SYLLABUS

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separation of mixtures and purification of chemical substance
chemical combination
kinetic theory of matter and gas laws
Atomic structure and bonding
Air
Water
Solubility
Environmental pollution
Acids,bases and salts
Oxidation and reduction
Energy changes
Chemical equilibra
Metals and their compounds
Organic compounds
Rates of chemical reaction
Non-metal and their compounds
Electrolysis


Articulate nature of matter
1. The concept of atoms and molecule
2. The constituents o the atom; protons, neutrons and electrons
3. Chemical symbols of the first 20 elements and other common elements
4. Atomic number, mass number and isotopes
5. Relative molecular mass, Mole, Molar Mass and Valency
6. Chemical formula; Empirical and molecular
7. Chemical equations-Balancing equations
8. Laws of Chemical Combination:
i. Law of conversation of matter
ii. Law of constant composition
iii. Law of multiple proportions
Atomic Structure 1. Dalton’s atomic theory
2. Arrangement of electrons in the Orbitals: s,p,d and f.
3. Shapes of S and P orbitals.
4. Rules guiding the filling of electrons e.g Aufbau’s Principles, Hund’s rule
of maximum multiplicity and Pauli’s exclusion principle.
5. Electronic configuration of elements H to Zn.
6. Quantum mechanics: reference to the works of Rutherford, Millikan,
Thompson and Bohr.
7. Dual nature of light as a particle and wave.
Chemical combination Types of bonds
1. Electrovalency; experiments to investigate the properties of ionic
compounds of the first twenty elements
2. Covalency
3. Co-ordinate covalency; Complex ion formation such as Fe(CN)63-, Fe
(CN)64-, Cu (NH3)42+ and Ag (NH3)2+
4. Hydrogen bond: effect on molecule where it is found, eg H20
5. Metallic bond; delocalized electrons, effects of this bond in soft and hard
metals.
6. van-der Waals forces; used in explaining intermolecular attraction in
Covalent compounds.
Periodic Table of Element - The Periodic Table: Periodic law
- Group – column of elements
- Period – row of elements
- Periodic properties such as Ionisation potential, Ionisation Energy,
Electronegativity, Electron Affinity. (properties that increase across a
period)
- Atomic size, ionic size. Their trends should be treated both down the
group and across the period.
- Periodic gradation of properties of elements in group seven (halogens)
using their physical state, melting and boiling points, redox properties of
the elements, displacement of one halogen by another.
- Reactions of chlorine with water and alkali, demonstration of variable
oxidation states.
- Elements of the first transition series from Scandium to Zinc. Treatment of their electronic configuration, physical and chemical properties, physical states, metallic properties and magnetic properties, variable oxidation states, formation of coloured compounds, complex ion formation and catalytic abilities.
Gaseous state and Gas Laws 1. The kinetic theory and its application to gaseous postulates only;
Brownian movement, inter-conversions of states
2. Gas laws
- Boyle’s law
- Charles’ law
- General gas law; ideal gas equation PV=nRT
- Gay Lussac’s law
- Avogadro’s law
- Graham’s law
- Dalton’s law
3. Molar volume of gases
4. Avogadro’s number and the mole concept
5. Calculations involving all the above mentioned gas laws.
Acids, Bases and Salts 1. Characteristics, preparation, reactions and uses of acids, bases and salts
2. Common acids and bases, relative acidity and alkalinity, pH value.
3. Weak acids and weak bases; behavior in water as example of equilibrium
system.
Strong and weak acids-Difference between strong and weak acids; Dilute
and concentrated acids
4. Theory of indicators-definition; properties and even their choice for
different reactions.
5. pH scale; (as a measure of acidity and alkalinity)
6. Knowledge of Kw, pKw in terms of pOH and pH. Also simple calculations
based on them.
7. Theory on substances-Effloresence, Deliquescence and Hygroscopy
8. Heat of neutralization
Acid – Base Titration 1. The use of standard solutions of acids and alkalis and their indicators for
Titration
2. Indicators as weak organic acids or bases.
3. Titrations involving strong acids versus strong bases strong acids versus
weak bases, weak acids versus strong bases using appropriate indicators.
4. Brief discussion on buffer solutions
5. Applications in quantitative determinations e.g. molar
masses/identification of acids and bases, concentrations, percentage
purity, water of crystallization and composition, solubility of acids and
bases.
Quantitative Aspect of Chemical Reactions 1. Mass – Volume Relationship
- Uses in determining the stoichiometry of precipitation reactions, reactions involving measurement of gaseous volume, analysis of chlorides, synthesis and reduction of metallic oxides and displacement of metal ions.
2. Mass – Mass Relationship
- Uses in determining the stochiometry of precipitation reactions,
decomposition reactions, reactions that involve depositions of metals,
reduction and oxidation reactions.
3. Volume – Volume Relationship
- Reactions involving gases only. The application of molar volume is very
necessary here.

Types of Reactions 1. Combination
2. Decomposition
3. Displacement
4. Double decomposition
5. Catalytic
i. characteristics of a catalyst
ii. types of catalyst
6. Reversible Reactions
7. Thermal dissociation
8. Redox reactions
i. Oxidation and Reduction
Definitions, in terms addition and removal of oxygen and hydrogen;
electron loss and gain, changes in oxidation state.
ii. Oxidation number and use in IUPAC Nomenclature of compound.
iii. Oxidising and Reducing agents in terms of:
- addition and removal of oxygen and hydrogen
- loss and gain of electrons
- change in oxidation number/state
- state which one is being reduced and which one is oxidized.
iv. Balancing redox reactions by ion, electron or change in oxidation state
v. half reactions and overall reactions using IUPAC
vi. Test for Oxidants and Reductants
vii. Corrosion of Metals
- treated as a redox process (equations essential)
- rusting of iron and its economic importance
- Prevention: galvanizing, electroplating, and non-redox methods.
Electrochemical Series and Electrolysis 1. Electrochemical cells.
i. Standard Electrode Potential (Standard Hydrogen Electrode)
Only metal/metal ion systems should be used
ii. E.M.F. of cells.
- Meaning, magnitude and significance of e.m.f.
- Application of e.m.f. in Secondary and Primary cells, Daniel cells,
lead battery cells, dry cells, fuel cells, and their use of generator.
2. Electrolysis
i. Effect of electricity on matter
ii. Electrolytes and non-electrolytes
iii. Preferential discharge of ions during electrolysis (Limit electrolytes to
molten NaCI/PbBr2, concentrated NaCI solution, CuSO4 (aq), dil
H2SO4, dil NaOH).
iv. Faraday’s Laws: Treat simple calculations involved. (mass deposited,
moles passed, volume of gas evolved, charges involved).
v. Practical applications: Electroplating, extraction of Aluminium.
vi. Uses of electrolysis: extraction, purification and electroplating.
Rates of Chemical Reactions and Energy Effects 1. Factors affecting Rates of Chemical Reactions
- nature of reactants
- concentration (uses of collision theory to explain)
- reaction mechanisms
- temperature (use of collision theory as basis)
- catalyst
- pressure instead of concentration for gases
2. Theory of reaction rates
- Collision theory and activation energy theory to be treated
quantitatively
- Effective collision which give rise to reactions.
- Activation energy
- Factors affecting collisions: temperature and concentration
- Energy profile showing activation enerby
3. Energy and reaction rates.
- reaction profile
- activation energy
- catalysed and uncatalysed reactions
4. Exothermic and endothermic reactions:
- Enthalpy: H, Entropy change S, Free energy change G.
- Relationship among the three (equations essential) like
G = nFE,
G = H – T S
H = U + P V where U = Internal Energy
P = pressure and V = volume
5. Definitions and examples of surroundings, open and closed systems.
6. Definitions of enthalpies of hydration, atomization, sublimation, and
lattice energy.
7. Equilibrium in chemical reactions
8. Le – Chateliers Principle
9. Equilibrium Constant in terms of concentration and pressure





Organic Chemistry 1. Hydrocarbons
i. Sources of hydrocarbons such as coal, natural gas and petroleum.
ii. Composition and structure of organic compounds
- determining the empirical formulae
- determining the molecular formulae
- determining structure
iii. Saturated Hydrocarbons; Alkanes Laboratory and industrial
preparations; Nomenclature and structures, reactions substitution,
combustion, cracking of large alkanes; uses as fuels and starting
materials for synthesis; and uses of haloalkanes and pollution effects.
iv. Homologous series.
v. Isomerism; exemplified with a compound that has maximum of five
carbon atoms.
vi. Unsaturated Hydrocarbons.
2. Alkenes; Laboratory preparation, Nomenclature and structure, Addition
reactions with halogen, bromine water, hydrogen halides, Oxidation,
hydroxylation with aqueous KMnO4., Test using Bromine vapour, KMnO4
and K2Cr2O7 and uses of alkenes.
3. Alkynes; Nomenclature, structure, Laboratory preparation, Test for and
use of Alkynes.
Reactions with ammoniacal CuCl and ammoniacal AgCl to distinguish
between double bond and triple bond.
4. Aromatic Hydrocarbons; Benzene, Resonance in benzene, stability from
substituted reactions, properties. Monosubstituted benzene such as
chlorobenzene, bromobenzene and methylbenzene (toluene)
5. Petroleum; Composition, fractional distillation and major products,
cracking and rebuilding, petrol quality (octane rating) and petro-chemical
starting material of organic synthesis.
6. Alkanols;
Laboratory preparation including hydration of alkenes. Industrial and
local production of ethanol, alcoholic beverages, Brewing process.
Classification-primary, secondary and tertiary alkanols, physical
properties e.g. intermolecular hydrogen bonding. Chemical properties
such as reaction with sodium, alkanoic acids (esterification), conc,
H2SO4, oxidation by aqueous KMnO4, K2Cr2O7 and I2/NaOH.
Monohydric alkanols e.g. ethanol,, Polyhydric alkanols e.g. ethane- 1,2-
diol (glycol) And propane- 1,2,3,-triol (glycerol).
7. Alkanoic acids
- Sources, nomenclature and structure
- physical properties e.g. intermolecular hydrogen bonding.
- chemical properties; reaction with H2O, NaOH, NaHCO3 (which is a
Laboratory test for alkanoic acid)
- Uses and properties of ethanoic and benzoic (phenylmethanoic) acids.
8. Alkanoate
- Preparation from the reaction of alkanoic acids with alkanols
- Sources, nomenclature, and structure
- physical properties, e.g. sweet or fruity smell.
- chemical properties; Alkaline hydrolysis and Acid hydrolysis.
9. Fats and Oils
- Sources, physical and chemical properties e.g. saponification,
hardening of oils, detergents as soapless detergent. The advantages of
detergent over soap.
- Hydrogenation of oil-margarine production
10. Protein
- as a polymer of amino acids molecules linked by peptide or amide
linkage
- difunctional nature of amino acids
- Uses in living systems
- hydrolysis
11. Natural and synthetic polymers
- Definitions of polymerization, Addition and condensation polymers,
plastics and resins, thermoplastic and thermosetting polymers.
- Important properties of polymers
- Synthetic polymers – classification, and preparation based on the
monomers and co-polymers e.g. Nylon.
- Natural polymers
12. Carbohydrates; Formulae, properties and uses, classification
Monosaccharides, Disaccharides and Polysaccharides, reducing and non-
reducing sugars exemplified by glucose, fructose, sucrose/maltose and
starch/cellulose.
- Hydrolysis of sucrose and starch; noting the enzymes involved and the
end product.
- Glucose as a source of energy. Oxidative metabolism, simple food
tests.
13. Functions of enzymes; importance of cellulose, fats, proteins, sugar,
starch in living system.
Non-Metals and their Compounds 1. Hydrogen
- Position in the Periodic Table
- Properties, reactions and uses
- Laboratory and Industrial preparations
- Compounds of Hydrogen (Hydrides)
2. Oxygen
- Bonding capacity
- Laboratory and Industrial preparations
- Properties and reactions
- Compounds of oxygen and uses of oxygen
- Classification of oxides
3. Air and pollution
- Composition of air
- Oxygen: combustion, flames, corrosion
Atmospheric Carbon (IV)oxide – Respiration, photosynthesis.
Atmospheric Nityrogen – water vapour, noble gases. Dissolved gases.
- Pollution: Causes, the pollutants, effects of pollutants, control of
pollution.
4. Water and solution
- Structure of H2O
- Solutions: process and types of solutions
- Solubility: calculations involved should be treated
- Solubility in g dm-3 and moles dm-3
- Water treatment and supply
- Hardness of water and softening methods
- Water pollution: Types of water, sources of pollutants, control of
pollution.
5. Halogens
- Electronic configuration, physical and chemical properties of halogens
- Laboratory and industrial preparation of Chlorine
- Compounds of halogens and their uses
- Reactions of chlorides and tests of chlorides.
6. Carbon and its compounds
- Allotropes; Charcoal, Graphite and Diamond – their structures and
properties, combustion and others.
- Coal types, destructive distillation of coal. Uses of the different
products.
- Coke: Gasefication and uses synthetic gas
Manufacture and uses of carbon as a reducing agent, charcoal
used as gases adsorbent
- Carbon (IV) oxide and carbon (II) oxide effect such as greenhouse. CO
that is poisonous, properties such as fire extinguishing for CO2,
reducing for CO
- Trioxocarbonate (IV) salts, and hydrogentrioxocarbonate (iv) salts.
7. Nitrogen
- Laboratory and industrial preparations.
- Properties and uses of nitrogen.
- Compounds of nitrogen – Ammonia, oxides of nitrogen, Trioxonitrate
(V) acid and salts
- Tests for nitrates.
8. Sulphur
- Allotropes and uses.
- Oxides of sulphur
- Trioxosulphate (IV) acids and salts
- Tetraoxosulphate (VI) acid-contact process, industrial preparation,
reactions and uses.
- Tests for SO42-, S2- and SO32-

Metals and their compounds 1. Extraction of metals by electrolysis, and reduction of compounds such as
oxides, chlorides and sulphides.
2. General properties of alkali metals
3. Properties and uses of Sodium and its compounds such as NaCI, NaOH,
Na2CO3, NaHCO3, NaNO3, NaCIO and Na2SO4
4. General properties of the alkaline earth metals
Calcium: Extraction, properties and uses Calcium.
5. Aluminium: Extraction, properties and uses.
6. Iron: Extraction, uses, properties and reactions; Prevention of Rusting.
7. Tin: Extraction and uses.
8. Copper: Extraction and uses
9. Alloys
Applied Chemistry 1. Chemical industries: Raw materials, sources of raw materials and their
uses.
2. Classification of chemicals into fine and heavy chemicals.
3. Production of various chemicals in the industries such as fertilizers,
plastics, pharmaceutical, glass, paints, ceramics, soap and detergents,
cement and metallurgy
Nuclear Chemistry 1. Radioactivity: Types and nature of radiation
Differences between chemical and nuclear reactions.
Half life: as a factor for stability of nucleus.
2. Nuclear Chemistry and Reactions
Nuclear fission and fusion in nuclear reactor.
Destructive power of atomic bomb, detection of radiation by the use of
Geiger Muller tube.
Applications in radio-carbon dating, agriculture, medicine, electronics,
and industry.
Astronomical Chemistry 1. Chemical Analysis of Earth and Space
- The age of the earth as determined by radioactive decay.
- Composition and properties of
(i) Atmosphere, (ii) Hydrosphere, (iii) Lithosphere
2. Planetary Data: Planets and the atmosphere, Space travel.
List of the parts of the earth comprising the solid, liquid and gas phases.
Chemistry of stars and space – Spectroscopy.