JAMB Syllabus for 2023/2024 Chemistry CBT Exam (Jamb.org.ng) | CHECK NOW

For students to prepare properly for the upcoming JAMB examination, they are to read according to the JAMB syllabus. The JAMB Syllabus for Chemistry is essential for candidates who would be taking this subject in this examination. Moreover, this is because candidates would have an idea of the upcoming topics in JAMB.

JAMB 2023 Syllabus for Chemistry CBT Exam

JAMB Syllabus is a document that contains subjects that students would likely face in the examination and this one is very important. Nevertheless, this page will tell you what you need to know about the JAMB Syllabus. As well as, bring the Syllabus for Chemistry.


What is JAMB (Joint Admission and Matriculation Board) Syllabus

This is just material that would cover information about topics and areas of focus in JAMB (Joint Admission and Matriculation Board). Whereas, questions students would face on the exam date would come from the topics in the JAMB syllabus.

This is among the reasons why students need this file as it would help them cover every or most topics in JAMB. However, it would also increase their chances of passing the JAMB exam so this syllabus is very useful.

JAMB (Joint Admission and Matriculation Board) Syllabus for Chemistry

There are various topics in this subject but with the aid of the JAMB Syllabus for Chemistry students would be able to prepare properly for the examination. Nevertheless, this is because students would be able to cover the assumed JAMB chemistry topics. Below are the topics students need to prepare for in chemistry for JAMB

1. Separation of mixtures and purification of chemical substances

  • 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
These applicants are to
  • Differentiate between pure and impure substances
  • Use boiling and melting points as criteria for the purity of chemical substances
  • Distinguish between elements, compounds, and mixtures;
  • Differentiate between chemical and physical changes;
  • Identify the properties of the components of a mixture;
  • Specify the principle involved in each separation method

2. Chemical Combination

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 12C=12, the mole concept and Avogadro’s number

Candidates are to

  • Perform simple calculations involving formulae, equations/chemical composition, and the mole concept;
  • Deduce the chemical laws from given expressions/statements;
  • Interpret data based on these laws;
  • Interpret graphical representations related to these laws

3. Kinetic Theory of matter & Gas Law

  • An outline of the kinetic theory of matter, melting, vaporization, and reverse processes; melting and boiling are explained in terms of molecular motion and Brownian movement.
  • The laws of Boyle, Charles, Graham, and Dalton (law of partial pressure); combined gas law, molar volume, and atomicity of gases
Candidates are to
  • Apply the theory to distinguish between solids, liquids, and gases;
  • Deduce reasons for the change of state;
  • Draw inferences based on the molecular motion;
  • Deduce chemical laws from given expressions/ statements;
  • Interpret graphical representations related to these laws;
  • Perform simple calculations based on these laws and the relationship between the vapor density of gases and the relative molecular mass.

4. Atomic Structure & Bonding

  • (i)The concept of atoms, molecules, and ions, the works of Dalton, Millikan, Rutherford, Mosely, Thompson, and Bohr. Simple hydrogen spectrum, Ionization of gases illustrating the electron as a fundamental particle of matter. (ii) Atomic structure, electron configuration, atomic number, mass number, and isotopes; 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 elements, presentation of the periodic table to recognize families of elements e.g alkali metals, halogens, noble gases, and transition metals. The variation of the following properties should be noticed: ionization energy, ionic radii, electron affinity, and electronegativity.
  • Chemical bonding: Electrovalence and covalency, the electron configuration of elements and their tendency to attain the noble gas structure. Furthermore, hydrogen bonding and metallic bonding as special types of electrovalence and covalency respectively; coordinate bond is 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 molecules: linear ((H2, 02, C12, HCI and CO2), non-linear (H2O) and tetrahedral; (CH4)

(b) Nuclear Chemistry: (i) Radioactivity (elementary treatment only) (ii) Nuclear reactions. Simple equations use and applications of natural and artificial radioactivity.

Candidates are to
  • Distinguish between atoms, molecules, and ions;
  • Assess the contributions of these scientists to the development of the atomic structure;
  • Deduce the number of protons, neutrons, and electrons from the atomic and mass numbers of an atom;
  • Apply the rules guiding the arrangement of electrons in an atom;
  • Relate isotopy to mass number;
  • Perform simple calculations on relative atomic mass
  • 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.
  • Differentiate between the different types of bonding.
  • Deduce bond types based on electron configurations;
  • Relate the nature of bonding to properties of compounds;
  • Apply it in everyday chemistry;
  • Differentiate between the various shapes of molecules
  • Distinguish between an ordinary chemical reaction and a nuclear reaction;
  • Differentiate between natural and artificial radioactivity;
  • Compare the properties of the different types of nuclear radiation;
  • Compute simple calculations on the half-life of radioactive material;
  • Balance simple nuclear equations;
  • Identify the various applications of radioactivity

5. Air

The usual gaseous constituents – nitrogen, oxygen, water vapor, carbon (IV) oxide, and the noble gases (argon and neon), the proportion of oxygen in the air e.g. by burning phosphorus or by using alkaline pyrogallol, air as a mixture, and some uses of the noble gas.

Candidates are to
  • Deduce reason (s) for the existence of air as a mixture;
  • Identify the principle involved in the separation of air components;
  • Deduce reasons for the variation in the composition of air in the environment;
  • Specify the uses of some of the constituents of air

6. Water

Composition by volume: Water as a solvent, atmospheric gases dissolved in water and their biological significance. Moreover, water is a product of the combustion of hydrogen. Hard and soft water: Temporary and permanent hardness and methods of softening hard water. Purification of town water supplies. Furthermore, the water of crystallization, efflorescence, deliquescence, and hygroscope. However, examples of the substances exhibiting these properties and their uses.

Candidates are to
  • Identify the various uses of 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 purification of water for town supply;
  • Distinguish between these phenomena;
  • Identify the various compounds that exhibit these phenomena.

7. Solubility

  • Unsaturated, saturated, and supersaturated solutions. Solubility curves and simple deductions from them, (solubility defined in terms of a mole per dm3) and simple calculations.


  • Solvents for fats, oil, and paints and the use of such solvents for the removal of stains.


  • Suspensions and colloids: Harmattan haze and paints as examples of suspensions and fog, milk, aerosol spray, and rubber solution as examples of colloids.
Candidates are to
  • 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;
  • Classify solvents based on their uses;
  • Differentiate between a true solution, suspension, and colloids;
  • Compare the properties of a true solution and a ‘false’ solution.
  • Provide typical examples of suspensions and colloids.

8. Environmental Pollution

(a)       Sources and effects of pollutants.

(b)      Air pollution: Examples of air pollutants such as H2S, CO, SO2, oxides of nitrogen, fluorocarbons, and dust.

(c)        Water pollution Sewage and oil pollution should be known.

(d)       Soil pollution: Oil spillage, Biodegradable and non-biodegradable pollutants.

Candidates are to
  • Identify the different types of pollution and pollutants;
  • Classify pollutants as biodegradable and non-biodegradable;
  • Assess the effects of pollution on the environment;
  • Recommend measures for control of environmental pollution.

9. Acids, Base & Salt

  • General characteristics and properties of acids, bases and salts. Acids/base indicators, the basicity of acids, normal, acidic, basic, and double salts. Whereas, an acid is defined as a substance whose aqueous solution furnishes H3O+ions or as a proton donor. However, Ethanoic, citric, and tartaric acids as examples of naturally occurring organic acids, alums as examples of double salts, and the preparation of salts by neutralization, precipitation, and 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, the relationship between conductance, the number of ions present, and their relative mobilities.


  • pH and pOH scale. pH defined as – log[H3O+]


  • Acid/base titrations.


(e)   Hydrolysis of salts: Simple examples such as NH4C1, AICI3, Na2CO3, and CH3COONa are to be mentioned.


Candidates are to
  • Distinguish between the properties of acids and bases;
  • Identify the different types of acids and bases;
  • Differentiate between acidity and alkalinity using acid/base indicators;
  • Identify the various methods of preparation of salts;
  • Classify different types of salts;
  • Relate the degree of dissociation to the strength of acids and bases;
  • Relate degree of dissociation to conductance;
  • Perform simple calculations on pare H;
  • 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;
  • Deduce the properties (acidic, basic, neutral) of the resultant solution.

10. Oxidation and Reduction

(a)           Oxidation in terms of the addition of oxygen or removal of hydrogen.

(b)          Reduction as removal of oxygen or addition of hydrogen.

(c)           Oxidation and reduction in terms of electron transfer.

(d)          Use of oxidation numbers. Oxidation and reduction treated as change I oxidation.

number and use of oxidation numbers in balancing simple equations. However, IUPAC nomenclature of inorganic compounds.

  • Tests for oxidizing and reducing agents
Candidates are to
  • 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 transfers in redox reactions;
  • Identify the name of redox species using IUPAC nomenclature.
  • Distinguish between oxidizing and reducing agents in redox reactions.

11. Electrolysis

(a)           Electrolytes and non-electrolytes. Faraday’s laws of electrolysis.

(b)          Electrolysis of dilute H2SO4, aqueous CuSO4, CuC12 solution, dilute and concentrated NaC1 solutions and fused NaC1 and factors affecting discharge of ions at the electrodes.

(c)           Uses of electrolysis: Purification of metals e.g. copper and production of elements and compounds e.g. A1, Na, O2, Cl2, and NaOH.

(d)          Electrochemical cells: Redox series (K, Na, Ca, Mg, AI, Zn, Fe, PbII, H, Cu, Hg, 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
Candidates are to
  • Identity between electrolytes and non-electrolytes;
  • Perform calculations based on faraday as a 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 product of electrolysis;
  • Specify the different areas of application of electrolysis;
  • Identify the various electrochemical cells;
  • Calculate electrode potentials using half- cell reaction equations;
  • Determine the different areas of applications of electrolytic processes;
  • Apply the methods to protect metals.

12. Energy Charge

  • Energy changes(∆H) accompanying physical and chemical changes: dissolution of substances in or reaction with water e.g. Na, NaOH, K, NH4, Cl. Endothermic (+∆H) and

exothermic (-∆H) reactions.

(b)    Entropy as an order-disorder phenomenon: simple illustrations like the mixing of gases and dissolution of salts.

(c)    Spontaneity of reactions: ∆G0 = 0 as a criterion for equilibrium, ∆G greater or

less than zero as a criterion for non-spontaneity or spontaneity.

Candidates are to
  • Determine the types of heat changes (∆H) 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 the spontaneity of a reaction;
  • Relate (∆H), ∆S0 and ∆G0 as the driving forces for chemical reactions;
  • Solve simple problems based on the relationships ∆G0= ∆H0-T∆S0)

13. Rates of Chemical Reaction

(a)           Elementary treatment of the following factors which can change the rate of a chemical reaction:

(i)            Temperature e.g. the reaction between HCI and Na2S2O3 or Mg and HCI

(ii)           Concentration e.g. the reaction between HCl and Na2S2O3, HCl and marble, and the iodine clock reactio1n, for gaseous systems, pressure may be used as a concentration term.

(iii)          SURFACE area e.g. the reaction between marble and HCI with marble in

(i)            Powdered form

(ii)           Lumps of the same mass.


(iv)          Catalyst e.g. the decomposition of H2O2 or KCIO3 in the presence or absence  MnO2


(b)          Concentration/time curves.

(c)           Activation energy Qualitative treatment of Arrhenius’ law and the collision theory, effect of light on some reactions. e.g. halogenation of alkanes

Candidates are to
  • Identify the factors that affect the rates of a chemical reaction;
  • Determine the effects of these factors on the rate of reactions;
  • Recommend ways of moderating these effects;
  • Examine the effect of concentration 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.
  • 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.
  • Deduce the value of activation energy (Ea) from reaction rate curves

14. Chemical Equilibrium

Reversible reactions and factors governing the equilibrium position. Dynamic equilibrium. Le Chatelier’s principle and equilibrium constant. Moreover, simple examples include the action of steam on iron and 2NO2. Nevertheless, no calculation will be required

Candidates are to
  • Identify the factors that affect the position of equilibrium of a chemical reaction;
  • Predict the effects of each factor on the position of the equilibrium

This is the JAMB Syllabus for Chemistry. However, these topics are meant to be a guideline for candidates who would be taking chemistry in the examination.

Open this link to get the Full JAMB Syllabus for Chemistry and this link to get the Recommended Textbooks to read for the 2023/2024 CBT Exam.

This post is authored by Madago Emuobo A.K.A Mobo, the founder and Admin of Naijschools. With nearly a decade of expertise in the education sector, Mobo started with Naijschools providing up-to-date information on educational and tech-related topics on breaking news, and daily opportunities for students and graduates.

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