ACIDS, BASES AND SALTS

Definition of Acids
Strength of Acids
Definition of Bases
Strength of Bases
Acid-Base Reactions

By the end of the lesson, the learner should be able to:
- Define an acid in terms of hydrogen ions
-Investigate reactions of magnesium and zinc carbonate with different acids
-Write equations for reactions taking place
-Explain why magnesium strip should be cleaned

Class experiment: React cleaned magnesium strips with 2M HCl, 2M ethanoic acid, 2M H₂SO₄, 2M ethanedioic acid. Record observations in table. Repeat using zinc carbonate. Write chemical equations. Discuss hydrogen ion displacement and gas evolution.

Magnesium strips, zinc carbonate, 2M HCl, 2M ethanoic acid, 2M H₂SO₄, 2M ethanedioic acid, test tubes, test tube rack
2M HCl, 2M ethanoic acid, universal indicator, pH chart, electrical conductivity apparatus, milliammeter, carbon electrodes, beakers, wires
Calcium hydroxide, red litmus paper, phenolphthalein indicator, distilled water, test tubes, spatula, evaporating dish
2M NaOH, 2M ammonia solution, universal indicator, pH chart, electrical conductivity apparatus, milliammeter, carbon electrodes
Various acids and bases from previous lessons, indicators, beakers, measuring cylinders, stirring rods

KLB Secondary Chemistry Form 4, Pages 1-3

ACIDS, BASES AND SALTS

Effect of Solvent on Acids
Effect of Solvent on Bases
Amphoteric Oxides and Hydroxides
Definition of Salts and Precipitation
Solubility of Chlorides, Sulphates and Sulphites
Complex Ions Formation
Solubility and Saturated Solutions

By the end of the lesson, the learner should be able to:
- Explain effect of polar and non-polar solvents on hydrogen chloride
-Investigate HCl behavior in water vs methylbenzene
-Define polar and non-polar solvents
-Explain why acids show properties only in polar solvents

Teacher demonstration: Dissolve HCl gas in water and methylbenzene separately. Test both solutions with litmus paper, magnesium, and calcium carbonate. Compare observations. Explain polarity of water vs methylbenzene. Discuss dissociation vs molecular solution.

HCl gas, distilled water, methylbenzene, magnesium ribbon, calcium carbonate, litmus paper, test tubes, gas absorption apparatus
Dry ammonia gas, distilled water, methylbenzene, red litmus paper, test tubes, gas collection apparatus
Al₂O₃, ZnO, PbO, Zn(OH)₂, Al(OH)₃, Pb(OH)₂, 2M HNO₃, 2M NaOH, boiling tubes, heating source
Na₂CO₃ solution, salt solutions containing various metal ions, test tubes, droppers
2M NaCl, 2M Na₂SO₄, 2M Na₂SO₃, 0.1M salt solutions, dilute HCl, test tubes, heating source
2M NaOH, 2M NH₃ solution, 0.5M salt solutions, test tubes, droppers
Saturated KNO₃ solution, evaporating dish, watch glass, measuring cylinder, thermometer, balance, heating source

KLB Secondary Chemistry Form 4, Pages 7-9

ACIDS, BASES AND SALTS

Effect of Temperature on Solubility
Solubility Curves and Applications
Fractional Crystallization
Hardness of Water - Investigation
Types and Causes of Water Hardness
Effects of Hard Water

By the end of the lesson, the learner should be able to:
- Investigate the effect of temperature on solubility of potassium chlorate
-Record temperature at which crystals appear
-Calculate solubility at different temperatures
-Plot solubility curve

Class experiment: Dissolve 4g KClO₃ in 15cm³ water by warming. Cool while stirring and note crystallization temperature. Add 5cm³ water portions and repeat until total volume is 40cm³. Calculate solubility in g/100g water for each temperature. Plot solubility vs temperature graph.

KClO₃, measuring cylinders, thermometer, burette, boiling tubes, heating source, graph paper
Graph paper, ruler, pencil, calculator, data tables from textbook
Calculator, graph paper, data tables, worked examples from textbook
Soap solution, burette, various salt solutions, conical flasks, distilled water, tap water, rainwater, heating source
Student books, examples from previous experiment, chalkboard for equations
Samples of fur deposits, pictures of scaled pipes, calculator for cost analysis

KLB Secondary Chemistry Form 4, Pages 18-20

ACIDS, BASES AND SALTS
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES

Methods of Removing Hardness I
Methods of Removing Hardness II
Endothermic and Exothermic Reactions
Enthalpy Notation and Energy Content
Bond Breaking and Bond Formation
Latent Heat of Fusion and Vaporization
Bond Energy Calculations
Determination of Enthalpy of Solution I
Thermochemical Equations
Enthalpy of Solution of Concentrated Sulphuric Acid
Enthalpy of Combustion

By the end of the lesson, the learner should be able to:
- Explain removal of hardness by boiling
-Explain removal by distillation
-Write equations for these processes
-Compare effectiveness of different methods
- Calculate energy changes in reactions using bond energies
-Apply the formula: Heat of reaction = Bond breaking energy + Bond formation energy
-Determine whether reactions are exothermic or endothermic
-Use bond energy data to solve problems

Demonstrate boiling method: Boil hard water samples from previous experiments and test with soap. Write equations for Ca(HCO₃)₂ and Mg(HCO₃)₂ decomposition. Discuss distillation method using apparatus setup. Compare costs and effectiveness. Explain why boiling only removes temporary hardness.
Work through formation of HCl from H₂ and Cl₂ using bond energies. Calculate energy required to break H-H and Cl-Cl bonds. Calculate energy released when H-Cl bonds form. Apply formula: ΔH = Energy absorbed - Energy released. Practice with additional examples. Discuss why calculated values may differ from experimental values.

Hard water samples, heating source, soap solution, distillation apparatus diagram
Na₂CO₃ solution, hard water samples, ion exchange resin diagram, Ca(OH)₂, NH₃ solution
250ml plastic beakers, tissue paper, rubber bands, NH₄NO₃, NaOH pellets, distilled water, thermometers, spatulas, measuring cylinders
Student books, calculators, worked examples from textbook, chalkboard for calculations
Crushed pure ice, 250ml glass beakers, thermometers, heating source, stopwatch, graph paper, stirring rods
Data tables showing molar heats of fusion/vaporization, calculators, heating curves from previous lesson
Bond energy data tables, calculators, worked examples, practice problems
250ml plastic beakers, 2.0g samples of NH₄NO₃ and NaOH, distilled water, thermometers, measuring cylinders, analytical balance, calculators
Results from previous experiment, graph paper for energy level diagrams, practice examples
Concentrated H₂SO₄, distilled water, 250ml plastic beaker, tissue paper, measuring cylinders, thermometer, safety equipment
Ethanol, small bottles with wicks, 250ml glass beakers, tripod stands, wire gauze, thermometers, analytical balance, measuring cylinders

KLB Secondary Chemistry Form 4, Pages 25-26
KLB Secondary Chemistry Form 4, Pages 35-36

ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES

Enthalpy of Displacement
Enthalpy of Neutralization
Standard Conditions and Standard Enthalpy Changes
Hess's Law - Introduction and Theory
Energy Cycle Diagrams
Hess's Law Calculations

By the end of the lesson, the learner should be able to:
- Define molar heat of displacement
-Investigate displacement of copper(II) ions by zinc
-Calculate molar heat of displacement
-Explain relationship between position in reactivity series and heat of displacement

Class experiment: Add 4.0g zinc powder to 100cm³ of 0.5M CuSO₄ solution in wrapped plastic beaker. Record temperature change and observations. Calculate moles of Zn used and Cu²⁺ displaced. Determine molar heat of displacement. Write ionic equation. Discuss why excess zinc is used. Compare with theoretical value.

Zinc powder, 0.5M CuSO₄ solution, 250ml plastic beakers, tissue paper, thermometers, analytical balance, stirring rods
2M HCl, 2M NaOH, 2M ethanoic acid, 2M ammonia solution, measuring cylinders, thermometers, 250ml plastic beakers, tissue paper
Student books, examples of standard enthalpy data, notation practice exercises
Energy cycle diagrams for methane formation, chalkboard illustrations, worked examples from textbook
Graph paper, energy cycle templates, combustion data tables, calculators
Worked examples, combustion data, calculators, step-by-step calculation sheets

KLB Secondary Chemistry Form 4, Pages 44-47

ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES

Lattice Energy and Hydration Energy
Factors Affecting Lattice and Hydration Energies
Definition and Types of Fuels
Heating Values of Fuels
Factors in Fuel Selection
Environmental Effects of Fuels

By the end of the lesson, the learner should be able to:
- Define lattice energy and hydration energy
-Explain relationship between heat of solution, lattice energy and hydration energy
-Draw energy cycles for dissolution of ionic compounds
-Calculate heat of solution using Born-Haber type cycles

Explain dissolution of NaCl: first lattice breaks (endothermic), then ions hydrate (exothermic). Define lattice energy as energy to form ionic solid from gaseous ions. Define hydration energy as energy when gaseous ions become hydrated. Draw energy cycle: ΔH(solution) = ΔH(lattice) + ΔH(hydration). Calculate for NaCl.

Energy cycle diagrams, lattice energy and hydration energy data tables, calculators
Data tables from textbook, calculators, trend analysis exercises
Examples of different fuels, classification charts, pictures of fuel types
Heating value data table, calculators, fuel comparison charts
Fuel comparison tables, local fuel availability data, cost analysis sheets
Pictures of environmental damage, pollution data, examples of clean technology

KLB Secondary Chemistry Form 4, Pages 54-56

ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES

Fuel Safety and Precautions
Endothermic and Exothermic Reactions
Bond Breaking, Formation and Phase Changes
Determination of Enthalpy of Solution
Enthalpy of Solution of H₂SO₄ and Safety

By the end of the lesson, the learner should be able to:
- State precautions necessary when using fuels
-Explain safety measures for different fuel types
-Identify hazards associated with improper fuel handling
-Apply safety principles to local situations

Discuss safety precautions: ventilation for charcoal stoves (CO poisoning), not running engines in closed garages, proper gas cylinder storage, fuel storage away from populated areas, keeping away from fuel spills. Relate to local situations and accidents. Students identify potential hazards in their environment.

Safety guideline charts, examples of fuel accidents, local safety case studies
250ml plastic beakers, tissue paper, NH₄NO₃, NaOH pellets, distilled water, thermometers, calculators
Ice, glass beakers, thermometers, heating source, graph paper, bond energy data tables
2.0g samples of NH₄NO₃ and NaOH, plastic beakers, thermometers, analytical balance, calculators
Concentrated H₂SO₄, distilled water, plastic beaker, tissue paper, thermometer, safety equipment

KLB Secondary Chemistry Form 4, Pages 57-58

ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
ENERGY CHANGES IN PHYSICAL AND CHEMICAL PROCESSES
REACTION RATES AND REVERSIBLE REACTIONS

Enthalpy of Combustion
Enthalpy of Displacement
Enthalpy of Neutralization
Standard Conditions and Standard Enthalpy Changes
Hess's Law - Theory and Energy Cycles
Hess's Law Calculations
Lattice Energy and Hydration Energy
Definition and Types of Fuels
Fuel Selection Factors
Environmental Effects and Safety
Definition of Reaction Rate and Collision Theory

By the end of the lesson, the learner should be able to:
- Carry out experiments to determine enthalpy of combustion of ethanol
-Define molar heat of combustion
-Calculate molar enthalpy of combustion from experimental data
-Explain why actual heats are lower than theoretical values
- Explain relationship between heat of solution, hydration and lattice energy
-Define lattice energy and hydration energy
-Draw energy cycles for dissolving ionic compounds
-Calculate heat of solution using energy cycles

Class experiment: Burn ethanol to heat 100cm³ water. Record mass of ethanol burned and temperature change. Calculate moles of ethanol and heat evolved using ΔH = mcΔT. Determine molar enthalpy of combustion. Compare with theoretical (-1368 kJ/mol). Discuss heat losses to surroundings.
Explain NaCl dissolution: lattice breaks (endothermic) then ions hydrate (exothermic). Define lattice energy as energy when ionic compound forms from gaseous ions. Define hydration energy as energy when gaseous ions become hydrated. Draw energy cycle: ΔH(solution) = ΔH(lattice) + ΔH(hydration). Calculate for NaCl: +781 + (-774) = +7 kJ/mol.

Ethanol, bottles with wicks, glass beakers, tripod stands, thermometers, analytical balance
Zinc powder, 0.5M CuSO₄ solution, plastic beakers, thermometers, analytical balance
2M HCl, 2M NaOH, 2M ethanoic acid, 2M ammonia solution, measuring cylinders, thermometers, plastic beakers
Student books, standard enthalpy data examples, notation practice exercises
Energy cycle diagrams for methane and CO formation, combustion data, calculators
Worked examples, combustion data tables, graph paper for diagrams, calculators
Energy cycle diagrams, hydration diagram (Fig 2.17), Tables 2.6 and 2.7 with lattice/hydration energies
Examples of local fuels, Table 2.8 showing heating values, calculators
Fuel comparison tables, local fuel cost data, examples of specialized fuel applications
Pictures of environmental damage, pollution reduction examples, safety guideline charts
Examples of fast/slow reactions, energy diagram templates, chalk/markers for diagrams

KLB Secondary Chemistry Form 4, Pages 41-44
KLB Secondary Chemistry Form 4, Pages 54-56

REACTION RATES AND REVERSIBLE REACTIONS

Effect of Concentration on Reaction Rate
Change of Reaction Rate with Time
Effect of Temperature on Reaction Rate
Effect of Surface Area on Reaction Rate
Effect of Catalysts on Reaction Rate
Effect of Light and Pressure on Reaction Rate

By the end of the lesson, the learner should be able to:
- Explain the effect of concentration on reaction rates
-Investigate reaction of magnesium with different concentrations of sulphuric acid
-Illustrate reaction rates graphically and interpret experimental data
-Calculate concentrations and plot graphs of concentration vs time

Class experiment: Label 4 conical flasks A-D. Add 40cm³ of 2M H₂SO₄ to A, dilute others with water (30+10, 20+20, 10+30 cm³). Drop 2cm magnesium ribbon into each, time complete dissolution. Record in Table 3.1. Calculate concentrations, plot graph. Explain: higher concentration → more collisions → faster reaction.

4 conical flasks, 2M H₂SO₄, distilled water, magnesium ribbon, stopwatch, measuring cylinders, graph paper
0.5M HCl, magnesium ribbon, conical flask, gas collection apparatus, graduated syringe, stopwatch, graph paper
0.15M Na₂S₂O₃, 2M HCl, conical flasks, water baths at different temperatures, paper with cross marked, stopwatch, thermometers
Marble chips, marble powder, 1M HCl, gas collection apparatus, balance, conical flasks, measuring cylinders, graph paper
20-volume H₂O₂, MnO₂ powder, gas collection apparatus, balance, conical flasks, filter paper, measuring cylinders
0.1M KBr, 0.05M AgNO₃, test tubes, dark cupboard, direct light source, examples of photochemical reactions

KLB Secondary Chemistry Form 4, Pages 65-67

REACTION RATES AND REVERSIBLE REACTIONS

Reversible Reactions
Chemical Equilibrium
Le Chatelier's Principle and Effect of Concentration
Effect of Pressure and Temperature on Equilibrium
Industrial Applications - Haber Process
Industrial Applications - Contact Process

By the end of the lesson, the learner should be able to:
- State examples of simple reversible reactions
-Investigate heating of hydrated copper(II) sulphate
-Write equations for reversible reactions using double arrows
-Distinguish between reversible and irreversible reactions

Class experiment: Heat CuSO₄·5H₂O crystals in boiling tube A, collect liquid in tube B as in Fig 3.15. Observe color changes: blue → white + colorless liquid. Pour liquid back into tube A, observe return to blue. Write equation with double arrows: CuSO₄·5H₂O ⇌ CuSO₄ + 5H₂O. Give other examples: NH₄Cl ⇌ NH₃ + HCl. Compare with irreversible reactions.

CuSO₄·5H₂O crystals, boiling tubes, delivery tube, heating source, test tube holder
0.5M NaOH, 0.5M HCl, universal indicator, boiling tubes, droppers, examples of equilibrium systems
Bromine water, 2M NaOH, 2M HCl, beakers, chromate/dichromate solutions for demonstration
Copper turnings, concentrated HNO₃, test tubes, heating source, ice bath, gas collection apparatus, safety equipment
Haber Process flow diagram, equilibrium data showing temperature/pressure effects on NH₃ yield, industrial catalyst information
Contact Process flow diagram, comparison table with Haber Process, catalyst effectiveness data

KLB Secondary Chemistry Form 4, Pages 78-80

ELECTROCHEMISTRY

Redox Reactions and Oxidation Numbers
Oxidation Numbers in Naming and Redox Identification
Displacement Reactions - Metals and Halogens
Electrochemical Cells and Cell Diagrams
Standard Electrode Potentials
Calculating Cell EMF and Predicting Reactions
Types of Electrochemical Cells
Electrolysis of Aqueous Solutions I
Electrolysis of Aqueous Solutions II
Effect of Electrode Material on Electrolysis

By the end of the lesson, the learner should be able to:
Define redox reactions in terms of electron transfer
- State rules for assigning oxidation numbers
- Calculate oxidation numbers in compounds
- Identify oxidation and reduction processes

Q/A: Review previous knowledge
- Experiment 4.1: Iron filings + copper(II) sulphate
- Experiment 4.2: Iron(II) ions + hydrogen peroxide
- Discussion on oxidation number rules with examples

Iron filings, 1M CuSO₄, 1M FeSO₄, 2M NaOH, 20V H₂O₂, test tubes
Compound charts, calculators, student books, practice exercises
Various metals (Ca, Mg, Zn, Fe, Pb, Cu), metal salt solutions, halogens (Cl₂, Br₂, I₂), halide solutions
Metal electrodes, 1M metal salt solutions, voltmeters, salt bridges, connecting wires
Standard electrode potential table, diagrams, charts showing standard conditions
Calculators, electrode potential data, worked examples, practice problems
Cell diagrams, sample batteries, charts showing cell applications
Dilute and concentrated NaCl solutions, carbon electrodes, gas collection tubes, test equipment
U-tube apparatus, 2M H₂SO₄, 0.5M MgSO₄, platinum/carbon electrodes, gas syringes
Copper and carbon electrodes, 3M CuSO₄ solution, accurate balance, beakers, connecting wires

KLB Secondary Chemistry Form 4, Pages 108-116

ELECTROCHEMISTRY
ELECTROCHEMISTRY
METALS
METALS
METALS
METALS
METALS

Factors Affecting Electrolysis
Applications of Electrolysis I
Applications of Electrolysis II
Faraday's Laws and Quantitative Electrolysis
Electrolysis Calculations I
Electrolysis Calculations II
Advanced Applications and Problem Solving
Chemical Properties I - Reaction with Air
Chemical Properties II - Reaction with Water
Chemical Properties III - Reaction with Chlorine
Chemical Properties IV - Reaction with Acids
Uses of Metals I - Sodium and Aluminium

By the end of the lesson, the learner should be able to:
Identify factors affecting preferential discharge
- Explain electrochemical series influence
- Discuss concentration and electrode effects
- Predict electrolysis products
Determine charge on ions from electrolysis data
- Calculate current-time relationships
- Solve complex multi-step problems
- Apply concepts to industrial situations

Review electrochemical series and discharge order
- Analysis of concentration effects on product formation
- Summary of all factors affecting electrolysis
- Practice prediction problems
Complex problems: Determine ionic charges
- Current-time-mass relationships
- Multi-step calculations
- Industrial calculation examples

Electrochemical series chart, summary tables, practice exercises, student books
Iron nails, copper electrodes, CuSO₄ solution, power supply, industrial process diagrams
Flow charts, mercury cell diagrams, environmental impact data, industrial case studies
Accurate balance, copper electrodes, CuSO₄ solution, ammeter, timer, calculators
Calculators, worked examples, practice problems, gas volume data, Faraday constant
Calculators, complex problem sets, industrial data, student books
Past papers, comprehensive problem sets, industrial case studies, calculators
Deflagrating spoons, metal samples (Na, Al, Zn, Fe, Cu), Bunsen burners, safety equipment
Metal samples, cold water, steam generator, test tubes, universal indicator, safety equipment
Chlorine gas, gas jars, metal samples, tongs, deflagrating spoons, fume cupboard, safety equipment
Various acids (dilute and concentrated), metal strips, test tubes, gas collection apparatus, safety equipment
Charts showing metal applications, alloy samples, aircraft parts, cooking vessels

KLB Secondary Chemistry Form 4, Pages 153-155
KLB Secondary Chemistry Form 4, Pages 161-164

METALS
ORGANIC CHEMISTRY II
ORGANIC CHEMISTRY II
ORGANIC CHEMISTRY II
ORGANIC CHEMISTRY II
ORGANIC CHEMISTRY II

Uses of Metals II - Zinc, Copper and Iron
Steel Types and Alloys
Environmental Effects of Metal Extraction
Introduction to Alkanols and Nomenclature
Isomerism in Alkanols
Laboratory Preparation of Ethanol
Industrial Preparation and Physical Properties
Chemical Properties of Alkanols I

By the end of the lesson, the learner should be able to:
Explain galvanization process
- Describe copper electrical applications
- Compare iron, steel, and cast iron uses
- Analyze alloy compositions and properties

Study galvanization and rust prevention
- Copper in electrical applications
- Different types of steel and their compositions
- Alloy property comparisons

Galvanized sheets, copper wires, steel samples, alloy composition charts, brass and bronze samples
Steel samples with different compositions, carbon content charts, specialized tools, stainless steel items
Environmental impact case studies, pollution images, NEMA regulation documents, waste management examples
Molecular models, Table 6.1 and 6.2, alkanol structure charts, student books
Isomer structure charts, molecular models, practice worksheets, student books
Sugar, yeast, warm water, conical flask, delivery tube, lime water, thermometer
Table 6.3, industrial process diagrams, ethene structure models, property comparison charts
Ethanol, sodium metal, universal indicator, concentrated H₂SO₄, ethanoic acid, test tubes

KLB Secondary Chemistry Form 4, Pages 159-161

ORGANIC CHEMISTRY II

Chemical Properties of Alkanols II
Uses of Alkanols and Health Effects
Introduction to Alkanoic Acids
Laboratory Preparation of Ethanoic Acid
Physical and Chemical Properties of Alkanoic Acids
Esterification and Uses of Alkanoic Acids
Introduction to Detergents and Soap Preparation

By the end of the lesson, the learner should be able to:
Investigate oxidation and esterification reactions
- Test oxidizing agents on ethanol
- Prepare esters from alkanols
- Explain dehydration reactions

Complete Experiment 6.2: Test with acidified K₂Cr₂O₇ and KMnO₄
- Observe color changes
- Esterification with ethanoic acid
- Study dehydration conditions

Acidified potassium chromate/manganate, ethanoic acid, concentrated H₂SO₄, heating apparatus
Charts showing alkanol uses, health impact data, methylated spirit samples, discussion materials
Alkanoic acid structure charts, Table 6.5 and 6.6, molecular models, student books
Ethanol, KMnO₄, concentrated H₂SO₄, distillation apparatus, thermometer, round-bottom flask
2M ethanoic acid, universal indicator, Mg strip, Na₂CO₃, NaOH, phenolphthalein, test tubes
Ethanoic acid, ethanol, concentrated H₂SO₄, test tubes, heating apparatus, cold water
Castor oil, 4M NaOH, NaCl, evaporating dish, water bath, stirring rod, filter paper

KLB Secondary Chemistry Form 4, Pages 173-176

ORGANIC CHEMISTRY II

Mode of Action of Soap and Hard Water Effects
Soapless Detergents and Environmental Effects
Introduction to Polymers and Addition Polymerization
Addition Polymers - Types and Properties
Condensation Polymerization and Natural Polymers
Polymer Properties and Applications

By the end of the lesson, the learner should be able to:
Explain soap molecule structure
- Describe cleaning mechanism
- Investigate hard water effects
- Compare soap performance in different waters

Study hydrophobic and hydrophilic ends
- Demonstrate micelle formation
- Test soap in distilled vs hard water
- Observe scum formation
- Write precipitation equations

Soap samples, distilled water, hard water (CaCl₂/MgSO₄ solutions), test tubes, demonstration materials
Flow charts of detergent manufacture, Table 6.9, environmental impact data, sample detergents
Polymer samples, monomer structure charts, molecular models, calculators, polymer formation diagrams
Various polymer samples, structure identification exercises, calculation worksheets, Table 6.10
Nylon samples, rubber samples, condensation reaction diagrams, natural polymer examples
Table 6.10, polymer application samples, environmental impact studies, product examples

KLB Secondary Chemistry Form 4, Pages 186-188

ORGANIC CHEMISTRY II
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
RADIOACTIVITY
GAS LAWS
GAS LAWS

Comprehensive Problem Solving and Integration
Introduction, Nuclear Stability and Types of Radioactivity
Types of Radiation and Their Properties
Radioactive Decay and Half-Life Concept
Half-Life Calculations and Problem Solving
Nuclear Reactions and Equations
Radioactive Decay Series and Sequential Reactions
Nuclear Fission and Chain Reactions
Nuclear Fusion and Energy Comparisons
Medical and Diagnostic Applications
Industrial, Agricultural and Dating Applications
Radiation Hazards and Environmental Impact
Safety Measures and International Control
Half-Life Problem Solving and Graph Analysis
Nuclear Equations and Conservation Laws
Boyle's Law - Introduction and Experimental Investigation
Boyle's Law - Mathematical Expression and Graphical Representation

By the end of the lesson, the learner should be able to:
Solve complex problems involving alkanols and acids
- Apply knowledge to practical situations
- Integrate polymer concepts
- Practice examination questions
Explain industrial leak detection
- Describe agricultural monitoring techniques
- Discuss carbon-14 dating principles
- Analyze food preservation methods

Worked examples on organic synthesis
- Problem-solving on isomers, reactions, polymers
- Integration of all unit concepts
- Practice examination-style questions
Study leak detection using short half-life isotopes
- Carbon-14 dating of archaeological materials
- Phosphorus tracking in agriculture
- Gamma radiation food preservation

Comprehensive problem sets, past examination papers, calculators, organic chemistry summary charts
Periodic table, atomic structure charts, Table 7.1, nuclear stability diagrams
Radiation type charts, penetration diagrams, electric field illustrations, safety equipment charts
Graph paper, Table 7.2 data, calculators, decay curve examples, half-life data table
Calculators, comprehensive problem sets, worked examples, isotope half-life comparison tables
Nuclear equation examples, periodic table, conservation law charts, practice worksheets
Decay series charts, thorium series diagram, nuclide stability charts, practice decay series
Fission reaction diagrams, chain reaction illustrations, nuclear reactor diagrams, energy calculation examples
Fusion reaction diagrams, comparison tables, stellar fusion charts, energy comparison data
Medical radioisotope charts, treatment procedure diagrams, diagnostic equipment images, case studies
Carbon dating examples, agricultural application charts, industrial use diagrams, food preservation data
Accident case studies, environmental impact data, radiation exposure charts, contamination maps
IAEA guidelines, safety protocol charts, monitoring equipment diagrams, international cooperation data
Graph paper, experimental data sets, calculators, statistical analysis examples, comprehensive problem sets
Nuclear equation worksheets, periodic table, decay series diagrams, conservation law examples
Bicycle pump, Syringes, Gas jars, Chart showing volume-pressure relationship
Graph papers, Scientific calculators, Chart showing mathematical expressions

KLB Secondary Chemistry Form 4, Pages 167-201
KLB Secondary Chemistry Form 4, Pages 208-209

GAS LAWS

Boyle's Law - Numerical Problems and Applications
Charles's Law - Introduction and Temperature Scales
Charles's Law - Experimental Investigation and Mathematical Expression
Charles's Law - Numerical Problems and Applications
Combined Gas Law and Standard Conditions
Introduction to Diffusion - Experimental Investigation
Rates of Diffusion - Comparative Study
Graham's Law of Diffusion - Theory and Mathematical Expression
Graham's Law - Numerical Applications and Problem Solving

By the end of the lesson, the learner should be able to:
Solve numerical problems involving Boyle's law
Convert between different pressure units
Apply Boyle's law to real-life situations
Calculate volumes and pressures using P₁V₁ = P₂V₂

Worked examples: Demonstrate step-by-step problem solving. Supervised practice: Students solve problems involving pressure and volume calculations. Convert units (mmHg, atm, Pa). Discuss applications in tire inflation, aerosol cans. Assignment: Additional practice problems.

Scientific calculators, Worked example charts, Unit conversion tables
Round-bottomed flask, Narrow glass tube, Colored water, Rubber bung, Hot and cold water baths
Glass apparatus, Thermometers, Graph papers, Water baths at different temperatures
Scientific calculators, Temperature conversion charts, Application examples
Scientific calculators, Combined law derivation charts, Standard conditions reference table
KMnO₄ crystals, Bromine liquid, Gas jars, Combustion tube, Litmus papers, Stopwatch
Glass tube (25cm), Cotton wool, Concentrated NH₃ and HCl, Stopwatch, Ruler, Safety equipment
Graham's law charts, Molecular mass tables, Mathematical derivation displays
Scientific calculators, Worked example charts, Molecular mass reference tables

KLB Secondary Chemistry Form 3, Pages 4-5

THE MOLE

Relative Mass - Introduction and Experimental Investigation
Avogadro's Constant and the Mole Concept
Interconversion of Mass and Moles for Elements
Molecules and Moles - Diatomic Elements
Empirical Formula - Experimental Determination

By the end of the lesson, the learner should be able to:
Define relative mass using practical examples
Compare masses of different objects using a reference standard
Explain the concept of relative atomic mass
Identify carbon-12 as the reference standard

Experiment: Weighing different sized nails using beam balance. Use smallest nail as reference standard. Q/A: Discuss everyday examples of relative measurements. Teacher exposition: Introduction of carbon-12 scale and IUPAC recommendations. Calculate relative masses from experimental data.

Different sized nails ( 5-15cm), Beam balance, Fruits of different masses, Reference charts
Beam balance, Various sized nails, Scientific calculators, Avogadro's constant charts
Scientific calculators, Periodic table, Worked example charts, Formula triangles
Molecular models, Charts showing diatomic elements, Scientific calculators
Crucible and lid, Magnesium ribbon, Bunsen burner, Beam balance, Tongs, Safety equipment

KLB Secondary Chemistry Form 3, Pages 25-27

THE MOLE

Empirical Formula - Reduction Method
Empirical Formula - Percentage Composition Method
Molecular Formula - Determination from Empirical Formula
Molecular Formula - Combustion Analysis
Concentration and Molarity of Solutions
Preparation of Molar Solutions

By the end of the lesson, the learner should be able to:
Determine empirical formula using reduction reactions
Calculate empirical formula from reduction data
Apply reduction method to copper oxides
Analyze experimental errors and sources

Experiment: Reduction of copper(II) oxide using laboratory gas. Measure masses before and after reduction. Calculate moles of copper and oxygen. Determine empirical formula from mole ratios. Discuss experimental precautions.

Combustion tube, Porcelain boat, Copper(II) oxide, Laboratory gas, Beam balance, Bunsen burner
Scientific calculators, Percentage composition charts, Worked example displays
Scientific calculators, Molecular mass charts, Worked example displays
Scientific calculators, Combustion analysis charts, Molecular models of hydrocarbons
Scientific calculators, Molarity charts, Various salt samples for demonstration
Volumetric flasks (250, 500, 1000cm³), Sodium hydroxide pellets, Beam balance, Wash bottles, Beakers

KLB Secondary Chemistry Form 3, Pages 35-37

THE MOLE

Dilution of Solutions
Stoichiometry - Experimental Determination of Equations
Stoichiometry - Precipitation Reactions
Stoichiometry - Gas Evolution Reactions
Volumetric Analysis - Introduction and Apparatus
Titration - Acid-Base Neutralization
Titration - Diprotic Acids
Standardization of Solutions
Back Titration Method
Redox Titrations - Principles
Redox Titrations - KMnO₄ Standardization

By the end of the lesson, the learner should be able to:
Define dilution process
Apply dilution formula M₁V₁ = M₂V₂
Calculate concentrations after dilution
Prepare dilute solutions from concentrated ones
Investigate titrations involving diprotic acids
Determine basicity of acids from titration data
Compare volumes needed for mono- and diprotic acids
Write equations for diprotic acid reactions

Experiment: Dilute 25cm³ of 2M HCl to different final volumes (250cm³ and 500cm³). Calculate resulting concentrations. Worked examples using dilution formula. Safety precautions when diluting acids.
Experiment: Titrate 25cm³ of 0.1M NaOH with 0.1M H₂SO₄. Compare volume used with previous HCl titration. Calculate mole ratios. Explain concept of basicity. Introduce dibasic and tribasic acids.

Volumetric flasks, Hydrochloric acid (2M), Measuring cylinders, Pipettes, Safety equipment
Iron filings, Copper(II) sulphate solution, Beam balance, Beakers, Filter equipment
Test tubes, Lead(II) nitrate solution, Potassium iodide solution, Burettes, Ethanol, Rulers
Conical flask, Thistle funnel, Plastic bags, Rubber bands, Sodium carbonate, HCl solution
Pipettes (10, 20, 25cm³), Burettes (50cm³), Pipette fillers, Conical flasks, Various solutions
Burettes, Pipettes, 0.1M NaOH, 0.1M HCl, Phenolphthalein indicator, Conical flasks
Burettes, Pipettes, 0.1M H₂SO₄, 0.1M NaOH, Phenolphthalein, Basicity reference chart
Anhydrous Na₂CO₃, Approximately 0.1M HCl, Methyl orange, Volumetric flasks, Analytical balance
Metal carbonate sample, 0.5M HCl, 0M NaOH, Phenolphthalein, Conical flasks
Potassium manganate(VII), Potassium dichromate(VI), Iron(II) solutions, Color change charts
Iron(II) ammonium sulfate, KMnO₄ solution, Dilute H₂SO₄, Pipettes, Burettes

KLB Secondary Chemistry Form 3, Pages 46-50
KLB Secondary Chemistry Form 3, Pages 62-65

THE MOLE
ORGANIC CHEMISTRY I
ORGANIC CHEMISTRY I

Water of Crystallization Determination
Atomicity and Molar Gas Volume
Combining Volumes of Gases - Experimental Investigation
Gas Laws and Chemical Equations
Introduction to Organic Chemistry and Hydrocarbons
Sources of Alkanes - Natural Gas, Biogas, and Crude Oil

By the end of the lesson, the learner should be able to:
Determine water of crystallization in hydrated salts
Use redox titration to find formula of hydrated salt
Calculate value of 'n' in crystallization formulas
Apply analytical data to determine complete formulas

Experiment: Determine 'n' in FeSO₄(NH₄)₂SO₄·nH₂O. Dissolve known mass in acid, titrate with standardized KMnO₄. Calculate moles of iron(II), hence complete formula. Compare theoretical and experimental values.

Hydrated iron(II) salt, Standardized KMnO₄, Dilute H₂SO₄, Analytical balance
Gas syringes (50cm³), Various gases, Analytical balance, Gas supply apparatus
Gas syringes, Dry NH₃ generator, Dry HCl generator, Glass connecting tubes, Clips
Scientific calculators, Gas law charts, Volume ratio examples
Carbon models, Hydrocarbon structure charts, Molecular model kits
Biogas digester model/diagram, Natural gas composition charts, Organic waste samples

KLB Secondary Chemistry Form 3, Pages 72-73

ORGANIC CHEMISTRY I

Fractional Distillation of Crude Oil
Cracking of Alkanes - Thermal and Catalytic Methods
Alkane Series and Homologous Series Concept
Nomenclature of Alkanes - Straight Chain and Branched
Isomerism in Alkanes - Structural Isomers
Laboratory Preparation of Methane

By the end of the lesson, the learner should be able to:
Explain fractional distillation process
Perform fractional distillation of crude oil
Identify different fractions and their uses
Relate boiling points to molecular size

Experiment: Fractional distillation of crude oil using improvised column. Collect fractions at different temperatures (120°C intervals up to 350°C). Test fractions for appearance, flammability, and viscosity. Record observations and relate to molecular size.

Crude oil sample, Boiling tubes, High-temperature thermometer, Sand/porcelain chips, Bunsen burner, Test tubes
Cracking process diagrams, Chemical equation charts, Catalyst samples for demonstration
Alkane series chart, Molecular formula worksheets, Periodic table
Structural formula charts, IUPAC naming rules poster, Molecular model kits
Molecular model kits, Isomerism charts, Structural formula worksheets
Sodium ethanoate, Soda lime, Round-bottomed flask, Gas collection apparatus, Bromine water, Wooden splints

KLB Secondary Chemistry Form 3, Pages 87-89

ORGANIC CHEMISTRY I

Laboratory Preparation of Ethane
Physical Properties of Alkanes
Chemical Properties of Alkanes - Combustion and Substitution
Uses of Alkanes in Industry and Daily Life
Introduction to Alkenes and Functional Groups

By the end of the lesson, the learner should be able to:
Prepare ethane using sodium propanoate and soda lime
Compare preparation methods of methane and ethane
Test properties of ethane gas
Write general equation for alkane preparation

Experiment: Prepare ethane from sodium propanoate and soda lime. Compare with methane preparation method. Carry out similar tests as for methane. Discussion: General pattern for alkane preparation from sodium alkanoates.

Sodium propanoate, Soda lime, Gas collection apparatus, Testing materials
Physical properties data tables, Graph paper, Calculators, Solubility demonstration materials
Molecular models, Halogenation reaction charts, Chemical equation worksheets
Industrial application charts, Product samples, Environmental impact materials
Alkene series charts, Molecular models showing double bonds, Functional group posters

KLB Secondary Chemistry Form 3, Pages 94-96

ORGANIC CHEMISTRY I

Nomenclature of Alkenes
Isomerism in Alkenes - Branching and Positional
Laboratory Preparation of Ethene
Alternative Preparation of Ethene and Physical Properties
Chemical Properties of Alkenes - Addition Reactions
Oxidation Reactions of Alkenes and Polymerization
Tests for Alkenes and Uses
Introduction to Alkynes and Triple Bond
Nomenclature and Isomerism in Alkynes
Laboratory Preparation of Ethyne
Physical and Chemical Properties of Alkynes

By the end of the lesson, the learner should be able to:
Apply IUPAC rules for naming alkenes
Number carbon chains to give lowest numbers to double bonds
Name branched alkenes with substituents
Distinguish position isomers of alkenes
Perform chemical tests to identify alkenes
Use bromine water and KMnO₄ as test reagents
List industrial and domestic uses of alkenes
Explain importance in plastic manufacture

Teacher demonstration: Step-by-step naming of alkenes. Rules application: Longest chain with double bond, numbering from end nearest double bond. Practice exercises: Name various alkene structures. Group work: Complex branched alkenes with substituents.
Practical session: Test known alkenes with bromine water and acidified KMnO₄. Observe rapid decolorization compared to alkanes. Discussion: Uses in plastics, ethanol production, fruit ripening, detergents. Assignment: Research alkene applications.

IUPAC naming charts for alkenes, Structural formula worksheets, Molecular model kits
Molecular model kits, Isomerism worksheets, Geometric isomer models
Ethanol, Concentrated H₂SO₄, Round-bottomed flask, Sand bath, Gas collection apparatus, Testing solutions
Aluminum oxide catalyst, Glass wool, Alternative apparatus setup, Physical properties charts
Addition reaction charts, Mechanism diagrams, Chemical equation worksheets
Oxidizing agents for demonstration, Polymer samples, Polymerization charts, Monomer-polymer models
Test alkenes, Bromine water, Acidified KMnO₄, Plastic samples, Uses reference charts
Alkyne series charts, Triple bond molecular models, Unsaturation comparison charts
IUPAC naming rules for alkynes, Structural formula worksheets, Molecular model kits
Calcium carbide, Sand, Flat-bottomed flask, Dropping funnel, Gas collection apparatus, Testing solutions
Physical properties charts, Comparison tables, Combustion equation examples

KLB Secondary Chemistry Form 3, Pages 101-102
KLB Secondary Chemistry Form 3, Pages 108-109

ORGANIC CHEMISTRY I
NITROGEN AND ITS COMPOUNDS
NITROGEN AND ITS COMPOUNDS
NITROGEN AND ITS COMPOUNDS
NITROGEN AND ITS COMPOUNDS

Addition Reactions of Alkynes and Chemical Tests
Uses of Alkynes and Industrial Applications
Introduction to Nitrogen - Properties and Occurrence
Isolation of Nitrogen from Air - Industrial and Laboratory Methods
Laboratory Preparation of Nitrogen Gas
Properties and Uses of Nitrogen Gas

By the end of the lesson, the learner should be able to:
Write equations for halogenation of alkynes
Describe hydrogenation and hydrohalogenation
Compare reaction rates: alkynes vs alkenes
Perform chemical tests for alkynes

Worked examples: Two-step addition reactions of ethyne with Br₂, Cl₂, H₂. Discussion: Faster reaction rates in alkynes compared to alkenes. Practical session: Test alkynes with oxidizing agents. Comparison: Rate of decolorization vs alkenes.

Addition reaction charts, Chemical equation worksheets, Test solutions, Stopwatch for rate comparison
Industrial application charts, Welding equipment demonstration/video, Synthetic fiber samples
Periodic table charts, Atmospheric composition diagrams, Molecular models showing N≡N triple bond
Aspirator, KOH solution, Copper turnings, Heating apparatus, Fractional distillation flow chart
Sodium nitrite, Ammonium chloride, Round-bottomed flask, Gas collection apparatus, Test reagents, Deflagrating spoon
Property summary charts, Uses of nitrogen displays, Industrial application diagrams

KLB Secondary Chemistry Form 3, Pages 113-115

NITROGEN AND ITS COMPOUNDS

Nitrogen(I) Oxide - Preparation and Properties
Nitrogen(II) Oxide - Preparation and Properties
Nitrogen(IV) Oxide - Preparation and Properties
Comparison of Nitrogen Oxides and Environmental Effects
Laboratory Preparation of Ammonia
Preparation of Aqueous Ammonia and Solubility

By the end of the lesson, the learner should be able to:
Prepare nitrogen(I) oxide from ammonium nitrate
Test physical and chemical properties
Explain decomposition and oxidizing properties
Describe uses of nitrogen(I) oxide

Experiment: Heat ammonium nitrate carefully in test tube. Collect gas over warm water. Tests: Color, smell, glowing splint test, reaction with heated copper and sulfur. Safety: Stop heating while some solid remains to avoid explosion.

Ammonium nitrate, Test tubes, Gas collection apparatus, Copper turnings, Sulfur, Glowing splints
Copper turnings, Dilute nitric acid, Gas collection apparatus, Iron(II) sulfate solution, Test reagents
Copper turnings, Concentrated nitric acid, Lead(II) nitrate, Gas collection apparatus, U-tube with ice, Testing materials
Comparison charts, Environmental impact diagrams, Vehicle emission illustrations
Calcium hydroxide, Ammonium chloride, Round-bottomed flask, Calcium oxide, HCl solution, Glass rod, Litmus paper
Ammonia generation apparatus, Funnel, Universal indicator, Fountain apparatus, pH meter/paper

KLB Secondary Chemistry Form 3, Pages 123-125

NITROGEN AND ITS COMPOUNDS

Reactions of Aqueous Ammonia with Metal Ions
Chemical Properties of Ammonia - Reactions with Acids and Combustion
Industrial Manufacture of Ammonia - The Haber Process
Uses of Ammonia and Introduction to Nitrogenous Fertilizers
Nitrogenous Fertilizers - Types and Calculations

By the end of the lesson, the learner should be able to:
Test reactions of aqueous ammonia with various metal ions
Observe precipitate formation and dissolution
Explain complex ion formation
Use reactions for metal ion identification

Experiment: Add aqueous ammonia dropwise to solutions of Ca²⁺, Mg²⁺, Al³⁺, Zn²⁺, Fe²⁺, Fe³⁺, Pb²⁺, Cu²⁺. Record observations with few drops vs excess ammonia. Identify complex ion formation with Zn²⁺ and Cu²⁺.

Various metal salt solutions, Aqueous ammonia, Test tubes, Droppers, Observation recording tables
Various dilute acids, Methyl orange, Oxygen supply, Platinum wire, Copper(II) oxide, Combustion apparatus, U-tube for collection
Haber process flow charts, Industrial diagrams, Catalyst samples, Economic analysis sheets
Fertilizer samples, Percentage calculation worksheets, Use application charts, Calculator
Various fertilizer formulas, Scientific calculators, Laboratory preparation materials, Environmental impact data

KLB Secondary Chemistry Form 3, Pages 136-138

NITROGEN AND ITS COMPOUNDS

Laboratory Preparation of Nitric(V) Acid
Industrial Manufacture of Nitric(V) Acid
Reactions of Dilute Nitric(V) Acid with Metals
Reactions of Dilute Nitric(V) Acid with Carbonates and Hydroxides
Reactions of Concentrated Nitric(V) Acid - Oxidizing Properties
Uses of Nitric(V) Acid and Introduction to Nitrates
Action of Heat on Nitrates - Decomposition Patterns
Test for Nitrates - Brown Ring Test
Environmental Pollution by Nitrogen Compounds
Pollution Control and Environmental Solutions
Comprehensive Problem Solving - Nitrogen Chemistry
Laboratory Practical Assessment - Nitrogen Compounds

By the end of the lesson, the learner should be able to:
Prepare nitric acid from nitrate and concentrated sulfuric acid
Set up all-glass apparatus safely
Explain brown fumes and yellow color
Purify nitric acid by air bubbling
Test thermal decomposition of different nitrates
Classify decomposition patterns based on metal reactivity
Identify products formed on heating
Write equations for decomposition reactions

Experiment: Heat mixture of KNO₃ and concentrated H₂SO₄ in all-glass apparatus. Collect yellow nitric acid. Explain brown fumes (NO₂) and yellow color. Bubble air through to remove dissolved NO₂. Safety: Gentle heating, fume cupboard.
Experiment: Heat KNO₃, NaNO₃, Zn(NO₃)₂, Cu(NO₃)₂, NH₄NO₃ separately. Test gases with glowing splint. Observe residues. Classification: Group I nitrates → nitrite + O₂; Group II → oxide + NO₂ + O₂; NH₄NO₃ → N₂O + H₂O.

Potassium nitrate, Concentrated sulfuric acid, All-glass apparatus, Condenser, Retort stand, Safety equipment
Industrial process flow charts, Catalyst samples, Process condition charts, Efficiency calculation sheets
Various metals (Mg, Zn, Cu), Dilute nitric acid, Test tubes, Gas testing apparatus, Burning splints
Various carbonates and hydroxides, Dilute nitric acid, Lime water, Universal indicator, Test tubes
Concentrated nitric acid, Iron(II) sulfate, Sulfur powder, Copper turnings, Test tubes, Fume cupboard access
Industrial use charts, Nitrate salt samples, Preparation method diagrams, Safety data sheets
Various nitrate salts, Test tubes, Bunsen burner, Gas collection apparatus, Glowing splints, Observation recording sheets
Sodium nitrate, Fresh FeSO₄ solution, Concentrated H₂SO₄, Copper turnings, Test tubes, Unknown nitrate samples
Environmental pollution charts, Acid rain effect photos, Vehicle emission diagrams, Control measure illustrations
Case studies, Pollution control technology information, Group activity worksheets, Local environmental data
Scientific calculators, Comprehensive problem sets, Industrial data sheets, Experimental result tables
Unknown nitrogen compounds, All laboratory chemicals and apparatus used in chapter, Safety equipment, Assessment rubrics

KLB Secondary Chemistry Form 3, Pages 144-145
KLB Secondary Chemistry Form 3, Pages 151-153

NITROGEN AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS
SULPHUR AND ITS COMPOUNDS

Industrial Applications and Economic Importance
Chapter Review and Integration
Extraction of Sulphur
Allotropes of Sulphur
Physical Properties of Sulphur - Solubility
Physical Properties of Sulphur - Effect of Heat
Chemical Properties of Sulphur - Reactions with Elements
Chemical Properties of Sulphur - Reactions with Acids
Uses of Sulphur and Introduction to Oxides

By the end of the lesson, the learner should be able to:
Evaluate economic importance of nitrogen industry
Analyze industrial production costs and benefits
Compare different manufacturing processes
Assess impact on agricultural productivity

Case study analysis: Haber process economics, fertilizer industry impact, nitric acid production costs. Agricultural benefits: Crop yield improvements, food security. Economic calculations: Production costs, profit margins, environmental costs. Global nitrogen cycle importance.

Economic data sheets, Industry case studies, Agricultural statistics, Cost-benefit analysis templates
Concept mapping materials, Comparison charts, Flow diagram templates, Integration worksheets
Charts showing periodic table, Diagram of Frasch process, Samples of sulphur compounds (pyrites, gypsum)
Powdered sulphur, Carbon(IV) sulphide, Evaporating dish, Glass rod, Hand lens, Boiling tubes, Filter paper, Beakers
Powdered sulphur, Water, Benzene, Methylbenzene, Carbon(IV) sulphide, Test tubes, Charts showing molecular structure
Powdered sulphur, Test tubes, Bunsen burner, Cold surface for condensation, Thermometer, Safety equipment
Sulphur, Iron powder, Copper powder, Oxygen gas jar, Deflagrating spoon, Moist litmus papers, Test tubes, Bunsen burner
Sulphur powder, Concentrated HNO3, Concentrated H2SO4, Concentrated HCl, Barium chloride solution, Test tubes, Fume cupboard access
Charts showing uses of sulphur, Samples of vulcanized rubber, Fungicides, Industrial photographs, Textbook diagrams

KLB Secondary Chemistry Form 3, Pages 119-157

SULPHUR AND ITS COMPOUNDS

Preparation of Sulphur(IV) Oxide
Physical and Chemical Properties of Sulphur(IV) Oxide
Bleaching Action of Sulphur(IV) Oxide
Reducing Action of Sulphur(IV) Oxide
Oxidising Action of Sulphur(IV) Oxide
Test for Sulphate and Sulphite Ions & Uses of SO2

By the end of the lesson, the learner should be able to:
Describe laboratory preparation of sulphur(IV) oxide. Set up apparatus for gas preparation and collection. Write balanced equations for the preparation reactions. Explain the drying and collection methods used.

Practical work: Experiment 4 - Preparation of SO2 using sodium sulphite and dilute HCl. Apparatus setup: Round-bottomed flask, delivery tube, gas jars. Collection: Downward delivery method. Testing: Using acidified potassium chromate(VI) paper. Alternative method: Copper + concentrated H2SO

Sodium sulphite, Dilute HCl, Round-bottomed flask, Delivery tubes, Gas jars, Concentrated H2SO4 for drying, Acidified potassium chromate(VI) paper
SO2 gas from previous preparation, Litmus papers, Universal indicator, 0.1M NaOH solution, Water, Test tubes, Safety equipment
Colored flower petals (red/blue), SO2 gas jars, Hand lens for observation, Charts comparing bleaching agents
SO2 gas, Acidified K2Cr2O7, Acidified KMnO4, Bromine water, Iron(III) chloride solution, Concentrated HNO3, Test tubes
SO2 gas jars, Magnesium ribbon, Deflagrating spoon, Hydrogen sulphide gas, Water droppers, Safety equipment
Sodium sulphate solution, Sodium sulphite solution, Barium chloride solution, Dilute HCl, Test tubes, Charts showing industrial uses

KLB Secondary Chemistry Form 4, Pages 170-171

SULPHUR AND ITS COMPOUNDS

Large-scale Manufacture of Sulphuric(VI) Acid - Contact Process
Properties of Concentrated Sulphuric(VI) Acid - Dehydrating Properties
Properties of Concentrated Sulphuric(VI) Acid - Oxidizing Properties
Properties of Concentrated Sulphuric(VI) Acid - Displacement Reactions
Reactions of Dilute Sulphuric(VI) Acid - With Metals
Reactions of Dilute Sulphuric(VI) Acid - With Carbonates

By the end of the lesson, the learner should be able to:
Describe the contact process for manufacturing H2SO Identify raw materials and conditions used. Explain the role of catalyst in the process. Draw flow diagrams of the contact process.

Study of flow diagram: Figure 12 - Contact process. Discussion: Raw materials (sulphur, air), burning sulphur to SO Purification: Electrostatic precipitation, drying with H2SO Catalytic chamber: V2O5 catalyst at 450°C, 2-3 atmospheres. Formation of oleum: H2S2O7. Safety and environmental considerations.

Flow chart diagrams, Charts showing industrial plant, Samples of catalyst (V2O5), Photographs of Thika chemical plant, Calculator for percentage calculations
Concentrated H2SO4, Copper(II) sulphate crystals, Sucrose, Ethanol, KMnO4 solution, Test tubes, Beakers, Safety equipment, Fume cupboard
Copper foil, Zinc granules, Charcoal powder, Concentrated H2SO4, Acidified K2Cr2O7 paper, Lime water, Test tubes, Bunsen burner
Potassium nitrate crystals, Sodium chloride crystals, Concentrated H2SO4, Moist blue litmus paper, Concentrated ammonia, Test tubes, Bunsen burner
Magnesium ribbon, Zinc granules, Copper turnings, Dilute H2SO4, Test tubes, Burning splints, Reactivity series chart
Sodium carbonate, Zinc carbonate, Calcium carbonate, Copper(II) carbonate, Dilute H2SO4, Lime water, Test tubes

KLB Secondary Chemistry Form 4, Pages 179-181

SULPHUR AND ITS COMPOUNDS
CHLORINE AND ITS COMPOUNDS
CHLORINE AND ITS COMPOUNDS
CHLORINE AND ITS COMPOUNDS
CHLORINE AND ITS COMPOUNDS

Reactions of Dilute Sulphuric(VI) Acid - With Oxides and Hydroxides
Hydrogen Sulphide - Preparation and Physical Properties
Chemical Properties of Hydrogen Sulphide
Pollution Effects and Summary
Introduction and Preparation of Chlorine
Physical Properties of Chlorine
Chemical Properties of Chlorine - Reaction with Water
Chemical Properties of Chlorine - Reaction with Metals
Chemical Properties of Chlorine - Reaction with Non-metals
Oxidising Properties of Chlorine
Reaction of Chlorine with Alkali Solutions
Oxidising Properties - Displacement Reactions
Test for Chloride Ions
Uses of Chlorine and its Compounds
Hydrogen Chloride - Laboratory Preparation
Chemical Properties of Hydrogen Chloride
Large-scale Manufacture of Hydrochloric Acid
Uses of Hydrochloric Acid
Environmental Pollution by Chlorine Compounds and Summary

By the end of the lesson, the learner should be able to:
Investigate reactions of dilute H2SO4 with metal oxides and hydroxides. Identify neutralization reactions. Explain formation of insoluble sulphates. Write equations for acid-base reactions.
Investigate reactions of chlorine with non-metals. Demonstrate reaction with phosphorus and hydrogen. Write equations for non-metal chloride formation. Explain the vigorous nature of these reactions.

Practical work: Experiment 13 - Reactions with magnesium oxide, zinc oxide, copper(II) oxide, lead(II) oxide, sodium hydroxide. Recording observations in Table 1 Discussion: Salt and water formation, immediate stopping with lead(II) oxide due to insoluble PbSO Acid-base neutralization concept.
Practical work: Experiment 6.5 - Warming red phosphorus and lowering into chlorine. Demonstration: Burning hydrogen jet in chlorine. Observations: White fumes of phosphorus chlorides, hydrogen chloride formation. Writing equations: P4 + 6Cl2 → 4PCl3, H2 + Cl2 → 2HCl. Discussion: Formation of covalent chlorides.

Metal oxides (MgO, ZnO, CuO, PbO), NaOH solution, 2M H2SO4, Test tubes, Bunsen burner for warming
Iron(II) sulphide, Dilute HCl, Apparatus for gas generation, Anhydrous CaCl2, Gas jars, Safety equipment, Fume cupboard
H2S gas, Bromine water, Iron(III) chloride, KMnO4, K2Cr2O7, Metal salt solutions, Test tubes, Droppers
Charts showing pollution effects, Photographs of acid rain damage, Environmental data, Summary charts of reactions, Industrial pollution control diagrams
Manganese(IV) oxide, Concentrated HCl, Gas collection apparatus, Water, Concentrated H2SO4, Blue litmus paper, Gas jars
Preserved chlorine gas, Water trough, Gas jars, Observation tables, Safety equipment
Chlorine gas, Distilled water, Blue and red litmus papers, Colored flower petals, Gas jars, Boiling tubes
Magnesium ribbon, Iron wire, Chlorine gas, Deflagrating spoon, Combustion tube, Anhydrous CaCl2, Gas jars
Red phosphorus, Hydrogen gas, Chlorine gas, Deflagrating spoon, Gas jars, Bunsen burner, Safety equipment
Sodium sulphite solution, Barium nitrate, Lead nitrate, Hydrogen sulphide gas, Aqueous ammonia, Chlorine gas, Test tubes
Sodium hydroxide solutions (dilute cold, concentrated hot), Chlorine gas, Beakers, Bunsen burner, Thermometer
Potassium bromide solution, Potassium iodide solution, Chlorine gas, Test tubes, Observation charts
Sodium chloride, Concentrated H2SO4, Lead(II) nitrate solution, Aqueous ammonia, Glass rod, Test tubes, Bunsen burner
Charts showing industrial uses, Samples of bleaching agents, PVC materials, Photographs of water treatment plants, Industrial application diagrams
Rock salt (NaCl), Concentrated H2SO4, Gas collection apparatus, Ammonia solution, Litmus papers, Water trough, Gas jars
Distilled water, Filter funnel, Metals (Zn, Fe, Mg, Cu), NaOH solution, Carbonates, Lead nitrate, Methylbenzene, Indicators
Flow diagrams, Industrial photographs, Glass beads samples, Charts showing electrolysis processes, Safety equipment models
Samples of rusted and cleaned metals, Photographic materials, pH control charts, Industrial application videos, Water treatment diagrams
Environmental pollution charts, Ozone layer diagrams, DDT restriction documents, PVC waste samples, NEMA guidelines, Summary charts of reactions

KLB Secondary Chemistry Form 4, Pages 186-187
KLB Secondary Chemistry Form 4, Pages 201