WATER AND HYDROGEN

Burning candle wax in air.
Reaction of cold water with metals.
Reaction of steam with metals.
Hydrogen. - lab preparation.

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



Test for the products of burning candle wax in air.


Identify products of reaction of steam with metals.
Recall the reactivity series of metals based on reaction with water.

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

Candles, lime water.
Calcium, sodium grain.
Magnesium ribbon, sand, iron / steel wool.
Zinc granules,
dil HCl,
conc. sulphuric acid.

K.L.B.
BOOK I
PP. 91-92
K.L.B.
BOOK I
PP. 94-96

WATER AND HYDROGEN

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

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.

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

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.

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

WATER AND HYDROGEN
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

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

By the end of the lesson, the learner should be able to:
State uses of hydrogen.
List the first twenty elements of the periodic table.
Write chemical symbols of the first twenty elements of the periodic table.

Probing questions;
Open 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 I
PP. 102-103
K.L.B.
BOOK II

PP. 1-3

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Isotopes.
Electronic configuration.
Electronic configuration in diagrams.
Periods of the periodic table.

By the end of the lesson, the learner should be able to:
Define isotopes.
Give examples of isotopes.

Represent electronic configuration diagrammatically.

Exposition of definition and examples of isotopes.
Giving examples of isotopes.

Supervised practice;
Written exercise.

Periodic table.
text book
Periodic table.

K.L.B.
BOOK II
P. 4





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

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Groups of the periodic table.
R.M.M. and isotopes.
Positive ions and ion formation.

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

Exposition ? definition of a group.
Q/A: examples of elements of the same group.
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.

Periodic table.
text book

K.L.B. BOOK IIP. 9
K.L.B. BOOK IIPP 14-15

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Positive ions representation.
Negative ions and ion formation.
Valencies of metals.
Valencie of non-metals.

By the end of the lesson, the learner should be able to:
To represent formation of positive ions symbolically.
Recall valencies of metals among the first twenty elements in the periodic table.

Diagrammatic representation of cations.
Q/A to review previous lesson;
Exposition;
Guided discovery.

Chart  ion model.
Periodic table.

K.L.B. BOOK IIP 16
K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencies of radicals.
Oxidation number.
Electronic configuration, ion formed, valency and 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.
text book

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

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
THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE
CARBON AND SOME OF ITS COMPOUNDS.
CARBON AND SOME OF ITS COMPOUNDS.

Chemical equations.
Balanced chemical equations.
Balanced chemical equations.(contd)
Allotropy.
Physical and chemical properties of diamond, graphite and amorphous carbon

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

To balance chemical equations correctly.

Review word equations;
Exposition of new concepts with probing questions;
Brief discussion.
Supervised practice;
Written exercise.

text book
text book
Charcoal, graphite.

K.L.B. BOOK IIPP 21-23
K.L.B. BOOK IIPP 25-8

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

By the end of the lesson, the learner should be able to:
Describe reaction of carbon with oxygen.
Write balanced CO2.

Teacher demonstration- Prepare oxygen and pass dry oxygen into a tube containing carbon. Heat the carbon. Observe effects on limewater.
Give examples of reactions. Write corresponding balanced chemical equations.

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.
text book

K.L.B. BOOK II PP. 134-135
K.L.B. BOOK II PP.139-140

CARBON AND SOME OF ITS COMPOUNDS.

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 write chemical equations for reactions of carbonates and hydrogen carbonates with acids.
To draw schematic diagram for extraction of sodium carbonates.

Discuss the observations above.
Write chemical equations for the reactions.
Discuss each step of the process.

Write relevant equations.

text book
text book, chart
text book

K.L.B. BOOK II