| Lesson Plan |
| Grade: |
Date: 25/02/2026 |
| Subject: Chemistry |
| Lesson Topic: Explain in terms of structure and bonding the properties of simple molecular compounds: (a) low melting points and boiling points in terms of weak intermolecular forces (specific types of intermolecular forces are not required) (b) poor electrical co |
Learning Objective/s:
- Describe the structure of simple molecular compounds and the covalent bonding within molecules.
- Explain why these compounds have low melting and boiling points because only weak intermolecular forces must be overcome.
- Explain why simple molecular compounds show poor electrical conductivity due to the absence of mobile charge carriers.
- Compare the properties of simple molecular solids with ionic, covalent‑network and metallic solids.
- Apply the concepts to predict the behaviour of a given molecular compound when heated or dissolved.
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Materials Needed:
- Projector or interactive whiteboard
- Slide deck on molecular structures and intermolecular forces
- Handout with compound data tables and worksheet
- Molecular model kits (optional)
- Whiteboard and markers
- Exit‑ticket cards
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Introduction:
Begin with a quick question about why ice melts at 0 °C while salt melts at much higher temperatures, linking to prior knowledge of bond types. Highlight that today’s focus is on how structure and bonding dictate melting points and conductivity. State that students will be able to explain these properties and compare them with other solid types by the end of the lesson.
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Lesson Structure:
- Do‑now (5') – short quiz on states of matter and basic bond types.
- Mini‑lecture (10') – present key concepts: discrete molecules, covalent bonds, weak intermolecular forces.
- Guided analysis (10') – examine the melting/boiling point table; discuss why only weak forces are broken.
- Demonstration (5') – show sublimation of dry ice or boiling water to illustrate low temperature changes.
- Group activity (10') – using the comparison table, students fill a worksheet contrasting simple molecular, ionic, covalent‑network and metallic solids.
- Concept check (5') – think‑pair‑share question on why simple molecular compounds conduct poorly; teacher polls answers.
- Summary & exit ticket (5') – students write one reason for low melting point and one reason for poor conductivity on a card.
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Conclusion:
Recap the two main reasons why simple molecular compounds have low melting/boiling points and poor electrical conductivity. Collect exit tickets to gauge understanding and clarify any lingering misconceptions. Assign homework: students research a simple molecular compound of their choice and prepare a brief note on its melting point, boiling point, and conductivity in both solid and aqueous states.
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