Lesson Plan

• Describe why atoms form covalent bonds to achieve noble‑gas electron configurations.
• Explain how sharing of electron pairs creates single, double, and triple covalent bonds.
• Predict the number of covalent bonds an atom can form based on its valence electrons.
• Illustrate the formation of a covalent bond using H₂ or Cl₂ as examples.

• Projector or interactive whiteboard
• Slide deck with electron‑sharing diagrams
• Ball‑and‑stick model kits
• Worksheet with bond‑formation exercises
• Exit‑ticket cards

Begin with a quick animation showing two atoms pulling together, prompting students to consider why they might want to stick together. Recall that atoms strive for the lowest‑energy, noble‑gas electron arrangement studied last lesson. Today we will determine the success criteria: students will be able to state how a covalent bond forms and sketch the electron‑sharing process.

1. Do‑now (5') – students answer a short question on electron configurations on a mini‑quiz sheet.
2. Teacher mini‑lecture (10') – present the concept of covalent bonding with slides and the H₂ example.
3. Guided practice (12') – use ball‑and‑stick models to build H₂, O₂ and H₂O, discussing shared pairs.
4. Collaborative worksheet (10') – groups complete a worksheet converting electron‑dot diagrams into covalent structures.
5. Check for understanding (8') – ask a few students to explain the formation of a Cl₂ bond on the board, using diagrams.
6. Exit ticket (5') – write one sentence describing why covalent bonds give atoms a noble‑gas configuration.

Summarise that covalent bonds allow atoms to complete their valence shells by sharing electrons, producing stable noble‑gas configurations. Ask a few pupils to share their exit‑ticket statements for quick retrieval. Assign homework to research a simple covalent molecule and draw its Lewis structure.