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

Reaction of alkaline earth metals with dilute acids.
Chemical formulae of alkaline earth metals.

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.
Write chemical formulae for compounds of alkaline earth metals.
Explain formation of hydroxides, oxides and chlorides of alkaline earth metals.

Changing word to chemical equations.
Supervised practice.
Exercise: Completing a table of hydroxides, oxides and chlorides of alkaline earth metals.
Discuss combination of ions of alkaline earth metals with anions.

revision book
text book

K.L.B. BOOK II PP. 43
K.L.B. BOOK II PP. 45-47

CHEMICAL FAMILIES

Uses of some alkaline earth metals and their compounds.

By the end of the lesson, the learner should be able to:
State uses of alkaline earth metals.

Descriptive approach: Teacher elucidates uses of alkaline earth metals.

text book

K.L.B. BOOK II PP. 45-47

CHEMICAL FAMILIES

Halogens. Physical properties of halogens.
Comparative physical properties of halogens.

By the end of the lesson, the learner should be able to:
Identify halogens in the periodic table.
Give examples of halogens.
Identify physical states of halogens.

Teacher demonstration: - To examine electrical properties of iodine, solubility in water of chlorine.

Iodine crystals, electrical wire, a bulb.
text book

KLB BK II
P. 47

CHEMICAL FAMILIES

Chemical properties of halogens.
Equations of reaction of halogens with metals.

By the end of the lesson, the learner should be able to:
To describe laboratory preparation of chlorine gas.

To describe reaction of halogens with metals.
To write balanced chemical equations of reactions involving halogens.

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.

Chlorine, iron wool, bromine.
text book

K.L.B. BOOK IIPP. 48-50
K.L.B. BOOK II P. 50

CHEMICAL FAMILIES

Reaction of halogens with water.

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

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

Chlorine gas, litmus papers.

K.L.B. BOOK II P. 51

CHEMICAL FAMILIES

Some uses of halogens and their compounds.

By the end of the lesson, the learner should be able to:
To state uses of halogens and their compounds.

Teacher elucidates uses of halogens and their compounds.

text book

K.L.B. BOOK II pp 52

CHEMICAL FAMILIES
STRUCTURE & BONDING

Noble Gases. Comparative physical properties of noble gases.
Uses of noble gases.
Chemical bonds. Ionic bond.
Ionic bond representation.

By the end of the lesson, the learner should be able to:
To describe physical properties of noble gases.
To explain physical properties of noble gases.
Describe role of valence electrons in determining chemical bonding.


Explain formation of ionic bonding.

Make A comparative analysis of tabulated physical properties of noble gases.
Q/A: Review valence electrons of atoms of elements in groups I, II, III, VII and VIII.
Q/A: Review group I and group VII elements.
Discuss formation of ionic bond.

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

  K.L.B. BOOK IIPP. 52-53
K.L.B. BOOK IIP54




PP 57-58

STRUCTURE & BONDING

Grant ionic structures.
Physical properties of ionic compounds.

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

Covalent bond.
Co-ordinate bond.

By the end of the lesson, the learner should be able to:
Explain the formation of covalent bond
Use dot and cross diagrams to represent covalent bond.

Exposition: Shared pair of electrons in a hydrogen molecule, H2O, NH3, Cl2, and CO2.
Drawing of dot-and-cross diagrams of covalent bonds.

text book

K.L.B. BOOK II PP 60-63

STRUCTURE & BONDING

Molecular structure.
Trend in physical properties of molecular structures.
Giant atomic structure in diamond.
Giant atomic structure in graphite.

By the end of the lesson, the learner should be able to:
To describe the molecular structure.
To give examples of substance exhibiting molecular structure
To describe giant atomic structure in diamond.
To state uses of diamond.

Discussion ? To explain formation of the giant structure and give examples of substance exhibiting molecular structure.
Diagrammatic representation of diamond.
Discuss uses of diamond.

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

K.L.B. BOOK IIP 65
K.L.B. BOOK II P 69

STRUCTURE & BONDING

Metallic bond. Uses of some metals.

By the end of the lesson, the learner should be able to:
To describe mutual electronic forces between electrons and nuclei.
To describe metallic bond.
To compare physical properties of metals.
To state uses of some metals.

Discussion:
Detailed analysis of comparative physical properties of metals and their uses.



Probing questions & brief explanations.

text book

K.L.B. BOOK IIP 70

PROPERTIES AND TRENDS ACROSS PERIOD THREE

Physical properties of elements in periods.

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

Physical properties of elements in period 3.
Chemical properties of elements in period 3.
Chemical properties of elements in the third period.
Oxides of period 3 elements.

By the end of the lesson, the learner should be able to:
To compare other physical properties of elements across period 3.
To compare reactions of elements in period 3 with water

Analyse comparative physical properties presented in form of a table.
Explain the trend in the physical properties given.

Q/A: Review reaction of sodium, Mg, chlorine, with water.
Infer that sodium is most reactive metal; non-metals do not react with water.

The periodic table.

K.L.B. BOOK II P. 77
K.L.B. BOOK II PP. 80-81

PROPERTIES AND TRENDS ACROSS PERIOD THREE
SALTS

Chlorides of period 3 elements.
Types of salts.

By the end of the lesson, the learner should be able to:
To explain chemical behavior of their chlorides.
To describe hydrolysis reaction.

Comparative analysis, discussion and explanation.

The periodic table.
text book

K.L.B. BOOK II PP. 77-78

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.
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.
To describe various methods of preparing some salts.

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


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

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

K.L.B. BOOK IIPP. 94-95
K.L.B. BOOK II pp96

SALTS

Direct synthesis of a salts.

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

K.L.B. BOOK II P. 104

SALTS

Ionic equations.
Effects of heat on carbonates.

By the end of the lesson, the learner should be able to:
To identify spectator ions in double decomposition reactions.
To write ionic equations correctly.

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

PbNO3, MgSO4 solutions.
Various carbonates.

K.L.B. BOOK II

SALTS

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

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.
To define hygroscopic deliquescent and efflorescent salts.
To give examples of hygroscopic deliquescent and efflorescent salts.

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.

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

Common metal nitrates.
Common sulphates.

K.L.B. BOOK II PP. 110-111
K.L.B. BOOK II P. 114

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Electrical conductivity.

By the end of the lesson, the learner should be able to:
To test for electrical conductivities of substances.

Group experiments- to identify conductors and non-conductors.
Explain the difference in (non) conductivities.

Various solids, bulb, battery, & wires.

K.L.B. BOOK II PP. 118-119