Lesson Plan

• Describe oxidation as loss of electrons and an increase in oxidation number.
• Explain how oxidation is paired with reduction in a redox reaction.
• Identify oxidation‑number changes in common examples such as Mg → Mg²⁺ and Fe²⁺ → Fe³⁺.
• Apply oxidation‑number rules to write half‑reactions for simple redox equations.

• Projector and screen
• Whiteboard and markers
• Printed worksheet with oxidation‑number table
• Magnesium ribbon, candle, and safety goggles for a demo
• Student notebooks and calculators

Begin with a quick question: “What happens to an atom when it loses electrons?” Connect this to students’ prior work on electron transfer. State that by the end of the lesson they will be able to define oxidation precisely and recognise it in redox reactions.

1. Do‑now (5') – Short quiz on electron loss/gain and oxidation numbers from the previous lesson.
2. Mini‑lecture (10') – Define oxidation (loss of electrons, ↑ oxidation number) and link to reduction.
3. Guided example (12') – Work through the Mg + O₂ → MgO half‑reactions, filling the oxidation‑number table.
4. Group activity (10') – Teams analyse given reactions (Fe²⁺ → Fe³⁺, Cl⁻ → Cl₂, CH₄ → CO₂) and identify the oxidised species.
5. Check for understanding (5') – Exit ticket: write the oxidation half‑reaction for a supplied species.
6. Summary & homework (3') – Recap key points and assign the worksheet for further practice.

Summarise that oxidation is always electron loss and an increase in oxidation number, occurring alongside reduction. Collect exit tickets to gauge understanding, and remind students to complete the worksheet on identifying oxidation and reduction in new reactions for homework.