THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Atomic and mass numbers.
First twenty elements of the periodic table.
Isotopes.
Electronic configuration.

By the end of the lesson, the learner should be able to:


Name the subatomic particles in an atom.
Define atomic number and mass number of an atom.
Represent atomic and mass numbers symbolically.

Define isotopes.
Give examples of isotopes.

Exposition on new concepts;
Probing questions;
Brief discussion.
Exposition of definition and examples of isotopes.
Giving examples of isotopes.

text book
Periodic table.

K.L.B.
BOOK II

PP. 1-3
K.L.B.
BOOK II
P. 4





PP. 5-8

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration in diagrams.

By the end of the lesson, the learner should be able to:
Represent electronic configuration diagrammatically.

Supervised practice;
Written exercise.

text book

K.L.B.
BOOK II
PP. 5-8

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Periods of the periodic table.
Groups of the periodic table.

By the end of the lesson, the learner should be able to:
Identify elements of the same period.

Exposition ? Definition of a period.
Q/A: Examples of elements of the same period.

Periodic table.

K.L.B. BOOK IIP. 9

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

R.M.M. and isotopes.

By the end of the lesson, the learner should be able to:
Calculate R.M.M. from isotopic composition.

Supervised practice involving calculation of RMM from isotopic composition.

text book

K.L.B. BOOK IIPP. 11-13

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions and ion formation.
Positive ions representation.
Negative ions and ion formation.
Valencies of metals.

By the end of the lesson, the learner should be able to:
To define an ion and a cation.

To define an anion.
To describe formation of negative ions symbolically.

Teacher gives examples of stable atoms.
Guided discovery that metals need to lose one, two or three electrons to attain stability.
Examples of positive ions.


Teacher gives examples of stable atoms.
Guided discovery of formation of negative ions.
Diagrammatic representation of anions.

text book
Chart  ion model.
Chart  ion model.
Periodic table.

K.L.B. BOOK IIPP 14-15
K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencie of non-metals.

By the end of the lesson, the learner should be able to:
Recall valencies of non-metals among the first twenty elements in the periodic table.

Q/A to review previous lesson;
Exposition;
Guided discovery.

Periodic table.

K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencies of radicals.
Oxidation number.

By the end of the lesson, the learner should be able to:
Define a radical.
Recall the valencies of common radicals.

Exposition ? teacher defines a radical, gives examples of radicals and exposes their valencies.
Students draw a table of radicals and their valencies.

text book
The periodic table.

K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration, ion formed, valency and oxidation number

By the end of the lesson, the learner should be able to:
Relate electronic configuration, ion formed, valency and oxidation number of different elements.

Written exercise;
Exercise review.

text book

K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical formulae of compounds. - Elements of equal valencies.
Chemical formulae of compounds. -Elements of unequal valencies.
Chemical formulae of compounds. -Elements of variable valencies.
Chemical equations.

By the end of the lesson, the learner should be able to:
To derive the formulae of some compounds involving elements of equal valencies.
To derive the formulae of some compounds involving elements of variable valencies.

Discuss formation of compounds such as NaCl, MgO.
Discuss formation of compounds such as
-Copper (I) Oxide.
-Copper (II) Oxide.
-Iron (II) Sulphate.
-Iron (III) Sulphate.

text book

K.L.B. BOOK IIPP 19-20
K.L.B. BOOK IIP 20

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Balanced chemical equations.

By the end of the lesson, the learner should be able to:
To balance chemical equations correctly.

Exposition;
Supervised practice.

text book

K.L.B. BOOK IIPP 24-25

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
SALTS
SALTS

Balanced chemical equations.(contd)
Types of salts.
Solubility of salts in water.

By the end of the lesson, the learner should be able to:
To balance chemical equations correctly.

Supervised practice;
Written exercise.

text book
Sulphates, chlorides, nitrates, carbonates of various metals.

K.L.B. BOOK IIPP 25-8

SALTS

Solubility of bases in water.
Methods of preparing various salts.

By the end of the lesson, the learner should be able to:
To test solubility of various bases in water.
To carry out litmus test on the resulting solutions.

Class experiments- Dissolve salts in 5cc of water.
Record the solubility in a table,
Carry out litmus tests.
Discuss the results.

Oxides, hydroxides, of various metals, litmus papers.
CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.

K.L.B. BOOK IIPP. 94-95

SALTS

Direct synthesis of a salts.
Ionic equations.
Effects of heat on carbonates.

By the end of the lesson, the learner should be able to:
To describe direct synthesis of a salt.
To write balanced equations for the reactions.

Group experiments- preparation of iron (II) sulphide by direct synthesis.
Give other examples of salts prepared by direct synthesis.
Students write down corresponding balanced equations.

Iron,
Sulphur
PbNO3, MgSO4 solutions.
Various carbonates.

K.L.B. BOOK II P. 104

SALTS

Effects of heat on nitrates.
Effects of heat on sulphates.
Hygroscopy, Deliquescence and Efflorescence.

By the end of the lesson, the learner should be able to:
To state effects of heat on nitrates.
To predict products resulting from heating metal nitrates.

Group experiments- To investigate effects of heat on various metal nitrates.
Observe various colour changes before, during and after heating.
Write equations for the reactions.

Common metal nitrates.
Common sulphates.

K.L.B. BOOK II PP. 110-111

SALTS
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Uses of salts.
Molten electrolytes.
Electrolysis.
Aqueous electrolytes. Electrodes.
Reaction on electrodes.
Binary electrolyte.
Application of electrolysis.

By the end of the lesson, the learner should be able to:
To state uses of salts
To describe half- equation reactions at the cathode and anode

Teacher elucidates uses of salts.
To demonstrate ?Electrolysis of molten lead (II) bromide
Observe colour changes
Explanation of half-equations and reactions at the electrodes.

Molten candle wax
Sugar
Sulphur
Lead oxide.
Graphite electrodes
Battery
Various aqueous solutions switch bulb.
Graphite electrodes
Battery
Various aqueous solutions switch.
text book

K.L.B. BOOK II P. 114
K.L.B. BOOK II PP.126-127

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.

Electroplating.
Allotropy.
Physical and chemical properties of diamond, graphite and amorphous carbon

By the end of the lesson, the learner should be able to:
To describe electroplating process.

Experiment- Left overnight.
Electroplating an iron nail with silver nitrate/ copper sulphate.
Brief discussion.

Silver nitrate
Iron nail
Complete circuit battery.
text book
Charcoal, graphite.

K.L.B. BOOK II PP. 129-30

CARBON AND SOME OF ITS COMPOUNDS.

Burning carbon and oxygen.
Reduction properties of carbon.
Reaction of carbon with acids. Preparation of CO2.
Properties of CO2.

By the end of the lesson, the learner should be able to:
Describe reaction of carbon with oxygen.

Teacher demonstration- Prepare oxygen and pass dry oxygen into a tube containing carbon. Heat the carbon. Observe effects on limewater.

Carbon, limewater, tube, limewater stand& Bunsen burner.
CuO, pounded charcoal, Bunsen burner& bottle top
Conc. HNO3, limewater.
Lime water,
Magnesium ribbon,
Universal indicator,
lit candle.

K.L.B. BOOK II PP. 134-135

CARBON AND SOME OF ITS COMPOUNDS.

Chemical equations for reactions involving CO2.
Uses of CO2.
Carbon monoxide lab preparation.

By the end of the lesson, the learner should be able to:
Write balanced CO2.

Give examples of reactions. Write corresponding balanced chemical equations.

text book

K.L.B. BOOK II PP.139-140

CARBON AND SOME OF ITS COMPOUNDS.

Chemical properties of carbon monoxide.
Carbonates and hydrogen carbonates.
Heating carbonates and hydrogen carbonates.
Extraction of sodium carbonate from trona.
Solvay process of preparing sodium carbonate.
Importance of carbon in nature. & its effects on the environment.

By the end of the lesson, the learner should be able to:
To describe chemical properties of carbon monoxide.
To draw schematic diagram for extraction of sodium carbonates.

Description of properties of carbon monoxide.
Discussion and writing of chemical equations.
Discuss each step of the process.

Write relevant equations.

text book
text book, chart
text book

K.L.B. BOOK II PP. 144-145

GAS 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:
State Boyle's law
Explain Boyle's law using kinetic theory of matter
Investigate the relationship between pressure and volume of a fixed mass of gas
Plot graphs to illustrate Boyle's law

Teacher demonstration: Use bicycle pump to show volume-pressure relationship. Students observe force needed to compress gas. Q/A: Review kinetic theory. Class experiment: Investigate pressure-volume relationship using syringes. Record observations in table format. Discuss observations using kinetic theory.

Bicycle pump, Syringes, Gas jars, Chart showing volume-pressure relationship
Graph papers, Scientific calculators, Chart showing mathematical expressions

KLB Secondary Chemistry Form 3, Pages 1-3

GAS LAWS

Boyle's Law - Numerical Problems and Applications

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

KLB Secondary Chemistry Form 3, Pages 4-5

GAS LAWS

Charles's Law - Introduction and Temperature Scales
Charles's Law - Experimental Investigation and Mathematical Expression

By the end of the lesson, the learner should be able to:
State Charles's law
Convert temperatures between Celsius and Kelvin scales
Define absolute zero temperature
Explain the concept of absolute temperature

Teacher demonstration: Flask with colored water column experiment. Q/A: Observe volume changes with temperature. Exposition: Introduce Kelvin scale and absolute zero concept. Practice: Temperature conversions between °C and K. Discuss absolute zero and ideal gas concept.

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

KLB Secondary Chemistry Form 3, Pages 6-8

GAS LAWS

Charles's Law - Numerical Problems and Applications
Combined Gas Law and Standard Conditions
Introduction to Diffusion - Experimental Investigation

By the end of the lesson, the learner should be able to:
Solve numerical problems using Charles's law
Apply V₁/T₁ = V₂/T₂ in calculations
Predict gas behavior with temperature changes
Relate Charles's law to everyday phenomena
Derive the combined gas law equation
Apply PV/T = constant in problem solving
Define standard temperature and pressure (s.t.p)
Define room temperature and pressure (r.t.p)

Worked examples: Step-by-step problem solving with temperature conversions. Supervised practice: Calculate volumes at different temperatures. Discuss applications: hot air balloons, tire pressure changes, weather balloons. Assignment: Practice problems with real-life contexts.
Q/A: Combine Boyle's and Charles's laws. Teacher exposition: Derive P₁V₁/T₁ = P₂V₂/T₂. Define s.t.p (273K, 760mmHg) and r.t.p (298K, 760mmHg). Worked examples: Problems involving changes in all three variables. Supervised practice: Complex gas law calculations.

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

KLB Secondary Chemistry Form 3, Pages 10-12
KLB Secondary Chemistry Form 3, Pages 12-14

GAS LAWS

Rates of Diffusion - Comparative Study
Graham's Law of Diffusion - Theory and Mathematical Expression

By the end of the lesson, the learner should be able to:
Compare diffusion rates of different gases
Investigate factors affecting diffusion rates
Measure relative distances covered by diffusing gases
Calculate rates of diffusion using distance and time data

Class experiment: Ammonia and HCl diffusion in glass tube. Insert cotton wool soaked in concentrated NH₃ and HCl at opposite ends. Time the formation of white NH₄Cl ring. Measure distances covered by each gas. Calculate rates: distance/time. Compare molecular masses of NH₃ and HCl.

Glass tube (25cm), Cotton wool, Concentrated NH₃ and HCl, Stopwatch, Ruler, Safety equipment
Graham's law charts, Molecular mass tables, Mathematical derivation displays

KLB Secondary Chemistry Form 3, Pages 16-18

GAS LAWS

Graham's Law - Numerical Applications and Problem Solving

By the end of the lesson, the learner should be able to:
Solve numerical problems using Graham's law
Calculate relative rates of diffusion
Determine molecular masses from diffusion data
Compare diffusion times for equal volumes of gases

Worked examples: Calculate relative diffusion rates using √(M₂/M₁). Problems involving time comparisons for equal volumes. Calculate unknown molecular masses from rate data. Supervised practice: Various Graham's law calculations. Real-life applications: gas separation, gas masks.

Scientific calculators, Worked example charts, Molecular mass reference tables

KLB Secondary Chemistry Form 3, Pages 20-22