JAMB Chemistry Syllabus 2026/2027: Topics, Objectives & Study Guide

Q: How many questions does JAMB set in Chemistry?

JAMB sets 40 multiple-choice questions in Chemistry, each carrying equal marks for a total of 100 marks. Only Use of English has more (60 questions); every other subject follows this 40-question pattern, and your four subjects together make 180 questions and 400 marks.

Q: How long is the exam and how much time per question?

The whole UTME lasts two hours (120 minutes) for all four subjects combined — about 40 seconds per question on average. Pace yourself: answer the questions you know quickly, flag the hard ones, and come back to them.

Q: What textbooks are recommended for JAMB Chemistry?

The syllabus recommends standard texts such as New School Chemistry (Ababio) and other SSS Chemistry texts. Pair your textbook with plenty of calculation and equation practice.

Subject overview

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:

questions in Chemistry

100

marks (of 400 total)

Official syllabus Content is taken from the official JAMB UTME syllabus (IBASS). Last checked: 17 Sept 2026. Always confirm at jamb.gov.ng.

Your progress

Mark topics as you go to track your readiness.

Study the syllabus below, then test yourself. Move each topic from Not started → Learning → Practising → Mastered.

Practise Chemistry questions

General objectives

The Chemistry syllabus is designed to test candidates' ability to:

CHEMISTRY
(i) understand the basic principles and concepts in chemistry;
(ii) interpret scientific data relating to chemistry;
(iii) deduce the relationships between chemistry and other sciences; and
(iv) apply the knowledge of chemistry to industry and everyday life.
1. Separation of Mixtures and
Purification of Chemical
Substances
(a) Elements, compounds and mixtures
(b) Chemical and physical changes
(c) Pure and impure substances
(d) Boiling ,density, freezing and melting points
(e) Separation processes:
Evaporation, simple and fractional distillation, sublimation, re-crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation, filtration and centrifugation
2. Chemical Combination
Laws of definite, multiple and reciprocal proportions, law of conservation of matter,

How this paper is examined

JAMB Chemistry is a Computer-Based Test of 40 multiple-choice questions worth 100 marks. There is no negative marking, so attempt every question. It is taken with Use of English and two other subjects, for 180 questions in two hours overall.

How to use this syllabus: don't just read it — turn each topic into a checklist. Study a topic, then immediately practise questions on it so the knowledge sticks. Give extra time to the sections that carry the most topics, and revisit weak areas with timed practice as the exam approaches.

Practise as you learn: Belmadeng CBT practice is expanding across subjects. Explore CBT practice →

Every section and topic below is from the official JAMB syllabus, reproduced faithfully.

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, Avogadro,
Gay-Lussac, Graham and Dalton (law of partial pressure), 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
(iv) Ideal and real gases

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, the four quantum numbers, the principles that govern the arrangement of atoms into orbitals, electron configuration, atomic number, mass number and isotopes; specific
(ii) perform simple calculations involving formulae, equations/chemical composition and the mole concept; and
(iii) deduce the stoichiometry of chemical reactions.

5. Nuclear Chemistry

(i) Radioactivity – Types, properties and detection of radiations
(ii) Natural and artificial radioactivity
(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; and
(xvi) differentiate between the various shapes of molecules.

6. Solubility

(a) Unsaturated, saturated and supersaturated solutions. Solubility curves and simple deductions from them, (solubility defined in terms of mole per
dm3) and simple calculations
(b) Solvents for fats, oil, perspiration and paints and the use of such solvents for the removal of stains
(c) True and false solutions (Suspensions and colloids):
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

7. Environmental Pollution

(a) Air
(i) The natural gaseous constituents and their proportion in the air
– nitrogen, oxygen, water vapour, carbon (IV) oxide and the noble gases (argon and neon)
(iii) compare the properties of the different types of nuclear radiations;
(iv) compute simple calculations on the half-life of a radioactive material;
(v) balance simple nuclear equation; and
(vi) identify the various applications of radioactivity.

8. Acids, Bases and Salts

(a) General characteristics, properties and uses of acids, bases and salts.
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
(b) Qualitative comparison of the conductance of molar solutions of strong and weak acids and bases, relationship between conductance and amount of ions present
(v) identify the different types of pollution and pollutants;
(vi) specify different sources of pollutants;
(vii) classify pollutants as biodegradable and non-biodegradable;
(viii) specify the effects of pollution on the environment; and
(ix) identify measures for control of environmental pollution.

9. Oxidation and Reduction - Redox

(a) Oxidation in terms of the addition of oxygen
(b) Reduction as removal of oxygen with the aid of hydrogen
(c) Oxidation and reduction in terms of electron transfer
(d) Use of oxidation numbers.
Oxidation and reduction treated as change in oxidation number and use of oxidation numbers in balancing simple equations
(e) IUPAC nomenclature of inorganic compounds using oxidation number
(f) Tests for oxidizing and reducing agents pOH;
(x) enumerate the significance of pH in everyday life;
(xi) state applications of Buffer solution;
(xii) identify the appropriate acid-base indicator;
(xiii) interpret graphical representation of titration curves;
(xiv) perform simple calculations based on the mole concept;
(xv) balance equations for the hydrolysis of salts; and
(xvi) deduce the properties (acidic, basic, neutral) of the resultant solution.

10. Electrolysis

(a) Electrolytes and non-electrolytes
Faraday’s laws of electrolysis
(b) (i) Electrolysis of dilute H2SO4, aqueous CuSO4, CuC12 solution, dilute and concentrated NaC1 solutions and fused NaC1
(ii)Factors affecting discharge of ions at the electrodes
(c) Uses of electrolysis:
Purification of metals e.g. copper and production of elements and compounds (Al, Na, O2, Cl2 and NaOH)
(d) Electrochemical cells:
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)
(e) Corrosion as an electrolytic process, cathodic protection of metals, painting, electroplating and coating with grease or oil as ways of preventing iron from corrosion

11. Energy Changes

(a) Energy changes (∆H) accompanying physical and chemical changes:
Dissolution of substances in/or reaction with water e.g. Na, NaOH,
K, NH4Cl. Endothermic (+∆H) and exothermic (-∆H) reactions
(b) Entropy as an order-disorder phenomenon: simple illustrations like 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 respectively

12. 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 HCl and Na2S2O3 or Mg and HCl
(ii) Concentration/ Pressure 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
(iii) Surface area e.g. the reaction between marble and HCl with marble in:
(i) powdered form; and
(ii) lumps of the same mass.
(iv) Catalyst e.g. the decomposition of H2O2 or KClO3 in the presence or absence of MnO2
(b) Reaction rate curves
(c) Activation energy
Qualitative treatment of Arrhenius’ law and the collision theory, effect of light on some reactions e.g. halogenation of alkanes

13. Chemical Equilibra

Reversible reactions and factors governing the equilibrium position.
Dynamic equilibrium.

14. Non-metals and their Compounds

(a) Hydrogen: commercial production from water gas and cracking of petroleum fractions, laboratory preparation, properties, uses and test for hydrogen
(b) Halogens: 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 acid: Preparation and properties.
Chlorides and test for chlorides.
(c) Oxygen and Sulphur
(i) Oxygen:
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
Water - 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 water: Temporary and permanent hardness and methods of softening hard water.
Treatment of water for town supply.
(ii) predict the effects of each factor on the position of equilibrium;
(iii)specify the industrial processes where Le
Chatelier’s principle is required; and
(iv) determine the effects of these factors on equilibrium constant.

15. Metals and their Compounds

(a) General properties of metals
(b) Alkali metals e.g. sodium
(i) Sodium hydroxide:-
Production by electrolysis of brine, its action on aluminium, zinc and lead ions.
Uses including precipitation of metallic hydroxides
(ii) Sodium trioxocarbonate (IV) and sodium hydrogen trioxocarbonate (IV):
Production by Solvay process, properties and uses, e.g.
Na2CO3 in the manufacture of glass.
(iii) Sodium chloride: its occurrence in sea water and uses, the economic importance of sea water and the recovery of sodium chloride, test for Na+
(xxx) identify allotropes of carbon;
(xxxi) predict reagents for the laboratory preparation of CO2;
(xxxii) specify the properties of CO2 and its uses;
(xxxiii) determine the reagents for the laboratory preparation of CO;
(xxxiv) predict the effects of CO on human;
(xxxv) determine the specific tests for HCO3-,
CO32-, CO2 ;
(xxxvi) identify the different forms of coal;
(xxxvii) determine their uses;
(xxxviii) specify the products of the destructive distillation of wood and coal; and (xxxix) specify the uses of coke and synthesis
gas.

16. Organic Compounds

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
(a) Aliphatic hydrocarbons
(i) Alkanes
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
(ii) Alkenes
Isomerism: structural and geometric isomerism, additional and polymerization reactions, polythene and synthetic rubber as examples of products of polymerization and its use in vulcanization
(iii) Alkynes
Ethyne – production from action of water on carbides, simple reactions and properties of ethyne
(b) Aromatic hydrocarbons e.g. benzene - structure, properties and uses

17. Chemistry and Industry

Chemical industries: Types, raw materials and relevance. Biotechnology

18.Astronomical Chemistry

Solar system, planets, satellite and the composition of the earth - atmosphere, lithosphere and hydrosphere (xxxvii) identify the basic structure of proteins;
(xxxviii) specify the methods and products of hydrolysis;
(xxxix) specify the various tests for proteins;
(xl) distinguish between natural and synthetic polymers;
(xli) differentiate between addition and condensation polymerization processes;
(xlii) classify natural and commercial polymers and their uses; and (xliii) distinguish between thermoplastics and thermosetting plastics.

1. Ababio, O. Y. (2009). New School Chemistry for Senior Secondary Schools (Fourth

edition), Onitsha: Africana FIRST Publishers Limited.

2. Bajah, S.T., Teibo, B. O., Onwu, G. and Obikwere, A. Book 1 (1999). Senior Secondary

Chemistry, Books 2 and 3 (2000). Lagos: Longman.

3. Ojokuku, G. O. (2012).Understanding Chemistry for Schools and Colleges, (Revised

Edition), Zaria: Press-On Chemresources.

4. Odesina, I. A. (2008). Essential: Chemistry for Senior Secondary Schools, (2nd Edition),

Lagos: Tonad Publishers Limited.

5. Uche, I. O., Adenuga, I. J. and Iwuagwu, S. L. (2003).Countdown to WASSCE/SSCE,

NECO, JME Chemistry, Ibadan: Evans.

Recommended next steps

All subjects · Subject combination checker · JAMB information · CBT practice

Frequently asked questions

How many questions does JAMB set in Chemistry?

JAMB sets 40 multiple-choice questions in Chemistry, each carrying equal marks for a total of 100 marks. Only Use of English has more (60 questions); every other subject follows this 40-question pattern, and your four subjects together make 180 questions and 400 marks.

How long is the exam and how much time per question?

The whole UTME lasts two hours (120 minutes) for all four subjects combined — about 40 seconds per question on average. Pace yourself: answer the questions you know quickly, flag the hard ones, and come back to them.

Is Chemistry compulsory in JAMB?

Use of English is the only universally compulsory subject. Chemistry is required for Medicine, Pharmacy, Engineering, the physical and chemical sciences and related courses, so most science candidates take it.

How is the JAMB Chemistry syllabus structured?

The Chemistry syllabus spans separation of mixtures, chemical combination and bonding, the kinetic theory, atomic structure, the periodic table, acids/bases/salts, electrochemistry, energetics, rates, equilibrium, organic chemistry and more.

What should I focus on most in Chemistry?

Atomic structure and bonding, mole/stoichiometry calculations, acids-bases-salts, redox and electrolysis, rates and equilibrium, and organic chemistry are heavily examined. Practise calculations until they are automatic.

Does JAMB repeat past questions in Chemistry?

JAMB does not announce a policy of repeating questions, but the syllabus changes little from year to year, so the same topics and question styles recur. Studying strictly by the syllabus and practising many questions per topic is the dependable approach — never rely on 'expo', which is a scam.

Is there negative marking in JAMB Chemistry?

No. JAMB does not use negative marking, so a wrong answer scores zero with no penalty. Always attempt every question, even if you have to make an educated guess.

What textbooks are recommended for JAMB Chemistry?

The syllabus recommends standard texts such as New School Chemistry (Ababio) and other SSS Chemistry texts. Pair your textbook with plenty of calculation and equation practice.

Where can I find the official Chemistry syllabus?

The official source is the JAMB e-syllabus on the IBASS portal (jamb.gov.ng). The full topics are reproduced on this page for easy study, but always confirm the current syllabus on the official portal before your exam.

How can I practise Chemistry on Belmadeng?

Belmadeng offers free, timed CBT practice with worked explanations. Study a topic here, then test yourself — your weak topics are highlighted afterwards so you know exactly what to revise. Explore CBT practice to get started.

Source: official JAMB UTME Chemistry syllabus (IBASS, jamb.gov.ng). Reproduced for study use. Last checked: 17 Sept 2026. Belmadeng is not affiliated with JAMB — always confirm the current syllabus on the official portal.

← All subjects