CHEMICAL FAMILIES

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

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

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.

text book

K.L.B. BOOK IIP. 38

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.

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.

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.

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

text book

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

Uses of some alkaline earth metals and their compounds.
Halogens. Physical properties of halogens.
Comparative physical properties of halogens.

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

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.
text book

K.L.B. BOOK II PP. 45-47
KLB BK II
P. 47

CHEMICAL FAMILIES

Chemical properties of halogens.

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.

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.

Chlorine, iron wool, bromine.

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

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

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 write balanced chemical equations of reactions involving halogens.
To describe reaction of halogens with water and the results obtained.

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 gas, litmus papers.

K.L.B. BOOK II P. 50
K.L.B. BOOK II P. 51

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.

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.

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

STRUCTURE & BONDING

Physical properties of ionic compounds.

By the end of the lesson, the learner should be able to:
Describe physical properties of ionic compounds.
Explain the differences in the physical properties of ionic compounds.

Analyse tabulated comparative physical properties of ionic compounds.

Teacher asks probing questions.

text book

K.L.B. BOOK IIPP 58-59

STRUCTURE & BONDING

Covalent bond.
Co-ordinate bond.
Molecular structure.

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.
To describe the molecular structure.
To give examples of substance exhibiting molecular structure

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

Discussion ? To explain formation of the giant structure and give examples of substance exhibiting molecular structure.

text book

K.L.B. BOOK II PP 60-63
K.L.B. BOOK IIP 65

STRUCTURE & BONDING

Trend in physical properties of molecular structures.

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

Discuss comparative physical properties of substances. exhibiting molecular structure.
Explain variation in the physical properties.

Sugar, naphthalene, iodine rhombic sulphur.

K.L.B. BOOK IIP 65

STRUCTURE & BONDING

Giant atomic structure in diamond.
Giant atomic structure in graphite.

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

Diagrammatic representation of diamond.
Discuss uses of diamond.

Diagrams in textbooks.

K.L.B. BOOK II P 69

STRUCTURE & BONDING
PROPERTIES AND TRENDS ACROSS PERIOD THREE

Metallic bond. Uses of some metals.
Physical properties of elements in periods.

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.




To compare electrical conductivity of elements in period 3

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



Probing questions & brief explanations.

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.

text book
The periodic table.

K.L.B. BOOK IIP 70
K.L.B. BOOK IIP. 76

PROPERTIES AND TRENDS ACROSS PERIOD THREE

Physical properties of elements in period 3.

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

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

The periodic table.

K.L.B. BOOK II P. 77

PROPERTIES AND TRENDS ACROSS PERIOD THREE

Chemical properties of elements in period 3.

By the end of the lesson, the learner should be able to:
To compare reactions of elements in period 3 with oxygen.

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.

The periodic table.

K.L.B. BOOK II PP. 79-80

PROPERTIES AND TRENDS ACROSS PERIOD THREE

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

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

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

Comparative analysis, discussion and explanation.

The periodic table.

K.L.B. BOOK II PP. 80-81
K.L.B. BOOK II P. 84

SALTS

Types of salts.

By the end of the lesson, the learner should be able to:
Define a salt.
Describe various types of salts and give several examples in each case.

Descriptive approach. Teacher exposes new concepts.

text book

K.L.B. BOOK II P. 91

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

Methods of preparing various salts.

By the end of the lesson, the learner should be able to:
To describe various methods of preparing some salts.

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

CuO, H2SO4, HCl, NaOH, PbCO3, dil HNO3.

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.

To state effects of heat on carbonates.
To predict products resulting from heating metal carbonates.

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

Group experiments- To investigate effects of heat on Na2CO3, K2CO3, CaCO3, ZnCO3, PbCO3, e.t.c.
Observe various colour changes before, during and after heating.
Write equations for the reactions.

PbNO3, MgSO4 solutions.
Various carbonates.

K.L.B. BOOK II
K.L.B. BOOK II PP. 108-109

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.

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

SALTS
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Uses of salts.
Electrical conductivity.
Molten electrolytes.

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

Teacher elucidates uses of salts.
Group experiments- to identify conductors and non-conductors.
Explain the difference in (non) conductivities.

Various solids, bulb, battery, & wires.
Molten candle wax
Sugar
Sulphur
Lead oxide.

K.L.B. BOOK II P. 114
K.L.B. BOOK II PP. 118-119

EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.

Binary electrolyte.

By the end of the lesson, the learner should be able to:
To define a binary electrolyte.
To state the products of a binary electrolyte.

Completing a table of electrolysis of binary electrolytes.

text book

K.L.B. BOOK II P.127