Exploring the Chemical Effects of Electric Current: DIY Activities for High School Teachers & Homeschooling Parents
Introduction:
Engaging students in hands-on activities is an effective way to teach the chemical effects of electric current. In this blog post, we present three exciting and educational DIY activities that high school teachers and homeschooling parents can use to demonstrate these concepts. Each activity is designed to be fun, interactive, and easy to set up, requiring simple materials that are readily available. Let's dive into the fascinating world of the chemical effects of electric current!
Activity 1: Electrolysis
Materials Required:
- Salt
- Water
- Graphite rods
- Battery
- beaker
Procedure:
- Fill the beaker with water.
- Dissolve a small amount of salt in the water to create a saltwater solution.
- Insert two graphite rods into the solution, making sure they are not touching each other.
- Connect the positive terminal of the battery to one graphite rod and the negative terminal to the other.
- Observe the process as the electric current passes through the solution, causing electrolysis to occur.
- Bubbles should form around the graphite rods, indicating the movement of ions.
- Discuss the chemical reactions that take place, such as the decomposition of water into hydrogen and oxygen gases.
What’s Happening?
Salt is mixed with water | For electrolysis to work, the ions must be free to move. Ions are free to move when an ionic substance is dissolved in water or molten (melted). |
|---|---|
When current is passed | Ionic compound is broken down to ions & the ions move towards electrodes of opposite charge. NaCl− → Na+ + Cl− H2 O− → H+ + OH− |
At the cathode | 2H+ + 2e− → H2 (g) (NOTE: H+ is easier to reduce than Na+) |
At the anode | 2Cl− → Cl2 (g) + 2e− (NOTE: Cl− is easier to oxidize than hydroxide OH−) |
Inside the electrolyte | Na+ + OH− → NaOH |
Ionic substances contain charged particles called ions. For example, lead bromide contains positively charged lead ions and negatively charged bromide ions.
Real Life Connect: Electric cells
An electric cell is an electrolytic system in which a chemical reaction causes a current to flow in an external circuit; it essentially reverses electrolysis. A battery is a single electric cell (or two or more such cells linked together for additional power) used as a source of electrical energy.
Activity 2: Electroplating
Materials Required:
- CuSO4 (Copper sulfate)
- Water
- Copper rod
- Iron nail
- Aluminum nail
- Steel ring
- Battery
- beaker
Procedure:
- Prepare a copper sulfate solution by dissolving CuSO4 in water.
- Place the iron nail, aluminum nail, and steel ring in separate containers.
- Connect the positive terminal of the battery to the copper rod and the negative terminal to the objects (iron nail, aluminum nail, and steel ring) using wires.
- Submerge the objects in their respective containers, ensuring they do not touch each other.
- Observe the electroplating process as copper ions migrate from the copper rod to the objects, forming a thin copper coating.
- Discuss the concepts of reduction and oxidation, as well as the applications of electroplating in various industries.
What’s Happening?
Copper goes into the Copper Sulphate solution at the Anode (+). A constant concentration of Cu2+is maintained in the electrolyte solution surrounding the electrodes. The Copper is coated onto the conductive surface placed at the Cathode (-).
Reactions:
Anode (+) : Cu(s) Cu2+(aq) + 2 e
Cathode (-) : Cu2+(aq) + 2 e- Cu(s)
Try putting different materials at cathode(-)
Activity 3: Conduction of Electricity in Liquids
Materials Required:
- Salt
- Battery
- Water
- LED bulb
- Wires
Procedure:
- Prepare a saltwater solution by dissolving salt in water.
- Connect the positive terminal of the battery to one end of a wire and the negative terminal to the shorter leg of the LED bulb.
- Dip the other end of the wire into the saltwater solution.
- Connect the longer leg of the LED bulb to the saltwater solution using a separate wire.
- Observe as the LED bulb lights up, indicating the conduction of electricity through the liquid.
- Discuss the role of ions in conducting electricity and relate it to the properties of electrolytes.
What’s Happening?
When electricity is passed through pure water, the bulb didn’t glow since pure water is a bad conductor of electricity. However, when salt is added to water & electricity is passed, the bulb glows because of the presence of ions in the electrolyte.
Inside the electrolyte, it is the ions which move towards the electrodes. Outside the electrolyte, through the bulb, wire & the battery – it is the electrons which move.
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Hands-On Chemistry: Exploring the Chemical Effects of Electric Current
Conclusion: By combining these three electrifying experiments into a single session, high school teachers and homeschooling parents can create an unforgettable learning experience. Students will gain a comprehensive understanding of the chemical effects of electric current while enjoying a day filled with hands-on science fun. Get ready to spark curiosity, ignite passion, and empower the next generation of scientists and engineers on this electrifying adventure!
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