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.
SYLLABUS
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
- 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.
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-
- 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
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
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.
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.
- 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.