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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 2 | 2 |
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
|
|
| 2 | 3-4 |
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 |
|
| 3 | 1 |
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
|
|
| 3 | 2 |
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
|
|
| 3 | 3-4 |
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
|
|
| 4 | 1 |
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
|
|
| 4 | 2 |
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
|
|
| 4 | 3-4 |
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. 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. |
K.L.B. BOOK II PP. 45-47
KLB BK II P. 47 |
|
| 5 | 1 |
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
|
|
| 5 | 2 |
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
|
|
| 5 | 3-4 |
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 |
|
| 6 | 1 |
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
|
|
| 6 | 2 |
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
|
|
| 6 | 3-4 |
CHEMICAL FAMILIES
STRUCTURE & BONDING |
Noble Gases.
Comparative physical properties of noble gases.
Uses of noble gases. Chemical bonds. Ionic bond. |
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
|
K.L.B. BOOK IIPP. 52-53
K.L.B. BOOK IIP54 PP 57-58 |
|
| 7 | 1 |
STRUCTURE & BONDING
|
Ionic bond representation.
Grant ionic structures. |
By the end of the
lesson, the learner
should be able to:
Use dot and cross diagrams to represent ionic bonding. |
Drawing diagrams of ionic bonds.
|
Chart- dot and cross diagrams.
Models for bonding. Giant sodium chloride model. |
K.L.B. BOOK II P. 58
|
|
| 7 | 2 |
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
|
|
| 7 | 3-4 |
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 co-ordinate bond To represent co-ordinate bond diagrammatically. |
Exposition: Shared pair of electrons in a hydrogen molecule, H2O, NH3, Cl2, and CO2.
Drawing of dot-and-cross diagrams of covalent bonds. Exposition- teacher explains the nature of co-ordinate bond. Students represent co-ordinate bond diagrammatically. |
text book
|
K.L.B. BOOK II PP 60-63
K.L.B. BOOK II P 65 |
|
| 8 | 1 |
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
|
|
| 8 | 2 |
STRUCTURE & BONDING
|
Giant atomic structure in diamond.
|
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
|
|
| 8 | 3-4 |
STRUCTURE & BONDING
PROPERTIES AND TRENDS ACROSS PERIOD THREE |
Giant atomic structure in graphite.
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 giant atomic structure in graphite. To state uses of graphite. To compare electrical conductivity of elements in period 3 |
Diagrammatic representation of graphite.
Discuss uses of graphite. 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. |
Diagrams in textbooks.
text book The periodic table. |
K.L.B. BOOK II pp 69
K.L.B. BOOK IIP. 76 |
|
| 9 | 1 |
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
|
|
| 9 | 2 |
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
|
|
| 9 | 3-4 |
PROPERTIES AND TRENDS ACROSS PERIOD THREE
|
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 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 |
|
| 10 | 1 |
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
|
|
| 10 | 2 |
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
|
|
| 10 | 3-4 |
SALTS
|
Solubility of salts in water.
Solubility of bases 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. To test solubility of various bases in water. To carry out litmus test on the resulting solutions. |
Class experiments- Dissolve salts in 5 cc of water.
Record the solubility in a table, Analyse the results. Class experiments- Dissolve salts in 5cc of water. Record the solubility in a table, Carry out litmus tests. Discuss the results. |
Sulphates, chlorides, nitrates, carbonates of various metals.
Oxides, hydroxides, of various metals, litmus papers. |
K.L.B. BOOK II PP. 92-93
K.L.B. BOOK IIPP. 94-95 |
|
| 11 | 1 |
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
|
|
| 11 | 2 |
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
|
|
| 11 | 3 |
SALTS
|
Ionic equations.
|
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.
|
K.L.B. BOOK II
|
|
| 11 | 3-4 |
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 |
|
| 12 | 1 |
SALTS
|
Effects of heat on nitrates.
|
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.
|
K.L.B. BOOK II PP. 110-111
|
|
| 12 | 2 |
SALTS
|
Effects of heat on sulphates.
|
By the end of the
lesson, the learner
should be able to:
To state effects of heat on sulphates. To predict products results from heating metal sulphates. |
Group experiments- To investigate effects of heat on various sulphates.
Observe various colour changes before, during and after heating. Write equations for the reactions. |
Common sulphates.
|
K.L.B. BOOK II P. 113
|
|
| 12 | 3-4 |
SALTS
EFFECTS OF AN ELECTRIC CURRENT ON SUBSTANCES. |
Hygroscopy, Deliquescence and Efflorescence.
Uses of salts. Electrical conductivity. |
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. To test for electrical conductivities of substances. |
Prepare a sample of various salts.
Expose them to the atmosphere overnight. Students classify the salts as hygroscopic, deliquescent and / or efflorescent. Group experiments- to identify conductors and non-conductors. Explain the difference in (non) conductivities. |
Various solids, bulb, battery, & wires. |
K.L.B. BOOK II P. 114
K.L.B. BOOK II PP. 118-119 |
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