Jamb Chemistry 2022 Syllabus

Jamb Chemistry Syllabus

Below are the topics you need to read for your JAMB examination


Understand the basic principles and concept’s in Chemistry

Interpret scientific data relating to Chemistry

Deduce the relationship between Chemistry and other science

Apply the Knowledge to industry and everyday life.

The complete PDF file is also available.

Below are the Topics

  1. Separation of mixtures and purification of chemical substance
    1. pure and impure substances
    2. Boiling and melting points
    3. Elements, Compounds and Mixture
    4. Chemical and physical changes
    5. Separation process: Evaporation, simple and fractional distillation, sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization, magnetization and decantation.
  2. Chemical combination
    • Laws of definite, multiple and reciprocal proportion, law of conservation of matter, Gay Lussa’s law of combining volumes, Avogadro’s law; Chemical symbols, formulae, equations and their uses, relative atomic mass base on 12C=12, the mole concept and Avogadro’s number and stoichiometry of reactions.
  3. Kinetic theory of matter and Gas laws
    • Phenomenal to support Kinetic theory of matter using
      • Melting
      • Vaporization
      • Boiling
      • Freezing
      • Condensation In terms of molecular motion and Brownian movement
    • a. The law of Boyle, Charles, Graham, and Dalton (low of partial pressure); combined gas law, molar volume and atomicity of gases
    • b. The ideal gas equation(PV= nRT).
    • c. The relationship between vapour density gases and relative molecular mass.
  4. Atomic structure and bonding
    • i. The concept of atoms, molecule and ions, the work of Dalton, Millikan, Rutherford, Mosley, Thompson and Bohr.
    • ii. Atomic structure, electron configuration, atomic number, mass number and isotopes; specific examples should be drawn from elements of atomic number 1-20
    • iii. Shapes of s and p orbital
  5. Air
    • The natural gaseous constituents and their proportion in the air. -nitrogen, Oxygen, water vapour, Carbon(iv) oxide and noble gas (argon and neon)
    • Air as a mixture and some uses of noble gas.
  6. Water
    • Water as the product of combustion of hydrogen and its composition by volume
    • Water as solvent, atmospheric gases dissolved in water and their biological significant
    • Hard and soft water: Temporary and permanent hardness and method of softening hard water.
    • Treatment of water for town supply
  7. Solubility
    • Unsaturated, saturated and supersaturated solutions, solubility curves and simple deduction from them, (solubility defined in terms of mole per dm3) and simple calculations).
    • Solvents for fats, oil and paints and the use of such solvents for removal of stains.
  8. Environmental pollution
    • Source and effects of pollutants
    • Water pollution sewage and oil pollution should be known
    • Soil pollution: Oil spillage, biodegradable pollutants.
  9. Acids, base and salts
    • Quantitative comparison of the conductance of molar solutions of the conductance of strong and weak acids and bases, relationship between conductance and amount of ions present
    • pH and pHO scale; simple calculations.
    • Acid/base titration.
  10. Oxidation and Reduction – Redox
    • Oxidation in terms of the addition of oxygen or removal of hydrogen.
    • Reduction as removal of oxygen or addition of hydrogen.
    • Oxidation and reduction in terms of electron transfer.
    • Uses of oxidation numbers. Oxidation and reduction treated as change in oxidation number and use of oxidation number in balancing simple equations
    • ICUPAC nomenclature of inorganic compounds using oxidation number.
    • Text for oxidizing and reducing agents.
  11. Electrolysis
    • Electrolyte’s and non-electrolyte’s
    • Corrosion as an electrolytic process, cathodic protection of metals, painting, electroplating and coating with grease or oil as ways of preventing irons from corrosion.
  12. Energy Changes
    • Entropy is an order-disorder phenomenon: simple illustrations like mixing of gases and dissolution of salts.
  13. Rate of Chemical Reaction
    • Reaction rates curves.
    • Activation energy. Quantitative treatment of Arrhenius’ law and collision theory, effects of light on some reactions e.g, halogenation of alkanes.
  14. Chemical Equilibra: Reversible reactions and factors governing the equilibrium position. Dynamic equilibrium.
  15. Non-metals and their Compounds
    • Hydrogen: Commercial production from water gas and cracking of petroleum fractions, laboratory preparations, properties, uses and texts for hydrogen.
  16. Metal and their Compounds
  17. Organic compounds
  18. Chemistry and Industry

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