide (preparation, properties, uses and reaction with alkalis); trioxosulphate(IV) acid and its salts and the effect of acids on them; tetraoxosulphate(VI) acid (H2SO4) - contact process, properties of the dilute acid, as an oxidizing and dehydrating agent, and uses, with the test for SO42-; hydrogen sulphide (preparation, as a weak acid, reducing agent and precipitating agent, with the test for S2-)
    • Nitrogen: laboratory preparation and production from liquid air; ammonia - laboratory and industrial (Haber process) preparation, properties and uses, ammonium salts and their uses, oxidation of ammonia to nitrogen(IV) oxide and trioxonitrate(V) acid, and the test for NH4+; trioxonitrate(V) acid - laboratory preparation from ammonia, properties and uses, action of heat on trioxonitrate(V) salts and their uses, and the test for NO3-; oxides of nitrogen and their properties; the nitrogen cycle
    • Carbon: allotropes, their properties and uses; carbon(IV) oxide - laboratory preparation, properties, uses, action of heat on trioxocarbonate(IV) salts and the test for CO32-; carbon(II) oxide - laboratory preparation, properties, effect on blood, and its sources (charcoal, fire, exhaust fumes); coal - types and products of destructive distillation of wood and coal; coke - gasification and uses; synthetic (synthesis) gas - manufacture and uses

    Objectives — candidates should be able to

    1. predict the reagents for the laboratory and industrial preparation of the gases and compounds
    2. identify the properties of the gases and compounds
    3. compare the properties of the gases and compounds
    4. specify the uses of the gases and compounds
    5. determine the specific tests for the gases and compounds
    6. determine the specific tests for the ions Cl-, SO42-, SO32-, S2-, NH4+, NO3-, CO32- and HCO3-
    7. predict the reagents for the preparation of HCl(g) and HCl(aq), their properties and uses
    8. identify the allotropes of oxygen and the environmental significance of ozone
    9. classify the oxides of oxygen and identify their properties
    10. identify the allotropes and uses of sulphur
    11. specify the preparation, properties and uses of SO2, H2SO4, H2SO3 and H2S
    12. specify the laboratory and industrial preparation, properties and uses of ammonia
    13. identify the laboratory preparation, properties and uses of trioxonitrate(V) acid
    14. specify the properties of N2O, NO and NO2
    15. examine the environmental relevance of the nitrogen cycle
    16. identify the allotropes of carbon
    17. predict the reagents for the laboratory preparation of CO2 and specify its properties and uses
    18. determine the reagents for the laboratory preparation of CO and predict its effect on humans
    19. identify the forms and uses of coal
    20. specify the products of the destructive distillation of wood and coal
    21. specify the uses of coke and synthetic gas

16. Metals and Their Compounds

    Contents

    • General properties of metals
    • Alkali metals (e.g. sodium): sodium hydroxide (production by electrolysis of brine, action on aluminium, zinc and lead ions, and use in the precipitation of metallic hydroxides); sodium trioxocarbonate(IV) and sodium hydrogen trioxocarbonate(IV) (production by the Solvay process, properties and uses such as glass manufacture); sodium chloride (occurrence in seawater, uses, economic importance of seawater and recovery of sodium chloride)
    • Alkaline-earth metals (e.g. calcium): calcium oxide, calcium hydroxide and calcium trioxocarbonate(IV) - properties and uses; preparation of calcium oxide from seashells; chemical composition of cement and the setting of mortar; test for Ca2+
    • Aluminium: purification of bauxite, electrolytic extraction, properties and uses, properties and uses of its compounds, and the test for Al3+
    • Tin: extraction from its ore, properties and uses
    • First transition series metals: characteristic properties - electron configuration, oxidation states, formation of complex ions, formation of coloured ions, and catalytic properties
    • Iron: extraction from sulphide and oxide ores, properties and uses, forms of iron and their properties, advantages of steel over iron, and tests for Fe2+ and Fe3+
    • Copper: extraction from sulphide and oxide ores, properties and uses, preparation and uses of copper(II) tetraoxosulphate(VI), and the test for Cu2+
    • Alloys: steel, stainless steel, brass, bronze, type-metal, duralumin, soft solder, permalloy and alnico (constituents and uses only)

    Objectives — candidates should be able to

    1. specify the general properties of metals
    2. determine the suitable method for the extraction of a metal
    3. relate the method of extraction to the properties of the metal
    4. compare the chemical reactivities of the metals
    5. specify the uses of the metals
    6. determine the specific test for the metallic ions
    7. determine the processes involved in the production of the named compounds
    8. compare the chemical reactivities of the compounds
    9. specify the uses of the compounds
    10. specify the chemical composition of cement
    11. describe the method of purification of bauxite
    12. specify the ores of tin and relate the extraction method to its properties
    13. specify the uses of tin
    14. identify the general properties of the first transition metals
    15. deduce the reasons for the specific properties of transition metals
    16. determine the IUPAC names of simple transition metal complexes
    17. determine the suitable method for the extraction of iron and specify its properties and uses
    18. identify the forms of iron, their compositions, properties and uses
    19. identify the suitable method for the extraction of copper and relate its properties and those of its compounds to their uses
    20. specify the methods of preparation of copper(II) tetraoxosulphate(VI)
    21. specify the constituents and uses of alloys
    22. compare the properties and uses of alloys with those of pure metals

17. Organic Compounds

    Contents

    • Introduction: tetravalency of carbon, general formulae, IUPAC nomenclature and determination of empirical formula of each class of compound
    • Aliphatic hydrocarbons - Alkanes: homologous series in relation to physical properties, substitution reactions and uses of halogenated products, structural isomerism (examples not exceeding six carbons); petroleum - composition, fractional distillation and major products, cracking and reforming, petrochemicals as starting materials for synthetic products, and the meaning of petrol quality (octane number)
    • Aliphatic hydrocarbons - Alkenes: structural and geometric isomerism, addition and polymerization reactions, polythene and synthetic rubber as products of polymerization, and uses of vulcanization
    • Aliphatic hydrocarbons - Alkynes: ethyne produced from action of water on carbide, and its simple reactions and properties
    • Aromatic hydrocarbons - benzene: structure, properties and uses
    • Alkanols: primary, secondary and tertiary; production of ethanol by fermentation and from petroleum by-products; local examples of fermentation and distillation (e.g. gin from palm wine); glycerol as a polyhydric alkanol; reactions of OH group and the oxidation test (Lucas test) to distinguish the classes
    • Alkanals and alkanones: chemical test to distinguish between them
    • Alkanoic acids: chemical reactions, neutralization and esterification; ethanedioic (oxalic) acid as an example of a dicarboxylic acid; benzene carboxylic acid as an aromatic acid
    • Alkanoates: formation from alkanoic acids and alkanols; fats and oils as alkanoates; saponification and the production of soap and margarine; distinction between detergents and soap
    • Amines (alkanamines): primary, secondary and tertiary amines
    • Carbohydrates: classification into mono-, di- and polysaccharides; composition; chemical tests for simple sugars; reaction with concentrated tetraoxosulphate(VI) acid; hydrolysis of complex sugars (e.g. cellulose from cotton, starch from cassava); uses of sugar and starch (alcoholic beverages, pharmaceuticals, textiles)
    • Proteins: primary structures, hydrolysis and tests (Ninhydrin, Biuret, Millon's and xanthoproteic); enzymes and their functions
    • Polymers: natural and synthetic rubber; addition and condensation polymerization; methods of preparation, examples and uses; thermoplastic and thermosetting plastics

    Objectives — candidates should be able to

    1. derive the names of organic compounds from their general formulae
    2. relate the names of organic compounds to their structures
    3. relate the tetravalency of carbon to the formation of chains (catenation)
    4. classify the various compounds according to their functional groups
    5. derive the empirical and molecular formulae from given data
    6. relate the structure or functional groups to the properties of the compounds
    7. derive the various isomeric forms from a given formula
    8. distinguish between the various types of isomerism
    9. specify the uses of the various organic compounds
    10. identify crude oil as a mixture of hydrocarbons
    11. relate the various petroleum fractions to their properties and uses
    12. relate the transformation processes (cracking, reforming) to the quality of the fractions
    13. distinguish between the various polymerization processes
    14. specify the process of vulcanization
    15. specify the chemical test for terminal alkynes
    16. distinguish between aliphatic and aromatic hydrocarbons
    17. relate the properties of benzene to its structure
    18. compare the classes of alkanols
    19. determine the processes for the production of ethanol
    20. examine the importance of ethanol as an alternative source of energy
    21. differentiate between alkanals and alkanones
    22. compare the various types of alkanoic acids
    23. identify the natural sources of alkanoates
    24. specify the methods of production of soap, detergents and margarine
    25. distinguish between detergents and soap
    26. compare the various classes of alkanamines
    27. identify the natural sources of carbohydrates
    28. compare the various classes of carbohydrates
    29. infer the products of hydrolysis and dehydration of carbohydrates
    30. determine the uses of carbohydrates
    31. specify the tests for simple sugars
    32. identify the basic structure of proteins
    33. specify the methods and products of protein hydrolysis
    34. specify the tests for proteins
    35. distinguish between natural and synthetic polymers
    36. differentiate between addition and condensation polymerization
    37. classify natural and commercial polymers and specify their uses
    38. distinguish between thermoplastic and thermosetting plastics

18. Chemistry and Industry

    Contents

    • Types of chemical industries, their raw materials and relevance
    • Biotechnology

    Objectives — candidates should be able to

    1. classify chemical industries according to their products
    2. identify the raw materials for each industry
    3. distinguish between fine and heavy chemicals
    4. enumerate the relevance of the chemical industries
    5. relate industrial processes to biotechnology

Recommended Texts

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

Frequently Asked Questions

How many topics are in the JAMB Chemistry syllabus?

The JAMB UTME Chemistry syllabus is organised into 18 main topics, ranging from Separation of Mixtures and Purification of Chemical Substances through to Chemistry and Industry. The topics span physical chemistry, inorganic chemistry and organic chemistry, with each topic broken into a CONTENTS column (what to study) and an OBJECTIVES column (what you should be able to do).

What are the aims of the JAMB Chemistry syllabus?

The syllabus is designed so that candidates can understand the basic principles and concepts in chemistry, interpret scientific data relating to chemistry, deduce the relationships between chemistry and other sciences, and apply chemistry knowledge to industry and everyday life.

What are the main branches of chemistry covered?

The syllabus covers three broad branches: physical chemistry (e.g. kinetic theory and gas laws, energy changes, rates of reaction, chemical equilibrium, electrolysis, acids/bases/salts and solubility), inorganic chemistry (e.g. atomic structure and bonding, non-metals and their compounds, metals and their compounds) and organic chemistry (e.g. alkanes, alkenes, alkynes, alkanols, alkanoic acids, carbohydrates, proteins and polymers).

Which topics carry the most weight in JAMB Chemistry?

Large, content-heavy topics such as Atomic Structure and Bonding, Non-Metals and Their Compounds, Metals and Their Compounds, and Organic Compounds tend to generate the most questions because each contains many sub-topics. Quantitative areas like Chemical Combination (mole concept and stoichiometry), Electrolysis and Acids, Bases and Salts (pH and titration) are also frequently tested through calculations.

Does JAMB Chemistry include nuclear chemistry and radioactivity?

Yes. Nuclear chemistry is treated under Atomic Structure and Bonding. Candidates should be able to distinguish ordinary chemical reactions from nuclear reactions, compare the types and properties of radiation, balance nuclear equations, compute half-lives, and identify the applications of natural and artificial radioactivity.

Are calculations required in JAMB Chemistry?

Yes. Calculations appear across several topics, including the mole concept and stoichiometry, gas laws (PV = nRT), solubility, pH and pOH, acid-base titration, Faraday's laws in electrolysis, electrode potentials, half-life, and the free energy relationship delta G = delta H - T delta S. Note that Chemical Equilibrium specifically does not require calculations.

How is the IUPAC naming convention used in the syllabus?

JAMB uses IUPAC nomenclature throughout. Many compounds appear under their systematic names, for example tetraoxosulphate(VI) acid (sulphuric acid), trioxonitrate(V) acid (nitric acid), trioxocarbonate(IV) (carbonate) and carbon(IV) oxide (carbon dioxide). Candidates are also expected to apply oxidation numbers when naming inorganic compounds and simple transition-metal complexes.

What textbooks are recommended for JAMB Chemistry?

Widely recommended texts include Ababio's New School Chemistry for Senior Secondary Schools, the Bajah et al. Senior Secondary Chemistry series, Ojokuku's Understanding Chemistry for Schools and Colleges, Odesina's Essential Chemistry for Senior Secondary Schools, and Uche et al.'s Countdown to WASSCE/SSCE, NECO, JME Chemistry.