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JAMB 2024 syllabus for Chemistry

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JAMB 2024 syllabus for Chemistry

Welcome to Zamgist, Where we posted The latest JAMB 2024 syllabus for Chemistry, Chemistry JAMB Syllabus 2024 and JAMB syllabus 2023 for Chemistry.

If you are preparing for the Unified Tertiary Matriculation Examination (UTME) conducted by the Joint Admissions and Matriculation Board (JAMB), then you have come to the right place. will provide all the necessary guides that will help you succeed, without resorting to runz.

If you are planning to take the UTME and need a list of the outlined topics in chemistry that you should study in order to prepare for the examination, then this article is for you.

This article is all about the latest JAMB 2024 Syllabus for chemistry.

Is JAMB 2024 syllabus for Chemistry out?

Yes, Jamb 2024 syllabus for chemistry is out and we have posted it here in this page

About Jamb Syllabus for chemistry

The JAMB syllabus for chemistry is a list of outlined topics that students are required to study in order to prepare for the Unified Tertiary Matriculation Examination (UTME).

Objectives of Jamb 2024 Syllabus for chemistry

The objectives of the JAMB syllabus in chemistry is to prepare candidates for the UTME examination and to test their achievement of the following course objectives:

  • Apply knowledge of chemistry to industry and everyday life.
  • Deduce the relationships between chemistry and other sciences.
  • Apply basic principles of scientific methods in new situations.
  • Interpret scientific data.

JAMB 2024 syllabus for Chemistry

JAMB 2024 syllabus for Chemistry

1. Separation of Mixtures and Purification of Chemical Substances

(i) Pure and impure substances

(ii) Boiling and melting points

(iii) Elements, compounds, and mixtures

(iv) Chemical and physical changes

(v) Separation processes: evaporation, simple and fractional distillation, sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization

2. Chemical Combination

(i) Stoichiometry

(ii) Laws of definite and multiple proportions

(iii) Law of conservation of matter

(iv) Gay Lussac’s law of combining volumes

(v) Avogadro’s law

(vi) Chemical symbols, formulae, equations, and their uses

(vii) Relative atomic mass based on 12C=12

(viii) The mole concept and Avogadro’s number

3. Kinetic Theory of Matter & Gas Laws

(i) An outline of the kinetic theory of matter, melting, vaporization, and reverse processes.

(ii) Melting and boiling explained in terms of molecular motion and Brownian movement

(iii) The laws of Boyle, Charles, Graham, and Dalton (law of partial pressure)

(iv) Combined gas law

(v) Molar volume and atomicity of gases.

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4. Atomic Structure & Bonding

(i) (a) The concept of atoms, molecules, and ions, the work of Dalton, Millikan, Rutherford, Mosely, Thompson, and Bohr.

(b) Simple hydrogen spectrum, ionization of gases illustrating the electron as a fundamental particle of matter.

(c) 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

(ii) 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.

(iii) 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

(iv) Shapes of simple molecules: linear (H2, O2, C12, HCI, and CO2), non-linear (H2O), and tetrahedral (CH4).

(v) Nuclear Chemistry:

(a) Radioactivity (elementary treatment only)

(b) Nuclear reactions. Simple equations, uses, and applications of natural and artificial 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 gases.

6. Water

Composition by volume: Water as a solvent, atmospheric gases dissolved in water, and their biological significance.

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.

The water of crystallization, efflorescence, deliquescence, and hygroscopy.

Examples of the substances exhibiting these properties and their uses.

7. Solubility

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

(ii) Solvents for fats, oil, and paints and the use of such solvents for the removal of stains

(iii) Suspensions and colloids: Harmattan haze and paints as examples of suspensions and fog, milk, aerosol spray, and rubber solution as examples of colloids.

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8. Acids, Bases, & Salts

(i) General characteristics and properties of acids, bases, and salts. Acid/base indicators, basicity of acids, normal, acidic, basic, and double salts

(ii) 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

(iii) Qualitative comparison of the conductances of molar solutions of strong and weak acids and bases, relationship between conductance, amount of ions present, and their relative mobilities

(iv) pH and pOH scale. pH defined as – log[H3O+]

(v) Acid/base titrations

(vi) Hydrolysis of salts: simple examples such as NH4C1, AICI3, Na2CO3, CH3COONa to be mentioned.

9. 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 a change in oxidation number and use of oxidation numbers in balancing simple equations. IUPAC nomenclature of inorganic compounds

(e) Tests for oxidizing and reducing agents

10. 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

(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. 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 concentration term.

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

  •  powdered form
  •  lumps of the same mass.
  •  Catalyst e.g. the decomposition of H2O2 or KCIO3 in the presence or absence of 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

12. Energy Change

(a) 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 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.

13. 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 halogen.

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.

(ii) Sulphur: Uses and allotropes: preparation of allotropes is not expected. Preparation, properties, and uses of sulphur (IV) oxide, the reaction of SO2 with alkalis.

Trioxosulphate (IV) acid and its salts, the effect of acids on salts of trioxosulphate (IV), Tetraoxosulphate (VI) acid:

Commercial preparation (contact process only), properties as a dilute acid, an oxidizing and a dehydrating agents and uses. Test for SO42-.

Hydrogen sulphide: Preparation and properties as a weak acid, reducing and precipitating agents.

14. Chemical Equilibrium

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

Le Chatelier’s principle and equilibrium constant. Simple examples to include the action of steam on iron and N2O4, 2NO2. No calculation will be required.

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 seawater, and the recovery of sodium chloride.

(c) Alkaline-earth metals, e.g. calcium; calcium oxide, calcium hydroxide, and calcium trioxocarbonate (IV); properties and uses. Preparation of calcium oxide from seashells, the chemical composition of cement, and the setting of mortar. Test for Ca2+.

(d) Aluminium: Purification of bauxite, electrolytic extraction, properties, and uses of aluminium and its compounds. Test for Al3+.

(e) Tin: Extraction from its ores. Properties and uses.

(f) Metals of the first transition series:

Characteristic properties:
(i) electron configuration
(ii) oxidation states
(iii) complex ion formation
(iv) formation of coloured ions
(v) catalysis

(g) Iron: Extraction from sulphide and oxide ores, properties and uses, different forms of iron, and their properties and advantages of steel over iron. Test for Fe2+ and Fe3+.

(h) Copper: Extraction from sulphide and oxide ores, properties, and uses of copper. Preparation and uses of copper (II) tetraoxosulphate (VI). Test for Cu2+.

(i) Alloy Steel, stainless steel, brass, bronze, type-metal, duralumin, soft solder, permallory and alnico (constituents and uses only).

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Topics to read in Chemistry for JAMB 2024

Below are the topics that you need to read in chemistry for jamb 2024 UTME exam:

  1. Chemical Combination

  2. Kinetic Theory of Matter and Gas Laws

  3. Atomic Structure and Bonding

  4. Separation of Mixtures and Purification of Chemical Substances

  5. Acids, Bases, and Salts

  6. Oxidation and Reduction – Redox

  7. Electrolysis

  8. Energy Changes

  9. Rates of Chemical Reaction

  10. Chemical Equilibria

  11. Non-metals and Their Compounds

  12. Metals and Their Compounds

  13. Organic Compounds

  14. Solubility

  15. Water

  16. Air

  17. Environmental Pollution

  18. Chemistry and Industry

JAMB recommended textbooks for chemistry 2024

  1. Ababio, O.Y. (2005). New School Chemistry for Senior Secondary Schools, (Third Edition), Onitsha: Africana FIRST Publishers Limited

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

  3. Bajah, S.T., Teibo, B.O., Onwu, G and Obikwere, A. (2000). Senior Secondary Chemistry, Books 2 and 3, Lagos: Longman

  4. Ohia, G.N.C., Adewoyin, F.A. and Akpan, B.B. (1997). Exam Focus Chemistry for WASSCE & JME: Ibadan: University Press Plc

  5. STAN (1987). Chemistry for Senior Secondary Schools, Ibadan: Heinemann

  6. Sylvester: O.O. (2004). A Comprehensive Practical Chemistry for Senior Secondary Schools, Ibadan: Evans

  7. Uche, I.O., Adenuga, I.J. and Iwuagwu, S.L. (2003). Countdown to WASSCE/SSCE, NECO, JME Chemistry, Ibadan: Evans

  8. Wisdomline Pass at Once JAMB.

Where does JAMB ask questions mostly in chemistry?

According to research conducted by our experts, the table below shows the frequency with which JAMB asks questions on each topic based on analysis of JAMB past questions from 1979-2023.

Rank   Topic  Average % Number Of Question   
12 AIR 2.79
16 WATER 2.12
21 ACIDS 1.45


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