REACTION RATES AND REVERSIBLE REACTIONS

Definition of Reaction Rate and Collision Theory

By the end of the lesson, the learner should be able to:
- Define rate of reaction and explain the term activation energy
-Describe collision theory and explain why not all collisions result in products
-Draw energy diagrams showing activation energy
-Explain how activation energy affects reaction rates

Q/A: Compare speeds of different reactions (precipitation vs rusting). Define reaction rate as "measure of how much reactants are consumed or products formed per unit time." Introduce collision theory: particles must collide with minimum energy (activation energy) for successful reaction. Draw energy diagram showing activation energy barrier. Discuss factors affecting collision frequency and energy.

Examples of fast/slow reactions, energy diagram templates, chalk/markers for diagrams

KLB Secondary Chemistry Form 4, Pages 64-65

REACTION RATES AND REVERSIBLE REACTIONS

Definition of Reaction Rate and Collision Theory

By the end of the lesson, the learner should be able to:
- Define rate of reaction and explain the term activation energy
-Describe collision theory and explain why not all collisions result in products
-Draw energy diagrams showing activation energy
-Explain how activation energy affects reaction rates

Q/A: Compare speeds of different reactions (precipitation vs rusting). Define reaction rate as "measure of how much reactants are consumed or products formed per unit time." Introduce collision theory: particles must collide with minimum energy (activation energy) for successful reaction. Draw energy diagram showing activation energy barrier. Discuss factors affecting collision frequency and energy.

Examples of fast/slow reactions, energy diagram templates, chalk/markers for diagrams

KLB Secondary Chemistry Form 4, Pages 64-65

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
- Describe methods used to measure rate of reaction
-Investigate how reaction rate changes as reaction proceeds
-Plot graphs of volume of gas vs time
-Calculate average rates at different time intervals

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.
Class experiment: React 2cm magnesium ribbon with 100cm³ of 0.5M HCl in conical flask. Collect H₂ gas in graduated syringe as in Fig 3.4. Record gas volume every 30 seconds for 5 minutes in Table 3.2. Plot volume vs time graph. Calculate average rates between time intervals. Explain why rate decreases as reactants are consumed.

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
KLB Secondary Chemistry Form 4, Pages 67-70

REACTION RATES AND REVERSIBLE REACTIONS

Change of Reaction Rate with Time

By the end of the lesson, the learner should be able to:
- Describe methods used to measure rate of reaction
-Investigate how reaction rate changes as reaction proceeds
-Plot graphs of volume of gas vs time
-Calculate average rates at different time intervals

Class experiment: React 2cm magnesium ribbon with 100cm³ of 0.5M HCl in conical flask. Collect H₂ gas in graduated syringe as in Fig 3.4. Record gas volume every 30 seconds for 5 minutes in Table 3.2. Plot volume vs time graph. Calculate average rates between time intervals. Explain why rate decreases as reactants are consumed.

0.5M HCl, magnesium ribbon, conical flask, gas collection apparatus, graduated syringe, stopwatch, graph paper

KLB Secondary Chemistry Form 4, Pages 67-70

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

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

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

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

KLB Secondary Chemistry Form 4, Pages 73-76

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
- Explain effects of suitable catalysts on reaction rates
-Investigate decomposition of hydrogen peroxide with and without catalyst
-Define catalyst and explain how catalysts work
-Compare activation energies in catalyzed vs uncatalyzed reactions

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.
Class experiment: Decompose 5cm³ of 20-volume H₂O₂ in 45cm³ water without catalyst, collect O₂ gas. Repeat adding 2g MnO₂ powder. Record gas volumes as in Fig 3.12. Compare rates and final mass of MnO₂. Write equation: 2H₂O₂ → 2H₂O + O₂. Define catalyst and explain how it lowers activation energy. Show energy diagrams for both pathways.

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
KLB Secondary Chemistry Form 4, Pages 76-78

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

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

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

KLB Secondary Chemistry Form 4, Pages 78-80

REACTION RATES AND REVERSIBLE REACTIONS

Reversible Reactions

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

KLB Secondary Chemistry Form 4, Pages 78-80

REACTION RATES AND REVERSIBLE REACTIONS

Chemical Equilibrium

By the end of the lesson, the learner should be able to:
- Explain chemical equilibrium
-Define dynamic equilibrium
-Investigate acid-base equilibrium using indicators
-Explain why equilibrium appears static but is actually dynamic

Experiment: Add 0.5M NaOH to 2cm³ in boiling tube with universal indicator. Add 0.5M HCl dropwise until green color (neutralization point). Continue adding base then acid alternately, observe color changes. Explain equilibrium as state where forward and backward reaction rates are equal. Use NH₄Cl ⇌ NH₃ + HCl example to show dynamic nature. Introduce equilibrium symbol ⇌.

0.5M NaOH, 0.5M HCl, universal indicator, boiling tubes, droppers, examples of equilibrium systems

KLB Secondary Chemistry Form 4, Pages 80-82

REACTION RATES AND REVERSIBLE REACTIONS

Le Chatelier's Principle and Effect of Concentration

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

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

KLB Secondary Chemistry Form 4, Pages 82-84

REACTION RATES AND REVERSIBLE REACTIONS

Effect of Pressure and Temperature on Equilibrium

By the end of the lesson, the learner should be able to:
- Explain effect of pressure changes on equilibrium
-Explain effect of temperature changes on equilibrium
-Investigate NO₂/N₂O₄ equilibrium with temperature
-Apply Le Chatelier's Principle to industrial processes

Teacher demonstration: React copper turnings with concentrated HNO₃ to produce NO₂ gas in test tube. Heat and cool the tube, observe color changes: brown ⇌ pale yellow representing 2NO₂ ⇌ N₂O₄. Explain pressure effects using molecule count. Show Table 3.7 with pressure effects. Discuss temperature effects: heating favors endothermic direction, cooling favors exothermic direction. Use Table 3.8.

Copper turnings, concentrated HNO₃, test tubes, heating source, ice bath, gas collection apparatus, safety equipment

KLB Secondary Chemistry Form 4, Pages 84-87

REACTION RATES AND REVERSIBLE REACTIONS

Effect of Pressure and Temperature on Equilibrium

By the end of the lesson, the learner should be able to:
- Explain effect of pressure changes on equilibrium
-Explain effect of temperature changes on equilibrium
-Investigate NO₂/N₂O₄ equilibrium with temperature
-Apply Le Chatelier's Principle to industrial processes

Teacher demonstration: React copper turnings with concentrated HNO₃ to produce NO₂ gas in test tube. Heat and cool the tube, observe color changes: brown ⇌ pale yellow representing 2NO₂ ⇌ N₂O₄. Explain pressure effects using molecule count. Show Table 3.7 with pressure effects. Discuss temperature effects: heating favors endothermic direction, cooling favors exothermic direction. Use Table 3.8.

Copper turnings, concentrated HNO₃, test tubes, heating source, ice bath, gas collection apparatus, safety equipment

KLB Secondary Chemistry Form 4, Pages 84-87

REACTION RATES AND REVERSIBLE REACTIONS

Industrial Applications - Haber Process
Industrial Applications - Contact 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
- Apply equilibrium principles to Contact Process
-Explain optimum conditions for sulphuric acid manufacture
-Compare different industrial equilibrium processes
-Evaluate economic factors in industrial chemistry

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.
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.

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 87-89
KLB Secondary Chemistry Form 4, Pages 89

REACTION RATES AND REVERSIBLE REACTIONS

Industrial Applications - Contact Process

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

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

KLB Secondary Chemistry Form 4, Pages 89

ELECTROCHEMISTRY

Redox Reactions and Oxidation Numbers
Oxidation Numbers in Naming and Redox Identification

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

KLB Secondary Chemistry Form 4, Pages 108-116

ELECTROCHEMISTRY

Displacement Reactions - Metals and Halogens

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

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

KLB Secondary Chemistry Form 4, Pages 116-122

ELECTROCHEMISTRY

Electrochemical Cells and Cell Diagrams
Standard Electrode Potentials
Calculating Cell EMF and Predicting Reactions

By the end of the lesson, the learner should be able to:
Define electrode potential and EMF
- Describe electrochemical cell components
- Draw cell diagrams using correct notation
- Explain electron flow and salt bridge function
Define standard electrode potential
- Describe standard hydrogen electrode
- List standard conditions
- Use electrode potential tables effectively

Experiment 4.5: Set up Zn/Cu cell and other metal combinations
- Measure EMF values
- Practice writing cell notation
- Learn conventional representation methods
Study standard hydrogen electrode setup
- Discussion of standard conditions (25°C, 1M, 1 atm)
- Introduction to electrode potential series
- Practice reading potential tables

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

KLB Secondary Chemistry Form 4, Pages 123-128
KLB Secondary Chemistry Form 4, Pages 129-133

ELECTROCHEMISTRY

Types of Electrochemical Cells

By the end of the lesson, the learner should be able to:
Describe functioning of primary and secondary cells
- Compare different cell types
- Explain fuel cell operation
- State applications of electrochemical cells

Study dry cell (Le Clanche) and lead-acid accumulator
- Hydrogen-oxygen fuel cell operation
- Compare cell types and applications
- Discussion on advantages/disadvantages

Cell diagrams, sample batteries, charts showing cell applications

KLB Secondary Chemistry Form 4, Pages 138-141

ELECTROCHEMISTRY

Electrolysis of Aqueous Solutions I

By the end of the lesson, the learner should be able to:
Define electrolysis and preferential discharge
- Investigate electrolysis of dilute sodium chloride
- Compare dilute vs concentrated solution effects
- Test products formed

Experiment 4.6(a): Electrolysis of dilute NaCl
- Experiment 4.6(b): Electrolysis of brine
- Test gases evolved
- Compare results and explain differences

Dilute and concentrated NaCl solutions, carbon electrodes, gas collection tubes, test equipment

KLB Secondary Chemistry Form 4, Pages 141-146

ELECTROCHEMISTRY

Electrolysis of Aqueous Solutions II

By the end of the lesson, the learner should be able to:
Analyze electrolysis of dilute sulphuric acid
- Investigate electrolysis of metal salt solutions
- Measure gas volumes and ratios
- Apply theoretical predictions

Experiment 4.7: Electrolysis of dilute H₂SO₄ using U-tube
- Experiment 4.8: Electrolysis of MgSO₄ solution
- Collect and measure gases
- Analyze volume ratios

U-tube apparatus, 2M H₂SO₄, 0.5M MgSO₄, platinum/carbon electrodes, gas syringes

KLB Secondary Chemistry Form 4, Pages 146-148

ELECTROCHEMISTRY

Effect of Electrode Material on Electrolysis
Factors Affecting 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
Identify factors affecting preferential discharge
- Explain electrochemical series influence
- Discuss concentration and electrode effects
- Predict electrolysis products

Experiment 4.9: Electrolysis of CuSO₄ with carbon vs copper electrodes
- Weigh electrodes before/after
- Observe color changes
- Discussion on electrode effects
Review electrochemical series and discharge order
- Analysis of concentration effects on product formation
- Summary of all factors affecting electrolysis
- Practice prediction problems

Copper and carbon electrodes, 3M CuSO₄ solution, accurate balance, beakers, connecting wires
Electrochemical series chart, summary tables, practice exercises, student books

KLB Secondary Chemistry Form 4, Pages 141-148
KLB Secondary Chemistry Form 4, Pages 153-155

ELECTROCHEMISTRY

Applications of Electrolysis I

By the end of the lesson, the learner should be able to:
Describe electrolytic extraction of reactive metals
- Explain electroplating process
- Apply electrolysis principles to metal coating
- Design electroplating setup

Discussion: Extraction of Na, Mg, Al by electrolysis
- Practical: Electroplate iron nail with copper
- Calculate plating requirements
- Industrial applications

Iron nails, copper electrodes, CuSO₄ solution, power supply, industrial process diagrams

KLB Secondary Chemistry Form 4, Pages 155-157

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

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

Applications of Electrolysis II
Faraday's Laws and Quantitative Electrolysis

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
State Faraday's laws of electrolysis
- Define Faraday constant
- Calculate mass deposited in electrolysis
- Relate electricity to amount of substance

Study mercury cell for NaOH production
- Flow chart analysis of industrial processes
- Discussion on applications and environmental impact
- Purification of metals
Experiment 4.10: Quantitative electrolysis of CuSO₄
- Measure mass vs electricity passed
- Calculate Faraday constant
- Verify Faraday's laws

Flow charts, mercury cell diagrams, environmental impact data, industrial case studies
Accurate balance, copper electrodes, CuSO₄ solution, ammeter, timer, calculators

KLB Secondary Chemistry Form 4, Pages 155-157
KLB Secondary Chemistry Form 4, Pages 161-164

ELECTROCHEMISTRY

Electrolysis Calculations I

By the end of the lesson, the learner should be able to:
Calculate mass of products from electrolysis
- Determine volumes of gases evolved
- Apply Faraday's laws to numerical problems
- Solve basic electrolysis calculations

Worked examples: Mass and volume calculations
- Problems involving different ions
- Practice with Faraday constant
- Basic numerical problems

Calculators, worked examples, practice problems, gas volume data, Faraday constant

KLB Secondary Chemistry Form 4, Pages 161-164

ELECTROCHEMISTRY

Electrolysis Calculations II

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

Complex problems: Determine ionic charges
- Current-time-mass relationships
- Multi-step calculations
- Industrial calculation examples

Calculators, complex problem sets, industrial data, student books

KLB Secondary Chemistry Form 4, Pages 161-164

ELECTROCHEMISTRY

Electrolysis Calculations II

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

Complex problems: Determine ionic charges
- Current-time-mass relationships
- Multi-step calculations
- Industrial calculation examples

Calculators, complex problem sets, industrial data, student books

KLB Secondary Chemistry Form 4, Pages 161-164

ELECTROCHEMISTRY

Advanced Applications and Problem Solving

By the end of the lesson, the learner should be able to:
Solve examination-type electrochemistry problems
- Apply all concepts in integrated problems
- Analyze real-world electrochemical processes
- Practice complex calculations

Comprehensive problems combining redox, cells, and electrolysis
- Past examination questions
- Industrial case study analysis
- Advanced problem-solving techniques

Past papers, comprehensive problem sets, industrial case studies, calculators

KLB Secondary Chemistry Form 4, Pages 108-164

METALS

Chief Ores of Metals and General Extraction Methods
Occurrence and Extraction of Sodium

By the end of the lesson, the learner should be able to:
Name chief ores of common metals
- State formulas of metal ores
- Explain general methods of ore concentration
- Describe factors affecting extraction methods

Q/A: Review metallic bonding and reactivity
- Study Table 5.1 - metal ores and formulas
- Discussion on ore concentration methods
- Froth flotation demonstration

Chart of metal ores, ore samples if available, Table 5.1, flotation apparatus demonstration
Down's cell diagram, charts showing sodium occurrence, electrode reaction equations

KLB Secondary Chemistry Form 4, Pages 139-140

METALS

Occurrence and Extraction of Aluminium I

By the end of the lesson, the learner should be able to:
Describe occurrence and ores of aluminium
- Explain ore concentration process
- Write equations for bauxite purification
- Describe amphoteric nature of aluminium oxide

Study aluminium occurrence and bauxite composition
- Demonstration of amphoteric properties
- Equations for bauxite dissolution in NaOH
- Discussion on impurity removal

Bauxite samples, NaOH solution, charts showing aluminium extraction steps, chemical equations

KLB Secondary Chemistry Form 4, Pages 142-143

METALS

Extraction of Aluminium II - Electrolysis

By the end of the lesson, the learner should be able to:
Explain role of cryolite in aluminium extraction
- Describe electrolytic extraction process
- Write electrode equations
- Explain why anodes need replacement

Study Hall-Heroult process setup
- Analysis of electrolytic cell diagram
- Write electrode reactions
- Discussion on energy requirements and anode corrosion

Electrolytic cell diagram, cryolite samples, graphite electrodes, energy consumption data

KLB Secondary Chemistry Form 4, Pages 142-143

METALS

Occurrence and Extraction of Iron
Extraction of Zinc
Extraction of Lead and Copper

By the end of the lesson, the learner should be able to:
Describe iron ores and occurrence
- Explain blast furnace operation
- Write equations for iron extraction reactions
- Describe slag formation process
Explain extraction of lead from galena
- Describe copper extraction from copper pyrites
- Write relevant chemical equations
- Compare purification methods

Study iron ores and blast furnace structure
- Analysis of temperature zones in furnace
- Write reduction equations
- Discussion on limestone role and slag formation
Study galena roasting and reduction
- Copper pyrites multi-step extraction
- Electrolytic purification processes
- Discussion on blister copper formation

Blast furnace diagram, iron ore samples, coke, limestone, temperature zone charts
Zinc ore samples, flow charts showing both methods, electrolytic cell diagrams
Lead and copper ore samples, extraction flow charts, electrolytic purification diagrams

KLB Secondary Chemistry Form 4, Pages 143-145
KLB Secondary Chemistry Form 4, Pages 148-151

METALS

Physical Properties of Metals

By the end of the lesson, the learner should be able to:
Compare physical properties of sodium, aluminium, zinc, iron and copper
- Explain metallic bonding effects
- Relate structure to properties
- Analyze property data

Study Table 5.2 - physical properties comparison
- Discussion on metallic bonding and electron sea model
- Analysis of melting points, conductivity, and density trends

Table 5.2, metal samples, conductivity apparatus, density measurement equipment

KLB Secondary Chemistry Form 4, Pages 151-152