JAMB Chemistry Syllabus for 2025 UTME | Recommended Textbooks

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JAMB Chemistry Syllabus 2025/26 Textbooks
JAMB Syllabus for Chemistry and Textbooks

GENERAL OBJECTIVES

The Unified Tertiary Matriculation Examination (UTME) syllabus for Chemistry is designed to prepare candidates for the Board’s examination. The syllabus aims to test candidates’ understanding of:

  • Fundamental principles and concepts in chemistry
  • Interpretation of scientific data related to chemistry
  • The relationship between chemistry and other sciences
  • Application of chemistry knowledge in industry and everyday life

DETAILED SYLLABUS

1. Separation of Mixtures and Purification of Chemical Substances

Topics:

  • Pure and impure substances
  • Boiling and melting points
  • Elements, compounds, and mixtures
  • Chemical and physical changes
  • Separation techniques:
    • Evaporation
    • Simple and fractional distillation
    • Sublimation
    • Filtration
    • Crystallization
    • Chromatography (paper & column)
    • Fractional crystallization
    • Magnetization
    • Decantation

Objectives:
Candidates should be able to:

  1. Distinguish between pure and impure substances.
  2. Use boiling and melting points as criteria for purity.
  3. Differentiate between elements, compounds, and mixtures.
  4. Identify chemical and physical changes.
  5. Understand the properties of mixture components.
  6. Explain the principles behind separation techniques.
  7. Apply separation methods in real life.

2. Chemical Combination

Topics:

  • Stoichiometry
  • Laws of chemical combination:
    • Law of definite proportions
    • Law of multiple proportions
    • Law of conservation of mass
    • Gay-Lussac’s Law
    • Avogadro’s Law
  • Chemical symbols, formulae, and equations
  • Relative atomic mass (C=12)
  • The mole concept & Avogadro’s number

Objectives:
Candidates should be able to:

  1. Perform simple calculations involving chemical formulae, equations, and the mole concept.
  2. Deduce chemical laws from given expressions, statements, or data.
  3. Interpret graphical representations of chemical laws.
  4. Determine stoichiometric relationships in chemical reactions.

3. Kinetic Theory of Matter and Gas Laws

Topics:

  • The kinetic theory of matter
    • Melting
    • Vaporization
    • Boiling
    • Freezing
    • Condensation
  • Molecular motion and Brownian movement
  • Gas Laws:
    • Boyle’s Law
    • Charles’ Law
    • Graham’s Law
    • Dalton’s Law of Partial Pressure
    • Combined Gas Law
    • Molar Volume
    • Atomicity of gases
    • Ideal Gas Equation (PV = nRT)
    • Relationship between vapor density and relative molecular mass

Objectives:
Candidates should be able to:

  1. Apply kinetic theory to differentiate between solids, liquids, and gases.
  2. Explain reasons for changes in states of matter.
  3. Draw conclusions from molecular motion.
  4. Deduce gas laws from given expressions or data.
  5. Interpret graphical representations of gas laws.
  6. Perform calculations based on gas laws.

4. Atomic Structure and Bonding

(a) Atomic Structure

Topics:

  • Concepts of atoms, molecules, and ions
  • Contributions of Dalton, Millikan, Rutherford, Moseley, Thomson, and Bohr
  • Atomic structure, electron configuration, atomic number, and mass number
  • Isotopes and examples (elements with atomic numbers 1–20)
  • Shapes of s and p orbitals

Objectives:
Candidates should be able to:

  1. Differentiate between atoms, molecules, and ions.
  2. Recognize scientists’ contributions to atomic structure.
  3. Calculate the number of protons, neutrons, and electrons.
  4. Apply rules for electron configuration.
  5. Identify elements exhibiting isotopy.
  6. Relate isotopy to mass number and perform calculations.
  7. Differentiate the shapes of atomic orbitals.
  8. Determine the number of electrons in s and p orbitals.

(b) Periodic Table and Periodicity

Topics:

  • Periodic table structure and element classification (alkali metals, halogens, noble gases, transition metals)
  • Periodic variations in:
    • Ionization energy
    • Ionic radii
    • Electron affinity
    • Electronegativity

Objectives:
Candidates should be able to:

  1. Relate atomic number to element positioning in the periodic table.
  2. Compare properties of element groups.
  3. Explain variations in periodic properties across periods and down groups.

(c) Chemical Bonding

Topics:

  • Types of bonding:
    • Electrovalent (ionic)
    • Covalent
    • Hydrogen bonding
    • Metallic bonding
    • Coordinate covalent bonding
  • Noble gas electron configuration
  • Van der Waals’ forces
  • Molecular shapes:
    • Linear (H₂, O₂, Cl₂, HCl, CO₂)
    • Non-linear (H₂O)
    • Tetrahedral (CH₄)
    • Pyramidal (NH₃)

Objectives:
Candidates should be able to:

  1. Differentiate between types of bonding.
  2. Deduce bond types from electron configurations.
  3. Relate bonding nature to compound properties.
  4. Identify molecular shapes.

JAMB CHEMISTRY SYLLABUS 

5. Nuclear Chemistry

Topics/Contents/Notes

(a) Radioactivity:

  • Types and properties of radiations

(b) Nuclear Reactions:

  • Simple equations
  • Uses and applications of natural and artificial radioactivity

Objectives

Candidates should be able to:

  1. Distinguish between ordinary chemical reactions and nuclear reactions.
  2. Differentiate between natural and artificial radioactivity.
  3. Compare the properties of different types of nuclear radiation.
  4. Perform simple calculations on the half-life of radioactive materials.
  5. Balance simple nuclear equations.
  6. Identify various applications of radioactivity.

6. Air

Topics/Contents/Notes

(a) Natural gaseous constituents of air and their proportions:

  • Nitrogen, oxygen, water vapour, carbon(IV) oxide, and noble gases (argon and neon).

(b) Air as a mixture and uses of noble gases.

Objectives

Candidates should be able to:

  1. Explain why air is considered a mixture.
  2. Identify the principles involved in the separation of air components.
  3. Deduce reasons for variations in the composition of air in different environments.
  4. Specify the uses of some air constituents.

7. Water

Topics/Contents/Notes

(a) Water as a product of hydrogen combustion and its volumetric composition. (b) Water as a solvent, including dissolved atmospheric gases and their biological significance. (c) Hard and soft water:

  • Temporary and permanent hardness
  • Methods of softening hard water (d) Treatment of water for municipal supply. (e) Water of crystallization, efflorescence, deliquescence, and hygroscopy with examples and applications.

Objectives

Candidates should be able to:

  1. Identify various uses of water.
  2. Understand the effects of dissolved atmospheric gases in water.
  3. Distinguish between the properties of hard and soft water.
  4. Determine the causes of water hardness.
  5. Identify methods for removing water hardness.
  6. Describe the processes involved in water treatment for municipal supply.
  7. Differentiate between efflorescence, deliquescence, and hygroscopy.
  8. Identify compounds exhibiting these phenomena.

8. Solubility

Topics/Contents/Notes

(a) Types of solutions:

  • Unsaturated, saturated, and supersaturated solutions.
  • Solubility curves and related calculations (solubility expressed in moles per dm³).

(b) Solvents for fats, oils, and paints and their application in stain removal.

(c) False solutions (suspensions and colloids):

  • Properties and examples.
  • Harmattan haze and water paints as examples of suspensions.
  • Fog, milk, aerosol sprays, emulsion paints, and rubber solutions as examples of colloids.

Objectives

Candidates should be able to:

  1. Differentiate between different types of solutions.
  2. Interpret solubility curves.
  3. Calculate the amount of solute that can dissolve in a given solvent at a specified temperature.
  4. Explain that solubility is temperature-dependent.
  5. Relate the nature of solvents to their practical uses.
  6. Differentiate between true solutions, suspensions, and colloids.
  7. Compare the properties of true and false solutions.
  8. Provide typical examples of suspensions and colloids.

9. Environmental Pollution

Topics/Contents/Notes

(a) Sources and effects of pollutants. (b) Air pollution:

  • Examples: Hydrogen sulfide (H₂S), carbon monoxide (CO), sulfur oxides (SO₂), nitrogen oxides, chlorofluorocarbons (CFCs), and dust. (c) Water pollution:
  • Examples: Sewage and oil pollution. (d) Soil pollution:
  • Examples: Oil spillage, biodegradable, and non-biodegradable pollutants.

Objectives

Candidates should be able to:

  1. Identify different types of pollution and their sources.
  2. Classify pollutants as biodegradable or non-biodegradable.
  3. Describe the effects of pollution on the environment.
  4. Identify measures for controlling environmental pollution.

10. Acids, Bases, and Salts

Topics/Contents/Notes

(a) General characteristics and properties of acids, bases, and salts:

  • Acid/base indicators
  • Basicity of acids
  • Types of salts: Normal, acidic, basic, and double salts
  • Acids as substances whose aqueous solutions furnish H₃O⁺ ions or as proton donors
  • Examples of naturally occurring organic acids (ethanoic, citric, and tartaric acids)
  • Alums as examples of double salts
  • Preparation of salts by neutralization, precipitation, and reactions of acids with metals, oxides, and trioxocarbonates(IV)

(b) Qualitative comparison of molar conductance of strong and weak acids and bases, and the relationship between conductance and ion concentration.

Objectives

Candidates should be able to:

  1. Distinguish between the properties of acids and bases.
  2. Identify different types of acids and bases.
  3. Determine the basicity of acids.
  4. Differentiate between acidity and alkalinity using acid/base indicators.
  5. Identify various methods of preparing salts.
  6. Classify different types of salts.
  7. Relate the degree of dissociation to the strength of acids and bases.
  8. Relate the degree of dissociation to conductance.

9. Acids, Bases, and Salts

(a) General Characteristics and Properties

  • Acid/base indicators
  • Basicity of acids: normal, acidic, basic, and double salts
  • Acids as substances whose aqueous solutions furnish H₃O⁺ ions or act as proton donors
  • Examples of naturally occurring organic acids (ethanoic, citric, and tartaric 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) Conductance of Acids and Bases

  • Qualitative comparison of the conductance of molar solutions of strong and weak acids and bases
  • Relationship between conductance and the amount of ions present

(c) pH and pOH Scale

  • Simple calculations involving pH and pOH

(d) Acid-Base Titrations

  • Interpretation of titration curves
  • Selection of appropriate acid-base indicators
  • Simple calculations based on the mole concept

(e) Hydrolysis of Salts

  • Principles of hydrolysis
  • Simple examples: NH₄Cl, AlCl₃, Na₂CO₃, and CH₃COONa

OBJECTIVES

  • Distinguish between the properties of acids and bases
  • Identify different types of acids and bases
  • Determine the basicity of acids
  • Differentiate between acidity and alkalinity using indicators
  • Identify various methods of salt preparation
  • Classify different types of salts
  • Relate the degree of dissociation to the strength of acids and bases
  • Relate dissociation to conductance
  • Perform simple pH and pOH calculations
  • Balance equations for hydrolysis reactions
  • Determine the properties (acidic, basic, neutral) of hydrolysis products

10. Oxidation and Reduction

(a) Concepts of Oxidation and Reduction

  • Oxidation as the addition of oxygen or removal of hydrogen
  • Reduction as the removal of oxygen or addition of hydrogen
  • Oxidation and reduction in terms of electron transfer

(b) Use of Oxidation Numbers

  • Oxidation and reduction treated as changes in oxidation number
  • Application of oxidation numbers in balancing equations

(c) IUPAC Nomenclature

  • Naming of inorganic compounds using oxidation numbers

(d) Tests for Oxidizing and Reducing Agents

OBJECTIVES

  • Identify various ways of expressing oxidation and reduction
  • Classify reactions based on oxidation or reduction
  • Balance redox reaction equations
  • Deduce oxidation numbers of chemical species
  • Compute the number of electrons transferred in redox reactions
  • Distinguish between oxidizing and reducing agents
  • Apply oxidation numbers in naming inorganic compounds
  • Relate reagents to their oxidizing and reducing abilities

11. Electrolysis

(a) Electrolytes and Non-Electrolytes

  • Faraday’s laws of electrolysis

(b) Electrolysis of Various Solutions

  • Dilute H₂SO₄, aqueous CuSO₄, CuCl₂ solutions
  • Dilute and concentrated NaCl solutions
  • Fused NaCl
  • Factors affecting ion discharge at electrodes

(c) Applications of Electrolysis

  • Purification of metals (e.g., copper)
  • Production of elements and compounds (Al, Na, O₂, Cl₂, NaOH)

(d) Electrochemical Cells

  • Redox 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 and Its Prevention

  • Corrosion as an electrolytic process
  • Methods of corrosion prevention: cathodic protection, painting, electroplating, grease/oil coating

OBJECTIVES

  • Differentiate between electrolytes and non-electrolytes
  • Perform calculations using Faraday’s laws
  • Identify suitable electrodes for different electrolytes
  • Specify chemical reactions at electrodes
  • Determine products of electrolysis
  • Identify factors affecting electrolysis products
  • Specify applications of electrolysis
  • Identify various electrochemical cells
  • Calculate electrode potentials using half-cell reaction equations
  • Identify methods for protecting metals from corrosion

12. Energy Changes in Chemical Reactions

(a) Enthalpy (ΔH) in Physical and Chemical Changes

  • Dissolution of substances in water (e.g., Na, NaOH, K, NH₄Cl)
  • Endothermic (ΔH > 0) and exothermic (ΔH < 0) reactions

(b) Entropy (ΔS) and Disorder

  • Mixing of gases and dissolution of salts as examples

(c) Spontaneity of Reactions

  • ΔG = 0 as the criterion for equilibrium
  • ΔG > 0 or ΔG < 0 as criteria for non-spontaneity or spontaneity

OBJECTIVES

  • Identify different types of enthalpy changes in physical and chemical processes
  • Interpret graphical representations of energy changes
  • Relate the physical state of a substance to its degree of orderliness
  • Determine conditions for spontaneity of reactions
  • Relate ΔH, ΔS, and ΔG as driving forces of chemical reactions
  • Solve simple problems using ΔG = ΔH – TΔS

13. Rates of Chemical Reactions

(a) Factors Affecting Reaction Rates

  • Temperature effects (e.g., reaction between HCl and Na₂S₂O₃ or Mg and HCl)

OBJECTIVES

  • Identify factors influencing reaction rates
  • Determine temperature effects on reaction rates

13. Rates of Chemical Reactions

(a) Factors Affecting Reaction Rates:

  1. Temperature:
    • Example: Reaction between HCl and Na₂S₂O₃ or Mg and HCl.
  2. Concentration:
    • Example: Reaction between HCl and Na₂S₂O₃, HCl and marble, iodine clock reaction.
    • For gaseous systems, pressure is used as a concentration term.
  3. Surface Area:
    • Example: Reaction between marble and HCl in:
      • (i) Powdered form
      • (ii) Lumps of the same mass.
  4. Catalyst:
    • Example: 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 reactions, e.g., halogenation of alkanes.

OBJECTIVES: Candidates should be able to:

  1. Identify factors affecting reaction rates.
  2. Determine the effect of temperature on reaction rates.
  3. Examine the effect of concentration/pressure on reaction rates.
  4. Describe how surface area affects reaction rates.
  5. Identify suitable catalysts and their effects.
  6. Determine ways to moderate these effects in chemical reactions.
  7. Interpret reaction rate curves.
  8. Solve simple problems on reaction rates.
  9. Relate reaction rates to the kinetic theory of matter.
  10. Examine the significance of activation energy.
  11. Deduce activation energy (Ea) from reaction rate curves.

14. Chemical Equilibria

  • Reversible reactions and factors affecting equilibrium position.
  • Dynamic equilibrium.
  • Le Chatelier’s Principle and equilibrium constant.
  • Examples: Action of steam on iron. (No calculations required.)

OBJECTIVES: Candidates should be able to:

  1. Identify factors affecting equilibrium position.
  2. Predict the effects of each factor on equilibrium.
  3. Determine how these factors influence equilibrium constant.

15. Non-Metals and Their Compounds

(a) Hydrogen:

  • Commercial production from water gas and petroleum cracking.
  • Laboratory preparation, properties, uses, and test for hydrogen.

(b) Halogens:

  • Chlorine:
    • Laboratory and industrial preparation (electrolysis).
    • Properties and uses (e.g., water sterilization, bleaching, HCl production, plastics, insecticides).
  • Hydrogen chloride and Hydrochloric Acid:
    • Preparation, properties, chlorides, and test for chlorides.

(c) Oxygen and Sulphur:

  • Oxygen:
    • Laboratory and commercial preparation (liquid air distillation).
    • Properties and uses.
    • Oxides: Acidic, basic, amphoteric, and neutral.
    • Ozone (O₃) as an allotrope and its atmospheric importance.
  • Sulphur:
    • Uses and allotropes (preparation not required).
    • Preparation, properties, and uses of SO₂.
    • Reaction of SO₂ with alkalis.
    • Acids and Salts:
      • H₂SO₃ and its salts.
      • Effects of acids on H₂SO₃ salts.
      • H₂SO₄ (Contact Process), properties, and uses.
    • Hydrogen Sulphide:
      • Preparation, properties (weak acid, reducing, precipitating agent).
      • Test for S²⁻.

(d) Nitrogen:

  • Laboratory preparation and production from liquid air.
  • Ammonia (NH₃):
    • Laboratory and industrial preparation (Haber Process).
    • Properties and uses.
    • Ammonium salts and their applications.
    • Oxidation to NO₂ and HNO₃.
    • Test for NH₄⁺.
  • Trioxonitrate (V) Acid (HNO₃):
    • Laboratory preparation from NH₃.
    • Properties and uses.
    • Trioxonitrate (V) salts: Heat action and applications.
    • Test for NO₃⁻.
  • Oxides of Nitrogen:
    • Properties.

OBJECTIVES: Candidates should be able to:

  1. Predict reagents for laboratory and industrial preparation of these gases and compounds.
  2. Identify properties and compare characteristics of these gases and compounds.
  3. Specify uses of each gas and its compounds.
  4. Determine specific tests for Cl⁻, SO₄²⁻, SO₃²⁻, S²⁻, NH₄⁺, NO₃⁻, CO₃²⁻, HCO₃⁻.
  5. Identify allotropes of oxygen and sulphur.
  6. Determine the significance of ozone in the atmosphere.
  7. Classify oxides based on their properties.
  8. Predict reagents for preparation, properties, and uses of SO₂ and H₂S.
  9. Specify the preparation, properties, and uses of H₂SO₃ and H₂SO₄.
  10. Specify laboratory and industrial preparation of NH₃ and its applications.
  11. Identify reagents for the preparation of HNO₃, its properties, and uses.
  12. Specify the properties of nitrogen oxides (N₂O, NO, NO₂).

15. Non-Metals and Their Compounds

(e) The Nitrogen Cycle

Carbon and Its Compounds

  1. Allotropes of Carbon: Properties and uses.
  2. Carbon(IV) Oxide (CO₂):
    • Laboratory preparation
    • Properties and uses
    • Action of heat on trioxocarbonate(IV) salts
    • Test for CO₂
  3. Carbon(II) Oxide (CO):
    • Laboratory preparation
    • Properties, including its effect on blood
    • Sources (charcoal, fire, exhaust fumes)
  4. Coal:
    • Types and characteristics
    • Products from destructive distillation of wood and coal
  5. Coke:
    • Gasification and uses
  6. Synthesis Gas:
    • Manufacture and applications

16. Metals and Their Compounds

  1. General Properties of Metals
  2. Alkali Metals (e.g., Sodium):
    • Sodium Hydroxide (NaOH):
      • Production via electrolysis of brine
      • Reactions with aluminum, zinc, and lead ions
      • Uses, including precipitation of metallic hydroxides
    • Sodium Trioxocarbonate(IV) and Sodium Hydrogen Trioxocarbonate(IV):
      • Production via Solvay process
      • Properties and applications, e.g., glass manufacturing
    • Sodium Chloride (NaCl):
      • Occurrence in seawater
      • Uses and economic significance of seawater
  3. Alkaline Earth Metals (e.g., Calcium):
    • Calcium Oxide (CaO), Calcium Hydroxide (Ca(OH)₂), and Calcium Trioxocarbonate(IV) (CaCO₃)
    • Properties and uses
    • Preparation of calcium oxide from sea shells
    • Chemical composition of cement and setting of mortar
    • Test for Ca²⁺

Objectives:

  • Identify the general properties of metals
  • Determine suitable methods of extraction
  • Compare chemical reactivities and properties of metals and their compounds
  • Specify industrial and laboratory uses
  • Identify specific tests for metallic ions

17. Organic Chemistry

(a) Alkanoates

  • Formation from alkanoic acids and alkanols
  • Fats and oils as alkanoates
  • Saponification: Production of soap and margarine
  • Differences between detergents and soaps

(b) Amines (Alkanamines)

  • Classification: Primary, secondary, and tertiary

(c) Carbohydrates

  • Classification: Monosaccharides, disaccharides, and polysaccharides
  • Composition and chemical tests for simple sugars
  • Hydrolysis of complex sugars (e.g., cellulose from cotton, starch from cassava)
  • Uses of sugars and starch in alcohol production, pharmaceuticals, and textiles

(d) Proteins

  • Primary structures, hydrolysis, and chemical tests (Biuret, Ninhydrin, Xanthoproteic, Millon’s tests)
  • Enzymes and their functions

(e) Polymers

  • Natural and synthetic rubber
  • Addition and condensation polymerization
  • Preparation, examples, and applications
  • Differentiation between thermoplastic and thermosetting plastics

Objectives:

  • Identify natural sources and methods of production for alkanoates, amines, and carbohydrates
  • Compare the different classes of organic compounds
  • Determine the products of hydrolysis and dehydration reactions
  • Differentiate between soaps and detergents
  • Identify protein structures and enzymatic functions
  • Classify polymers and distinguish between thermoplastics and thermosetting plastics

18. Chemistry and Industry

  • Types of chemical industries
  • Raw materials and relevance
  • Biotechnology in chemical industries

Objectives:

  • Classify chemical industries based on products
  • Identify raw materials for various industries
  • Differentiate between fine and heavy chemicals
  • Relate industrial processes to biotechnology and their societal relevance.

SEE ALSO: 

Recommended Textbooks for Chemistry

1. General Chemistry Textbooks

  • Ababio, O. Y. (2009). New School Chemistry for Senior Secondary Schools (4th Edition). Onitsha: Africana FIRST Publishers Limited.
  • Ojokuku, G. O. (2012). Understanding Chemistry for Schools and Colleges (Revised Edition). Zaria: Press-On Chemresources.
  • Odesina, I. A. (2008). Essential Chemistry for Senior Secondary Schools (2nd Edition). Lagos: Tonad Publishers Limited.

2. Senior Secondary Chemistry Series

  • Bajah, S. T., Teibo, B. O., Onwu, G., & Obikwere, A. (1999). Senior Secondary Chemistry (Book 1). Lagos: Longman.
  • Bajah, S. T., Teibo, B. O., Onwu, G., & Obikwere, A. (2000). Senior Secondary Chemistry (Books 2 & 3). Lagos: Longman.

3. Examination Preparation Guides

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

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