2022/2023 Second Term Chemistry Scheme Of Work For SS2

Chemistry scheme of work
UNIFIED SCHEME OF WORK FOR CHEMISTRY
CLASS: SENIOR SECONDARY SCHOOL TWO
TERM: SECOND TERM SCHEME OF WORK  

WEEK ONE

Revision and cleaning of the compound

WEEK TWO

TOPIC

Titration

CONTENT

Determination of :

1) solubility

2) number of molecules

and ions

3) molar volume

BEHAVIOURAL OBJECTIVE

At the end of the lesson student should be able to:

1) list type of solutions

2) calculate solubility using the parameter given

3) determine the number of molecules, ions, and hydrogen using titrimetric analysis

4) volume of gas liberated when acids react with trioxo  carbonate (iv)

INSTRUCTIONAL MATERIALS

  1. Pipette, burette, weighing balance, funnel
  2. Retort stand
  3. Test tube indicators.

TEACHERS ACTIVITIES

1) Teacher prepares standard acid and base solution

2) extracts indicators to be used from flower

3) demonstrates acid-base titration for the students.

4) guides the students to solve the simple question

LEADER’S ACTIVITIES

1) Assists teacher in preparing standard acid and base solution

2) Carries out titration with a given acid-base solution

3) calculates;

i) solubility

ii)volume of carbon (iv) oxide liberated

iii) number of molecules, and ions from a simple question

WEEK THREE

TOPIC

Energy and chemical reactions

CONTENT

1 heat content and heat of reaction

2 endothermic and exothermic

3 Reaction profile

4  Activation energy.

BEHAVIOURAL OBJECTIVE

At the end of the lesson student should be able to:

1) define heat content and heat of reaction

2) differentiate between exothermic and endothermic reactions

3) list examples of exothermic

And endothermic reaction

4) draw an energy profile for an exothermic and endothermic reaction

5) define activation energy

6) state the effect of  catalyst on activation energy

7) solve the simple questions on the energy profile

INSTRUCTIONAL MATERIALS

1) conical flask

2) testy tube

3) water

4) sodium hydroxide pellet

5) ammonium chloride solid 6 charts showing energy profile diagram

TEACHERS ACTIVITIES

1) teacher guides the student to define the heat of the reaction

2) assists students in enthalpy change for an endothermic and exothermic reaction

3) explains the energy profile for an endothermic and exothermic reaction

LEADER’S ACTIVITIES

1) dissolves ammonium salt and sodium hydroxide  pellet in water to identify exothermic and endothermic reaction

2) solves simple questions on energy profiles for exothermic and endothermic reactions

3) takes down short notes and asks questions

WEEK FOUR

TOPIC

Types of Heat Change

CONTENT

  1. Heat Change of Formation
  2. Heat Change of Combustion
  3. Heat Change of Neutralization
  4. Heat Change of Dissolution

BEHAVIOURAL OBJECTIVE

At the end of the lesson student should be able to:

1) Differentiate between Heat change of reaction and Standard heat change of Reaction

2) State notation for heat change and standard heat change

3) List various heat changes of reaction

4) Differentiate between standard heat change of neutralization and standard heat change of combustion and show their similarities.

INSTRUCTIONAL MATERIALS

1) Test tube

2) Water

3) Sodium hydroxide pellet

4) Ammonium salt

5) Calorimeter

TEACHERS ACTIVITIES

1) Leads the students to differentiate between Standard heat change and Heat change of reaction

2) States various Standard heat changes of reaction

3) Assists the students to differentiate between heat change of neutralization and heat change of combustion.

LEADER’S ACTIVITIES

1) Watching the teacher during his explanation.

2) Differentiate between Standard heat change and ordinary heat change of reaction

3) Takes short notes and asks questions.

WEEK FIVE

TOPIC

Chemical Thermodynamics

CONTENT

  1. Enthalpy Change and Entropy Change
  2. Free energy
  3. The first law of thermodynamics
  4. The second law of thermodynamics
  5. The spontaneity of a chemical reaction

BEHAVIOURAL OBJECTIVE

At the end of the lesson student should be able to:

  1. Define Enthalpy change
  2. Define Entropy change
  3. Define Free energy
  4. Show the equations that connect them
  5. State first law of thermodynamics
  6. State second law of thermodynamics

INSTRUCTIONAL MATERIALS

Charts that show the relationships among Free energy change, Enthalpy change, and Entropy change.

TEACHERS ACTIVITIES

  1. Guides the students to the effects of free energy change being: (i) negative (ii) positive
  2. Leads the students to show the relationships among Free energy change, Enthalpy change, Entropy change, and Absolute temperature.
  3. Guides the students to show how Entropy change affects the spontaneity of chemical reactions.

LEADER’S ACTIVITIES

  1. Define the following: Enthalpy, Entropy, Free energy
  2. Write the relationships among Free energy change, Enthalpy change, and Entropy change.
  3. Use the equation G=H-TS to solve simple questions.
  4. State the implication of  G=0, G=+ve, and G=-ve.

WEEK SIX

TOPIC

Chemical equilibrium

CONTENT

  1. Equilibrium and reversible reaction
  2. Le – Chatelier’s principle
  3. Factors affecting equilibrium
  4. Equilibrium constant

BEHAVIOURAL OBJECTIVE

At the end of the lesson student should be able to:

  1. Define the equilibrium state of a reaction and reversible reaction.
  2. Write the equilibrium constant of a particular reversible reaction.
  3. State the significance of equilibrium constant
  4. State the factors that affect the equilibrium position
  5. Highlight how catalyst affects equilibrium.
  6. State Le – Chatelier’s principle

INSTRUCTIONAL MATERIALS

Lesson note, Chalkboard, and cardboard containing various reversible reactions

TEACHERS ACTIVITIES

  1. Teachers assist the students to define the equilibrium state of reaction
  2. Guides the students to write the equilibrium constant for a particular reversible reaction
  3. Leads the students to identify reversible reaction
  4. Guides the students to highlight how catalyst influences the equilibrium of a reaction.

LEADER’S ACTIVITIES

  1. students define: (i) Reversible reaction (ii) Equilibrium of a reaction
  2. State the importance of equilibrium constant
  3. State factors that affect the equilibrium position
  4. Highlight how catalysts influence equilibrium reaction

WEEK SEVEN

TOPIC

Chemical equilibrium

CONTENT

  1. Equilibrium constant, free energy, and electrode potential
  2. Industrial Applications of chemical equilibrium.
  3. Acid-base equilibrium

BEHAVIOURAL OBJECTIVE

At the end of the lesson student should be able to:

  1. Write an equation to relate equilibrium constant, free energy, and electrode potential together.
  2. Highlight the industrial application of chemical equilibrium to chemical industries.
  3. Define PH and shows the mathematical expression for PH.
  4. Show the relationship among; PH, POH, and PKW.
  5. Define buffer solution and state its applications.

INSTRUCTIONAL MATERIALS

Lesson note, Chalkboard, and cardboard containing various reversible reactions.

TEACHERS ACTIVITIES

The teacher leads the student.

  1. Write the relationship between equilibrium constant, electrode potential, and free energy.
  2. State the industrial application of equilibrium constant to chemical industries.
  3. Show the acid-base equilibrium equation
  4. Define PH and buffer solution and state the application’s buffer solution.

LEADER’S ACTIVITIES i. students write the relationship among equilibrium constants, free energy change, and standard electrode potential.

  1. listen to the teacher during the discussion
  2. iii. Take down notes and ask questions.
  3. Iv. Attend the classroom work.

WEEK EIGHT

TOPIC

Non-metals and their compounds hydrogen

CONTENT

1 Position in the periodic table.

2 Properties and reactions

3 Laboratory preparation and industrial preparations

4 Uses

5 Laboratory identification

BEHAVIOURAL OBJECTIVE

At the end of the lesson student should be able to:

  1. Write and draw the electronic configuration
  2. Identify the isotopes of hydrogen
  3. Highlight steps involved in the laboratory and industrial method C of properties of hydrogen.
  4. List the physical and chemical properties of hydrogen.
  5. Mention the uses of hydrogen.

INSTRUCTIONAL MATERIALS

  1. The periodic table
  2. Chart showing an electronic configuration of hydrogen
  3. Apparatus for laboratory preparation of hydrogen.

TEACHERS ACTIVITIES

Guides the students to:

  1. write the electronic configuration of hydrogen.
  2. name isotopes of hydrogen.
  3. discuss the unique position of hydrogen on the periodic table.
  4. sets up apparatus for the laboratory preparation of hydrogen using the action of dilute acid (HCl(Aq) ) on active metals (e.g Zinc )

LEADER’S ACTIVITIES

1 write and draw:

-the electronic configuration of hydrogen.

-the structure of isotopes of hydrogen.

-draw the setup apparatus for laboratory preparation of hydrogen gas.

-carry out the test for hydrogen gas using a lighted splint.

WEEK NINE

TOPIC

Oxygen.

CONTENT

  1. Bonding capacity
  2. Allotropes of oxygen
  3. Preparation
  4. Properties and reactions
  5. Uses
  6. Test for oxygen
  7. Oxides.

BEHAVIOURAL OBJECTIVE

At the end of the lesson, students should be able to:

  1. write the electronic configuration of oxygen to establish its bonding capacity.
  2. State some physical properties of oxygen as a major component of air breathing-in
  3. Highlight the major points involved in the laboratory preparation of oxygen.
  4. Draw the diagram of set up apparatus for laboratory preparation of oxygen
  5. State the chemical reactions of oxygen.
  6. List the compounds of oxygen.
  7. State the effect of oxygen on a glowing splint.

INSTRUCTIONAL MATERIALS

  1. The periodic table.
  2. Matches
  3. Splint
  4. Set up apparatus for laboratory preparation of oxygen.

TEACHERS ACTIVITIES

Guides the students:

  1. To write the electronic configuration of oxygen to show its bounding capacity.
  2. State the uses of oxygen.
  3. Set up the apparatus uses for laboratory preparation of oxygen.
  4. Demonstrate the test for oxygen using a glowing splint.
  5. Illustrates oxidation as the addition of oxygen.
  6. Take the allotropes of oxygen.

LEADER’S ACTIVITIES

  1. Write the electronic configuration of oxygen to establish its bounding capacity.
  2. List allotrope of oxygen.
  3. Draw a label diagram of the setup apparatus for making oxygen.
  4. Test for oxygen using a glowing splint.

WEEK TEN

TOPIC

Water and solution

CONTENT

  1. composition of water
  2. structure
  3. source and purity
  4. properties
  5. The hardness of the water.

BEHAVIOURAL OBJECTIVE

Students should be able to:

  1. Draw and explain the structure of water.
  2. Define the following: solute, solvent, and solution
  3. List various sources of water
  4. State various properties of water and identify the abnormal behavior of water.
  5. Highlight steps involved in water treatment for various uses.
  6. Define hard water, and list various types and their cause.
  7. Highlight various methods for removing hard water.

INSTRUCTIONAL MATERIALS

  1. Samples of soft and hard water
  2. Soap.
  3. Sodium chloride(salt)
  4. Washing soda
  5. Source of heat
  6. Distilled apparatus.

TEACHERS ACTIVITIES

  1. Demonstrates formation of hard water by dissolving calcium ions in water.
  2. Demonstrate removal of hardness in water by using washing soda.
  3. List various forms of water sources.
  4. Highlight various stages of water treatment for consumption
  5. Lead student on an excursion to waterworks.

LEADER’S ACTIVITIES

Prepare solutions for common substances

Experiment to remove hardness by boiling and by adding washing soda

Watch the teacher during a demonstration

Take down notes and ask questions.

WEEK ELEVEN

TOPIC

Solution and solubility

CONTENT

1 Define solubility and various types of solution

2 Formula for finding solubility and its S I unit.

3 Factors affecting solubility

4 Solubility curves and their applications

5 Various solvents and their uses

6 Water as the universal solvent

BEHAVIOURAL OBJECTIVE

At the end of the lesson, students should be to:

1 defines solubility and states its unit.

2 name different types of solution

3 apply the solubility equation to solve simple questions.

4 draw the solubility curve and state its applications

5 list various solvents and their uses

INSTRUCTIONAL MATERIALS

1 kerosine

2 water

3 cloth stained with oil

4 soap

5 alcohol.

TEACHERS ACTIVITIES

1 an experiment to help students determine the solubility of a substance

2 demonstrate the application of solubility (removal of stains)

3 guides the students to draw a solubility curve.

LEADER’S ACTIVITIES

1 remove oil stains

2 watch the teacher during a demonstration

3 Takedown notes and asks questions.

WEEK TWELVE & THIRTEEN

Revision and Examination

Kindly Share

Similar Posts