CHEMICAL FAMILIES

Chemical properties of alkali metals.

By the end of the lesson, the learner should be able to:
To describe reaction of alkali metals with water.

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.

text book

K.L.B. BOOK IIP. 32

CHEMICAL FAMILIES

Reaction of alkali metals with chlorine gas.
Compounds of alkali metals.

By the end of the lesson, the learner should be able to:
To write balanced equations for reaction of alkali 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.

Sodium, chlorine.
text book

K.L.B. BOOK IIP. 33

CHEMICAL FAMILIES

Uses of alkali metals.

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

Descriptive approach: Teacher elucidates uses of alkali metals.

text book

K.L.B. BOOK II pp 34

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
K.L.B. BOOK II P. 35

CHEMICAL FAMILIES

Electrical properties of alkaline earth metals.

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

Teacher demonstration: -
To show alkaline metals are good conductors of electric charge.

Alkaline earth metals.

K.L.B. BOOK IIP. 37

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

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
Some alkaline earth metals.

K.L.B. BOOK IIP. 38

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.
Supervised practice.

Sodium, chlorine.
revision book

K.L.B. BOOK II P. 41
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.
Halogens. Physical properties of halogens.

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
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.

By the end of the lesson, the learner should be able to:
To state and explain the trends in physical properties of halogens.
To write balanced chemical equations of reactions involving halogens.

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

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

text book
Chlorine, iron wool, bromine.

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

CHEMICAL FAMILIES

Reaction of halogens with water.
Some uses of halogens and their compounds.

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.
text book

K.L.B. BOOK II P. 51

CHEMICAL FAMILIES
STRUCTURE & BONDING
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.

Make A comparative analysis of tabulated physical properties of noble gases.

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

  K.L.B. BOOK IIPP. 52-53

STRUCTURE & BONDING

Grant ionic structures.
Physical properties of ionic compounds.
Covalent bond.
Co-ordinate bond.
Molecular structure.

By the end of the lesson, the learner should be able to:
Describe the crystalline ionic compound.
Give examples of ionic substances.
Explain the formation of covalent bond
Use dot and cross diagrams to represent covalent bond.

Discuss the group ionic structures of NaCl.
Teacher gives examples of other ionic substances: KNO3, potassium bromide, Ca (NO3)2, sodium iodide.
Exposition: Shared pair of electrons in a hydrogen molecule, H2O, NH3, Cl2, and CO2.
Drawing of dot-and-cross diagrams of covalent bonds.

Giant sodium chloride model.
text book

K.L.B. BOOK II PP 56-58
K.L.B. BOOK II PP 60-63

STRUCTURE & BONDING

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 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.
Diagrams in textbooks.

K.L.B. BOOK IIP 65

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.
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.
Chlorides of period 3 elements.

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




To compare electrical conductivity of elements in period 3
To compare reactions of elements in period 3 with water

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.

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 IIP. 76
K.L.B. BOOK II PP. 80-81

SALTS

Types of salts.
Solubility of salts in water.

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
Sulphates, chlorides, nitrates, carbonates of various metals.

K.L.B. BOOK II P. 91

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.
Hygroscopy, Deliquescence and Efflorescence.

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
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES.
CARBON AND SOME OF ITS COMPOUNDS.

Uses of salts.
Electrical conductivity.
Allotropy.

By the end of the lesson, the learner should be able to:
To state uses of salts

Teacher elucidates uses of salts.

Various solids, bulb, battery, & wires.
text book

K.L.B. BOOK II P. 114

CARBON AND SOME OF ITS COMPOUNDS.

Physical and chemical properties of diamond, graphite and amorphous carbon
Burning carbon and oxygen.
Reduction properties of carbon.
Reaction of carbon with acids. Preparation of CO2.
Properties of CO2.

By the end of the lesson, the learner should be able to:
Describe physical and chemical properties of diamond, graphite and amorphous carbon.
State uses of carbon allotropes.
Describe reaction of carbon with acids.




Prepare CO2 in the lab.

Discuss physical and chemical properties of diamond, graphite and amorphous carbon.
Explain the Physical and chemical properties of diamond, graphite and amorphous carbon.
Discuss uses of carbon allotropes.
Teacher demonstration- reaction of carbon with hot conc HNO3.
Write balanced equations for the reaction.

Review effects of heat on carbonates.
Group experiments/teacher demonstration- preparation of CO2.

Charcoal, graphite.
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.

K.L.B. BOOK II pp 134
K.L.B. BOOK II P.126

CARBON AND SOME OF ITS COMPOUNDS.

Chemical equations for reactions involving CO2.
Uses of CO2.

By the end of the lesson, the learner should be able to:
Write balanced CO2.

Give examples of reactions. Write corresponding balanced chemical equations.

text book

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

CARBON AND SOME OF ITS COMPOUNDS.

Carbon monoxide lab preparation.
Chemical properties of carbon monoxide.
Carbonates and hydrogen carbonates.

By the end of the lesson, the learner should be able to:
To describe preparation of carbon monoxide in the lab

Teacher demonstration: preparation of carbon monoxide in the lab.
Make observations.

text book

K.L.B. BOOK II PP. 142-143

CARBON AND SOME OF ITS COMPOUNDS.

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 equations for reaction of carbonates and hydrogen carbonates on heating.
To discuss: - Importance of carbon in nature.
&
Effects of carbon on the environment.

Discuss the above observations.
Write corresponding balanced equations.
Discuss the carbon cycle and processes that increase/ reduce amount of CO2 in the air.
Uses of CO2 in soft drinks and fire extinguishers.

text book
text book, chart

K.L.B. BOOK II PP.150-151
K.L.B. BOOK II PP.157-158