In SS2, students explore chemistry in greater depth. This study year builds upon fundamental knowledge acquired previously, aiming to broaden understanding and practical application.
In the Lagos state unified scheme of work for chemistry in SS2, topics typically cover areas such as chemical bonding, basic organic chemistry, and stoichiometry, as well as more advanced concepts like equilibrium and reaction kinetics. Practical sessions often involve experiments to reinforce theoretical learning, encouraging a hands-on approach to comprehending chemical principles.
SS2 chemistry is a foundational stepping stone for future studies and careers in fields such as medicine, engineering, and environmental science, emphasizing the development of critical thinking and problem-solving skills crucial for scientific exploration. By the end of SS2, students will have a strong foundation in Chemistry, preparing them for more advanced topics in the future.
SSS2 First Term
At the end of SSS2 first term, students can;
SSS2 Second Term
At the end of SSS2 second term, students can;
SSS2 Third Term
At the end of SSS2 third term, students can;
In SS2 chemistry, assessment methods include written exams testing theoretical knowledge, practical experiments with lab reports assessing practical skills, assignments evaluating the application of concepts, classroom participation gauging communication, quizzes for specific topics, and midterm/end-of-term assessments for overall progress.
Grading follows a scale from A to F, with A representing excellent performance, typically scoring around 70% or 80%, and F indicating failure, usually below 50% or 45%.
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| CLASS | SS2 | |
| SUBJECT | CHEMISTRY | |
| TERM | SECOND TERM | |
| WEEKS | TOPICS | LEARNING OBJECTIVES |
| 1 | CHEMICAL REACTIONS – Basic concepts of reactants and products – Rate of reaction – Collision theory – Activation energy | At the end of the lesson, students should be able to: i. write balanced equations of reactions ii. indicate reactants and products in chemical equation iii. express/explain the meaning of chemical equations iv. define chemical equations v. explain collision theory vi. explain activation energy |
| 2 | CHEMICAL REACTIONS II – Types of chemical reactions – Factors affecting the rate of chemical reactions – Calculation of rates of chemical reactions | At the end of the lesson, students should be able to: i. enumerate 5 examples of chemical reactions ii. list and explain at least 5 factors affecting the rate of chemical reactions iii. calculate rates of chemical reactions |
| 3 | ENERGY, ENERGY CHANGES, BIOTECHNOLOGY A. RENEWABLE, NON-RENEWABLE ENERGY/BIOTECHNOLOGY – Definition and forms of energy – Forms and types of energy resources (renewable and non-renewable) – Sources of renewable and non-renewable energy – Advantages and disadvantages of renewable and non-renewable energy B. BIOTECHNOLOGY – Projects on renewable and non-renewable energy C. EXOTHERMIC AND ENDOTHERMIC REACTIONS – Exothermic and endothermic reactions with examples – Enthalpy and enthalpy changes – Laws of thermodynamics – Heat of reactions | At the end of the lesson, students should be able to: i. identify keywords in the topics and sub topics of the lesson eg renewable, non-renewable, etc ii. explain the meaning of the keywords and relate such to the lesson iii. list forms of energy iv. mention types and forms of energy resources v. differentiate between renewable and non-renewable energy vi. list 5 sources each of renewable and non-renewable energy vii. list 5 advantages each of renewable and non-renewable energy viii. participate in projects on Biotechnology using either renewable or non-renewable energy ix. differentiate between exothermic and endothermic reactions x. draw energy profiles for exothermic and endothermic reactions (catalyzed and un-catalyzed) xi. explain the concept of thermodynamics xii. state the 1st and 2nd laws of thermodynamics xiv. explain enthalpy xv. define various heat of reactions |
| 4 | ENERGY, ENERGY CHANGES AND BIOTECHNOLOGY II A. ENTROPY, GIBBS FREE ENERGY – Definition of Entropy, Gibbs free energy – ∆G, ∆S, ∆H – Relationship between ∆G, ∆S, ∆H – Conditions for spontaneity in chemical reactions – Calculation of ∆G, ∆S, ∆H | At the end of the lesson, students should be able to: i. write out key words in the topics and sub-topics of the lesson ii. explain ∆G, ∆S, ∆H and the connection between them iii. list the conditions for spontaneity in chemical reactions iv. calculate ∆G, ∆S, ∆H |
| 5 | CHEMICAL EQUILIBRIUM – Reversible and irreversible reactions – Equlibrium in reversible reactions – Equilibrium in nature – Le Chatelier’s principles – Factors affecting equilibrium position in a chemical reaction – Expression and calculation of equilibrium constant k | At the end of the lesson, students should be able to: i. identify keywords in the topic and sub-topic of the lesson ii. express the meaning of the keywords and relate such to the lesson iii. differentiate reversible and irreversible reactions iv. explain the concept of equilibrium in a reversible reaction v. give 5 examples of equilibrium in nature vi. state Le Chatelier’s principles and laws of mass action vii. list 3 factors affecting equlibrium position in a chemical reaction viii. write expressions for equilibrium constant K ix. calculate equilibrium constant |
| 6 | NON METALS- HYDROGEN – Unique position of Hydrogen in the periodic table – Electronic configuration of hydrogen – Isotopes of Hydrogen – Hydrogen molecule – Properties and uses – Test for Hydrogen | At the end of the lesson, students should be able to: i. explain the unique position of Hydrogen on the periodic table ii. list the 3 isotopes of hydrogen iii. write the electronic configuration of hydrogen and it’s 3 isotopes iv. show the formation of hydrogen molecule from its electronic structure v. demonstrate the laboratory preparation of hydrogen vi. describe the industrial preparation of hydrogen vii. outline 3 physical and chemical properties of hydrogen viii. list 6 uses of hydrogen ix. test for hydrogen in the laboratory |
| 7 | MID-TERM BREAK | |
| 8 | NON METALS – OXYGEN A. OXYGEN IN NATURE – Position of Oxygen on the periodic table – Electronic configuration – The Oxygen molecule – Allotrope of Oxygen – Properties and laboratory preparation of Oxygen B. OXIDES – Definition of oxides – Types of oxides (acidic, basic, neutral, amphoteric, higher) C. AIR – Constituents and it’s composition – Properties – Air pollution and pollutants – Effects and control of air pollution – Global warming (ozone layer and greenhouse effect) D. FLAME – Types of flame – Zones in flame | At the end of the lesson, students should be able to: i. discuss oxygen as a component of many natural and chemical substances ii. indicate the position of oxygen on the periodic table iii. write the electronic configuration of oxygen iv. explain the formation of oxygen molecules from it’s atomic structure v. mention the only allotrope of oxygen vi. prepare oxygen in the lab vii. describe industrial preparation of oxygen viii. write 4 physical and chemical properties of oxygen ix. outline 5 uses of oxygen x. define oxides xi. list and define at least 4 types of oxides with 1 example each xii. explain why air is a mixture xiii. draw a schematic diagram to show the constituents of air and % composition xiv. enumerate 4 properties of air xv. define air pollution xvi. outline 5 air pollutants xvii. state 5 effects of air pollution xviii. explain 5 methods to combat air pollution xix. discuss global warming in relation to ozone layer and greenhouse effect xx. list 3 types of flames xxi. draw and label a candle + bunsen burner |
| 9 | HALOGENS – Meaning, occurrence of halogens in nature and daily life – Position of halogens in the periodic table – Electronic configuration of halogens – Gradations of general properties of halogens (Physical and chemical) down the group – Examples of halogen compounds – General uses of halogens and their compounds – Laboratory preparation of Chlorine – Test for halides- Cl, Br, etc – Bleaching action of Chlorine | At the end of the lesson, students should be able to: i. identify key words in the topic and sub-topic of the lesson ii. express the meaning of the keywords and relate such to the lesson iii. briefly discuss occurrence of halogens in nature eg sea water iv. mention 5 substances used in daily life that contains specific halogens eg toothpaste, bleach, etc v. indicate the position of halogens on the periodic table vi. write the electronic configuration of the first four halogens (F, Cl, Br, I) vii. explain the gradation of the physical and chemical properties down the group viii. write and name 5 halogen compounds ix. enumerate 5 general uses of halogens and their compounds x. perform experiment on laboratory preparation of Chlorine gas (if a fume cupboard is available) xi. perform experiments to test for halides in the laboratory xii. demonstrate the bleaching action of Chlorine |
| 10 | NITROGEN AND IT’S COMPOUNDS A. NITROGEN – Nitrogen in nature and position in the periodic table – Electronic configuration of Nitrogen – General properties of VA – Laboratory preparation of Nitrogen – Industrial preparation of Nitrogen from liquid air – Properties of Nitrogen (Physical and chemical) – Uses of Nitrogen – The Nitrogen cycle B. OXIDES OF NITROGEN – List the oxides of nitrogen (names and formulas) and state their characteristics – Explain experiments to distinguish between the oxides C. HYDRIDE OF NITROGEN – AMMONIA GAS – Chemical formula, physical and chemical properties – Uses of ammonia – Laboratory preparation of ammonia gas – Industrial preparation of ammonia gas (Haber process) D. OTHER COMPOUNDS OF NITROGEN – Trioxonitrate (v) – Ammonium salts, examples and uses* – Test for NO3 – Test for NH4 | At the end of the lesson, students should be able to: i. discuss the occurrence of nitrogen in air, nature and food substances ii. indicate the position of nitrogen on the periodic table iii. write the electronic configuration of nitrogen iv. state 3 general properties of VA elements v. explain the laboratory preparation of Nitrogen vi. explain the industrial preparation of Nitrogen vii. list 3 physical and 2 chemical properties of nitrogen viii. list 3 uses of nitrogen ix. draw and explain the nitrogen cycle x. list the 3 main oxides of nitrogen xi. compare the properties of the oxides of nitrogen using a T-Chart xii. explain experiments to distinguish between the 3 oxides of nitrogen xiii. mention ammonia gas as the only hydride of nitrogen and write it’s chemical formula xiv. outline 3 properties (physical and chemical) of ammonia xv. explain/demonstrate the laboratory preparation of ammonia gas xvi. explain the industrial preparation of ammonia gas (Haber process) xvii. list 4 uses of ammonia gas xviii. list (names and formulas) of 5 other compounds of nitrogen in the laboratory eg Trioxonitrate (v), ammonium salts, etc xix. list 3 uses of Trioxonitrate (v) and ammonium salts xx. perform experiments to test for Trioxonitrate (v) ion xxi. perform experiments to test for NH4 |
| 11 | A. SULPHUR – Sulphur in nature and position on the periodic table – Electronic configuration of Sulphur – General properties of VA – Explain the concept of allotropy – List the allotropes of sulphur – Explain the extraction of sulphur (French process) – State the uses of sulphur – Oxidation number of Sulphur in it’s major compound B. COMPOUNDS OF SULPHUR – H2S – H2SO3 – H2SO4 – Oxides of sulphur – Industrial preparation of H2SO4 – Uses of H2SO4 | At the end of the lesson, students should be able to: i. mention the local name of sulphur in their language ii. write 5 substances used in daily life and nature that contain sulphur eg antiseptic soap iii. indicate the position of sulphur on the periodic table iv. write the electronic configuration of sulphur v. enumerate 3 general properties of sulphur vi. recall the concept of allotropy treated under carbon vii. explain the concept of allotropy viii. describe at least 3 isotopes of sulphur ix. explain the extraction of sulphur x. enumerate 5 uses of sulphur xi. calculate the oxidation scores of sulphur in its main compounds using rules taught under oxidation and reduction xii. list a few major compounds of sulphur xiii. list their characteristic properties xiv. explain the industrial preparation of H2SO4 xv. perform experiment test |
| 12 | REVISION/EXAMINATIONS | |
| CLASS | SS2 | |
| SUBJECT | CHEMISTRY | |
| TERM | THIRD TERM | |
| WEEKS | TOPICS | LEARNING OBJECTIVES |
| 1 | WATER – Structure of water – Laboratory preparation of water – Properties of water (Physical and chemical) – Types of water (Soft and hard) – Types of hardness (Temporary and Permanent) – Causes of hardness – Advantages and disadvantages of hard water – Methods of removal of hardness/ softening water – Purification of water from town (municipal) supply | At the end of the lesson, students should be able to: i. discuss water as an essential substance for life and major components of living tissue ii. mention elemental component of water iii. draw the structure of water iv. explain the laboratory preparation of water v. list 5 physical properties of water and explain the unusual high boiling of water vi. outline at least 3 chemical properties of water viii. mention the types and causes of hardness in water ix. discuss at least 3 advantages and disadvantages of soft and hard water x. outline and describe at least 4 methods of softening water/removal of hardness xi. outline and explain 5 processes involved in the treatment of water for town/municipal supply |
| 2 | WATER – Structure of water – Laboratory preparation of water – Properties of water (Physical and chemical) – Types of water (Soft and hard) – Types of hardness (Temporary and Permanent) – Causes of hardness – Advantages and disadvantages of hard water – Methods of removal of hardness/ softening water – Purification of water from town (municipal) supply | At the end of the lesson, students should be able to: i. discuss water as an essential substance for life and major components of living tissue ii. mention elemental component of water iii. draw the structure of water iv. explain the laboratory preparation of water v. list 5 physical properties of water and explain the unusual high boiling of water vi. outline at least 3 chemical properties of water viii. mention the types and causes of hardness in water ix. discuss at least 3 advantages and disadvantages of soft and hard water x. outline and describe at least 4 methods of softening water/removal of hardness xi. outline and explain 5 processes involved in the treatment of water for town/municipal supply |
| 3 | SOLUBILITY – Definition of terms: solute, solvent, solution, saturated, un-saturated and super saturated solution, solubility) – Factors affecting solubility – Solubility curve – Calculations on solubility – Applications of solubility and solubility curve | At the end of the lesson, students should be able to: i. identify keywords in the topic and sub-topic of the lesson ii. explain the meaning of the keywords and relate such to the lesson iii. give 5 examples each of solute, solvent and solution iv. prepare solution = solute + solvent v. prepare saturated, un-saturated, super saturated solution vi. differentiate between saturated, un-saturated and super saturated solutions vii. define solubility viii. list 3 factors affecting solubility ix. calculate the solubility of solvents and solutes x. plot solubility curves xi. list and discuss at least 3 applications of solubility and solubility curve in daily life and nature |
| 4 | MASS-VOLUME RELATIONSHIP – Mole concept, molar quantities – Relative densities, relative molar mass, molar volume, S.T.P, S.V.P – Molar concentration and mass concentration – Chemical equations – Calculations involving mass and volume | At the end of the lesson, students should be able to: i. identify keywords in the topic and sub-topic of the lesson ii. express the meaning of the keywords and relate such to the lesson iii. explain concept of mole, molar volume, molar mass, molar concentration, etc iv. calculate the mass/volume of reactants and products, number of moles of reacting substances and products, relative densities v. derive S.I units of calculative quantities |
| 5 | VOLUMETRIC/QUANTITATIVE ANALYSIS – Definition of terms: titration, trimetry, molar solution, standard solution, indicator, etc – Apparatus required for volumetric analysis – Precautions in titration – Steps in titration – Recording acceptable titre value – Acid-base and redox titrations – Determination of: a) concentration in g/dm and mol/dm b) % purity and impurity c) water of crystallization – Heat of neutralization | At the end of the lesson, students should be able to: i. identify topics and sub-topics of the lesson ii. express the meaning of the keywords and relate such to the lesson iii. explain the concept of volumetric/quantitative analysis iv. define terms in volumetric analysis v. list the apparatus required for volumetric analysis vi. state and explain the necessary precaution during titration vii. outline steps in titration viii. perform acid/base and redox reactions ix. create acceptable table of titre values x. calculate unknown quantities in xi. define heat neutralization |
| 6 | VOLUMETRIC/QUANTITATIVE ANALYSIS – Definition of terms: titration, trimetry, molar solution, standard solution, indicator, etc – Apparatus required for volumetric analysis – Precautions in titration – Steps in titration – Recording acceptable titre value – Acid-base and redox titrations – Determination of: a) concentration in g/dm and mol/dm b) % purity and impurity c) water of crystallization – Heat of neutralization | At the end of the lesson, students should be able to: i. identify topics and sub-topics of the lesson ii. express the meaning of the keywords and relate such to the lesson iii. explain the concept of volumetric/quantitative analysis iv. define terms in volumetric analysis v. list the apparatus required for volumetric analysis vi. state and explain the necessary precaution during titration vii. outline steps in titration viii. perform acid/base and redox reactions ix. create acceptable table of titre values x. calculate unknown quantities in xi. define heat neutralization |
| 7 | MID-TERM BREAK | |
| 8 | HYDROCARBONS – Definition of hydrocarbons – Structure and valency of carbons – Classification of hydrocarbons: Aliphatic or Aromatic – Classification of aliphatic and aromatic hydrocarbons – Definition of terms: homologous series, functional groups, isomerism | At the end of the lesson, students should be able to: i. highlight keywords from the topics and sub-topics of the lesson ii. explain the meaning of the keywords and relate such to the lesson iii. discuss the occurrence of hydrocarbons iv. explain the tetravalent nature of carbon v. define and classify hydrocarbons vi. explain and define terms vii. explain 5 characteristics of a typical homologous series |
| 9 | SATURATED HYDROCARBONS- ALKANES – General formula of alkanes – IUPAC nomenclature of alkanes – Laboratory preparation of alkanes (methane) – Properties and uses of alkanes (methane) | At the end of the lesson, students should be able to: i. write the general formula, IUPAC name and structural formula for the first 10 alkanes ii. draw and name isomers of alkanes from a given formula iii. describe the laboratory preparation of methane iv. explain at least two chemical properties of alkanes v. list 3 uses of alkanes and methane |
| 10 | UN-SATURATED HYDROCARBONS A. ALKENES – General formula and functional groups of alkenes – IUPAC nomenclature of alkenes – Laboratory preparation of ethene – Properties and uses of alkenes (ethene) B. ALKYNES -General formula of alkenes – Functional groups of alkenes – IUPAC nomenclature of alkenes – Laboratory preparation of ethyne – Properties and uses of alkenes(ethyne) – Test for unsaturation | At the end of the lesson, students should be able to: i. write the general formula for alkenes and alkynes ii. specify the functional groups in alkene and alkynes iii. write the IUPAC name and structure for the first 10 alkenes and alkynes iv. describe the laboratory preparation of ethene and ethyne v. list 3 physical properties of ethene and ethyne vi. explain at least 3 chemical reactions of ethene and ethyne viii. enumerate at least 4 uses of alkenes and alkynes ix. perform experiments to test for alkenes and alkynes x. perform experiments to distinguish alkenes from alkynes |
| 11 | ALKANOLS – Natural sources of alkanols – Classification based on: a) number of hydroxyl group b) akyl group – Physical and chemical properties of alkanol – Polarity of alkanols and solubility of substances – Laboratory preparation of Ethanol – Local and industrial preparation of ethanol by fermentation – Uses of alkanols – Test for alkanols | At the end of the lesson, students should be able to: i. discuss natural sources of alkanols ii. list 5 substances in daily life that contain alkanols iii. write the general formula for alkanols iv. classify alkanols v. describe the laboratory and industrial preparation of alkanols vi. list and explain 5 uses of alkanols vii. prepare ethanol from starchy foods viii. explain hydrogen bonding in alkanols ix. explain and rest for different classes of alkanols |
| 12 | REVISION/ EXAMINATION | |
The recommended Chemistry textbooks for SSS2 include but are not limited to the following:
