Chemistry Syllabus from JAMB

(a) Pure and impure substances
(b) Boiling and melting points.
(c) Elements, compounds and mixtures
(d) Chemical and physical changes.
(e) Separation processes:
evaporation, simple and fractional distillation, sublimation, filtration, crystallization, paper and column chromatography, simple and fractional crystallization, magnetization, decantation.

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.

(a) An outline of the kinetic theory of matter;
(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, Graham and Dalton (law of partial pressure); combined gas law, 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.

(a) (i)The concept of atoms, molecules and ions, the works of Dalton, Millikan, Rutherford, Moseley, 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 to 20.
(iii) 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: 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, O2, C12,HCl and CO2), non-linear (H2O) and tetrahedral; (CH4) and pyramidal (NH3).
(e) Nuclear Chemistry:
(i) Radioactivity – Types and properties of
radiations
(ii) Nuclear reactions. Simple equations,
uses and applications of natural and
artificial radioactivity.

(a) The natural gaseous constituents and their proportion in the air.
– nitrogen, oxygen, water vapour, carbon (IV) oxide and the noble gases (argon and neon).
(b) Air as a mixture and some uses of the noble gas.

(a) Water as a product of the combustion of hydrogen and its composition by volume.
(b) Water as a solvent, atmospheric gases dissolved in water and their biological significance.
(c) Hard and soft water:
Temporary and permanent
hardness and methods of softening
hard water.
(d) Treatment of water for town supply.
(e) Water of crystallization, efflorescence,
deliquescence and hyg
roscopy. 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) False solution (Suspensions and colloids):
Properties and examples.
Harmattan haze and water paints as examples
of suspensions and fog, milk, aerosol spray,
emulsion paints and rubber solution as
examples of colloids.

(a) Sources and effects of pollutants.
(b) Air pollution:
Examples of air pollutants such as
H2S, CO, SO2, oxides of nitrogen,
chlorofluorocarbons and dust.
(c) Water pollution
Sewage and oil pollution should be
known.
(d) Soil pollution:
Oil spillage, Biodegradable and
non-biodegradable pollutants.

(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 and
amount of ions present.
(c) pH and pOH scale; Simple calculations
(d) Acid/base titrations.
(e) Hydrolysis of salts: Principle
Simple examples such as
NH4Cl, AlCl3, Na2CO3 and CH3COONa

(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.
(e) IUPAC nomenclature of inorganic compounds using oxidation number.
(f) Tests for oxidizing and reducing agents.

(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:
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 as an electrolytic process,
cathodic protection of metals,
painting, electroplating and coating
with grease or oil as ways of
preventing iron from corrosion.

(a) Energy changes([Math Processing Error]H) accompanying physical
and chemical changes:
dissolution of substances in/or
reaction with water e.g. Na, NaOH,
K, NH4Cl. Endothermic (+[Math Processing Error]H) and exothermic (-[Math Processing Error]H) reactions.
(b) Entropy as an order-disorder
phenomenon: simple illustrations
like mixing of gases and dissolution
of salts.
(c) Spontaneity of reactions:
[Math Processing Error]G[Math Processing Error]= 0 as a criterion for equilibrium, [Math Processing Error]G
greater or less than zero as a criterion for
non-spontaneity or spontaneity respectively.

(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 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
(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

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.

(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 agent and uses. Test for SO42-.
Hydrogen sulphide: Preparation and properties as a weak acid, reducing agent and precipitating agent. Test for S2-
(d) Nitrogen:
(i) Laboratory preparation
(ii) Production from liquid air
(iii) Ammonia:
Laboratory and industrial
preparations (Haber Process only),
properties and uses, ammonium salts
and their uses, oxidation of
ammonia to nitrogen (IV)
oxide and trioxonitrate (V)
acid.
Test for NH4+
(iv) Trioxonitrate (V) acid:
Laboratory preparation
f
rom ammonia;
properties and uses. Trioxonitrate (V) salt-
action of heat and uses. Test for NO3-
(v) Oxides of nitrogen:
Properties.
The nitrogen cycle.
(e) Carbon:
(i) Allotropes: Uses and
properties
(ii) Carbon(IV) oxide-
Laboratory preparation, properties
and uses. Action of heat on
trioxocarbonate (IV) salts and test for
CO32-
(iii) Carbon(II) oxide:
Laboratory preparation, properties
including its effect on blood;
sources of carbon (II) oxide to
include charcoal, fire and exhaust
fumes.
(iv) Coal: Different types, products
obtained from destructive
distillation of wood and coal.
(v) Coke: Gasification and uses.
Manufacture of synthetic gas and
uses.

Formation from alkanoic acids and
alkanols – fats and oils as alkanoates.
Saponification:
Production of soap and margarine from
alkanoates and distinction between
detergents and soaps.
(g) Amines (Alkanamines) Primary, Secondary,
and tertiary
(h) Carbohydrates
Classification – mono-, di- and polysaccharides; composition, chemical tests for simple sugars and reaction with concentrated tetraoxosulphate (VI) acid. Hydrolysis of complex sugars e.g. cellulose from cotton and starch from cassava, the uses of sugar and starch in the production of alcoholic beverages, pharmaceuticals and textiles.
(i) Proteins:
Primary structures, hydrolysis and tests (Ninhydrin, Biuret, Millon’s and xanthoproteic)
Enzymes and their functions.
(j) Polymers:
Natural and synthetic rubber; addition and condensation polymerization.
– Methods of preparation, examples and uses.
Thermoplastic and thermosetting plastics.

Chemical industries: Types, raw materials and
relevancies; Biotechnology.