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| WK | LSN | TOPIC | SUB-TOPIC | OBJECTIVES | T/L ACTIVITIES | T/L AIDS | REFERENCE | REMARKS |
|---|---|---|---|---|---|---|---|---|
| 1 |
Opening of school and opener exam |
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| 2 | 1-2 |
CHEMICAL FAMILIES
|
Alkali metals.
Atomic and ionic radii of alkali metals
Ionisation energy of alkali metals. |
By the end of the
lesson, the learner
should be able to:
Identify alkali metals. State changes in atomic and ionic radii of alkali metals. State changes in number of energy levels and ionisation energy of alkali metals. |
Q/A to reviews elements of group I and their electronic configuration. Examine a table of elements, their symbols and atomic & ionic radii. Discussion & making deductions from the table. Examine a table of elements, number of energy levels and their ionization energy. Discuss the trend deduced from the table. |
The periodic
text book |
K.L.B. BOOK IIPP 28-29
|
|
| 2 | 3 |
CHEMICAL FAMILIES
|
Ionisation energy of alkali metals.
|
By the end of the
lesson, the learner
should be able to:
State changes in number of energy levels and ionisation energy of alkali metals. |
Examine a table of elements, number of energy levels and their ionization energy.
Discuss the trend deduced from the table. |
text book
|
K.L.B. BOOK II
|
|
| 2 | 4 |
CHEMICAL FAMILIES
|
Physical properties of alkali metals.
|
By the end of the
lesson, the learner
should be able to:
State and explain trends in physical properties of alkali metals. |
Examine a table showing comparative physical properties of Li, Na, and K.
Q/A: Teacher asks probing questions as students refer to the table for answers. Detailed discussion on physical properties of alkali metals. |
Chart ? comparative properties of Li, Na, K.
|
K.L.B. BOOK IIPP 30-31
|
|
| 3 | 1-2 |
CHEMICAL FAMILIES
|
Chemical properties of alkali metals.
Reaction of alkali metals with chlorine gas. |
By the end of the
lesson, the learner
should be able to:
To describe reaction of alkali metals with water. To write balanced equations for reaction of alkali metals with chlorine gas. |
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. 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. |
text book
Sodium, chlorine. |
K.L.B. BOOK IIP. 32
K.L.B. BOOK IIP. 33 |
|
| 3 | 3 |
CHEMICAL FAMILIES
|
Reaction of alkali metals with chlorine gas.
|
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.
|
K.L.B. BOOK IIP. 33
|
|
| 3 | 4 |
CHEMICAL FAMILIES
|
Compounds of alkali metals.
|
By the end of the
lesson, the learner
should be able to:
Write chemical formulae for compounds of alkali metals. Explain formation of hydroxides, oxides and chlorides of alkali metals. |
Exercise: Completing a table of hydroxides, oxides and chlorides of alkali metals.
Discuss combination of ions of alkali metals with anions. |
text book
|
K.L.B. BOOK II pp 33
|
|
| 4 | 1-2 |
CHEMICAL FAMILIES
|
Uses of alkali metals.
Alkaline Earth metals Atomic and ionic radii of alkaline earth metals. |
By the end of the
lesson, the learner
should be able to:
State uses of alkali metals. Identify alkaline earth metals. State changes in atomic and ionic radii of alkaline earth metals. |
Descriptive approach: Teacher elucidates uses of alkali 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. |
text book
Some alkaline earth metals. |
K.L.B. BOOK II pp 34
|
|
| 4 | 3 |
CHEMICAL FAMILIES
|
Physical properties of alkaline earth metals.
|
By the end of the
lesson, the learner
should be able to:
State and explain trends in physical properties of alkaline earth metals. |
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 P. 35
|
|
| 4 | 4 |
CHEMICAL FAMILIES
|
Physical properties of alkaline earth metals.
|
By the end of the
lesson, the learner
should be able to:
State and explain trends in physical properties of alkaline earth metals. |
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 P. 35
|
|
| 5 | 1-2 |
CHEMICAL FAMILIES
|
Electrical properties of alkaline earth metals.
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 electrical properties of alkaline earth metals. To describe reaction of alkaline earth metals with oxygen |
Teacher demonstration: -
To show alkaline metals are good conductors of electric charge. 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. |
Alkaline earth metals.
text book |
K.L.B. BOOK IIP. 37
K.L.B. BOOK IIP. 38 |
|
| 5 | 3 |
CHEMICAL FAMILIES
|
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 water. |
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. |
Some alkaline earth metals.
|
K.L.B. BOOK IIP. 39
|
|
| 5 | 4 |
CHEMICAL FAMILIES
|
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 water. |
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. |
Some alkaline earth metals.
|
K.L.B. BOOK IIP. 39
|
|
| 6 | 1-2 |
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 |
|
| 6 | 3 |
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
|
|
| 6 | 4 |
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
|
|
| 7 | 1-2 |
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 |
|
| 7 | 3 |
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
|
|
| 7 | 4 |
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
|
|
| 8 | 1-2 |
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. 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 |
|
| 8 | 3 |
CHEMICAL FAMILIES
|
Noble Gases.
Comparative physical properties of noble gases.
Uses of noble gases. |
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
|
K.L.B. BOOK IIPP. 52-53
|
|
| 8 | 4 |
STRUCTURE & BONDING
|
Chemical bonds.
Ionic bond.
Ionic bond representation. |
By the end of the
lesson, the learner
should be able to:
Describe role of valence electrons in determining chemical bonding. Explain formation of ionic bonding. |
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
Chart- dot and cross diagrams. Models for bonding. |
K.L.B. BOOK IIP54
PP 57-58 |
|
| 9 | 1-2 |
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. Describe physical properties of ionic compounds. Explain the differences in the physical properties of ionic compounds. |
Discuss the group ionic structures of NaCl.
Teacher gives examples of other ionic substances: KNO3, potassium bromide, Ca (NO3)2, sodium iodide. Analyse tabulated comparative physical properties of ionic compounds. Teacher asks probing questions. |
Giant sodium chloride model.
text book |
K.L.B. BOOK II PP 56-58
K.L.B. BOOK IIPP 58-59 |
|
| 9 |
Midterm break |
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| 10 | 1-2 |
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 |
|
| 10 | 3 |
STRUCTURE & BONDING
|
Giant atomic structure in graphite.
|
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.
|
K.L.B. BOOK II pp 69
|
|
| 10 | 4 |
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
|
|
| 11 | 1-2 |
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. |
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 oxygen. |
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: 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 IIP. 76
K.L.B. BOOK II PP. 79-80 |
|
| 11 | 3 |
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 |
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 PP. 80-81
|
|
| 11 | 4 |
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
|
|
| 12 | 1-2 |
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 |
|
| 12 | 3 |
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
|
|
| 12 | 4 |
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
|
|
| 13 | 1-2 |
SALTS
|
Ionic equations.
Effects of heat on carbonates. Effects of heat on nitrates. |
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. Common metal nitrates. |
K.L.B. BOOK II
K.L.B. BOOK II PP. 108-109 |
|
| 13 | 3 |
SALTS
|
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 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
|
|
| 13 | 4 |
SALTS
|
Uses of salts.
|
By the end of the
lesson, the learner
should be able to:
To state uses of salts |
Teacher elucidates uses of salts.
|
|
K.L.B. BOOK II P. 114
|
|
| 14 |
End term2 examination and closure |
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