Lesson Plan

• Describe how ionic bonds form between Group I metals and Group VII non‑metals.
• Illustrate electron transfer using dot‑and‑cross diagrams.
• Predict the charges on the ions and write the correct formula for the resulting ionic compound.
• Explain why ionic bonds are strong based on charge magnitude and ionic radii.

• Projector or interactive whiteboard
• Periodic‑table poster
• Handouts with dot‑and‑cross diagram worksheets
• Model kits or magnetic ions for a physical demonstration
• Whiteboard markers and eraser
• Exit‑ticket cards

Begin with a quick demonstration: show a piece of sodium metal and a chlorine gas balloon to spark curiosity about how they combine. Ask students what they know about electron shells and why atoms seek stability. Explain that today they will discover how electrons move from Group I metals to Group VII halogens and how to visualise this with dot‑and‑cross diagrams. State that success will be measured by correctly drawing the diagrams and explaining the bond formation.

1. Do‑Now (5') – Short quiz on valence electrons of Group I and VII elements.
2. Mini‑lecture (10') – Review electron configurations and introduce dot‑and‑cross notation using the projector.
3. Guided practice (15') – Whole‑class step‑by‑step creation of the NaCl dot‑and‑cross diagram on the board.
4. Pair activity (15') – Learners draw diagrams for NaF, KBr, LiCl on worksheets and peer‑check.
5. Concept check (5') – Exit question: “What determines the strength of an ionic bond?”
6. Summary & reflection (5') – Teacher recaps key points; students write one takeaway on an exit ticket.

Review that ionic bonds result from electron transfer from Group I metals to Group VII halogens, producing oppositely charged ions that attract each other. Highlight how dot‑and‑cross diagrams visually represent this process. Collect exit tickets as a retrieval check and assign homework to complete additional diagram worksheets for new ionic compounds.