JAMB Syllabus for Chemistry 2022/2023 (PDF Download)

Do you wish to score high in JAMB? Have you been searching for JAMB Syllabus for Chemistry 2022? Then this post you’re currently reading will surely benefit you.

We provide you this article to help 2022 JAMB candidates to perform better in their chemistry, This 2022 JAMB chemistry syllabus is gotten from the JAMB brochure. It is designed to test student’s achievement of the course objectives as well as enhance their performance.

What Is Chemistry JAMB Syllabus 2022?

The JAMB Syllabus for Chemistry 2022 is an outline containing JAMB candidate’s Area of Concentration 2022. These area of concentration are topics that candidates are expected to study to enhance their JAMB performance.

JAMB Chemistry Area of Concentration 2022

I’m sure you all have written one exam or the other, we all know how tough it is when in the exam hall despite all preparations.

JAMB Chemistry syllabus 2022 area of concentration is an appropriate materials that will make your Jamb preparation to be more effective, easy, and helpful.

Helpful Materials for JAMB Chemistry practice 2022

The above materials are helpful for your Jamb practice. Having known that, lets look at the recommended Jamb chemistry syllabus for 2022.


JAMB Syllabus for Chemistry 2022

The following is the approved JAMB Syllabus For Chemistry 2022/2023.

  1. Separation of mixtures and purification of chemical substances
  2. Chemical Combination
  3. Atomic Structure and Bonding
  4. Air
  5. Water
  6. Solubility
  7. Environmental Pollution
  8. Acids, Base and Salt
  9. Oxidation and Reduction
  10. Electrolysis
  11. Energy Change
  12. Rates of Chemical Reactions
  13. Chemical Equilibrium

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
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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.

Kinetic Theory of Matter and Gas Law

(a) An outline of the kinetic theory of matter, melting, vapourization and reverse processes; melting and boiling explained in terms of molecular motion and Brownian movement.

(b) The laws of Boyle, Charles, Graham and Dalton (law of partial pressure); combined gas law, molar volume and atomicity of gases

Atomic Structure and Bonding

(a) (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 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.

(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 should be noticed: 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, 02, C12,HCI and CO2), non-linear (H2O) and
tetrahedral; (CH4)

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


The usual gaseous constituents – nitrogen, oxygen, water vapour, carbon (IV) oxide and the noble gases (argon and neon), 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.


Composition by volume: Water as a solvent, atmospheric gases dissolved in water and their biological significance. Water as a product of the combustion of hydrogen. Hard and soft water:

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Temporary and permanent hardness and methods of softening hard water. Purification of town water supplies.

Water of crystallization, efflorescence, deliquescence and hygroscopy. Examples of the substances exhibiting these properties and their uses.


(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 and paints and the use of such solvents for the removal of stains.

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

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.

Acids, Base and Salt

(a) General characteristics and properties 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 conductances of molar solutions of strong and weak acids and bases, relationship between conductance, amount of ions present and their relative mobilities.

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

(d) Acid/base titrations.

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

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 in oxidation.
number and use of oxidation numbers in balancing simple equations. IUPAC nomenclature of inorganic compounds.
(e) Tests for oxidizing and reducing agents.


(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.

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.

Rates of Chemical Reactions

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

(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.

Chemical Equilibrium

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

JAMB Syllabus For Chemistry 2022 (Download PDF)

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