Basic Electricity - Senior Secondary 1

TERM: 3^RD TERM

WEEK TEN

Class: Senior Secondary School 1

Age: 15 years

Duration: 40 minutes of 5 periods each

Date:

Subject: BASIC ELECTRICITY

Topic: BATTERY CHARGING II

SPECIFIC OBJECTIVES: At the end of the lesson, pupils should be able to

I.) Define electrolyte

II.) Construct a Simple Cell

INSTRUCTIONAL TECHNIQUES: Identification, explanation, questions and answers, demonstration, videos from source

INSTRUCTIONAL MATERIALS: Videos, loud speaker, textbook, pictures,

INSTRUCTIONAL PROCEDURES

PERIOD 1-2

PRESENTATION	TEACHER’S ACTIVITY	STUDENT’S ACTIVITY
STEP 1 INTRODUCTION	The teacher explains the meaning of electrolyte to the students	Students listens attentively to the teacher
STEP 2 EXPLANATION	Teacher guide students to construct a simple cell in the workshop.	Students exhibit attentiveness and active engagement
STEP 3 NOTE TAKING	The teacher writes a summarized note on the board	The students copy the note in their books

NOTE

BATTERY CHARGING II

Electrolyte

An electrolyte is a substance that conducts electricity when dissolved in a solvent or melted. It contains ions that are free to move and carry electric charge. In electrochemical cells, electrolytes are essential for facilitating the flow of ions between the electrodes, allowing the cell to generate electrical energy through chemical reactions.

Procedure to Constructing a Simple Cell

Below is a simple procedure to construct a basic galvanic cell (also known as a voltaic cell):

Materials Needed:

- Two different metals (e.g., copper and zinc)

- Two electrolytes (e.g., copper sulfate solution and zinc sulfate solution)

- Two inert electrodes (e.g., graphite rods)

- Connecting wires

- Voltmeter (optional, for measuring voltage)

Procedure

Prepare the Electrolytes: Prepare two electrolyte solutions by dissolving copper sulfate in water to make a copper sulfate solution and zinc sulfate in water to make a zinc sulfate solution. Ensure that the concentrations are not too high to prevent excessive current flow.
Prepare the Electrodes: Attach each metal to an inert electrode (e.g., graphite rod) to create the anode and cathode. For example, attach a copper strip to one electrode and a zinc strip to the other electrode.
Assemble the Cell: Place the two electrodes (with attached metals) into their respective electrolyte solutions. Ensure that the electrodes are immersed in the electrolytes but do not touch each other.
Connect the Circuit: Connect the two electrodes with a conducting wire. This completes the circuit and allows electrons to flow from the anode to the cathode through the external circuit.
Observe the Reaction:

- As the circuit is completed, electrons will flow from the zinc electrode (anode) to the copper electrode (cathode) through the external circuit.

- At the zinc electrode (anode), zinc atoms will oxidize and release electrons, forming zinc ions in the electrolyte solution.

- At the copper electrode (cathode), copper ions from the electrolyte solution will gain electrons and deposit onto the copper electrode as solid copper.

EVALUATION: 1. What is an electrolyte?

Construct a simple cell

CLASSWORK: As in evaluation

CONCLUSION: The teacher commends the students positively

Basic Electricity - Senior Secondary 1 - Battery charging II