Chemistry Syllabus from
JAMB
The aim of this 2016/2017 Unified Tertiary
Matriculation Examination (UTME) syllabus in
Chemistry is to prepare the candidates for the
Board's examination. It is designed to test their
achievement of the course objectives, which are to:
(i) understand the basic principles and concepts in
chemistry;
(ii) interpret scientific data relating to chemistry;
(iii) deduce the relationships between chemistry
and other sciences;
(iv) apply the knowledge of chemistry to industry
and everyday life.
TOPICS/CONTENTS/NOTES OBJECTIVES
1. Separation of mixtures
and purification of chemical
substances
(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.
Candidates should be able
to:
(i) distinguish between
pure and impure
substances;
(ii) use boiling and melting
points as criteria for purity
of chemical substances;
(iii) distinguish between
elements, compounds and
mixture;
(iv) differentiate between
chemical and physical
changes;
(v) identify the properties of
the components of a
mixture;
(vi) specify the principle
involved in each separation
method.
(vii) apply the basic
principle of separation
processes in everyday life.
2. 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 C=12, the
mole concept and
Avogadro's number.
Candidates should be able
to:
(i) perform simple
calculations involving
formulae, equations/
chemical composition and
the mole concept;
(ii) deduce the chemical
laws from given
expressions/statements/
data;
(iii) interpret graphical
representations related
to these laws;
(iv) deduce the
stoichiometry of chemical
reactions.
3. Kinetic theory of matter
and Gas Laws
(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.
Candidates should be able
to:
(i) apply the theory to
distinguish between solids,
liquids and gases;
(ii) deduce reasons for
change of state;
(iii) draw inferences based
on molecular motion;
(iv) deduce gas laws from
given expressions/
statements;
(v) interpret graphical
representations related to
these laws;
(vi) perform simple
calculations based on
these laws, equations and
relationships
4. Atomic structure and
bonding
(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) ] , [Fe
(CN) ] , [Cu(NH ) ]
and [Ag(NH ) ] ; van der
Waals' forces should be
mentioned as a special
type of bonding forces.
(d) Shapes of simple
molecules: linear ((H , O ,
C ,HCl and CO ), non-
linear (H O) and
tetrahedral; (CH ) and
pyramidal (NH ).
(e) Nuclear Chemistry:
(i) Radioactivity - Types
and properties of
radiations
(ii) Nuclear reactions.
Simple equations,
uses and applications of
natural and
artificial radioactivity.
Candidates should be able
to:
(i) distinguish between
atoms, molecules and ions;
(ii) identify the
contributions of these
scientists to
the development of the
atomic structure;
(iii) deduce the number of
protons, neutrons and
electrons from atomic and
mass numbers of
an atom;
(iv) apply the rules guiding
the arrangement of
electrons in an atom;
(v) identity common
elements exhibiting
isotopy;
(vi) relate isotopy to mass
number;
(vii) perform simple
calculations relating to
isotopy;
(viii) differentiate between
the shapes of the orbitals;
(ix) determine the number
of electrons in s and
p atomic orbitals;
(x) relate atomic number to
the position of an
element on the periodic
table;
(xi) relate properties of
groups of elements on the
periodic table;
(xii) identify reasons for
variation in properties
across the period and
down the groups.
(xiii) differentiate between
the different types
of bonding.
(xiv) deduce bond types
based on electron
configurations;
(xv) relate the nature of
bonding to properties
of compounds;
(xvi) differentiate between
the various shapes
of molecules
xvii) distinguish between
ordinary chemical
reaction and nuclear
reaction;
(xviii) differentiate between
natural and
artificial radioactivity;
(xix) compare the
properties of the different
types of nuclear radiations;
(xx) compute simple
calculations on the
half-life of a radioactive
material;
(xxi) balance simple
nuclear equation;
(xxii) identify the various
applications of
radioactivity.
5. Air
(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.
Candidates should be able
to:
(i) deduce reason (s) for
the existence of
air as a mixture;
(ii) identify the principle
involved in the
separation of air
components;
(iii) deduce reasons for the
variation in the
composition of air in the
environment;
(iv) specify the uses of
some of the
constituents of air.
6. Water
(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
hygroscopy. Examples of
the substances exhibiting
these properties and their
uses.
Candidates should be able
to:
(i) identify the various uses
of water;
(ii) identity the effects of
dissolved atmospheric
gases in water;
(iii) distinguish between the
properties of hard and
soft water;
(iv) determine the causes
of hardness;
(v) identify methods of
removal of hardness;
(vi) describe the processes
involved in the
treatment of water for town
supply;
(vii) distinguish between
these phenomena;
(viii) identify the various
compounds that exhibit
these phenomena.
7. Solubility
(a) Unsaturated, saturated
and supersaturated
solutions. Solubility curves
and simple deductions
from them, (solubility
defined in terms of mole
per dm ) 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.
Candidates should be able
to:
(i) distinguish between the
different types of
solutions;
(ii) interpret solubility
curves;
(iii) calculate the amount of
solute that can
dissolve in a given amount
of solvent at a
given temperature;
(iv) deduce that solubility
is temperature-dependent;
(v) relate nature of solvents
to their uses;
(vi) differentiate among
true solution,
suspension and colloids;
(vii) compare the properties
of a true solution
and a �false' solution.
(viii) provide typical
examples of suspensions
and colloids.
8. Environmental Pollution
(a) Sources and effects of
pollutants.
(b) Air pollution:
Examples of air pollutants
such as
H S, CO, SO , 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.
Candidates should be able
to:
(i) identify the different
types of pollution and
pollutants;
(ii) specify different
sources of pollutants
(iii) classify pollutants as
biodegradable and
non-biodegradable;
(iv) specify the effects of
pollution on the
environment;
(v) identify measures for
control of
environmental pollution.
9. Acids, bases and salts
(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
NH Cl, AlCl , Na CO and
CH COONa
Candidates should be able
to:
(i) distinguish between the
properties of
acids and bases;
(ii) identify the different
types of acids
and bases;
(iii) determine the basicity
of acids;
(iv) differentiate between
acidity and
alkalinity using acid/base
indicators;
(v) identify the various
methods of
preparation of salts;
(vi) classify different types
of salts;
(vii) relate degree of
dissociation to strength
of acids and bases;
(viii) relate degree of
dissociation to
conductance;
(ix) perform simple
calculations on pH and
pOH;
(x) identify the appropriate
acid-base
indicator;
(xi) interpret graphical
representation of
titration curves;
(xii) perform simple
calculations based on
the mole concept;
(xiii) balance equations for
the hydrolysis
of salts;
(xiv) deduce the properties
(acidic, basic,
neutral) of the resultant
solution.
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.
(e) IUPAC nomenclature of
inorganic compounds
using oxidation number.
(f) Tests for oxidizing and
reducing agents.
Candidates should be able
to:
(i) identify the various
forms of expressing
oxidation and reduction;
(ii) classify chemical
reactions in terms of
oxidation or reduction;
(iii) balance redox reaction
equations;
(iv) deduce the oxidation
number of chemical
species;
(v) compute the number of
electron transfer
in redox reactions;
(vi) identify the name of
redox species in a reaction
(vii) distinguish between
oxidizing and reducing
agents in redox reactions.
(viii) apply oxidation
number in naming
inorganic compounds
(ix) relate reagents to their
oxidizing and reducing
abilities.
11. Electrolysis
(a) Electrolytes and non-
electrolytes.
Faraday's laws of
electrolysis.
(b) (i) Electrolysis of dilute
H SO4, aqueous
CuSO , CuC 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, O , C 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.
Candidates should be able
to:
(i) distinguish between
electrolytes and non-
electrolytes;
(ii) perform calculations
based on faraday as a
mole of electrons.
(iii) identify suitable
electrodes for different
electrolytes.
(iv) specify the chemical
reactions at the
electrodes;
(v) determine the products
at the electrodes;
(vi) identify the factors that
affect the products
of electrolysis;
(vii) specify the different
areas of application of
electrolysis;
(viii) identify the various
electrochemical cells;
(ix) calculate electrode
potentials using half-
cell reaction equations;
(x) determine the different
areas of
application of electrolytic
processes;
(xi) identify methods used
in protecting metals.
12. Energy changes
(a) Energy changes( Δ H)
accompanying physical
and chemical changes:
dissolution of substances
in/or
reaction with water e.g.
Na, NaOH,
K, NH Cl. Endothermic (+ Δ
H) and exothermic (- Δ H)
reactions.
(b) Entropy as an order-
disorder
phenomenon: simple
illustrations
like mixing of gases and
dissolution
of salts.
(c) Spontaneity of
reactions:
Δ G θ = 0 as a criterion for
equilibrium, Δ G
greater or less than zero
as a criterion for
non-spontaneity or
spontaneity respectively.
Candidates should be able
to:
(i) determine the types of
heat changes
(Δ H) in physical and
chemical processes;
(ii) interpret graphical
representations of heat
changes;
(iii) relate the physical state
of a substance
to the degree of
orderliness;
(iv) determine the
conditions for spontaneity
of a reaction ;
(v) relate Δ H θ , Δ Sθ and Δ
G θ as the driving
forces for chemical
reactions;
(vi) solve simple problems
based on the
relationships Δ G θ = Δ H θ -
TΔ S θ
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 HCl and
Na S O or Mg and HCl
(ii) Concentration e.g. the
reaction between HCl and
Na S O , 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 H O or KClO in the
presence or absence of
MnO
(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
Candidates should be able
to:
(i) identify the factors that
affect the rates of a
chemical reaction;
(ii) determine the effects of
temperature on
the rate of reactions;
(iii) examine the effect of
concentration/pressure on
the rate of a chemical
reaction;
(iv) describe how the rate
of a chemical reaction is
affected by surface area;
(v) determine the types of
catalysts suitable for
different reactions and their
effects;
(vi) determine ways of
moderating these effects in
chemical reactions.
(vii) interpret reaction rate
curves;
(viii) solve simple
problems on the rate of
reactions;
(ix) relate the rate of
reaction to the kinetic
theory of matter.
(x) examine the
significance of activation
energy to chemical
reactions.
(xi) deduce the value of
activation energy (Ea) from
reaction rate curves.
14. Chemical equilibra
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 N O 2NO .
No calculation will be
required.
Candidates should be able
to:
(i) identify the factors that
affects the position
of equilibrium of a
chemical reaction;
(ii) predict the effects of
each factor on the position
of equilibrium;
(iii) determine the effects of
these factors on
equilibrium constant.
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 SO 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 SO .
Hydrogen sulphide:
Preparation and properties
as a weak acid, reducing
agent and precipitating
agent. Test for S
(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 NH
(iv) Trioxonitrate (V) acid:
Laboratory preparation
from ammonia;
properties and uses.
Trioxonitrate (V) salt-
action of heat and uses.
Test for NO
(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
CO
(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.
Candidates should be able
to:
(i) predict reagents for the
laboratory and
industrial preparation of
these gases and
their compounds.
(ii) identify the properties of
the gases and their
compounds.
(iii) compare the properties
of these gases and
their compounds.
(iv) specify the uses of
each gas and its
compounds;
(v) determine the specific
test for each gas and its
compounds.
(vi) determine specific
tests for Cl , SO ,
SO ,
S , NH , NO , CO ,
HCO
(vii) predict the reagents
for preparation,
properties and uses HCl(g)
and HCl(aq);
(viii) identify the allotropes
of oxygen;
(ix) determine the
significance of ozone to
our environment.
(x) classify the oxides of
oxygen and their
properties
(xi) identify the allotropes
of sulphur and their
uses;
(xii) predict the reagents
for preparation, properties
and uses of SO and H S;
(xiii) specify the
preparations of H SO and
H SO ,
their properties and uses.
(xiv) specify the laboratory
and industrial
preparation of NH ;
(xv) identify the properties
and uses of NH ;
(xvi) identify reagents for
the laboratory
preparation of HNO , its
properties and
uses;
(xvii) specify the properties
of N O, NO, NO gases.
(xviii) examine the
relevance of nitrogen cycle
to the environment.
(xix) identify allotropes of
carbon;
(xx) predict reagents for
the laboratory
preparation of CO ;
(xxi) specify the properties
of CO and its
uses;
(xxii) determine the
reagents for the
laboratory preparation of
CO;
(xxiii) predict the effects of
CO on human;
(xxiv) identify the different
forms of coal:
(xxv) determine their uses;
(xxvi) specify the products
of the destructive
distillation of wood and
coal;
(xxvii) specify the uses of
coke and synthetic gas.
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.
Na CO in the manufacture
of glass.
(iii) Sodium chloride: its
occurrence in
sea water and uses, the
economic
importance of sea water
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 sea shells, the
chemical composition of
cement
and the setting of mortar.
Test for Ca .
(d) Aluminium
Purification of bauxite,
electrolytic
extraction, properties and
uses of aluminium and its
compounds. Test for A1
(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 Fe and Fe
(h) Copper
Extraction from sulphide
and oxide
ores, properties and uses
of copper.
Preparation and uses of
copper( II )
tetraoxosulphate(VI). Test
for Cu
(i) Alloy
Steel, stainless steel,
brass, bronze, type- metal,
duralumin, soft solder,
permallory and alnico
(constituents and
uses only).
Candidates should be able
to:
(i) specify the general
properties of metals;
(ii) determine the method
of extraction suitable
for each metal;
(iii) relate the methods of
extraction to the
properties for the metals;
(iv) compare the chemical
reactivities of the metals;
(v) specify the uses of the
metals;
(vi) determine specific test
for metallic ions;
(vii) determine the process
for the production
of the compounds of these
metals;
(viii) compare the chemical
reactivities of the
compounds;
(ix) specify the uses of
these compounds;
(x) specify the chemical
composition of cement.
(xi) describe the method of
purification of bauxite;
(xii) specify the ores of tin;
(xiii) relate the method of
extraction to its properties;
(xiv) specify the uses of
tin;
(xv) identify the general
properties of the first
transition metals;
(xvi) deduce reasons for
the specific properties
of the transition metals;
(xvii) determine the IUPAC
names of simple
transition metal complexes
(xviii) determine the
suitable method of
extraction of iron;
(xix) specify the properties
and uses of iron;
(xx) identify the different
forms of iron, their
compositions, properties
and uses.
(xxi) identify the
appropriate method of
extraction of copper from
its compounds;
(xxii) relate the properties
of copper and its
compound to their uses.
(xxiii) specify the method
for the preparation of
CuSO ;
(xxiv) specify the
constituents and uses of
the
various alloys mentioned.
(xxv) compare the
properties and uses of
alloys
to pure metals.
17. Organic Compounds
An introduction to the
tetravalency of
carbon, the general
formula, IUPAC
nomenclature and the
determination of
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.
Candidates should be able
to:
(i) derive the name of
organic compounds from
their general formulae;
(ii) relate the name of a
compound to its structure
(iii) relate the tetravalency
of carbon to its ability
to form chains of
compound (catenation);
(iv) classify compounds
according to their
functional groups;
(v) derive empirical formula
and molecular
formula, from given data;
(vi) relate structure/
functional groups to
specific
properties;
(vii) derive various
isomeric forms from a
given
formula;
(viii) distinguish between
the different types of
isomerism;
(ix) classify the various
types of hydrocarbons;
(x) distinguish each class
of hydrocarbons by their
properties;
(xi) specify the uses of
various hydrocarbons;
(xii) identify crude oil as a
complex mixture
of hydrocarbons;
(xiii) relate the fractions of
hydrocarbons to their
properties and uses;
(xiv) relate transformation
processes to quality
improvement of the
fractions;
(xv) distinguish between
various polymerization
processes;
(xvi) specify the process
involved in vulcanization;
(xvii) specify chemical test
for terminal alkynes
(xviii) distinguish between
aliphatic and aromatic
hydrocarbons;
(xix) relate the properties of
benzene to its structure
(xx) compare the various
classes of alkanols;
(xxi) determine the
processes involved in
ethanol
production;
(xxii) examine the
importance of ethanol as
an
alternative energy provider;
(xxiii) distinguish the
various classes of alkanols;
(xxiv) differentiate between
alkanals and alkanones;
(xxv) compare the various
types of alkanoic acids;
(xxvi) identify natural
sources of alkanoates;
(xxvii) specify the methods
for the production of
soap, detergent and
margarine.
(xxviii) distinguish between
detergent and soap;
(xxix) compare the various
classes of alkanamine;
(xxx) identify the natural
sources of
carbohydrates;
(xxxi) compare the various
classes of
carbohydrates;
(xxxii) infer the products of
hydrolysis and
dehydration of
carbohydrates;
(xxxiii) determine the uses
of carbohydrates;
(xxxiv) specify the tests for
simple sugars;
(xxxv) identify the basic
structure of proteins;
(xxxvi) specify the methods
and products of
hydrolysis;
(xxxvii) specify the various
tests for proteins;
(xxxviii) distinguish
between natural and
synthetic
polymers;
(xxxix) differentiate
between addition and
condensation
polymerization processes;
(xl) classify natural and
commercial polymers
and their uses;
(xli) distinguish between
thermoplastics and
thermosetting plastics.
18. Chemistry and Industry
Chemical industries: Types,
raw materials and
relevancies; Biotechnology.
Candidates should be able
to :
(i) classify chemical
industries interms of
products;
(ii) identify raw materials
for each industry;
(iii) distinguish between
fine and heavy
chemicals;
(iv) enumerate the
relevance of each of these
industries;
(v) relate industrial
processes to
biotechnology.
RECOMMENDED TEXTS
1. New School Chemistry for Senior Secondary
Schools, Ababio, O. Y. (2009), (Fourth edition),
Onitsha: Africana FIRST Publishers Limited.
2. Senior Secondary Chemistry, Bajah, S.T.; Teibo,
B. O., Onwu, G.; and Obikwere, A. Book 1 (1999),
Books 2 and 3 (2000). Lagos: Longman.
3. Understanding Chemistry for Schools and
Colleges, Ojokuku, G. O. (2012, Revised Edition),
Zaria: Press-On Chemresources.
4. Essential: Chemistry for Senior Secondary
Schools, (2008), 2nd Edition, I. A. Odesina, Lagos:
Tonad Publishers Limited.
5. Countdown to WASSCE/SSCE, NECO, JME
Chemistry, Uche, I. O.; Adenuga, I. J. and
Iwuagwu, S. L. (2003). Ibadan: Evans.
