ACIDS, BASES AND SALTS

Definition of Acids

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

In groups, learners are guided to:
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

KLB Secondary Chemistry Form 4, Pages 1-3

ACIDS, BASES AND SALTS

Strength of Acids
Definition of Bases
Strength of Bases

By the end of the lesson, the learner should be able to:
- Compare strengths of acids using pH values
-Determine strengths of acids by comparing their electrical conductivity
-Classify acids as either strong or weak
-Explain complete and partial dissociation of acids

In groups, learners are guided to:
Class experiment: Test pH of 2M HCl and 2M ethanoic acid using universal indicator. Set up electrical conductivity apparatus with both acids. Record milliammeter readings. Compare results and explain in terms of hydrogen ion concentration. Discuss strong vs weak acid definitions.

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

KLB Secondary Chemistry Form 4, Pages 3-5

ACIDS, BASES AND SALTS

Acid-Base Reactions
Effect of Solvent on Acids
Effect of Solvent on Bases
Amphoteric Oxides and Hydroxides

By the end of the lesson, the learner should be able to:
- Write equations for acid-base reactions
-Explain neutralization process
-Identify products of acid-base reactions
-Demonstrate formation of salt and water

In groups, learners are guided to:
Q/A: Review acid and base definitions. Demonstrate neutralization reactions: HCl + NaOH, H₂SO₄ + Ca(OH)₂, HNO₃ + KOH. Write molecular and ionic equations. Explain H⁺ + OH⁻ → H₂O. Discuss salt formation. Use indicators to show neutralization point.

Various acids and bases from previous lessons, indicators, beakers, measuring cylinders, stirring rods
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

KLB Secondary Chemistry Form 4, Pages 6-7

ACIDS, BASES AND SALTS

Definition of Salts and Precipitation
Solubility of Chlorides, Sulphates and Sulphites

By the end of the lesson, the learner should be able to:
- Define a salt as an ionic compound
-Define a precipitate
-Investigate precipitation reactions
-Write ionic equations showing formation of precipitates

In groups, learners are guided to:
Q/A: Review salt definition from Book 2. Demonstrate precipitation: Add sodium carbonate to solutions containing Mg²⁺, Ca²⁺, Zn²⁺, Al³⁺, Cu²⁺, Fe²⁺, Ba²⁺, Pb²⁺ ions. Record observations. Write ionic equations for precipitate formation. Explain why Fe³⁺ and Al³⁺ give different results.

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

KLB Secondary Chemistry Form 4, Pages 11-14

ACIDS, BASES AND SALTS

Complex Ions Formation

By the end of the lesson, the learner should be able to:
- Explain formation of complex ions
-Investigate reactions with excess sodium hydroxide and ammonia
-Identify metal ions that form complex ions
-Write equations for complex ion formation

In groups, learners are guided to:
Class experiment: Add NaOH dropwise then in excess to Mg²⁺, Ca²⁺, Zn²⁺, Al³⁺, Cu²⁺, Fe²⁺, Fe³⁺, Pb²⁺ solutions. Repeat with NH₃ solution. Record observations showing precipitate formation and dissolution. Write equations for complex ion formation: [Zn(OH)₄]²⁻, [Al(OH)₄]⁻, [Pb(OH)₄]²⁻, [Zn(NH₃)₄]²⁺, [Cu(NH₃)₄]²⁺.

2M NaOH, 2M NH₃ solution, 0.5M salt solutions, test tubes, droppers

KLB Secondary Chemistry Form 4, Pages 15-16

ACIDS, BASES AND SALTS

Solubility and Saturated Solutions
Effect of Temperature on Solubility

By the end of the lesson, the learner should be able to:
- Define the term solubility
-Determine solubility of a given salt at room temperature
-Calculate mass of solute and solvent
-Express solubility in different units

In groups, learners are guided to:
Class experiment: Weigh evaporating dish and watch glass. Measure 20cm³ saturated KNO₃ solution. Record temperature. Evaporate to dryness carefully. Calculate masses of solute, solvent, and solution. Determine solubility per 100g water and in moles per litre. Discuss definition and significance.

Saturated KNO₃ solution, evaporating dish, watch glass, measuring cylinder, thermometer, balance, heating source
KClO₃, measuring cylinders, thermometer, burette, boiling tubes, heating source, graph paper

KLB Secondary Chemistry Form 4, Pages 16-18

ACIDS, BASES AND SALTS

Solubility Curves and Applications

By the end of the lesson, the learner should be able to:
- Plot solubility curves for various salts
-Use solubility curves to determine mass of crystals formed
-Apply solubility curves to practical problems
-Compare solubility patterns of different salts

In groups, learners are guided to:
Using data from textbook, plot solubility curves for KNO₃, KClO₃, NaCl, CaSO₄. Calculate mass of crystals deposited when saturated solutions are cooled. Work through examples: KClO₃ cooled from 70°C to 30°C. Discuss applications in salt extraction and purification.

Graph paper, ruler, pencil, calculator, data tables from textbook

KLB Secondary Chemistry Form 4, Pages 20-21

ACIDS, BASES AND SALTS

Fractional Crystallization
Hardness of Water - Investigation

By the end of the lesson, the learner should be able to:
- Define fractional crystallization
-Apply knowledge of solubility curves in separation of salts
-Calculate masses of salts that crystallize
-Explain separation of salt mixtures

In groups, learners are guided to:
Work through separation problems using solubility data for KNO₃ and KClO₃ mixtures. Calculate which salt crystallizes first when cooled from 50°C to 20°C. Plot combined solubility curves. Discuss applications in Lake Magadi and Ngomeni salt works. Solve practice problems.

Calculator, graph paper, data tables, worked examples from textbook
Soap solution, burette, various salt solutions, conical flasks, distilled water, tap water, rainwater, heating source

KLB Secondary Chemistry Form 4, Pages 21-22

ACIDS, BASES AND SALTS

Types and Causes of Water Hardness
Effects of Hard Water

By the end of the lesson, the learner should be able to:
- Define temporary and permanent hardness
-Explain causes of temporary hardness
-Explain causes of permanent hardness
-Write equations for decomposition of hydrogen carbonates

In groups, learners are guided to:
Q/A: Review previous experiment results. Explain temporary hardness caused by Ca(HCO₃)₂ and Mg(HCO₃)₂. Write decomposition equations when boiled. Explain permanent hardness caused by CaSO₄, MgSO₄, Ca(NO₃)₂, Mg(NO₃)₂. Discuss why permanent hardness cannot be removed by boiling.

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 24-25

ACIDS, BASES AND SALTS

Methods of Removing Hardness I

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

In groups, learners are guided to:
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.

Hard water samples, heating source, soap solution, distillation apparatus diagram

KLB Secondary Chemistry Form 4, Pages 25-26

ACIDS, BASES AND SALTS
REACTION RATES AND REVERSIBLE REACTIONS

Methods of Removing Hardness II
Definition of Reaction Rate and Collision Theory

By the end of the lesson, the learner should be able to:
- Explain removal using sodium carbonate
-Describe ion exchange method
-Explain removal using calcium hydroxide and ammonia
-Write equations for all processes

In groups, learners are guided to:
Demonstrate addition of Na₂CO₃ to hard water - observe precipitation. Explain ion exchange using resin (NaX) showing Ca²⁺ + 2NaX → CaX₂ + 2Na⁺. Discuss regeneration with brine. Write equations for Ca(OH)₂ and NH₃ methods. Compare all methods for effectiveness and cost.

Na₂CO₃ solution, hard water samples, ion exchange resin diagram, Ca(OH)₂, NH₃ solution
Examples of fast/slow reactions, energy diagram templates, chalk/markers for diagrams

KLB Secondary Chemistry Form 4, Pages 25-26

REACTION RATES AND REVERSIBLE REACTIONS

Effect of Concentration on Reaction Rate
Change of Reaction Rate with Time

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

In groups, learners are guided to:
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

KLB Secondary Chemistry Form 4, Pages 65-67

REACTION RATES AND REVERSIBLE REACTIONS

Effect of Temperature on Reaction Rate

By the end of the lesson, the learner should be able to:
- Explain the effect of temperature on reaction rates
-Investigate temperature effects using sodium thiosulphate and HCl
-Plot graphs of time vs temperature and 1/time vs temperature
-Apply collision theory to explain temperature effects

In groups, learners are guided to:
Class experiment: Place 30cm³ of 0.15M Na₂S₂O₃ in flasks at room temp, 30°C, 40°C, 50°C, 60°C. Mark cross on paper under flask. Add 5cm³ of 2M HCl, time until cross disappears. Record in Table 3.4. Plot time vs temperature and 1/time vs temperature graphs. Explain: higher temperature → more kinetic energy → more effective collisions.

0.15M Na₂S₂O₃, 2M HCl, conical flasks, water baths at different temperatures, paper with cross marked, stopwatch, thermometers

KLB Secondary Chemistry Form 4, Pages 70-73

REACTION RATES AND REVERSIBLE REACTIONS

Effect of Surface Area on Reaction Rate
Effect of Catalysts on Reaction Rate

By the end of the lesson, the learner should be able to:
- Explain the effect of surface area on reaction rates
-Investigate reaction of marble chips vs marble powder with HCl
-Compare reaction rates using gas collection
-Relate particle size to surface area and collision frequency

In groups, learners are guided to:
Class experiment: React 2.5g marble chips with 50cm³ of 1M HCl, collect CO₂ gas using apparatus in Fig 3.10. Record gas volume every 30 seconds. Repeat with 2.5g marble powder. Record in Table 3.5. Plot both curves on same graph. Write equation: CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂. Explain: smaller particles → larger surface area → more collision sites → faster reaction.

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

KLB Secondary Chemistry Form 4, Pages 73-76

REACTION RATES AND REVERSIBLE REACTIONS

Effect of Light and Pressure on Reaction Rate

By the end of the lesson, the learner should be able to:
- Identify reactions affected by light
-Investigate effect of light on silver bromide decomposition
-Explain effect of pressure on gaseous reactions
-Give examples of photochemical reactions

In groups, learners are guided to:
Teacher demonstration: Mix KBr and AgNO₃ solutions to form AgBr precipitate. Divide into 3 test tubes: place one in dark cupboard, one on bench, one in direct sunlight. Observe color changes after 10 minutes. Write equations. Discuss photochemical reactions: photography, Cl₂ + H₂, photosynthesis. Explain pressure effects on gaseous reactions through compression.

0.1M KBr, 0.05M AgNO₃, test tubes, dark cupboard, direct light source, examples of photochemical reactions

KLB Secondary Chemistry Form 4, Pages 78-80

REACTION RATES AND REVERSIBLE REACTIONS

Reversible Reactions
Chemical Equilibrium

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

In groups, learners are guided to:
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

KLB Secondary Chemistry Form 4, Pages 78-80

REACTION RATES AND REVERSIBLE REACTIONS

Le Chatelier's Principle and Effect of Concentration
Effect of Pressure and Temperature on Equilibrium

By the end of the lesson, the learner should be able to:
- State Le Chatelier's Principle
-Explain effect of concentration changes on equilibrium position
-Investigate bromine water equilibrium with acid/base addition
-Apply Le Chatelier's Principle to predict equilibrium shifts

In groups, learners are guided to:
Experiment: Add 2M NaOH dropwise to 20cm³ bromine water until colorless. Then add 2M HCl until excess, observe color return. Write equation: Br₂ + H₂O ⇌ HBr + HBrO. Explain Le Chatelier's Principle: "When change applied to system at equilibrium, system moves to oppose that change." Demonstrate with chromate/dichromate equilibrium: CrO₄²⁻ + H⁺ ⇌ Cr₂O₇²⁻ + H₂O.

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

KLB Secondary Chemistry Form 4, Pages 82-84

REACTION RATES AND REVERSIBLE REACTIONS

Industrial Applications - Haber Process

By the end of the lesson, the learner should be able to:
- Apply equilibrium principles to Haber Process
-Explain optimum conditions for ammonia manufacture
-Calculate effect of temperature and pressure on yield
-Explain role of catalysts in industrial processes

In groups, learners are guided to:
Analyze Haber Process: N₂ + 3H₂ ⇌ 2NH₃ ΔH = -92 kJ/mol. Apply Le Chatelier's Principle: high pressure favors forward reaction (4 molecules → 2 molecules), low temperature favors exothermic forward reaction but slows rate. Explain optimum conditions: 450°C temperature, 200 atmospheres pressure, iron catalyst. Discuss removal of NH₃ to shift equilibrium right. Economic considerations.

Haber Process flow diagram, equilibrium data showing temperature/pressure effects on NH₃ yield, industrial catalyst information

KLB Secondary Chemistry Form 4, Pages 87-89

REACTION RATES AND REVERSIBLE REACTIONS
ELECTROCHEMISTRY
ELECTROCHEMISTRY

Industrial Applications - Contact Process
Redox Reactions and Oxidation Numbers
Oxidation Numbers in Naming and Redox Identification

By the end of the lesson, the learner should be able to:
- Apply equilibrium principles to Contact Process
-Explain optimum conditions for sulphuric acid manufacture
-Compare different industrial equilibrium processes
-Evaluate economic factors in industrial chemistry

In groups, learners are guided to:
Analyze Contact Process: 2SO₂ + O₂ ⇌ 2SO₃ ΔH = -197 kJ/mol. Apply principles: high pressure favors forward reaction (3 molecules → 2 molecules), low temperature favors exothermic reaction. Explain optimum conditions: 450°C, atmospheric pressure, V₂O₅ catalyst, 96% conversion. Compare with Haber Process. Discuss catalyst choice and economic factors.

Contact Process flow diagram, comparison table with Haber Process, catalyst effectiveness data
Iron filings, 1M CuSO₄, 1M FeSO₄, 2M NaOH, 20V H₂O₂, test tubes
Compound charts, calculators, student books, practice exercises

KLB Secondary Chemistry Form 4, Pages 89

ELECTROCHEMISTRY

Displacement Reactions - Metals and Halogens
Electrochemical Cells and Cell Diagrams
Standard Electrode Potentials

By the end of the lesson, the learner should be able to:
Explain displacement reactions using electron transfer
- Arrange metals and halogens by reactivity
- Predict displacement reactions
- Compare oxidizing powers of halogens

In groups, learners are guided to:
Experiment 4.3: Metal displacement reactions - systematic testing
- Experiment 4.4: Halogen displacement (FUME CUPBOARD)
- Tabulate results and arrange by reactivity

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

KLB Secondary Chemistry Form 4, Pages 116-122

ELECTROCHEMISTRY

Calculating Cell EMF and Predicting Reactions
Types of Electrochemical Cells
Electrolysis of Aqueous Solutions I
Electrolysis of Aqueous Solutions II

By the end of the lesson, the learner should be able to:
Calculate EMF using standard electrode potentials
- Predict reaction spontaneity using EMF
- Solve numerical problems on cell EMF
- Apply EMF calculations practically

In groups, learners are guided to:
Worked examples: Calculate EMF for various cells
- Practice EMF calculations
- Exercise 4.2 & 4.3: Cell EMF and reaction feasibility problems
- Distinguish spontaneous from non-spontaneous reactions

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

KLB Secondary Chemistry Form 4, Pages 133-137

ELECTROCHEMISTRY

Effect of Electrode Material on Electrolysis

By the end of the lesson, the learner should be able to:
Compare inert vs reactive electrodes
- Investigate electrode dissolution
- Explain electrode selection importance
- Analyze copper purification process

In groups, learners are guided to:
Experiment 4.9: Electrolysis of CuSO₄ with carbon vs copper electrodes
- Weigh electrodes before/after
- Observe color changes
- Discussion on electrode effects

Copper and carbon electrodes, 3M CuSO₄ solution, accurate balance, beakers, connecting wires

KLB Secondary Chemistry Form 4, Pages 141-148

ELECTROCHEMISTRY

Factors Affecting Electrolysis
Applications of Electrolysis I

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

In groups, learners are guided to:
Review electrochemical series and discharge order
- Analysis of concentration effects on product formation
- Summary of all factors affecting electrolysis
- Practice prediction problems

Electrochemical series chart, summary tables, practice exercises, student books
Iron nails, copper electrodes, CuSO₄ solution, power supply, industrial process diagrams

KLB Secondary Chemistry Form 4, Pages 153-155

ELECTROCHEMISTRY

Applications of Electrolysis II

By the end of the lesson, the learner should be able to:
Describe manufacture of NaOH and Cl₂ from brine
- Explain mercury cell operation
- Analyze industrial electrolysis processes
- Discuss environmental considerations

In groups, learners are guided to:
Study mercury cell for NaOH production
- Flow chart analysis of industrial processes
- Discussion on applications and environmental impact
- Purification of metals

Flow charts, mercury cell diagrams, environmental impact data, industrial case studies

KLB Secondary Chemistry Form 4, Pages 155-157

ELECTROCHEMISTRY

Faraday's Laws and Quantitative Electrolysis
Electrolysis Calculations I

By the end of the lesson, the learner should be able to:
State Faraday's laws of electrolysis
- Define Faraday constant
- Calculate mass deposited in electrolysis
- Relate electricity to amount of substance

In groups, learners are guided to:
Experiment 4.10: Quantitative electrolysis of CuSO₄
- Measure mass vs electricity passed
- Calculate Faraday constant
- Verify Faraday's laws

Accurate balance, copper electrodes, CuSO₄ solution, ammeter, timer, calculators
Calculators, worked examples, practice problems, gas volume data, Faraday constant

KLB Secondary Chemistry Form 4, Pages 161-164

ELECTROCHEMISTRY

Electrolysis Calculations II
Advanced Applications and Problem Solving

By the end of the lesson, the learner should be able to:
Determine charge on ions from electrolysis data
- Calculate current-time relationships
- Solve complex multi-step problems
- Apply concepts to industrial situations

In groups, learners are guided to:
Complex problems: Determine ionic charges
- Current-time-mass relationships
- Multi-step calculations
- Industrial calculation examples

Calculators, complex problem sets, industrial data, student books
Past papers, comprehensive problem sets, industrial case studies, calculators

KLB Secondary Chemistry Form 4, Pages 161-164

METALS

Chemical Properties I - Reaction with Air
Chemical Properties II - Reaction with Water

By the end of the lesson, the learner should be able to:
Investigate metal reactions with air and oxygen
- Write balanced equations for metal oxidation
- Compare reactivity patterns
- Explain tarnishing and oxide formation

In groups, learners are guided to:
Experiment 5.1: Heat metals in air - sodium, aluminium, zinc, iron, copper
- Observe color changes and products
- Record observations in Table 5.3
- Write oxidation equations

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

KLB Secondary Chemistry Form 4, Pages 152-154

METALS

Chemical Properties III - Reaction with Chlorine

By the end of the lesson, the learner should be able to:
Investigate metal reactions with chlorine gas
- Write equations for chloride formation
- Compare reaction vigor
- Observe product characteristics

In groups, learners are guided to:
Experiment 5.3: React hot metals with chlorine gas (FUME CUPBOARD)
- Observe color changes and fume formation
- Record all observations
- Write balanced equations

Chlorine gas, gas jars, metal samples, tongs, deflagrating spoons, fume cupboard, safety equipment

KLB Secondary Chemistry Form 4, Pages 156-157

METALS

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:
Test metal reactions with dilute and concentrated acids
- Compare reaction patterns
- Write chemical equations
- Explain passivation effects

In groups, learners are guided to:
Experiment 5.4: Test metals with various acids - HCl, HNO₃, H₂SO₄
- Use Table 5.5 for systematic recording
- Observe gas evolution
- Discuss passivation

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 157-158

METALS

Uses of Metals II - Zinc, Copper and Iron
Steel Types and Alloys

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

In groups, learners are guided to:
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

KLB Secondary Chemistry Form 4, Pages 159-161

METALS
ORGANIC CHEMISTRY II

Environmental Effects of Metal Extraction
Introduction to Alkanols and Nomenclature

By the end of the lesson, the learner should be able to:
Identify environmental impacts of mining
- Explain pollution from metal extraction
- Describe waste management strategies
- Discuss NEMA regulations in Kenya

In groups, learners are guided to:
Analysis of mining environmental impact
- Air, water, and land pollution from extraction
- Waste management and slag utilization
- NEMA role and regulations

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

KLB Secondary Chemistry Form 4, Pages 161-162

ORGANIC CHEMISTRY II

Isomerism in Alkanols
Laboratory Preparation of Ethanol
Industrial Preparation and Physical Properties

By the end of the lesson, the learner should be able to:
Explain positional and chain isomerism
- Draw isomers of given alkanols
- Name different isomeric forms
- Classify isomers as primary, secondary, or tertiary

In groups, learners are guided to:
Study positional isomerism examples (propan-1-ol vs propan-2-ol)
- Practice drawing chain isomers
- Exercises on isomer identification and naming
- Discussion on structural differences

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

KLB Secondary Chemistry Form 4, Pages 170-171

ORGANIC CHEMISTRY II

Chemical Properties of Alkanols I
Chemical Properties of Alkanols II
Uses of Alkanols and Health Effects

By the end of the lesson, the learner should be able to:
Test reactions of ethanol with various reagents
- Write equations for ethanol reactions
- Identify products formed
- Explain reaction mechanisms

In groups, learners are guided to:
Experiment 6.2: Test ethanol with burning, universal indicator, sodium metal, acids
- Record observations in Table 6.4
- Write balanced equations
- Discuss reaction types

Ethanol, sodium metal, universal indicator, concentrated H₂SO₄, ethanoic acid, test tubes
Acidified potassium chromate/manganate, ethanoic acid, concentrated H₂SO₄, heating apparatus
Charts showing alkanol uses, health impact data, methylated spirit samples, discussion materials

KLB Secondary Chemistry Form 4, Pages 173-175

ORGANIC CHEMISTRY II

Introduction to Alkanoic Acids
Laboratory Preparation of Ethanoic Acid

By the end of the lesson, the learner should be able to:
Define alkanoic acids and functional group
- Apply nomenclature rules
- Draw structural formulae
- Compare with alkanols

In groups, learners are guided to:
Study carboxyl group (-COOH) structure
- Practice naming using IUPAC rules
- Complete Table 6.5 and 6.6
- Compare functional groups of alkanols and acids

Alkanoic acid structure charts, Table 6.5 and 6.6, molecular models, student books
Ethanol, KMnO₄, concentrated H₂SO₄, distillation apparatus, thermometer, round-bottom flask

KLB Secondary Chemistry Form 4, Pages 177-179

ORGANIC CHEMISTRY II

Physical and Chemical Properties of Alkanoic Acids
Esterification and Uses of Alkanoic Acids

By the end of the lesson, the learner should be able to:
Investigate chemical reactions of ethanoic acid
- Test with various reagents
- Write chemical equations
- Analyze acid strength

In groups, learners are guided to:
Experiment following Table 6.8: Test ethanoic acid with indicators, metals, carbonates, bases
- Record observations
- Write equations
- Discuss weak acid behavior

2M ethanoic acid, universal indicator, Mg strip, Na₂CO₃, NaOH, phenolphthalein, test tubes
Ethanoic acid, ethanol, concentrated H₂SO₄, test tubes, heating apparatus, cold water

KLB Secondary Chemistry Form 4, Pages 180-182

ORGANIC CHEMISTRY II

Introduction to Detergents and Soap Preparation
Mode of Action of Soap and Hard Water Effects

By the end of the lesson, the learner should be able to:
Define detergents and classify types
- Explain saponification process
- Prepare soap in laboratory
- Compare soapy and soapless detergents

In groups, learners are guided to:
Study soap vs soapless detergent differences
- Experiment 6.5: Saponify castor oil with NaOH
- Add salt for salting out
- Test soap formation

Castor oil, 4M NaOH, NaCl, evaporating dish, water bath, stirring rod, filter paper
Soap samples, distilled water, hard water (CaCl₂/MgSO₄ solutions), test tubes, demonstration materials

KLB Secondary Chemistry Form 4, Pages 183-186

ORGANIC CHEMISTRY II

Soapless Detergents and Environmental Effects

By the end of the lesson, the learner should be able to:
Explain soapless detergent preparation
- Compare advantages/disadvantages
- Discuss environmental impact
- Analyze pollution effects

In groups, learners are guided to:
Study alkylbenzene sulphonate preparation
- Compare Table 6.9 - soap vs soapless
- Discussion on eutrophication and biodegradability
- Environmental awareness

Flow charts of detergent manufacture, Table 6.9, environmental impact data, sample detergents

KLB Secondary Chemistry Form 4, Pages 188-191

ORGANIC CHEMISTRY II

Introduction to Polymers and Addition Polymerization
Addition Polymers - Types and Properties

By the end of the lesson, the learner should be able to:
Define polymers, monomers, and polymerization
- Explain addition polymerization
- Draw polymer structures
- Calculate polymer properties

In groups, learners are guided to:
Study polymer concept and terminology
- Practice drawing addition polymers from monomers
- Examples: polyethene, polypropene, PVC
- Calculate molecular masses

Polymer samples, monomer structure charts, molecular models, calculators, polymer formation diagrams
Various polymer samples, structure identification exercises, calculation worksheets, Table 6.10

KLB Secondary Chemistry Form 4, Pages 191-195

ORGANIC CHEMISTRY II

Condensation Polymerization and Natural Polymers
Polymer Properties and Applications

By the end of the lesson, the learner should be able to:
Explain condensation polymerization
- Compare with addition polymerization
- Study natural polymers
- Analyze nylon formation

In groups, learners are guided to:
Study nylon 6,6 formation from diamine and dioic acid
- Natural polymers: starch, protein, rubber
- Vulcanization process
- Compare synthetic vs natural

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 197-200

ORGANIC CHEMISTRY II
RADIOACTIVITY

Comprehensive Problem Solving and Integration
Introduction, Nuclear Stability and Types of Radioactivity

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

In groups, learners are guided to:
Worked examples on organic synthesis
- Problem-solving on isomers, reactions, polymers
- Integration of all unit concepts
- Practice examination-style questions

Comprehensive problem sets, past examination papers, calculators, organic chemistry summary charts
Periodic table, atomic structure charts, Table 7.1, nuclear stability diagrams

KLB Secondary Chemistry Form 4, Pages 167-201

RADIOACTIVITY

Types of Radiation and Their Properties
Radioactive Decay and Half-Life Concept
Half-Life Calculations and Problem Solving

By the end of the lesson, the learner should be able to:
Identify alpha, beta, and gamma radiations
- Compare penetrating abilities and ionizing power
- Explain electric field deflection
- Analyze safety implications

In groups, learners are guided to:
Study alpha (α), beta (β), gamma (γ) characteristics
- Figure 7.2 - penetrating power demonstration
- Figure 7.3 - electric field effects
- Discussion on radiation protection and detection

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

KLB Secondary Chemistry Form 4, Pages 201-204

RADIOACTIVITY

Nuclear Reactions and Equations
Radioactive Decay Series and Sequential Reactions
Nuclear Fission and Chain Reactions

By the end of the lesson, the learner should be able to:
Write balanced nuclear equations
- Apply conservation laws for mass and atomic numbers
- Explain alpha and beta emission effects
- Balance complex nuclear reactions

In groups, learners are guided to:
Practice writing nuclear equations for alpha emission
- Study beta emission examples
- Apply mass and atomic number conservation
- Balance various nuclear reactions with missing nuclides

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

KLB Secondary Chemistry Form 4, Pages 205-207

RADIOACTIVITY

Nuclear Fusion and Energy Comparisons
Medical and Diagnostic Applications

By the end of the lesson, the learner should be able to:
Define nuclear fusion process
- Compare fusion with fission processes
- Write fusion equations
- Explain stellar energy production and fusion applications

In groups, learners are guided to:
Study hydrogen fusion examples
- Compare fusion vs fission characteristics and energy yields
- Stellar fusion processes
- Hydrogen bomb vs nuclear reactor principles

Fusion reaction diagrams, comparison tables, stellar fusion charts, energy comparison data
Medical radioisotope charts, treatment procedure diagrams, diagnostic equipment images, case studies

KLB Secondary Chemistry Form 4, Pages 207-208

RADIOACTIVITY

Industrial, Agricultural and Dating Applications
Radiation Hazards and Environmental Impact

By the end of the lesson, the learner should be able to:
Explain industrial leak detection
- Describe agricultural monitoring techniques
- Discuss carbon-14 dating principles
- Analyze food preservation methods

In groups, learners are guided to:
Study leak detection using short half-life isotopes
- Carbon-14 dating of archaeological materials
- Phosphorus tracking in agriculture
- Gamma radiation food preservation

Carbon dating examples, agricultural application charts, industrial use diagrams, food preservation data
Accident case studies, environmental impact data, radiation exposure charts, contamination maps

KLB Secondary Chemistry Form 4, Pages 208-209

RADIOACTIVITY

Safety Measures and International Control
Half-Life Problem Solving and Graph Analysis
Nuclear Equations and Conservation Laws

By the end of the lesson, the learner should be able to:
Explain radiation protection principles
- Describe proper storage and disposal methods
- Discuss IAEA role and standards
- Analyze monitoring and control systems

In groups, learners are guided to:
Study IAEA guidelines and international cooperation
- Radiation protection protocols and ALARA principle
- Safe storage, transport and disposal methods
- Environmental monitoring systems

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

KLB Secondary Chemistry Form 4, Pages 209-210