This is to notify our reader that The ss2 chemistry scheme of work (senior secondary school two) for this session is now available on our website for free especially for chemistry teachers and students in senior secondary in Nigeria. As we all know that chemistry is a one of the pure science subject offered in only secondary throughout Nigeria. Therefore this post imply chemistry teachers about the government approved chemistry scheme of work for ss2 which include first term, second term and third term.
Learning should be from known to unknown, easier to complex, the riders therefore this chemistry scheme of work for SS 2 first term, is the continuation of the third term chemistry scheme of work for ss1. As part of our practice the scheme of work provided here is arranged systematically for better understand for both ss2 teacher and student.
With the mandate from the ministry of education, it is willful that all private and public senior secondary schools in Nigeria should use the same scheme of work. In order to be in line with the desires of all external exam bodies such as WAEC and NECO, the ministry of education compulsory it that schools should should submit government approved scheme of work for all subject offered as one of the prerequisite requirements for approving the operation or license to run a secondary school in Nigeria.
The principals and teachers in secondary schools in Nigeria are to embrace to the appropriate approved scheme of work as ordered by the ministry of education because the approved scheme of work for Chemistry (Senior secondary school two) is the same for both private and public
From our observations the approved scheme of work for Chemistry in Senior secondary school two (SS 2) from first term to third term is the same irrespective of whether the school is a public or private, so for this reason the search for the government approved scheme of work for Chemistry in senior secondary school level has been on higher demand by chemistry teacher throughout the federation, the reason is that chemistry is a compulsory science subject offered for all student in science department as it is important requirements for admission and for candidates who wants to study Chemistry, health science, engineering, science and any science related course in higher institutions.
This post is mostly important for ss2 science students because the provided scheme here detailed the current Chemistry scheme of work it vividly analysis and emphasize on 1st term, 2nd term and 3rd term), which also comprises of the government approved scheme of work for all topics and sub-topics, teacher and students activities and behavioural objective.
First Term SS2 Chemistry Scheme Of Work
|1||Mass volume Relationship|
Mole ratio and mass relationship
Calculation of concentration, molar mass, moles, volume e.t.c
Stoichiometry of reactions
|Teachers guide the students to calculate: The masses of reactions and products and several moles of reacting substances and products.|
The learners calculate the masses, moles, and volumes in chemical reactions, participates in class review exercises. Compute or write the number of moles and molar mass of reactants and products from chemical equations of a chemical reactions
|2||Types of Reaction|
Decomposition, displacement, catalytic reaction, double-decomposition, thermal-dissociation, Reversible reaction
|The instructor guides the Students to identify reactants and products of any reaction.|
The learners ask questions and watch the teacher’s demonstration in the class.
Oxidation and reduction
Oxidizing and Reducing agents
Balancing of Redox Equation
|The teacher guides Students to define Oxidation and Reduction, Calculate Oxidation numbers of the central atom in H2SO4, HNO3e.t.c.|
It guides the students in distinguishing oxidizing agents from reducing agents.
Guides the students to write a balanced Redox reaction or equation
The Students note the various definitions of oxidation and reduction reaction.
Ask questions and calculate the oxidation of an atom in a compound
Differentiate between oxidizing agents and reducing agents.
Learn how to balance the Redox equation.
Definition of Electrolysis, Ionic Theory, Electrolyte and non-electrolyte
Preferential discharge of ions
Electrolysis of common electrolytes, e.g. acidified water, copper (II) sulfates, and brines.
|The teacher define Electrolysis to the Students. Draw electrolytic and electrochemical cells.|
The teacher guides the students to know the differences between Strong and weak electrolytes and no-electrolyte.
Guides Students to calculate the number of substances liberated or deposited at electrodes during electrolysis.
Demonstrate the uses of electrolysis.
Draw the electrolysis of some common electrolytes in the form of a chart to show to the Students
The learner ask questions in the class on the topic discussed.
Ask questions about the discussions in the class
Differentiate between the electrolyte and non-electrolyte
Calculate the amounts of substances discharged during electrolysis
State the uses of electrolysis and its applications.
|5||Laws of Electrolysis|
Faraday’s laws of electrolysis
Calculations and Uses of Electrolysis
|The instructor explain Faraday’s first and second laws of electrolysis.|
Guides students to calculate the amount of substance librated or deposited at an electrode during electrolysis
State the uses and application of electrolysis
The learners State Solve some problems involving faraday’s law of electrolysis and uses of electrolysis
|6||Electrode Potential (Electrochemical cells)|
Electrochemical cell and electromotive force (E.M.F.) of cells.
|The teacher draw and write cell diagrams.|
Guides the students to draw and write cell diagram
The students explain electrode potential and draw the cell diagram and able questions
|7||Energy and chemical reactions|
Rate of Reactions
Collision theory and Factors affecting the rate of reaction
|The teacher guides the students to know the meaning of the rate of reaction|
Guides the students when showing the chart to them.
Explain each factor properly to the Students
Te Students define and demonstrate the experimente the rate of reaction.
Explain the Collision theory through the charts and list factors affecting the rate of reaction
Qualitative comparisons of conductance of molar solution of story-weak acid and base
|The teacher guides Students to Prepare standard solutions, and identify appropriate indicators for acid-base titration. Displays and explain the apparatus necessary for carrying out simple titrations|
The students prepare standard solutions, carry out acid and base titrations using given indicators
Record correct by titer values to two decimal places.
|9||Simple Acid-Base Titration|
Preparation of standard solution for titration (Practical)
|Teacher should demonstrate the process of acid-base titration|
Guides students to carry out the acid-base titration according to the instructions
Teachers should ensure that students record properly and perform relevant calculations
The learners carry out relevant calculations from the values.
Construct a wooden retort stand and ask questions during the practical class.
|10||Determination of Percentage Purity|
Water of crystallization
|The instructor should carry out titrations to determine the percentage of purity|
Explain to students how to calculate the molar mass of substances
Explain to students how to calculate the molar mass of substances.
Carry out a titration to determine water of crystallization
Students determine the purity of the substance
Calculate the molar mass of a substance in a given solution.
Determine the water of crystallization in a titration reaction.
Summary Of First Term SS2 Chemistry Scheme Of Work
Please teacher should make sure that they cover and explain the concepts of the mole, molar, S.T.P; relative molar mass, and relative densities, solve problems involving reacting masses and volumes in chemical reactions, state the SI units of various fundamental quantities
Define the various types of reactions: such as catalytic reaction, decomposition, displacement reaction, e.t.c.
Define oxidation and reduction: as the addition of oxygen and removal of hydrogen, calculate the oxidation number of elements using a set of arbitrary rules like (a)Oxidation number of free elements=0, (b) Oxygen in any compound=-2 except in hydrogen peroxides=-1, define oxidizing and reducing agents in terms of the addition and removal of oxygen and hydrogen respectively, balance the Redox reactions effectively through the steps.
Define electrolysis, electrolytes (Strong, Weak, non-electrolytes), explain Ionic theory: discharge of ions in the solution, define electrolyte and non-electrolyte, differentiate between electrolyte and non-electrolyte, strong and weak electrolytes, identify the factors affecting the discharge of ions during electrolysis and llustrates the electrolysis of brines, and acidified water.
Calculate the amount of substance librated or deposited at the electrode during electrolysis
Explain electrode potential and the standard hydrogen electrode draw and write cell diagrams, define the electromotive force of cells.
Define rate of reaction, explain Collision theory and list the factors affecting the rate of reactions
Define concentration in mold-3 of solutions, define Standard solutions, explain the relationship between concentrations and volumes of reacting substances.
Prepare standard solution, define neutralization process, define indicators and list different types of indicators used for the titration.
Explain percentage purity, calculate the molar mass of the substances given and analyze different salts for anions and cations
Second Term SS2 Chemistry Scheme Of Work
|1||Determination of solubility|
number of molecules
and ions, molar volume
|Teacher prepares standard acid and base solution, extracts indicators to be used from flower, demonstrates acid-base titration for the students, guides the students to solve the simple question|
Learners Assists teacher in preparing standard acid and base solution, Carries out titration with a given acid-base solution
calculates solubility, volume of carbon (iv) oxide liberated, number of molecules, and ions from a simple question
|2||Energy and chemical reactions|
Heat content and heat of reaction
endothermic and exothermic
|The teacher guides the student to define the heat of the reaction, assists students in enthalpy change for an endothermic and exothermic reaction and explains the energy profile for an endothermic and exothermic reaction|
The learners dissolves ammonium salt and sodium hydroxide pellet in water to identify exothermic and endothermic reaction, solves simple questions on energy profiles for exothermic and endothermic reactions and takes down short notes and asks questions
|3||Heat Change of Formation, Combustion, Neutralization and Dissolution||The instructor leads the students to differentiate between Standard heat change and Heat change of reaction, States various Standard heat changes of reaction and Assists the students to differentiate between heat change of neutralization and heat change of combustion.|
The learner Watch the teacher during his explanation, differentiate between Standard heat change and ordinary heat change of reaction and takes short notes and asks questions.
Enthalpy and Entropy Change, Free energy. The first and second law of thermodynamics. The spontaneity of a chemical reaction
|The instructor guides the students to the effects of free energy change being: (i) negative (ii) positive, leads the students to show the relationships among Free energy change, Enthalpy change, Entropy change, and Absolute temperature and also guides the students to show how Entropy change affects the spontaneity of chemical reactions.|
The students Define the following: Enthalpy, Entropy, Free energy Write the relationships among Free energy change, Enthalpy change, and Entropy change. Use the equation G=H-TS to solve simple questions. State the implication of G=0, G=+ve, and G=-ve.
Equilibrium and reversible reaction
Le – Chatelier’s principle
Factors affecting equilibrium
|Teachers assist the students to define the equilibrium state of reaction, guides the students to write the equilibrium constant for a particular reversible reaction, leads the students to identify reversible reaction and guides the students to highlight how catalyst influences the equilibrium of a reaction.|
The students define reversible and equilibrium of a reaction. State the importance of equilibrium constant
State factors that affect the equilibrium position and highlight how catalysts influence equilibrium reaction
Meaning of Equilibrium constant, free energy, and electrode potential
Industrial Applications of chemical equilibrium. Acid-base equilibrium
|The teacher leads the student to write the relationship between equilibrium constant, electrode potential, and free energy, state the industrial application of equilibrium constant to chemical industries.|
Show the acid-base equilibrium equation and define PH and buffer solution and state the application’s buffer solution.
Students write the relationship among equilibrium constants, free energy change, and standard electrode potential, listen to the teacher during the discussion, Take down notes and ask questions and attend the classroom work.
|7||Non-metals and their compounds hydrogen|
Position in the periodic table, Properties and reactions, Laboratory preparation and industrial preparations, Uses and Laboratory identification of non metal and their compound
|The teacher guides the students to write the electronic configuration of hydrogen,name isotopes of hydrogen., discuss the unique position of hydrogen on the periodic table and sets up apparatus for the laboratory preparation of hydrogen using the action of dilute acid (HCl(Aq) ) on active metals (e.g Zinc )|
The learners write and draw the electronic configuration of hydrogen, the structure of isotopes of hydrogen, draw the setup apparatus for laboratory preparation of hydrogen gas and carry out the test for hydrogen gas using a lighted splint.
Bonding capacity, Allotropes, Preparation, Properties and reactions of oxygen
Uses and Test for oxygen
|The instructor guides the students to write the electronic configuration of oxygen to show its bounding capacity. State the uses of oxygen. Set up the apparatus uses for laboratory preparation of oxygen. Demonstrate the test for oxygen using a glowing splint. Illustrates oxidation as the addition of oxygen.|
The learners write the electronic configuration of oxygen to establish its bounding capacity. List allotrope of oxygen. Draw a label diagram of the setup apparatus for making oxygen and test for oxygen using a glowing splint.
|9||Water and solution|
composition of water structure, source and purity, properties and the hardness of the water.
|The teacher demonstrates formation of hard water by dissolving calcium ions in water. Demonstrate removal of hardness in water by using washing soda, list various forms of water sources. Highlight various stages of water treatment for consumption and lead student on an excursion to waterworks|
The students prepare solutions for common substances, experiment to remove hardness by boiling and by adding washing soda, watch the teacher during a demonstration
|10||Solution and solubility|
Define solubility and various types of solution, Formula for finding solubility and its S I unit. Factors affecting solubility, Solubility curves and their applications. Various solvents and their uses. Water as the universal solvent
|The instructor performs an experiment to help students determine the solubility of a substance, demonstrate the application of solubility (removal of stains) and guides the students to draw a solubility curve.|
The learners watch the teacher during a demonstration
Summary Of Scond Term SS2 Chemistry Scheme Of Work
You are provided with the summary of what the students student should be taught at the end of the term. The teacher should list type of solutions, calculate solubility using the parameter given, determine the number of molecules, ions, and hydrogen using titrimetric analysis, explain how the volume of gas liberated when acids react with trioxo carbonate (iv)
Define heat content and heat of reaction, differentiate between exothermic and endothermic reactions, list examples of exothermic and endothermic reaction, draw an energy profile for an exothermic and endothermic reaction, define activation energy, state the effect of catalyst on activation energy, ssolve the simple questions on the energy profile
Differentiate between Heat change of reaction and Standard heat change of Reaction. State notation for heat change and standard heat change, list various heat changes of reaction, differentiate between standard heat change of neutralization and standard heat change of combustion and show their similarities.
Define Enthalpy and Entropy change, define Free energy, show the equations that connect them, state the first and second law of thermodynamics
Define the equilibrium state of a reaction and reversible reaction, write the equilibrium constant of a particular reversible reaction, state the significance of equilibrium constant, state the factors that affect the equilibrium position, highlight how catalyst affects equilibrium and state Le – Chatelier’s principle
Write an equation to relate equilibrium constant, free energy, and electrode potential together, highlight the industrial application of chemical equilibrium to chemical industries, define PH and shows the mathematical expression for PH, show the relationship among; PH, POH, and PKW, define buffer solution and state its applications.
Write and draw the electronic configuration, identify the isotopes of hydrogen, highlight steps involved in the laboratory and industrial method C of properties of hydrogen, list the physical and chemical properties of hydrogen and mention the uses of hydrogen.
State some physical properties of oxygen as a major component of air breathing-in, highlight the major points involved in the laboratory preparation of oxygen, draw the diagram of set up apparatus for laboratory preparation of oxygen, state the chemical reactions of oxygen, list the compounds of oxygen and state the effect of oxygen on a glowing splint.
Draw and explain the structure of water, define the following: solute, solvent, and solution, list various sources of water, state various properties of water and identify the abnormal behavior of water, highlight steps involved in water treatment for various uses, define hard water, and list various types and their cause, hghlight various methods for removing hard water.
Defines solubility and states its unit, name different types of solution, apply the solubility equation to solve simple questions, draw the solubility curve and state its applications, list various solvents and their uses
Third Term SS2 Chemistry Scheme Of Work
Electronic confirmation, physical and chemical properties, laboratory preparations of halogens
Reactions of chlorine
|The instructor leads the student to write and draw the electronic configuration of chlorine and others, Perform simple experiments to illustrate the properties of chlorine (bleaching), Set up and demonstrate the laboratory preparation of chlorine|
Lead class discussion on the uses of halogen
The learners observe the experiment on the laboratory preparation of chlorine and record their observation correctly. Draw the apparatus for laboratory preparation of chlorine and participate in class discussion
|2||Laboratory preparation of Hydrogen chloride gas, the reaction of hydrogen chloride gas|
Test for chloride gas and test of halogens compounds
|Teacher Set up and demonstrate the laboratory preparation of HCl(g), Perform simple experiments to illustrate the reaction e.g. reaction with the metal, reaction with ammonia|
The students draw the apparatus for the preparation of HCl(g)
Laboratory preparation, industrial preparation from liquid air and uses of Nitrogen
|The instructor set up and demonstrate the laboratory preparation of nitrogen, lead the class on the uses of nitrogen|
The learners observe the experiments and record them correctly.
|4||Compound of Nitrogen|
Laboratory and industrial preparation and uses of Ammonia
Oxides of nitrogen v
|The instructor prepare and demonstrate the laboratory preparation of Ammonia, guides the student to smell the odor of urine and the gas prepared, lead class discussion on the uses of Ammonia|
Perform a simple experiment to illustrate why N2o is called laughing gas
The students smell the odour of urine and Ammonia to know the similarities
|5||Preparation of Trioxonitrate v acids|
Reactions, uses and test for trioxonitrate v ions
|The teacher set up and demonstrate the laboratory preparation of Trioxonitrate( v) acids guides the student to identify the uses of nitrates and emonstrate the test for trioxonitrate v ions|
The learners record, observe and draw the laboratory apparatus for the preparation of trioxonitrate(v) acid, find out more uses of nitrate. From the internet and other sources
General properties of group VI A element
Electronic structure, Allotropes and uses of sulphur
|The instructor explain the general properties of the group VIA element, guide the students to write the electronic configuration of sulfur, leads the student to identify the uses of sulfur.|
The students prepare and write and draw the electron structure of sulphur
|7||Compound of sulphur|
Industrial preparation, reaction and uses of H2So4
Test for So32- and SO42-
|The teacher name the compound of sulphur and write it for the student to copy, explain the preparation and properties of H2S and S02 to the students. Perform the chemical test for the identification of S042- and S032- ions|
The learners draw and describe the contact process, smell the odour of rotten egg.
|8||Organic chemistry: Hydrocarbon|
Structure and Valency of Carbon
Hydrocarbon, Homologous Series, Saturated and unsaturated Hydrocarbon, Isomerism
|The teacher explain the tetravalent nature of carbon, define Homologous series and their characteristics. Write structures of Alkane.|
Preparation, Properties, Uses and Test for Alkene and Alkyne
|The teacher Set up and demonstrate laboratory preparation of Ethyne to the Student. Identify and write the structure of alkene and alkyne. Experiment to differentiate between Ethene and Ethyne. Lead student to state the uses of ethene|
The learners Participate in writing other members of homologous series, distinguish between Alkane, Alkene, and Alkyne
|10||Aromatic Hydrocarbon (Alkanol)|
Benzene Structure and properties.
Classification, types, industrial production, uses, preparation and properties of Alkanols.
|The instructor shows action of Sodium on Methanol. Show that ethanol is soluble in water. Prepare alcohol by fermentation.|
Summary Of Third Term SS2 Chemistry Scheme Of Work
At the end of the term, teacher should cover and write the electronic configuration of halogens, state the properties and list some compounds of halogens and describe the laboratory preparation of chlorine
Describe the laboratory preparation of HCl(gas), list some reactions of Hydrogen chloride gas, describe a test for chloride ion and list the uses of halogen compounds
Describe the laboratory preparation of nitrogen and Industrial preparation and list the uses of nitrogen
Describe the laboratory preparation of Ammonia, describe the preparation of ammonia by the Haber process, give the use of Ammonia, list oxide of nitrogen and draw Nitrogen cycle
Explain laboratory preparation of Trioxonitrate iv acid, list the properties of the acid, give the uses of the acid and describe a chemical test for trinitrate (v) ions.
Write and draw the electronic configuration of sulphur, explain the meaning of allotropes, list the allotropes of sulphur
Describe the industrial preparation of H2So4
Write the general formular of Alkene and Alkyne, describe the laboratory preparation, list the properties and uses of Alkene and Alkyne, describe a test to distinguish between Etheneand Ethyne.
Write the structure and properties of Benzene, relate the structure of alkane to Alkanol, classify Alkanol based on the number of OH groups present, list the properties of Alkanol, explain the industrial production of Alkanol (Fermentation) and list the uses of Alkanol.