The official JAMB 2026/2027 syllabus for Chemistry is now available for download. If Chemistry is one of your core subjects, this syllabus is your roadmap to understanding the key topics and areas you need to study to excel in the exam.
| Examination Type | UTME / Direct Entry |
| Examination Year | 2026/2027 |
| Syllabus | Chemistry |
| File Format | |
| File Size | 283KB |
Some Key Areas Covered Syllabus
Here are some of the key areas covered:
- Structure of the Atom
- Periodic Table and Periodicity
- Chemical Bonding
- States of Matter and Gas Laws
- Energy Changes in Chemical Reactions
- Rates of Reaction
- Chemical Equilibrium
- Acids, Bases, and Salts
- Solubility and Solutions
- Electrochemistry
- Organic Chemistry
- Environmental Chemistry
- Metals and Non-Metals
General Objectives
| TOPICS/CONTENTS/NOTES | OBJECTIVES |
|---|---|
| 1. Separation of Mixtures and Purification of Chemical Substances (a) Pure and impure substances (b) Boiling and melting points (c) Elements, compounds and mixtures (d) Chemical and physical changes (e) Separation processes: – Evaporation, simple and fractional distillation, – sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation. | Candidates should be able to: (i) distinguish between pure and impure substances; (ii) use boiling and melting points as criteria for purity of chemical substances; (iii) distinguish between elements, compounds and mixture; (iv) differentiate between chemical and physical changes; (v) identify the properties of the components of a mixture; (vi) specify the principle involved in each separation method; and (vii) apply the basic principle of separation processes in everyday life. |
| 2. Chemical Combination Laws of definite, multiple and reciprocal 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 and stoichiometry of reactions. | Candidates should be able to: (i) perform simple calculations involving formulae, equations/chemical composition and the mole concept; (ii) deduce the chemical laws from given expressions/statements/data; (iii) interpret graphical representations related to these laws; and (iv) deduce the stoichiometry of chemical reactions. |
| 3. Kinetic Theory of Matter and Gas Laws (a) Phenomena to support the kinetic theory of matter using: (i) melting, (ii) vapourization (iii) boiling (iv) freezing (v) condensation in terms of molecular motion and Brownian movement. (b) (i) The laws of Boyle, Charles, Graham and Dalton (law of partial pressure); combined gas law, molar volume and atomicity of gases. (ii) The ideal gas equation (PV = nRT). (iii) The relationship between vapour density of gases and the relative molecular mass. | Candidates should be able to: (i) apply the theory to distinguish between solids, liquids and gases; (ii) deduce reasons for change of state; (iii) draw inferences based on molecular motion; (iv) deduce gas laws from given expressions/statements; (v) interpret graphical representations related to these laws; and (vi) perform simple calculations based on these laws, equations and relationships. |
| 4. Atomic Structure and Bonding (a) (i)The concept of atoms, molecules and ions, the works of Dalton, Millikan, Rutherford, Moseley, Thompson and Bohr. (ii) Atomic structure, electron configuration, atomic number, mass number and isotopes; specific examples should be drawn from elements of atomic number 1 to 20. (iii) Shapes of s and p orbitals. (b) The periodic table and periodicity of elements, presentation of the periodic table with a view to recognizing families of elements e.g. alkali metals, halogens, the noble gases and transition metals. The variation of the following properties: ionization energy, ionic radii, electron affinity and electronegativity. (c) Chemical bonding. 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. (d) Shapes of simple molecules: linear ((H2, O2, C12, HCl and CO2), non-linear (H2O), tetrahedral; (CH4) and pyramidal (NH3). (e) Nuclear Chemistry: (i) Radioactivity – Types and properties of radiations (ii) Nuclear reactions. Simple equations, uses and applications of natural and artificial radioactivity. | Candidates should be able to: (i) distinguish between atoms, molecules and ions; (ii) identify the contributions of these scientists to the development of the atomic structure; (iii) deduce the number of protons, neutrons and electrons from atomic and mass numbers of an atom; (iv) apply the rules guiding the arrangement of electrons in an atom; (v) identify common elements exhibiting isotopy; (vi) relate isotopy to mass number; (vii) perform simple calculations relating to isotopy; (viii) differentiate between the shapes of the orbitals; (ix) determine the number of electrons in s and p atomic orbitals; (x) relate atomic number to the position of an element on the periodic table; (xi) relate properties of groups of elements on the periodic table; (xii) identify reasons for variation in properties across the period and down the groups; (xiii) differentiate between the different types of bonding; (xiv) deduce bond types based on electron configurations; (xv) relate the nature of bonding to properties of compounds; (xvi) differentiate between the various shapes of molecules; xvii) distinguish between ordinary chemical reaction and nuclear reaction; (xviii) differentiate between natural and artificial radioactivity; (xix) compare the properties of the different types of nuclear radiations; (xx) compute simple calculations on the half-life of a radioactive material; (xxi) balance simple nuclear equation; and (xxii) identify the various applications of radioactivity. |
Download JAMB 2026 Syllabus for Chemistry Free PDF
Downloading the syllabus is easy and completely free. You can access it through the official JAMB website or use the direct download link below:
Frequently Asked Questions
Has the JAMB 2026/2027 Chemistry syllabus been released?
Yes, the official syllabus for Chemistry for the 2026/2027 UTME has been released and is now available for download.
Why is it important to study the JAMB Chemistry syllabus?
Studying the syllabus helps you stay focused on the right topics, understand what JAMB expects, and improve your chances of scoring high in the Chemistry section of the exam.
Does the syllabus include recommended textbooks?
Yes, the syllabus contains suggested textbooks to help you understand the topics better and practice effectively.
Is the JAMB Chemistry syllabus the same for all candidates?
Yes, the syllabus is the same for all candidates writing Chemistry in the UTME, regardless of their intended course of study or institution.
How many questions are asked from Chemistry in JAMB?
JAMB usually sets 40 questions for Chemistry, and they are to be answered in 30 minutes as part of the science subject combination.
Can I print the JAMB Chemistry syllabus?
Yes. Once downloaded in PDF format, you can print the syllabus for easy offline reading and highlighting important topics as you study.
