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Jamb 2018 Chemistry Syllabus and Recommended textbooks - solutionfans.com

The aim of this 2018/2019 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.

(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.

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.

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.

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.

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.

(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.

(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.

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.

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 S θ 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 -T Δ Sθ

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.

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.

(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

(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.

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.

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.

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