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

Reactivity series based on redox reactions, Uses of oxygen. Environmental pollution.
Burning candle wax in air.

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.

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

TEXT BOOK
Candles, lime water.

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

WATER AND HYDROGEN

Reaction of cold water with metals.

By the end of the lesson, the learner should be able to:
Identify products of reaction of cold water with metals.

Teacher demonstrations;
Discussion;
Write equations.

Calcium, sodium grain.

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

WATER AND HYDROGEN

Reaction of steam with metals.
Hydrogen. - lab preparation.
Hydrogen. - physical properties.
Hydrogen as a reducing agent.

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.
State physical properties of hydrogen.
Describe an experiment to show reducing properties of hydrogen.

Teacher demonstrations;
Test for evolved gas;
Discussion;
Write equations.
Review reactivity series.
Discussion.
Probing questions and discussion.
Teacher demonstration;
Discussion;
Write equations.

Magnesium ribbon, sand, iron / steel wool.
Zinc granules,
dil HCl,
conc. sulphuric acid.
Zinc granules,
dil HCl,
conc. sulphuric acid, litmus papers.
Copper (II) oxide, anhydrous Copper (II) sulphate., dry hydrogen.

K.L.B.
BOOK I
PP. 94-96
K.L.B.
BOOK I
PP. 97-98

WATER AND HYDROGEN

Burning hydrogen in air.
Uses of hydrogen.

By the end of the lesson, the learner should be able to:
Identify products of burning hydrogen in air.
State uses of hydrogen.

Teacher demonstration;
Discussion.
Probing questions;
Open discussion.

Anhydrous calcium chloride,
hydrogen, U tube, ice cold water.
TEXT BOOK

K.L.B.
BOOK I
PP. 101-102

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;
Written exercise.

Periodic table.
text book

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

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

Periodic table.

K.L.B. BOOK IIP. 9

THE STRUCTURE OF THE ATOM & 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:
Calculate R.M.M. from isotopic composition.
To define an ion and a cation.

Supervised practice involving calculation of RMM from isotopic composition.

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. 11-13

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

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

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

K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Oxidation number.
Electronic configuration, ion formed, valency and oxidation number

By the end of the lesson, the learner should be able to:
Define oxidation number.
Predict oxidation numbers from position of elements in the periodic table.
Relate electronic configuration, ion formed, valency and oxidation number of different elements.

Q/A: Valencies.
Expose oxidation numbers of common ions.
Students complete a table of ions and their oxidation numbers.
Written exercise;
Exercise review.

The periodic table.
text book

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.
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 unequal valencies.
To derive the formulae of some compounds involving elements of variable valencies.
To identify components of chemical equations.

Discuss formation of compounds such as NaCl, MgO.
Discuss formation of compounds such as MgCl2
Al (NO3)3
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 IIPP 19-20
K.L.B. BOOK IIP 20

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Balanced chemical equations.
Balanced chemical equations.(contd)

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

Exposition;
Supervised practice.
Supervised practice;
Written exercise.

text book

K.L.B. BOOK IIPP 24-25

CHEMICAL FAMILIES

Alkali metals. Atomic and ionic radii of alkali metals

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





Identify alkali metals.
State changes in atomic and ionic radii of alkali metals.

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.

The periodic

K.L.B. BOOK IIPP 28-29

CHEMICAL FAMILIES

Ionisation energy of alkali metals.
Physical properties of alkali metals.
Chemical properties of alkali metals.
Reaction of alkali metals with chlorine gas.

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.
To write balanced equations for reaction of alkali metals with chlorine gas.

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.
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.

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

K.L.B. BOOK II
K.L.B. BOOK IIP. 32

CHEMICAL FAMILIES

Compounds of alkali metals.
Uses 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.
State uses of alkali metals.

Exercise: Completing a table of hydroxides, oxides and chlorides of alkali metals.
Discuss combination of ions of alkali metals with anions.
Descriptive approach: Teacher elucidates uses of alkali metals.

text book

K.L.B. BOOK II pp 33

CHEMICAL FAMILIES

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

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

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.

Some alkaline earth metals.

K.L.B. BOOK II pp 34

CHEMICAL FAMILIES

Electrical properties of alkaline earth metals.
Chemical properties of alkaline earth metals. Reaction of alkaline earth metals with oxygen.
Chemical properties of alkaline earth metals. Reaction of alkaline earth metals with water.

By the end of the lesson, the learner should be able to:
To describe electrical properties of alkaline earth metals.
To describe reaction of alkaline earth metals with oxygen
To describe reaction of alkaline earth metals with water.

Teacher demonstration: -
To show alkaline metals are good conductors of electric charge.
Q/A: Review reactions of Mg, Ca, with oxygen.
The corresponding word and then chemical equations are then written and their correctness verified by the teacher.
Q/A: Review reaction of metals with water.
Writing down word and balanced chemical equations for the reactions.
Deduce and discuss the order of reactivity down the group.

Alkaline earth metals.
text book
Some alkaline earth metals.

K.L.B. BOOK IIP. 37
K.L.B. BOOK IIP. 39

CHEMICAL FAMILIES

Reaction of alkaline earth metals with chlorine gas.
Reaction of alkaline earth metals with dilute acids.

By the end of the lesson, the learner should be able to:
To write balanced equations for reaction of alkaline earth metals with chlorine gas.
To write balanced equations for reactions of alkaline earth metals with dilute acids.

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.
Supervised practice.
Changing word to chemical equations.

Sodium, chlorine.
revision book

K.L.B. BOOK II P. 41

CHEMICAL FAMILIES

Chemical formulae of alkaline earth metals.
Uses of some alkaline earth metals and their compounds.
Halogens. Physical properties of halogens.

By the end of the lesson, the learner should be able to:
Write chemical formulae for compounds of alkaline earth metals.
Explain formation of hydroxides, oxides and chlorides of alkaline earth metals.
State uses of alkaline earth metals.
Identify halogens in the periodic table.
Give examples of halogens.
Identify physical states of halogens.

Exercise: Completing a table of hydroxides, oxides and chlorides of alkaline earth metals.
Discuss combination of ions of alkaline earth metals with anions.
Descriptive approach: Teacher elucidates uses of alkaline earth metals.
Teacher demonstration: - To examine electrical properties of iodine, solubility in water of chlorine.

text book
Iodine crystals, electrical wire, a bulb.

K.L.B. BOOK II PP. 45-47

CHEMICAL FAMILIES

Comparative physical properties of halogens.
Chemical properties of halogens.
Equations of reaction of halogens with metals.
Reaction of halogens with water.

By the end of the lesson, the learner should be able to:
To state and explain the trends in physical properties of halogens.
To describe laboratory preparation of chlorine gas.
To describe reaction of halogens with metals.
To write balanced chemical equations of reactions involving halogens.
To describe reaction of halogens with water and the results obtained.

Examine a comparative table of physical properties of halogens.
Discuss the deductions made from the table.
Teacher demonstration: - preparation of chlorine gas.
Reaction of chlorine and iron wool.
Reaction of bromine and iron wool.
Reaction of iodine and iron wool.
Observe the rate of these reactions; hence deduce order of their reactivity of halogens.
Re-write word equations as chemical equations then balance them.
Supervised practice.
Bubbling chlorine gas through water.
Carry out litmus test for the water.
Explain the observations.

text book
Chlorine, iron wool, bromine.
text book
Chlorine gas, litmus papers.

K.L.B. BOOK II P. 47
K.L.B. BOOK II P. 50

CHEMICAL FAMILIES

Some uses of halogens and their compounds.
Noble Gases. Comparative physical properties of noble gases.
Uses of noble gases.

By the end of the lesson, the learner should be able to:
To state uses of halogens and their compounds.
To describe physical properties of noble gases.
To explain physical properties of noble gases.
State uses of noble gases.

Teacher elucidates uses of halogens and their compounds.
Make A comparative analysis of tabulated physical properties of noble gases.
Teacher elucidates uses of noble gases.

text book

K.L.B. BOOK II pp 52