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.

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.

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.
Negative ions and ion formation.

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.

Diagrammatic representation of cations.
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 16
K.L.B. BOOK IIP 17

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Valencies of 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.

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

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.
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.
Relate electronic configuration, ion formed, valency and oxidation number of different elements.

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

Written exercise;
Exercise review.

text book
The periodic table.

K.L.B. BOOK IIP 18

THE STRUCTURE OF THE ATOM & THE PERIODIC TABLE

Chemical formulae of compounds. - Elements of equal 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.

Discuss formation of compounds such as NaCl, MgO.

text book

K.L.B. BOOK IIPP 19-20

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.
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

Balanced chemical equations.(contd)

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

Supervised practice;
Written exercise.

text book

K.L.B. BOOK IIPP 25-8

CHEMICAL FAMILIES

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 reaction of alkaline earth metals with oxygen

To describe reaction of alkaline earth metals with water.

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.

text book
Some alkaline earth metals.

K.L.B. BOOK IIP. 38
K.L.B. BOOK IIP. 39

CHEMICAL FAMILIES

Reaction of alkaline earth metals with chlorine gas.

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.

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.

Sodium, chlorine.

K.L.B. BOOK II P. 41

CHEMICAL FAMILIES

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 reactions of alkaline earth metals with dilute acids.

Changing word to chemical equations.
Supervised practice.

revision book

K.L.B. BOOK II PP. 43

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.

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.

text book
text book
Iodine crystals, electrical wire, a bulb.

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

CHEMICAL FAMILIES

Comparative physical properties of halogens.
Chemical properties of halogens.

By the end of the lesson, the learner should be able to:
To state and explain the trends in physical properties of halogens.

Examine a comparative table of physical properties of halogens.
Discuss the deductions made from the table.

text book
Chlorine, iron wool, bromine.

K.L.B. BOOK II P. 47

CHEMICAL FAMILIES

Equations of reaction of halogens with metals.

By the end of the lesson, the learner should be able to:
To write balanced chemical equations of reactions involving halogens.

Re-write word equations as chemical equations then balance them.
Supervised practice.

text book

K.L.B. BOOK II P. 50

CHEMICAL FAMILIES

Reaction of halogens with water.
Some uses of halogens and their compounds.
Noble Gases. Comparative physical properties of noble gases.

By the end of the lesson, the learner should be able to:
To describe reaction of halogens with water and the results obtained.
To state uses of halogens and their compounds.

Bubbling chlorine gas through water.
Carry out litmus test for the water.
Explain the observations.

Teacher elucidates uses of halogens and their compounds.

Chlorine gas, litmus papers.
text book

K.L.B. BOOK II P. 51
K.L.B. BOOK II pp 52

CHEMICAL FAMILIES
STRUCTURE & BONDING
STRUCTURE & BONDING

Uses of noble gases.
Chemical bonds. Ionic bond.
Ionic bond representation.

By the end of the lesson, the learner should be able to:
State uses of noble gases.

Teacher elucidates uses of noble gases.

text book
Chart- dot and cross diagrams.
Models for bonding.

K.L.B. BOOK IIP. 54

STRUCTURE & BONDING

Grant ionic structures.
Physical properties of ionic compounds.
Covalent bond.

By the end of the lesson, the learner should be able to:
Describe the crystalline ionic compound.
Give examples of ionic substances.

Discuss the group ionic structures of NaCl.
Teacher gives examples of other ionic substances: KNO3, potassium bromide, Ca (NO3)2, sodium iodide.

Giant sodium chloride model.
text book

K.L.B. BOOK II PP 56-58

STRUCTURE & BONDING

Co-ordinate bond.
Molecular structure.
Trend in physical properties of molecular structures.
Giant atomic structure in diamond.

By the end of the lesson, the learner should be able to:
To describe the co-ordinate bond
To represent co-ordinate bond diagrammatically.
To describe van- der -waals forces.
To explain the trend in physical properties of molecular structures.

Exposition- teacher explains the nature of co-ordinate bond.
Students represent co-ordinate bond diagrammatically.
Discuss comparative physical properties of substances. exhibiting molecular structure.
Explain variation in the physical properties.

text book
Sugar, naphthalene, iodine rhombic sulphur.
Diagrams in textbooks.

K.L.B. BOOK II P 65
K.L.B. BOOK IIP 65

STRUCTURE & BONDING

Giant atomic structure in graphite.
Metallic bond. Uses of some metals.

By the end of the lesson, the learner should be able to:
To describe giant atomic structure in graphite.
To state uses of graphite.

Diagrammatic representation of graphite.

Discuss uses of graphite.

Diagrams in textbooks.
text book

K.L.B. BOOK II pp 69

PROPERTIES AND TRENDS ACROSS PERIOD THREE

Physical properties of elements in periods.
Physical properties of elements in period 3.

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




To compare electrical conductivity of elements in period 3

Group experiments- Construct electrical circuits incorporating a magnesium ribbon, then aluminum foil, then sulphur in turns.
The brightness of the bulb is noted in each case.
Discuss the observations in terms of delocalised electrons.

The periodic table.

K.L.B. BOOK IIP. 76

PROPERTIES AND TRENDS ACROSS PERIOD THREE
PROPERTIES AND TRENDS ACROSS PERIOD THREE
SALTS

Chemical properties of elements in period 3.
Chemical properties of elements in the third period.
Oxides of period 3 elements.
Chlorides of period 3 elements.
Types of salts.

By the end of the lesson, the learner should be able to:
To compare reactions of elements in period 3 with oxygen.
To identify bonds across elements in period 3.
To explain chemical behavior of their oxide.

Q/A: Products of reactions of Na, Mg, Al, P, & S with oxygen.
Discuss the trend in their reactivity; identify basic and acidic oxides.
Exercise ? balanced chemical equations for the above reactions.

Comparative analysis, discussion and explanation.

The periodic table.
The periodic table.
text book

K.L.B. BOOK II PP. 79-80
K.L.B. BOOK II P. 84

SALTS

Solubility of salts in water.

By the end of the lesson, the learner should be able to:
To test solubility of various salts in cold water/warm water.

Class experiments- Dissolve salts in 5 cc of water.
Record the solubility in a table,
Analyse the results.

Sulphates, chlorides, nitrates, carbonates of various metals.

K.L.B. BOOK II PP. 92-93

SALTS

Solubility of bases in water.

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.

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

SALTS

Methods of preparing various 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 various methods of preparing some salts.
To identify spectator ions in double decomposition reactions.
To write ionic equations correctly.

Experimental and descriptive treatments of preparation of salts e.g. ZnSO4, CuSO4, NaCl and Pb(NO3)2.


Q/A: Ions present in given reactants.
Deduce the products of double decomposition reactions.
Give examples of equations.
Supervised practice.

CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.
Iron,
Sulphur
PbNO3, MgSO4 solutions.
Various carbonates.

K.L.B. BOOK II pp96

SALTS

Effects of heat on nitrates.
Effects of heat on sulphates.

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

Hygroscopy, Deliquescence and Efflorescence.
Uses of salts.

By the end of the lesson, the learner should be able to:
To define hygroscopic deliquescent and efflorescent salts.
To give examples of hygroscopic deliquescent and efflorescent salts.

Prepare a sample of various salts.
Expose them to the atmosphere overnight.
Students classify the salts as hygroscopic, deliquescent and / or efflorescent.

K.L.B. BOOK II P. 114