1. Separation of Mixtures and Purification of Chemical Substance
(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.
2. Chemical
Combination
Stoichiometry,
laws of definite and multiple proportions, the 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.
3. Kinetic
Theory of Matter & Gas Law
(a) An outline
of the kinetic theory of matter, melting, vaporization 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
4. Atomic
Structure & 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 a 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)
(e) Nuclear
Chemistry:
(i)
Radioactivity (elementary treatment only)
(ii) 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 gas.
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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
(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.
9. Acids, Base
& 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.
10. 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.
11. 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.
12. Energy
Charge
(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. 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
(i) powdered
form
(ii) lumps of
the same mass.
(iv) 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
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. 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. 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 from 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 synthesis gas and uses.
16. 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 A13+
(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).
17. Organic
Compounds
An introduction
to the tetravalency of carbon, the general formula, IUPAC nomenclature and the
determination of
the empirical
formula of each class of the organic compounds mentioned below.
(a) Aliphatic
hydrocarbons
(i) Alkanes
Homologous series in relation to physical properties, substitution reaction and
a few examples and uses of halogenated products. Isomerism: structural only
(examples on isomerism should not go beyond six carbon atoms). Petroleum:
composition, fractional distillation and major products; cracking and
reforming, Petrochemicals – starting materials of organic syntheses, quality of
petrol and meaning of octane number
(ii) Alkenes
Isomerism: structural and geometric isomerism, additional and polymerization
reactions, polythene
and synthetic
rubber as examples of products of polymerization and its use in vulcanization.
(iii) Alkynes
Ethyne – production from action of water on carbides, simple reactions and
properties of ethyne.
(b) Aromatic
hydrocarbons e.g. benzene – structure, properties and uses.
(c) Alkanols
Primary, secondary, tertiary – production of ethanol by fermentation and from
petroleum by-products. Local examples of fermentation and distillation, e.g.
gin from palm wine and other local sources and glycerol as a polyhydric
alkanol. Reactions of OH group – oxidation as a distinguishing test among
primary, secondary and tertiary alkanols (Lucas test)
(d) Alkanals and
alkanones. Chemical test to distinguish between alkanals and alkanones.
(e) Alkanoic
acids. Chemical reactions; neutralization and esterification, ethanedioic
(oxalic) acid as an example of a dicarboxylic acid and benzene carboxylic acid
as an example of an aromatic acid.
(f) Alkanoates
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.
18. Chemistry
and Industry
Chemical
industries: Types, raw materials, and relevance; Biotechnology.
Jamb Chemistry Syllabus Recommended Textbook
Ababio, O.Y.
(2005). New School Chemistry for Senior Secondary Schools, (Third Edition),
Onitsha:
Africana FIRST Publishers Limited
Bajah, S.T.
Teibo, B.O., Onwu, G and Obikwere, A. (1999). Senior Secondary Chemistry,
Book 1, Lagos:
Longman
Bajah, S.T.,
Teibo, B.O., Onwu, G and Obikwere, A. (2000). Senior Secondary Chemistry,
Books 2 and 3,
Lagos: Longman
Ohia, G.N.C.,
Adewoyin, F.A. and Akpan, B.B. (1997). Exam Focus Chemistry for WASSCE
& JME:
Ibadan: University Press Plc
STAN (1987).
Chemistry for Senior Secondary Schools, Ibadan: Heinemann
Sylvester: O.O.
(2004). A Comprehensive Practical Chemistry for Senior Secondary Schools,
Ibadan: Evans
Uche, I.O.,
Adenuga, I.J. and Iwuagwu, S.L. (2003). Countdown to WASSCE/SSCE, NECO, JME
Chemistry,
Ibadan: Evans