JAMB Syllabus for Chemistry 2024/2025 | PDF Download

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The Joint Admission and Matriculation Board (JAMB) has recently released the Chemistry syllabus for the academic year 2024/2025. This strategic initiative aims to assist students in adequately preparing for their upcoming Unified Tertiary Matriculation Examination (UTME).

Objectives of JAMB Syllabus for Chemistry

The JAMB Chemistry syllabus is designed to equip candidates for the Board’s examination by assessing their comprehension, knowledge, and proficiency in the following aspects of the subject:

  1. Candidates will gain a solid understanding of chemistry’s fundamental principles and concepts.
  2. The syllabus emphasizes the ability to interpret scientific data related to chemistry effectively.
  3. Candidates will explore the interrelationships between chemistry and other scientific disciplines.
  4. Practical application of chemistry knowledge to industry and everyday life scenarios is a key focus.

Topics Under JAMB Chemistry Syllabus

The topics in the JAMB syllabus for chemistry are divided into 17 sections.

Separation of Mixtures and Purification of Chemicals

  • Pure and impure substances
  • Elements, compounds, and mixtures
  • Boiling and melting points.
  • Chemical and physical changes.
  • Separation methods

Chemical Bonds

  • Stoichiometry
  • Laws of determinism and multiple ratios
  • Laws of conservation of matter
  • Gay-Lussac law of volume bonds
  • Avogadro’s law
  • Chemical symbols, formulas, equations, and their use of 44mic44 molar concept and Avogadro’s number based on relative atomic mass 12C=12.

Theory of Motion of Matter and the Laws of Gases

  • Overview of theory of motion of matter: melting, evaporation, boiling, freezing, condensation in relation to molecular motion and Brownian Motion.
  • Boyle, Charles, Graham, and Dalton’s (law of partial pressure) laws. Combines gas laws, molar volume, and gas atomicity.
  • Ideal gas equation (PV = NRT).
  • Relation between vapor density and molecular weight of the gas.

Atomic Structures and Bonds

  • Concepts of atoms, molecules, and ions. Dalton, Millikan, Rutherford, Moseley, Thompson, Bohr.
  • Atomic structure, atomic number, electron configuration, mass number, and isotopes. Concrete examples should be drawn from the elements with atomic numbers 1 through 20.
  • Geometries of s and p orbitals.
  • A representation of the periodic table from the perspective of recognizing the periodic table, periodicity of the elements, and family of elements. Alkali metals, halogens, rare gases, transition metals. Changes in the following properties: ionization energy, ionic radius, electron affinity, and electronegativity.
  • Chemical bond.
  • Electronic and shared valences, electronic configurations of elements, and tendency to approach noble gas structures. Hydrogen and metallic bonds as special types of electronic and covalent valences, respectively. [Cu(NH3)4]2+, [Ag(NH3 )2] [Fe(CN)6]3-, [Fe(CN)6]4 with Van der Waals forces mentioned as a special binding force.
  • Simple molecular geometry: Linear ((H2, O2, C12, HCl, CO2), Nonlinear (H2O), Tetrahedral (CH4), Conical (NH3))
  • Nuclear Chemistry: Radioactivity (Types and Properties of Radiation).
  • Simple Equations of Nuclear Reactions, Uses and Applications of Natural and Artificial Radioactivity.


  • Applications of air and noble gases as mixtures.
  • Natural gas composition and proportion in air. Nitrogen, Oxygen, Water Vapor, carbon (IV) oxides, and noble gases (Argon and Neon)


  • Water is a combustion product of hydrogen and its volume composition.
  • Water as a solvent their biological significance in atmospheric gases dissolved in water.
  • Hard and soft water: Temporary and permanent hard water and methods of softening hard water.
  • Treatment of water for urban supply.
  • The water of crystallization, efflorescence, deliquescent and hygroscopic. Examples of substances with these properties and their uses.


  • Unsaturated, saturated, and supersaturated solutions. Solubility curves and simple derivation from them (solubility defined in moles per dm3) and simple calculations.
  • Use oils, paint solvents, and solvents to remove dirt.
  • Wrong solutions (Suspensions and Colloids): Properties and Examples. Harmattan haze and watercolors as examples of suspensions and mists, and milk is an example of colloids, aerosol sprays, emulsion paints, and gum solutions.

Environmental Pollution

  • Sources and effects of pollutants.
  • Air pollution examples of air pollutants include H2S, CO, SO2, nitrogen oxides, chlorofluorocarbons, and dust.
  • Water pollution, oil pollution, and sewage should be known.
  • Soil Pollution: Oil pollution, biodegradable and non-biodegradable contaminants.

Acids, Bases, and Salts

  • General properties and characteristics of Acids, Bases, and Salts. Acid/base indicator, the basicity of acid (normal, acidic, basic, and double salt).
  • A substance whose aqueous solution produces H3O+ ions or an acid is defined as a proton donor.
  • Ethanoic acid, citric acid, and tartaric acid are examples of natural organic acids, alum as double salt, formation of salts by neutralization, precipitation, and action of acids on metals. Oxide and Trioxocarbonate (IV) salts.
  • Qualitative comparison of conductivity of molar solutions of weak and strong Acids and bases, the relationship between conductivity and amount of Ions present.
  • pH and pOH Scale. Simple Calculations.
  • Acid/Base Titration.
  • Salt Hydrolysis: Principles, simple examples NH4Cl, AlCl3, Na2CO3, CH3COONa, etc.

Oxidation and Reduction

  • Oxidation is the sense of the addition of oxygen or removal of hydrogen.
  • Reduction is the removal of oxygen or the addition of hydrogen.
  • Oxidation and reduction by electron transfer.
  • Oxidation numbers. Oxidation and reduction are treated as changing and using oxidation numbers to balance simple equations.
  • IUPAC nomenclature for inorganic compounds using oxidation numbers.
  • Oxidizing and Reducing Agent Testing.


  • Electrolytes and Non-Electrolytes.
  • Faraday’s Law of Electrolysis.
  • Electrolysis of dilute H2SO4, aqueous CuSO4, CuCl2 solutions, dilute and concentrated NaCl solutions, and molten NaCl factors affecting Ionic discharge at
  • Electrodes.
  • Electrolysis applications.
  • Metal washing.
  • Production of copper and elements and compounds (Na, O2, Cl2, and NaOH).
  • Electrochemical cell: redox series (Zn, Fe, Sn, Pb, H, Cu, Hg, Ag, Au K, Ca, Na, Mg, Al)
  • Electrode potentials and half-cell reactions (simple calculations only).
  • Corrosion as electrolytic processes, cathodic protection of metals, electroplating, painting, and coating with grease or oil as corrosion protection for iron.

Energy Change

  • Energy change (ΔH) accompanying physical and chemical changes: Dissolution of substances in water/reaction with water.
  • G. Na, NaOH, K, NH4Cl. Endothermic (+ΔH) and exothermic (-ΔH) reactions.
  • Entropy as an Order-Disorder Phenomenon: A simple Illustration of gas mixing, salt dissolution, etc.
  • The reaction’s spontaneity: ΔGθ = 0 as a criterion for equilibrium and ΔG greater or less than 0 as a criterion for involuntary or spontaneous.

Rates of Chemical Reactions

  • Basic treatment of the following factors that can change the rate of chemical reactions.
  • Temperature Example: Reaction between HCl and Na2S2O3 or Mg and HCl
  • Concentration Example: HCl and Na2S2O3, for the reaction of HCl with marble and the iodine clock reaction (Pressure can be used as a concentration term for gas systems).
  • Surface Examples (The reaction of marble with HCl and powdered marble (ii) lumps of the same mass).
  • Catalyst.
  • Decomposition of KClO3 or H2O2 in the presence or absence of MnO2.
  • Kinetic curves.
  • Activation Energy.
  • Qualitative treatment of Arrhenius law and collision theory, effects of light on some reactions. e.g. halogenation of alkanes

Chemical Equilibria

  • Reversible reactions and factors governing the equilibrium position. 
  • Dynamic balance. Le Chatelier’s principle and equilibrium constants. Simple examples include the action of steam on iron and N2O4 2NO2. No calculation will be required.

Nonmetals and Their Compounds

  • Hydrogen: Laboratory preparation, commercial production from water gas and cracking of petroleum fractions, properties, uses, and testing of Hydrogen.
  • Halogen: Chlorine, which is a representative element of halogen. Laboratory preparations, industrial preparations by electrolysis, properties, and applications, e.g., water disinfection, bleaching, HCl, plastics, and pesticide production.
  • Hydrogen chloride and hydrochloric acid: properties and preparation.
  • Chloride and chloride test. Oxygen and Sulfur.
  • Oxygen: Laboratory preparations, properties, and uses. Commercial production from liquid air.
  • Oxides: Acidic, amphoteric, basic and neutral, trioxygen (ozone) as an allotrope, and the importance of atmospheric ozone.
  • Sulfur: Uses and allotropes: Allotropes are not expected to form.
  • Preparation, properties, and uses of sulfur(IV) oxides, the reaction of SO2 with alkalis. The action of Acids on Trioxosulfate(IV) acids and salts, Trioxosulfate(IV) and Tetraoxosulfate(VI) salts. Commercial preparation (contact method only), properties as dilute acid, oxidizing, and dehydrating agents and uses.
  • Hydrogen Sulfide: preparation and properties as a weak acid, reducing agent, and precipitating agent. Testing S2 Nitrogen: (i) Laboratory Preparations (ii) Preparations from Liquid Air (iii) Ammonia.
  • Laboratory and industrial preparations (Haber method only), properties, and uses. Ammonium salts and their uses, Ammonia oxidation to Nitrogen (IV) oxides, and Trioxonitric (V) acids.
  • Testing of NH4+ and Trioxonitrate (V) acid: laboratory preparation from ammonia. Properties and uses. Trioxonitrate (V) salts (heat exposure and use).
  • Test for NO3 Nitrogen Oxides: Characteristics. Nitrogen cycle.
  • Allotropes: Uses and properties.
  • Carbon (IV) Oxides laboratory preparations, properties, and uses.
  • Exposure of Trioxocarbonate (IV) salts to heat and testing of CO3. Carbon (II) oxides: properties including laboratory preparation and effects on the blood. Sources of carbon (II) oxides include charcoal, fire, and exhaust gases.
  • Charcoal: Other types of products obtained from the destructive distillation of wood and charcoal.
  • Coke: gasification and use.
  • Production and use of syngas.

Metals and Their Compounds

  • General properties of metals alkali Metals, e.g., Sodium
  • Sodium Hydroxide: Production of brine by electrolysis, affecting aluminum, zinc, and lead ions. Applications such as precipitation of metal hydroxides.
  • Sodium Trioxocarbonate (IV) and Sodium Trioxocarbonate (IV): Manufactured by the solvay process, properties, and uses. e.g., Na2CO3 in glass manufacturing.
  • Sodium Chloride: Presence and uses in seawater, economic importance of seawater and production of Sodium Chloride.
  • Alkaline earth metals, such as calcium, calcium hydroxide, calcium oxide, and calcium trioxocarbonate (IV); properties and uses.
  • Formation of calcium oxide from shells, cement chemical composition, and mortar hardening. Test for Ca2+.
  • Aluminum bauxite refining, electrowinning, properties and uses of aluminum and its compounds. Test the extraction of Al3+
  • Tin from the ore. Properties and uses.
  • Metals of the first transition series. Characteristic properties: (i) electron configuration (ii) oxidation state (iii) complex ion formation (iv) formation of colored ions (v) catalysis (g) iron
  • Extraction from sulfide and oxide ores, properties and applications, properties and benefits of different forms of steel and iron. Testing for Fe2+ and Fe3+
  • Copper extraction from sulfide and oxide ores, copper properties and uses.
  • Preparation and use of copper(II) tetraoxosulfate(VI). 
  • Test for Cu2+, alloy, steel, stainless steel, brass, bronze, carbide, duralumin, solder, permalloy, and alnico (components and applications only).

Organic Compounds

  •  An introduction to the tetravalence of carbons, the general formula, IUPAC nomenclature, and the determination of the molecular formula for each class of organic compounds are listed below.
  • Aliphatic Hydrocarbons
  • Alkanes
  • Homologous Series for some examples and uses of physical properties, substitution reactions, and halogenated products. Isomerism: structure only (examples of isomerism must not exceed six carbon atoms).
  • Petroleum: composition, fractional distillation, and principal products. Cracking and reforming, raw materials for petrochemical-organic synthesis, gasoline quality, the importance of octane number.
  • Alkenes.
  • Isomerisms: structural and geometric isomers, addition and polymerization reactions, polyethylene and synthetic rubber as examples of polymerization products, and their use in vulcanization.
  • Alkyne.
  • Ethyne – Produced by the action of water on carbides, a simple reaction, and the properties of ethyne.
  • Benzene and other aromatic hydrocarbons – structure, properties, and uses.
  • Alkanols.
  • Primary, secondary, and tertiary ethanol production from fermentation and petroleum by-products.
  • Local examples of distillation and fermentation, e.g., gin made from palm wine and other local sources, glycerin as a polyhydric alkanol.
  • The reaction of OH Groups: Oxidation (Lucas Test) as a test to distinguish primary, secondary, and tertiary Alkanols.
  • Alkanal and Alcanone.
  • A chemical test to distinguish between alkanols and alkanones.
  • Alkanoic acid.
  • Chemical Reaction; Examples of dicarboxylic acids include ethanedioic acid (oxalic acid), and aromatic acids include benzene-carboxylic acid.
  • Alkanoates.
  • Alkanoic acids, alkanols (oils and fats), and alkanoates.
  • Saponification: Making soaps and margarine from alkanoates, distinguishing between detergents and soaps.
  • Composition of amines (alkanamins) primary, secondary, and tertiary monosaccharides, chemical testing, reaction with concentrated tetraoxosulfate (VI) acid. Hydrolysis of complex sugars, for example, cellulose in cotton and starch in cassava, use of sugars and starches in manufacturing alcoholic beverages, pharmaceuticals, and textiles.
  • Proteins: Primary structure, hydrolysis, and testing (Ninhydrin, Biuret, Million and Xanthoproteins)
  • Enzymes and their functions.
  • Polymer (Natural and synthetic rubber, addition and condensation polymerization, manufacturing process, usage examples, and applications)
  • Thermoplastics and thermosets.

PDF Download of JAMB Syllabus For Chemistry 2024/2025

You can now download the JAMB Chemistry syllabus as you prepare for your exams.


The JAMB Chemistry syllabus serves as a crucial guide for candidates preparing for upcoming JAMB examinations. By focusing on the specified topics, candidates can streamline their study efforts effectively.

While it is essential to study the syllabus, it is important to note that not all examination questions will directly align with its content. However, a thorough understanding of the syllabus enhances overall preparation.

We recommend downloading the syllabus PDF from the post and sharing it with your friends to support their exceptional performance in the exams.

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