AIR AND COMBUSTION

Composition of air.

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



State the composition of air by volume.

Probing questions;
Brief discussion.

TEXT BOOK

K.L.B.
BOOK I
PP. 68-71

AIR AND COMBUSTION

Air and combustion.
Active part of air.

By the end of the lesson, the learner should be able to:
Describe an experiment to show percentage of air that supports burning.
Determine percentage of active part of air using copper.

Teacher demonstrations;
Discussion;
Worked examples.

Sodium hydroxide solution, candle, gas jar, trough, copper turnings, hard glass tube, glass syringes.
Copper turnings, glass wool, syringes, plastic tubing.

K.L.B.
BOOK I
PP. 68-71

AIR AND COMBUSTION

Rusting.
Percentage of air used up during rusting.
Preventing rusting.
Smouldering of phosphorus.

By the end of the lesson, the learner should be able to:
Identify conditions necessary for rusting.
Describe an experiment to show percentage of air used up during rusting.
State methods of preventing rusting.
Describe an experiment to show percentage of air used up when phosphorus smoulders.

Group experiments;
Discussion.
Teacher demonstration;
Questioning;
Questioning;
Discussion.
Teacher demonstration;

Iron
Iron nails, troughs.
TEXT BOOK
White phosphorus, trough.

K.L.B.
BOOK I
PP 76-77

AIR AND COMBUSTION

Presence of carbon (IV) oxide and water in the air.
Fractional distillation of liquid air.

By the end of the lesson, the learner should be able to:
Describe an experiment to show presence of carbon (IV) oxide and water in the air.
Describe fractional distillation of liquid air.

Teacher demonstration;
Probing questions on colour changes;
Discussion.
Q/A to review fractional distillation;
Discuss flow diagram.

Aspirator, lime water, u-tube, anhydrous calcium chloride.
Flowchart.

K.L.B.
BOOK I
PP. 73-74

AIR AND COMBUSTION

Lab preparation of oxygen.
Burning metals in air (oxygen)

By the end of the lesson, the learner should be able to:
Prepare oxygen in the lab.
State physical properties of oxygen.
State how metals burn in air.

Teacher demonstration / group expts;
Questioning;
Discussion.
Teacher demonstration;
Write equations.

Sodium peroxide, manganese (IV) oxide, potassium permanganate.
Sodium, calcium,
magnesium,
iron, copper.

K.L.B.
BOOK I
PP. 78-79

AIR AND COMBUSTION

Products of burning metals in air.
Reactivity series.
Burning non-metals in air (oxygen)
Competition for oxygen.

By the end of the lesson, the learner should be able to:
Identify products of burning metals in air.
Recall the reactivity series for some metals.
Identify products of burning non-metals in air.
Describe redox reactions.
Write equations for redox reactions.
State applications of redox reactions.

Group experiments;
Testing for products;
Write chemical equations.
Questioning;
Discussion.
Teacher demonstration;
Questioning;
Discussion.
Write equations.
Q/A to review redox reactions;
Teacher demonstrations;

Weighing balance.
Chart- reactivity series for metals.
Carbon, sulphur, phosphorus.
Metals and metal oxides.

K.L.B.
BOOK I
PP. 82-83,
P. 85
K.L.B.
BOOK I
PP. 84-85

AIR AND COMBUSTION
WATER AND HYDROGEN
WATER AND HYDROGEN

Reactivity series based on redox reactions, Uses of oxygen. Environmental pollution.
Burning candle wax in air.
Reaction of cold water with metals.

By the end of the lesson, the learner should be able to:
Recall the reactivity series.
State uses of oxygen.
Discuss environmental pollution.
Test for the products of burning candle wax in air.
Identify products of reaction of cold water with metals.

Q/A to review redox reactions;
Open discussion.
Teacher demonstrations;
Discussion.
Discussion;
Write equations.

TEXT BOOK
Candles, lime water.
Calcium, sodium grain.

K.L.B.
BOOK I
PP. 88-89

WATER AND HYDROGEN

Reaction of steam with metals.
Hydrogen. - lab preparation.

By the end of the lesson, the learner should be able to:
Identify products of reaction of steam with metals.
Recall the reactivity series of metals based on reaction with water.
Describe laboratory preparation of hydrogen.

Teacher demonstrations;
Test for evolved gas;
Discussion;
Write equations.
Review reactivity series.
Discussion.

Magnesium ribbon, sand, iron / steel wool.
Zinc granules,
dil HCl,
conc. sulphuric acid.

K.L.B.
BOOK I
PP. 94-96

WATER AND HYDROGEN

Hydrogen. - physical properties.
Hydrogen as a reducing agent.
Burning hydrogen in air.
Uses of hydrogen.

By the end of the lesson, the learner should be able to:
State physical properties of hydrogen.
Describe an experiment to show reducing properties of hydrogen.
Identify products of burning hydrogen in air.
State uses of hydrogen.

Probing questions and discussion.
Teacher demonstration;
Discussion;
Write equations.
Discussion.
Probing questions;
Open discussion.

Zinc granules,
dil HCl,
conc. sulphuric acid, litmus papers.
Copper (II) oxide, anhydrous Copper (II) sulphate., dry hydrogen.
Anhydrous calcium chloride,
hydrogen, U tube, ice cold water.
TEXT BOOK

K.L.B.
BOOK I
PP. 97-98
K.L.B.
BOOK I
PP. 99-101

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

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

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.
List the first twenty elements of the periodic table.
Write chemical symbols of the first twenty elements of the periodic table.

Exposition on new concepts;
Probing questions;
Brief discussion.
Expository approach: referring to the periodic table, teacher exposes the first twenty elements.
Writing down a list of first twenty elements of the periodic table.

text book
Periodic table.

K.L.B.
BOOK II

PP. 1-3

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Isotopes.
Electronic configuration.
Electronic configuration in diagrams.

By the end of the lesson, the learner should be able to:
Define isotopes.
Give examples of isotopes.
Represent isotopes symbolically.
Define an energy level.
Describe electronic configuration in an atom.
Represent electronic configuration diagrammatically.

Exposition of definition and examples of isotopes.
Giving examples of isotopes.
Exposition ? teacher exposes new concepts about electronic configuration.
Written exercise.
Supervised practice;

Periodic table.
text book

K.L.B.
BOOK II
P. 4





PP. 5-8

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Periods of the periodic table.
Groups of the periodic table.
R.M.M. and isotopes.

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

Exposition ? Definition of a period.
Q/A: Examples of elements of the same period.
Exposition ? definition of a group.
Q/A: examples of elements of the same group.
Supervised practice involving calculation of RMM from isotopic composition.

Periodic table.
Periodic table.
text book

K.L.B. BOOK IIP. 9

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions and ion formation.

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

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.

text book

K.L.B. BOOK IIPP 14-15

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions representation.

By the end of the lesson, the learner should be able to:
To represent formation of positive ions symbolically.

Diagrammatic representation of cations.

Chart  ion model.

K.L.B. BOOK IIP 16

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Negative ions and ion formation.

By the end of the lesson, the learner should be able to:
To define an anion.
To describe formation of negative ions symbolically.

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

Chart  ion model.

K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencies of metals.
Valencie of non-metals.

By the end of the lesson, the learner should be able to:
Recall valencies of metals among the first twenty elements in the periodic table.
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.
Define oxidation number.
Predict oxidation numbers from position of elements in the periodic table.

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

Q/A: Valencies.
Expose oxidation numbers of common ions.
Students complete a table of ions and their oxidation numbers.

text book
The periodic table.

K.L.B. BOOK IIP 18
K.L.B. BOOK IIvP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Electronic configuration, ion formed, valency and oxidation number
Chemical formulae of compounds. - Elements of equal valencies.

By the end of the lesson, the learner should be able to:
Relate electronic configuration, ion formed, valency and oxidation number of different elements.
To derive the formulae of some compounds involving elements of equal valencies.

Written exercise;
Exercise review.
Discuss formation of compounds such as NaCl, MgO.

text book

K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical formulae of compounds. -Elements of unequal valencies.

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

Discuss formation of compounds such as MgCl2
Al (NO3)3

text book

K.L.B. BOOK IIPP 19-20

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical formulae of compounds. -Elements of variable valencies.

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

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

text book

K.L.B. BOOK IIP 20

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

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 variable valencies.
To identify components of chemical equations.

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

Review word equations;
Exposition of new concepts with probing questions;
Brief discussion.

text book

K.L.B. BOOK IIP 20
K.L.B. BOOK IIPP 21-23

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
CHEMICAL FAMILIES

Balanced chemical equations.(contd)
Alkali metals. Atomic and ionic radii of alkali metals

By the end of the lesson, the learner should be able to:
To balance chemical equations correctly.
Identify alkali metals.
State changes in atomic and ionic radii of alkali metals.

Supervised practice;
Written exercise.
Q/A to reviews elements of group I and their electronic configuration.
Examine a table of elements, their symbols and atomic & ionic radii.
Discussion & making deductions from the table.

text book
The periodic

K.L.B. BOOK IIPP 25-8

CHEMICAL FAMILIES

Ionisation energy of alkali metals.
Physical properties of alkali metals.
Chemical properties of alkali metals.

By the end of the lesson, the learner should be able to:
State changes in number of energy levels and ionisation energy of alkali metals.
State and explain trends in physical properties of alkali metals.
To describe reaction of alkali metals with water.

Examine a table of elements, number of energy levels and their ionization energy.
Discuss the trend deduced from the table.

Examine a table showing comparative physical properties of Li, Na, and K.
Q/A: Teacher asks probing questions as students refer to the table for answers.
Detailed discussion on physical properties of alkali metals.

Q/A: Review reaction of metals with water.
Writing down chemical equations for the reactions.
Deduce and discuss the order of reactivity down the group.

text book
Chart ? comparative properties of Li, Na, K.
text book

K.L.B. BOOK II
K.L.B. BOOK IIPP 30-31

CHEMICAL FAMILIES

Reaction of alkali metals with chlorine gas.

By the end of the lesson, the learner should be able to:
To write balanced equations for reaction of alkali metals with chlorine gas.

Teacher demonstration- reaction of sodium with chlorine in a fume chamber.
Q/A: Students to predict a similar reaction between potassium and chlorine.
Word and balanced chemical equations for various reactions.

Sodium, chlorine.

K.L.B. BOOK IIP. 33

CHEMICAL FAMILIES

Compounds of alkali metals.

By the end of the lesson, the learner should be able to:
Write chemical formulae for compounds of alkali metals.
Explain formation of hydroxides, oxides and chlorides of alkali metals.

Exercise: Completing a table of hydroxides, oxides and chlorides of alkali metals.
Discuss combination of ions of alkali metals with anions.

text book

K.L.B. BOOK II pp 33

CHEMICAL FAMILIES

Uses of alkali metals.
Alkaline Earth metals Atomic and ionic radii of alkaline earth metals.
Physical properties of alkaline earth metals.
Electrical properties of alkaline earth metals.

By the end of the lesson, the learner should be able to:
State uses of alkali metals.
Identify alkaline earth metals.
State changes in atomic and ionic radii of alkaline earth metals.
State and explain trends in physical properties of alkaline earth metals.
To describe electrical properties of alkaline earth metals.

Descriptive approach: Teacher elucidates uses of alkali metals.
Q/A: Elements of group I and their electron configuration.
Examine a table of elements, their symbols and atomic & ionic radii.
Make deductions from the table.
Examine a table showing comparative physical properties of Be, Mg, Ca.
Q/A: Teacher asks probing questions as students refer to the table for answers.
Detailed discussion of physical properties of alkaline earth metals.
Teacher demonstration: -
To show alkaline metals are good conductors of electric charge.

text book
Some alkaline earth metals.
Alkaline earth metals.

K.L.B. BOOK II pp 34