1. Starter 1. What is electricity? 2. Write the formula for Calcium chloride 3. What type of bonding is present in the following: a) Phosphorous chloride b) Sodium c) Water

2. Aim of lesson: To perform an experiment on conductivity to investigate the difference between covalent and ionic substances.

3. Conduction of Ionic Compounds Aim: To investigate which ionic compounds conduct electricity.

4. Method Wires 3v DC Bulb Carbon electrodes Beaker containing compound

5. Results: CompoundFormula Conductor or insulator SolidSolution Copper sulphate Sodium chloride Potassium nitrate Potassium bromide

6. Conclusion: Ionic compounds do not conduct when they are in solid form. If they are in solution, or molten, they do conduct.

7. Ionic Substances Ionic compounds do not conduct when solid because the ions are not free to move. Ions are held tightly in a 3D structure called an ionic lattice. However, ionic compounds do conduct when molten or in solution because the ions are free to move.

8. Ionic bonding Ionic bonding is between a metals and non- metals. We get ions by losing and gaining electrons to achieve a noble gas arrangement Atoms that lose electrons become +vely charged ions (metals), while atoms that gain electrons become –vely charged ions (non- metals). Examples: sodium chloride and magnesium chloride

9. Quick Quiz 1. What types of elements are present in covalent compounds? 2. What can be said about the conductivity of covalent compounds? 3. What types of elements are present in an ionic compound? 4. Explain the conductivity of ionic compounds.