WK
| | SCHEME OF WORK FORM TWO CHEMISTRY TERM ONE 2019 | |
|WK |L/ |TOPIC/ |LESSON / SPECIFIC |TEACHING / LEARNING |MATERIALS |REFERE- |REMARKS |
|NO. |NO |SUBTOPIC |OBJECTIVES |ACTIVITIES |/ |NCES | |
| | | | | |RESOURCES | | |
|1 |1 |THE STRUCTURE OF THE ATOM & THE |By the end of the lesson, the learner |Exposition on new concepts; | |K.L.B. | |
| | |PERIODIC TABLE |should be able to: |Probing questions; | |BOOK II | |
| | | | |Brief discussion. | | | |
| | |Atomic and mass numbers. |Name the subatomic particles in an atom. | | |PP. 1-3 | |
| | | |Define atomic number and mass number of an| | | | |
| | | |atom. | | | | |
| | | |Represent atomic and mass numbers | | | | |
| | | |symbolically. | | | | |
| |2 |First twenty elements of the |List the first twenty elements of the |Expository approach: referring to the periodic |Periodic table. |K.L.B. | |
| | |periodic table. |periodic table. |table, teacher exposes the first twenty | |BOOK II | |
| | | |Write chemical symbols of the first twenty|elements. | | | |
| | | |elements of the periodic table. |Writing down a list of first twenty elements of| |PP. 1-3 | |
| | | | |the periodic table. | | | |
| |3 |Isotopes. |Define isotopes. |Exposition of definition and examples of |Periodic table. |K.L.B. | |
| | | |Give examples of isotopes. |isotopes. | |BOOK II | |
| |& | | |Giving examples of isotopes. | |P. 4 | |
| | | | | | | | |
| | | |Represent isotopes symbolically. |Exposition – teacher exposes new concepts about| | | |
| |4 |Electronic configuration. |Define an energy level. |electronic configuration. | | | |
| | | |Describe electronic configuration in an |Written exercise. | | | |
| | | |atom. | | | | |
| | | | | | |PP. 5-8 | |
| | | | | | | | |
|2 |1 |Electronic configuration in |Represent electronic configuration |Supervised practice; | |K.L.B. | |
| | |diagrams. |diagrammatically. |Written exercise. | |BOOK II | |
| | | | | | |PP. 5-8 | |
| |2 |Periods of the periodic table. |Identify elements of the same period. |Exposition – Definition of a period. |Periodic table. |P. 9 | |
| | | | |Q/A: Examples of elements of the same period. | | | |
| |3 |Groups of the periodic table. |Identify elements of the same period. |Exposition – definition of a group. |Periodic table. |P. 9 | |
| | | | |Q/A: examples of elements of the same group. | | | |
| |4 |R.M.M. and isotopes. |Calculate RMM from isotopic composition. |Teacher exposes definition of R.M.M. | |PP. 11-13 | |
| | | |To describe relative abundance of isotopes| | | | |
| | | |of an element. |Worked examples. | | | |
|3 |1 |R.M.M. and isotopes. |Calculate R.M.M. from isotopic |Supervised practice involving calculation of | |PP. 11-13 | |
| | | |composition. |RMM from isotopic composition. | | | |
| |2 |Positive ions and ion formation. |To define an ion and a cation. |Teacher gives examples of stable atoms. | |PP 14-15 | |
| | | | |Guided discovery that metals need to lose one, | | | |
| | | | |two or three electrons to attain stability. | | | |
| | | | |Examples of positive ions. | | | |
| | | | | | | | |
|3 |3 |Positive ions representation. |To represent formation of positive ions |Diagrammatic representation of cations. |Chart – ion model. |P 16 | |
| | | |symbolically. | | | | |
| |4 |Negative ions and ion formation. |To define an anion. |Teacher gives examples of stable atoms. |Chart – ion model. |P 17 | |
| | | |To describe formation of negative ions |Guided discovery of formation of negative ions.| | | |
| | | |symbolically. |Diagrammatic representation of anions. | | | |
|4 |1 |Valencies of metals. |Recall valencies of metals among the first|Q/A to review previous lesson; |Periodic table. |P 17 | |
| | | |twenty elements in the periodic table. |Exposition; | | | |
| | | | |Guided discovery. | | | |
| |2 |Valencie of non-metals. |Recall valencies of non-metals among the |Q/A to review previous lesson; |Periodic table. |P 17 | |
| | | |first twenty elements in the periodic |Exposition; | | | |
| | | |table. |Guided discovery. | | | |
| |3 |Valencies of radicals. |Define a radical. |Exposition – teacher defines a radical, gives | |P 18 | |
| | | |Recall the valencies of common radicals. |examples of radicals and exposes their | | | |
| | | | |valencies. | | | |
| | | | |Students draw a table of radicals and their | | | |
| | | | |valencies. | | | |
| |4 |Oxidation number. |Define oxidation number. |Q/A: Valencies. |The periodic table. |P 18 | |
| | | |Predict oxidation numbers from position of|Expose oxidation numbers of common ions. | | | |
| | | |elements in the periodic table. |Students complete a table of ions and their | | | |
| | | | |oxidation numbers. | | | |
|5 |1 |Electronic configuration, ion |Relate electronic configuration, ion |Written exercise; | |P 18 | |
| | |formed, valency and oxidation number|formed, valency and oxidation number of |Exercise review. | | | |
| | | |different elements. | | | | |
| |2 |Chemical formulae of compounds. |To derive the formulae of some compounds |Discuss formation of compounds such as NaCl, | |PP 19-20 | |
| | |- Elements of equal valencies. |involving elements of equal valencies. |MgO. | | | |
| |3 |Chemical formulae of compounds. |To derive the formulae of some compounds |Discuss formation of compounds such as MgCl2 | |PP 19-20 | |
| | |-Elements of unequal valencies. |involving elements of unequal valencies. |Al (NO3)3 | | | |
| |4 |Chemical formulae of compounds. |To derive the formulae of some compounds |Discuss formation of compounds such as | |P 20 | |
| | |-Elements of variable valencies. |involving elements of variable valencies. |-Copper (I) Oxide. | | | |
| | | | |-Copper (II) Oxide. | | | |
| | | | |-Iron (II) Sulphate. | | | |
| | | | |-Iron (III) Sulphate. | | | |
|6 |1 |Chemical equations. |To identify components of chemical |Review word equations; | |PP 21-23 | |
| | | |equations. |Exposition of new concepts with probing | | | |
| | | | |questions; | | | |
| | | | |Brief discussion. | | | |
| |2 |Balanced chemical equations. |To balance chemical equations correctly. |Exposition; | |PP 24-25 | |
| | | | |Supervised practice. | | | |
| |3 |Balanced chemical equations.(contd) |To balance chemical equations correctly. |Supervised practice; | |PP 25-8 | |
| | | | |Written exercise. | | | |
| |4 |TEST | | | | | |
|7 |1 |CHEMICAL FAMILIES | | |The periodic | | |
| | | | |Q/A to reviews elements of group I and their | |PP 28-29 | |
| | |Alkali metals. | |electronic configuration. | | | |
| | | | |Examine a table of elements, their symbols and | | | |
| | |Atomic and ionic radii of alkali | |atomic & ionic radii. | | | |
| | |metals |Identify alkali metals. |Discussion & making deductions from the table. | | | |
| | | |State changes in atomic and ionic radii of| | | | |
| | | |alkali metals. | | | | |
| |2 |Ionisation energy of alkali metals. |State changes in number of energy levels |Examine a table of elements, number of energy | | | |
| | | |and ionisation energy of alkali metals. |levels and their ionization energy. | | | |
| | | | |Discuss the trend deduced from the table. | | | |
| |3,4 |Physical properties of alkali |State and explain trends in physical |Examine a table showing comparative physical |Chart – comparative |PP 30-31 | |
| | |metals. |properties of alkali metals. |properties of Li, Na, and K. |properties of Li, Na, K. | | |
| | | | |Q/A: Teacher asks probing questions as students| | | |
| | | | |refer to the table for answers. | | | |
| | | | |Detailed discussion on physical properties of | | | |
| | | | |alkali metals. | | | |
| | | | | | | | |
|8 |1 |Chemical properties of alkali |To describe reaction of alkali metals with|Q/A: review reactions of Na, K, etc. with | |P 31 | |
| | |metals. |oxygen. |oxygen. | | | |
| | | | |The corresponding word and then chemical | | | |
| | | | |equations are then written. | | | |
|8 |2 |Chemical properties of alkali |To describe reaction of alkali metals with|Q/A: Review reaction of metals with water. | |P. 32 | |
| | |metals. |water. |Writing down chemical equations for the | | | |
| | | | |reactions. | | | |
| | | | |Deduce and discuss the order of reactivity down| | | |
| | | | |the group. | | | |
| |3,4 |Reaction of alkali metals with |To write balanced equations for reaction |Teacher demonstration- reaction of sodium with |Sodium, chlorine. |P. 33 | |
| | |chlorine gas. |of alkali metals with chlorine gas. |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. | | | |
| | | | | | | | |
|9 |1 |Compounds of alkali metals. |Write chemical formulae for compounds of |Exercise: Completing a table of hydroxides, | | | |
| | | |alkali metals. |oxides and chlorides of alkali metals. | | | |
| | | |Explain formation of hydroxides, oxides |Discuss combination of ions of alkali metals | | | |
| | | |and chlorides of alkali metals. |with anions. | | | |
| |2 |Uses of alkali metals. |State uses of alkali metals. |Descriptive approach: Teacher elucidates uses | | | |
| | | | |of alkali metals. | | | |
|9 |3 |Alkaline Earth metals |Identify alkaline earth metals. |Q/A: Elements of group I and their electron |Some alkaline earth metals. | | |
| | | | |configuration. | | | |
| | |Atomic and ionic radii of alkaline |State changes in atomic and ionic radii of|Examine a table of elements, their symbols and | | | |
| | |earth metals. |alkaline earth metals. |atomic & ionic radii. | | | |
| | | | |Make deductions from the table. | | | |
| |4 |Physical properties of alkaline |State and explain trends in physical |Examine a table showing comparative physical |Some alkaline earth metals. |P. 35 | |
| | |earth metals. |properties of alkaline earth metals. |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. | | | |
|10 |1 |Electrical properties of alkaline |To describe electrical properties of |Teacher demonstration: - |Alkaline earth metals. |P. 37 | |
| | |earth metals. |alkaline earth metals. |To show alkaline metals are good conductors of | | | |
| | | | |electric charge. | | | |
| |2 |Chemical properties of alkaline |To describe reaction of alkaline earth |Q/A: Review reactions of Mg, Ca, with oxygen. | |P. 38 | |
| | |earth metals. |metals with oxygen |The corresponding word and then chemical | | | |
| | |Reaction of alkaline earth metals | |equations are then written and their | | | |
| | |with oxygen. | |correctness verified by the teacher. | | | |
|10 |3 |Chemical properties of alkaline |To describe reaction of alkaline earth |Q/A: Review reaction of metals with water. |Some alkaline earth metals. |P. 39 | |
| | |earth metals. |metals with water. |Writing down word and balanced chemical | | | |
| | |Reaction of alkaline earth metals | |equations for the reactions. | | | |
| | |with water. | |Deduce and discuss the order of reactivity down| | | |
| | | | |the group. | | | |
| |4 |Reaction of alkaline earth metals |To write balanced equations for reaction |Teacher demonstration- Reaction of sodium with |Sodium, chlorine. |P. 41 | |
| | |with chlorine gas. |of alkaline earth metals with chlorine |chlorine in a fume chamber. | | | |
| | | |gas. |Q/A: Students to predict a similar reaction | | | |
| | | | |between potassium and chlorine. | | | |
| | | | |Word and balanced chemical equations for | | | |
| | | | |various reactions. | | | |
| | | | |Supervised practice. | | | |
|11 |1 |Reaction of alkaline earth metals |To describe reaction of alkaline earth |Group experiments- |Magnesium ribbon, dilute HCl,|P. 42 | |
| | |with dilute acids. |metals with acids. |Drop a ribbon of Mg in dilute HCl, H2SO4. |dilute H2SO4. | | |
| | | | |Test for evolved gas with a burning splint. | | | |
| |2 |Reaction of alkaline earth metals |To write balanced equations for reactions |Changing word to chemical equations. | |PP. 43 | |
| | |with dilute acids. |of alkaline earth metals with dilute |Supervised practice. | | | |
| | | |acids. | | | | |
|11 |3 |Chemical formulae of alkaline earth |Write chemical formulae for compounds of |Exercise: Completing a table of hydroxides, | |PP. 45-47 | |
| | |metals. |alkaline earth metals. |oxides and chlorides of alkaline earth metals. | | | |
| | | |Explain formation of hydroxides, oxides |Discuss combination of ions of alkaline earth | | | |
| | | |and chlorides of alkaline earth metals. |metals with anions. | | | |
| |4 |Uses of some alkaline earth metals |State uses of alkaline earth metals. |Descriptive approach: Teacher elucidates uses | |PP. 45-47 | |
| | |and their compounds. | |of alkaline earth metals. | | | |
|12-13 |END OF FIRST TERM EXAMS | |
| | SCHEME OF WORK FORM TWO CHEMISTRY TERM TWO 2019 | |
|WK |L/ |TOPIC/ |LESSON / SPECIFIC |TEACHING / LEARNING |MATERIALS |REFERE- |REMARKS |
|NO. |NO |SUBTOPIC |OBJECTIVES |ACTIVITIES |/ |NCES | |
| | | | | |RESOURCES | | |
|1 |1 |Halogens. |Identify halogens in the periodic table. |Teacher demonstration: - To examine electrical |Iodine crystals, electrical |KLB BK II | |
| | | |Give examples of halogens. |properties of iodine, solubility in water of |wire, a bulb. |P. 47 | |
| | |Physical properties of halogens. |Identify physical states of halogens. |chlorine. | | | |
| |2 |Comparative physical properties of |To state and explain the trends in |Examine a comparative table of physical | |P. 47 | |
| | |halogens. |physical properties of halogens. |properties of halogens. | | | |
| | | | |Discuss the deductions made from the table. | | | |
| |3,4 |Chemical properties of halogens. |To describe laboratory preparation of |Teacher demonstration: - preparation of |Chlorine, iron wool, bromine.|PP. 48-50 | |
| | | |chlorine gas. |chlorine gas. | | | |
| | | | |Reaction of chlorine and iron wool. | | | |
| | | |To describe reaction of halogens with |Reaction of bromine and iron wool. | | | |
| | | |metals. |Reaction of iodine and iron wool. | | | |
| | | | |Observe the rate of these reactions; hence | | | |
| | | | |deduce order of their reactivity of halogens. | | | |
|2 |1 |Equations of reaction of halogens |To write balanced chemical equations of |Re-write word equations as chemical equations | |P. 50 | |
| | |with metals. |reactions involving halogens. |then balance them. | | | |
| | | | |Supervised practice. | | | |
|2 |2 |Reaction of halogens with water. |To describe reaction of halogens with |Bubbling chlorine gas through water. |Chlorine gas, litmus papers. |P. 51 | |
| | | |water and the results obtained. |Carry out litmus test for the water. | | | |
| | | | |Explain the observations. | | | |
| |3,4 |Some uses of halogens and their |To state uses of halogens and their |Teacher elucidates uses of halogens and their | | | |
| | |compounds. |compounds. |compounds. | | | |
|3 |1 |Noble Gases. |To describe physical properties of noble |Make A comparative analysis of tabulated | |PP. 52-53 | |
| | | |gases. |physical properties of noble gases. | | | |
| | |Comparative physical properties of |To explain physical properties of noble | | | | |
| | |noble gases. |gases. | | | | |
| |2 |Uses of noble gases. |State uses of noble gases. |Teacher elucidates uses of noble gases. | |P. 54 | |
| |3 |STRUCTURE & BONDING |Describe role of valence electrons in |Q/A: Review valence electrons of atoms of | |P54 | |
| | | |determining chemical bonding. |elements in groups I, II, III, VII and VIII. | | | |
| | |Chemical bonds. | |Q/A: Review group I and group VII elements. | | | |
| | | | |Discuss formation of ionic bond. | | | |
| | |Ionic bond. |Explain formation of ionic bonding. | | | | |
| | | | | | |PP 57-58 | |
| |4 |Ionic bond representation. |Use dot and cross diagrams to represent |Drawing diagrams of ionic bonds. |Chart- dot and cross |P. 58 | |
| | | |ionic bonding. | |diagrams. | | |
| | | | | |Models for bonding. | | |
|4 | |Grant ionic structures. |Describe the crystalline ionic compound. |Discuss the group ionic structures of NaCl. |Giant sodium chloride model. |PP 56-58 | |
| |1 | |Give examples of ionic substances. |Teacher gives examples of other ionic | | | |
| | | | |substances: KNO3, potassium bromide, Ca (NO3)2,| | | |
| | | | |sodium iodide. | | | |
| |2 |Physical properties of ionic |Describe physical properties of ionic |Analyse tabulated comparative physical | |PP 58-59 | |
| | |compounds. |compounds. |properties of ionic compounds. | | | |
| | | |Explain the differences in the physical | | | | |
| | | |properties of ionic compounds. |Teacher asks probing questions. | | | |
| |3,4 |Covalent bond. |Explain the formation of covalent bond |Exposition: Shared pair of electrons in a | |PP 60-63 | |
| | | |Use dot and cross diagrams to represent |hydrogen molecule, H2O, NH3, Cl2, and CO2. | | | |
| | | |covalent bond. |Drawing of dot-and-cross diagrams of covalent | | | |
| | | | |bonds. | | | |
|5 |1 |Co-ordinate bond. |To describe the co-ordinate bond |Exposition- teacher explains the nature of | |P 65 | |
| | | |To represent co-ordinate bond |co-ordinate bond. | | | |
| | | |diagrammatically. |Students represent co-ordinate bond | | | |
| | | | |diagrammatically. | | | |
| |2 |Molecular structure. |To describe the molecular structure. |Discussion – To explain formation of the giant | |P 65 | |
| | | |To give examples of substance exhibiting |structure and give examples of substance | | | |
| | | |molecular structure |exhibiting molecular structure. | | | |
| |3 & 4 |Trend in physical properties of |To describe van- der -waals forces. |Discuss comparative physical properties of |Sugar, naphthalene, iodine |P 65 | |
| | |molecular structures. |To explain the trend in physical |substances. exhibiting molecular structure. |rhombic sulphur. | | |
| | | |properties of molecular structures. |Explain variation in the physical properties. | | | |
|6 |1 |Giant atomic structure in diamond. |To describe giant atomic structure in |Diagrammatic representation of diamond. |Diagrams in textbooks. |P 69 | |
| | | |diamond. |Discuss uses of diamond. | | | |
| | | |To state uses of diamond. | | | | |
| |2 |Giant atomic structure in graphite. |To describe giant atomic structure in |Diagrammatic representation of graphite. |Diagrams in textbooks. | | |
| | | |graphite. | | | | |
| | | |To state uses of graphite. |Discuss uses of graphite. | | | |
| |3 |Metallic bond. |To describe mutual electronic forces |Discussion: | |P 70 | |
| | | |between electrons and nuclei. |Detailed analysis of comparative physical | | | |
| | | |To describe metallic bond. |properties of metals and their uses. | | | |
| | | |To compare physical properties of metals. | | | | |
| | | |To state uses of some metals. | | | | |
| | | | | | | | |
| | | | |Probing questions & brief explanations. | | | |
| | | | | | | | |
| | |Uses of some metals. | | | | | |
| |4 |TEST | | | | | |
|7 |1 |PROPERTIES AND TRENDS ACROSS PERIOD | |Group experiments- Construct electrical |The periodic table. |P. 76 | |
| | |THREE | |circuits incorporating a magnesium ribbon, then| | | |
| | | | |aluminum foil, then sulphur in turns. | | | |
| | |Physical properties of elements in | |The brightness of the bulb is noted in each | | | |
| | |periods. |To compare electrical conductivity of |case. | | | |
| | | |elements in period 3 |Discuss the observations in terms of | | | |
| | | | |delocalised electrons. | | | |
| |2 |Physical properties of elements in |To compare other physical properties of |Analyse comparative physical properties |The periodic table. |P. 77 | |
| | |period 3. |elements across period 3. |presented in form of a table. | | | |
| | | | |Explain the trend in the physical properties | | | |
| | | | |given. | | | |
| |3 |Chemical properties of elements in |To compare reactions of elements in period|Q/A: Products of reactions of Na, Mg, Al, P, & |The periodic table. |PP. 79-80 | |
| | |period 3. |3 with oxygen. |S with oxygen. | | | |
| | | | |Discuss the trend in their reactivity; identify| | | |
| | | | |basic and acidic oxides. | | | |
| | | | |Exercise – balanced chemical equations for the | | | |
| | | | |above reactions. | | | |
| |4 |Chemical properties of elements in |To compare reactions of elements in period|Q/A: Review reaction of sodium, Mg, chlorine, |The periodic table. |PP. 80-81 | |
| | |the third period. |3 with water |with water. | | | |
| | | | |Infer that sodium is most reactive metal; | | | |
| | | | |non-metals do not react with water. | | | |
|8 |1 |Oxides of period 3 elements. |To identify bonds across elements in |Comparative analysis, discussion and |The periodic table. |P. 84 | |
| | | |period 3. |explanation. | | | |
| | | |To explain chemical behavior of their | | | | |
| | | |oxide. | | | | |
| |2 |Chlorides of period 3 elements. |To explain chemical behavior of their |Comparative analysis, discussion and |The periodic table. |PP. 77-78 | |
| | | |chlorides. |explanation. | | | |
| | | |To describe hydrolysis reaction. | | | | |
| |3,4 |SALTS |Define a salt. |Descriptive approach. Teacher exposes new | |P. 91 | |
| | | |Describe various types of salts and give |concepts. | | | |
| | |Types of salts. |several examples in each case. | | | | |
|9 |1,2 |Solubility of salts in water. |To test solubility of various salts in |Class experiments- Dissolve salts in 5 cc of |Sulphates, chlorides, |PP. 92-93 | |
| | | |cold water/warm water. |water. |nitrates, carbonates of | | |
| | | | |Record the solubility in a table, |various metals. | | |
| | | | |Analyse the results. | | | |
| | | | | | | | |
| | | | | | | | |
| |3,4 |Solubility of bases in water. |To test solubility of various bases in |Class experiments- Dissolve salts in 5cc of |Oxides, hydroxides, of |PP. 94-95 | |
| | | |water. |water. |various metals, litmus | | |
| | | |To carry out litmus test on the resulting |Record the solubility in a table, |papers. | | |
| | | |solutions. |Carry out litmus tests. | | | |
| | | | |Discuss the results. | | | |
| | | | | | | | |
|10 |1-4 |Methods of preparing various salts. |To describe various methods of preparing |Experimental and descriptive treatments of |CuO, H2SO4, HCl, NaOH, PbCO3,| | |
| | | |some salts. |preparation of salts e.g. ZnSO4, CuSO4, NaCl |dil HNO3. | | |
| | | | |and Pb(NO3)2. | | | |
| | | | | | | | |
|11 |1,2 |Direct synthesis of a salts. |To describe direct synthesis of a salt. |Group experiments- preparation of iron (II) |Iron, |P. 104 | |
| | | |To write balanced equations for the |sulphide by direct synthesis. |Sulphur | | |
| | | |reactions. |Give other examples of salts prepared by direct| | | |
| | | | |synthesis. | | | |
| | | | |Students write down corresponding balanced | | | |
| | | | |equations. | | | |
| | | | | | | | |
| |3,4 |Ionic equations. |To identify spectator ions in double |Q/A: Ions present in given reactants. |PbNO3, MgSO4 solutions. | | |
| | | |decomposition reactions. |Deduce the products of double decomposition | | | |
| | | |To write ionic equations correctly. |reactions. | | | |
| | | | |Give examples of equations. | | | |
| | | | |Supervised practice. | | | |
|12 |END OF SECOND TERM TEST | |
|13 | | |
SCHEME OF WORK FORM TWO CHEMISTRY TERM THREE 2019
|WK |L/ |TOPIC/ |LESSON / SPECIFIC |TEACHING / LEARNING |MATERIALS |REFERE- |REMARKS |
|NO. |NO |SUBTOPIC |OBJECTIVES |ACTIVITIES |/ |NCES | |
| | | | | |RESOURCES | | |
|1 |1 |Effects of heat on carbonates. |To state effects of heat on carbonates. |Group experiments- To investigate effects of |Various carbonates. |PP. 108-109 | |
| | | |To predict products resulting from heating|heat on Na2CO3, K2CO3, CaCO3, ZnCO3, PbCO3, | | | |
| | | |metal carbonates. |e.t.c. | | | |
| | | | |Observe various colour changes before, during | | | |
| | | | |and after heating. | | | |
| | | | |Write equations for the reactions. | | | |
| |2 |Effects of heat on nitrates. |To state effects of heat on nitrates. |Group experiments- To investigate effects of |Common metal nitrates. |PP. 110-111 | |
| | | |To predict products resulting from heating|heat on various metal nitrates. | | | |
| | | |metal nitrates. |Observe various colour changes before, during | | | |
| | | | |and after heating. | | | |
| | | | |Write equations for the reactions. | | | |
| |3,4 |Effects of heat on sulphates. |To state effects of heat on sulphates. |Group experiments- To investigate effects of |Common sulphates. |P. 113 | |
| | | |To predict products results from heating |heat on various sulphates. | | | |
| | | |metal sulphates. |Observe various colour changes before, during | | | |
| | | | |and after heating. | | | |
| | | | |Write equations for the reactions. | | | |
|2 |1 |Hygroscopy, Deliquescence and |To define hygroscopic deliquescent and |Prepare a sample of various salts. | |P. 114 | |
| | |Efflorescence. |efflorescent salts. |Expose them to the atmosphere overnight. | | | |
| | | |To give examples of hygroscopic |Students classify the salts as hygroscopic, | | | |
| | | |deliquescent and efflorescent salts. |deliquescent and / or efflorescent. | | | |
| |2 |Uses of salts. |To state uses of salts |Teacher elucidates uses of salts. | |P. 114 | |
| |3,4 |EFFECTS OF AN ELECTRIC CURRENT ON |To test for electrical conductivities of |Group experiments- to identify conductors and |Various solids, bulb, |PP. 118-119 | |
| | |SUBSTANCES. |substances. |non-conductors. |battery, & wires. | | |
| | | | |Explain the difference in (non) conductivities.| | | |
| | |Electrical conductivity. | | | | | |
|3 |1,2 |Molten electrolytes. |To test for electrical conductivities |Group experiments- to identify electrolytes in |Molten candle wax |PP. 120-121 | |
| | | |molten electrolytes. |molten form. |Sugar | | |
| | | | |Explain the difference in molten electrolytes. |Sulphur | | |
| | | | | |Lead oxide. | | |
| |3,4 |Electrolysis. |To define electrolysis |Descriptive approach punctuated with Q/A. | | | |
| | | |To describe the process of electrolysis in| | | | |
| | | |terms of charge movement. | | | | |
|4 |1,2 |Aqueous electrolytes. |To define an electrolyte |To investigate chemical effect of an electric |Graphite electrodes |PP.122-123 | |
| | |Electrodes. |To test for electrical conductivities of |current. |Battery | | |
| | | |electrodes. |Classify the solutions as electrolyte or non |Various aqueous solutions | | |
| | | | |-electrolytes. |switch bulb. | | |
| | | | |Discuss the electrical properties of the | | | |
| | | | |solutions. | | | |
| |3,4 |Reaction on electrodes. |To describe half- equation reactions at |To demonstrate –Electrolysis of molten lead |Graphite electrodes |PP.126-127 | |
| | | |the cathode and anode |(II) bromide |Battery | | |
| | | | |Observe colour changes |Various aqueous solutions | | |
| | | | |Explanation of half-equations and reactions at |switch. | | |
| | | | |the electrodes. | | | |
|5 |1,2 |Binary electrolyte. |To define a binary electrolyte. |Completing a table of electrolysis of binary | |P.127 | |
| | | |To state the products of a binary |electrolytes. | | | |
| | | |electrolyte. | | | | |
| |3 |Application of electrolysis. |To state application of electrolysis. |Discussion and explanations. | |P. 128 | |
| |4 |Electroplating. |To describe electroplating process. |Experiment- Left overnight. |Silver nitrate |PP. 129-30 | |
| | | | |Electroplating an iron nail with silver |Iron nail | | |
| | | | |nitrate/ copper sulphate. |Complete circuit battery. | | |
| | | | |Brief discussion. | | | |
| | | | | | | | |
|6 |1 |Topic assessment. |
| |2 |CARBON AND SOME OF ITS COMPOUNDS. |Define allotropes and allotropy. |Teacher exposes new terms. | |PP. 131-133 | |
| | | |Identify allotropes of carbon. |Review covalent bond. | | | |
| | |Allotropy. |Represent diamond and graphite |Discuss boding in diamond and graphite. | | | |
| | | |diagrammatically. | | | | |
| |3,4 |Physical and chemical properties of |Describe physical and chemical properties |Discuss physical and chemical properties of |Charcoal, graphite. | | |
| | |diamond, graphite and amorphous |of diamond, graphite and amorphous carbon.|diamond, graphite and amorphous carbon. | | | |
| | |carbon |State uses of carbon allotropes. |Explain the Physical and chemical properties of| | | |
| | | | |diamond, graphite and amorphous carbon. | | | |
| | | | |Discuss uses of carbon allotropes. | | | |
|7 |1 |Burning carbon and oxygen. |Describe reaction of carbon with oxygen. |Teacher demonstration- Prepare oxygen and pass |Carbon, limewater, tube, |PP. 134-135 | |
| | | | |dry oxygen into a tube containing carbon. Heat |limewater stand& Bunsen | | |
| | | | |the carbon. Observe effects on limewater. |burner. | | |
| |2 |Reduction properties of carbon. |Describe reduction properties of carbon. |Teacher demonstration – Burn strongly a mixture|CuO, pounded charcoal, Bunsen|P.126 | |
| | | |Show reduction properties of carbon. |of carbon and CuO on a bottle top. |burner& bottle top | | |
| | | | |Observe colour changes and give underlying | | | |
| | | | |explanation | | | |
| |3&4 |Reaction of carbon with acids. |Describe reaction of carbon with acids. |Teacher demonstration- reaction of carbon with |Conc. HNO3, limewater. |P.126 | |
| | | | |hot conc HNO3. | | | |
| | | | |Write balanced equations for the reaction. | | | |
| | | | | | | | |
| | | | |Review effects of heat on carbonates. | | | |
| | |Preparation of CO2. |Prepare CO2 in the lab. |Group experiments/teacher demonstration- | | | |
| | | | |preparation of CO2. | | | |
|8 |1,2 |Properties of CO2. |Describe properties of CO2 |Simple experiments to determine properties of |Lime water, |PP.138-139 | |
| | | | |CO2. |Magnesium ribbon, | | |
| | | | | |Universal indicator, | | |
| | | | |Discuss the observations. |lit candle. | | |
| |3,4 |Chemical equations for reactions |Write balanced CO2. |Give examples of reactions. Write corresponding| |PP.139-140 | |
| | |involving CO2. | |balanced chemical equations. | | | |
|9 |1 |Uses of CO2. |State uses of CO2 |Discuss briefly the uses of CO2. | |PP.140-1 | |
| |2 |Carbon monoxide lab preparation. |To describe preparation of carbon monoxide|Teacher demonstration: preparation of carbon | |PP. 142-143 | |
| | | |in the lab |monoxide in the lab. | | | |
| | | | |Make observations. | | | |
| |3 |Chemical properties of carbon |To describe chemical properties of carbon |Description of properties of carbon monoxide. | |PP. 44-145 | |
| | |monoxide. |monoxide. |Discussion and writing of chemical equations. | | | |
| |4 |Carbonates and hydrogen carbonates. |To state the difference between carbonates|Observe reactions of carbonates of Ca, Cu, Zn, |Carbonates of Ca, Cu, Zn, |PP.148-149 | |
| | | |and hydrogen carbonates. |NaHCO3 with HCl, HNO3, and H2SO4. |NaHCO3 with HCl, HNO3, and | | |
| | | |To describe chemical reactions of | |H2SO4. | | |
| | | |carbonates and hydrogen carbonates with |Record observations in a table. | | | |
| | | |acids. | | | | |
|10 |1 |Carbonates and hydrogen carbonates. |To write chemical equations for reactions |Discuss the observations above. | | | |
| | | |of carbonates and hydrogen carbonates with|Write chemical equations for the reactions. | | | |
| | | |acids. | | | | |
| |2 |Heating carbonates and hydrogen |To investigate reactions of carbonates and|Heat the above carbonates and record |Various carbonates and | | |
| | |carbonates. |hydrogen carbonates on heating. |observations in a table. |hydrogen carbonates. | | |
| |3,4 |Heating carbonates and hydrogen |To write equations for reaction of |Discuss the above observations. | |PP.150-151 | |
| | |carbonates. |carbonates and hydrogen carbonates on |Write corresponding balanced equations. | | | |
| | | |heating. | | | | |
|11 |1 |Extraction of sodium carbonate from |To draw schematic diagram for extraction |Discuss each step of the process. | |PP. 153-157 | |
| | |trona. |of sodium carbonates. |Write relevant equations. | | | |
| |2 |Solvay process of preparing sodium |To draw schematic diagram for extraction |Discuss each step of the process. | | | |
| | |carbonate. |of sodium carbonates. | | | | |
| | | | |Write relevant equations. | | | |
| |3,4 |Importance of carbon in nature. |To discuss: - Importance of carbon in |Discuss the carbon cycle and processes that | |PP.157-158 | |
| | |& its |nature. |increase/ reduce amount of CO2 in the air. | | | |
| | |effects on the environment. |& |Uses of CO2 in soft drinks and fire | | | |
| | | |Effects of carbon on the environment. |extinguishers. | | | |
|12 | |END OF YEAR EXAMS |
|13 | | |
................
................
In order to avoid copyright disputes, this page is only a partial summary.
To fulfill the demand for quickly locating and searching documents.
It is intelligent file search solution for home and business.