Lesson Plan

• Describe the roles of the anode and cathode during electrolysis.
• Write ionic half‑equations for oxidation at the anode and reduction at the cathode.
• Balance each half‑equation for mass and charge.
• Apply the procedure to both molten and aqueous electrolytes.
• Evaluate the competing reactions of water versus ions in aqueous solutions.

• Projector or interactive whiteboard
• Printed handout with half‑equation examples
• Worksheet with practice electrolytes
• Periodic table poster
• Diagram of an electrolytic cell
• Markers and whiteboard

Begin with a quick recall of oxidation‑reduction concepts, asking students to name the anode and cathode from previous work. Connect this knowledge to the new idea that electrolysis forces a non‑spontaneous redox reaction. Explain that today’s success criteria are to correctly write and balance half‑equations for both molten and aqueous systems.

1. Do‑now (5'): Students list what they know about oxidation, reduction, anode and cathode.
2. Mini‑lecture (10'): Explain electrolysis, show cell diagram, introduce the step‑by‑step method for half‑equations.
3. Guided practice (12'): Work through aqueous NaCl example together, students complete a worksheet.
4. Group activity (10'): Each group selects a different electrolyte (e.g., molten AlCl₃, aqueous HCl) and writes the corresponding half‑equations.
5. Whole‑class feedback (8'): Groups present; teacher checks balancing and discusses water’s competing role.
6. Exit ticket (5'): Individually write one balanced oxidation and one reduction half‑equation for a given electrolyte.

We have reviewed how to construct and balance ionic half‑equations for both molten and aqueous electrolysis, emphasizing water’s influence as a competing reactant. For homework, complete the additional worksheet on other electrolytes and be ready to discuss your answers in the next lesson.