1. Structure and Properties of Ionic and Covalent Compounds

2. Ionic Compounds
Crystalline - Arranged in crystal lattices with each ion surrounded by many oppositely charged ions.
Brittle -When force is applied causes like charges to align causing it to break.

3. Ionic Compounds
High Melting/Boiling Points – Melting/Boiling involves breaking bonds between ions which takes a lot of energy
Solubility –Soluble in water as the charged ions are attracted to the partial charges of polar water molecules

4. Ionic Compounds
Electrical Conductivity – Solids are not conductive as the ions are locked in place, however when molten or dissolved in water the ions can move easily and so are very conductive.

5. Covalent Compound
Soft and Squishy – There are only bonds present inside the molecules, not between them, and so therefore covalent compounds are a lot more flexible rather than hard.

6. Covalent Compound
Low Melting/Boiling Points – Melting only involves separating the molecules from each other where there are no bonds, so it melts/boils more easily.
Solubility – Most do not dissolve in water as most are non-polar and so are not attracted to the charges in water.

7. Covalent Compound
Electrical Conductivity – Even when the molecules can move around as a liquid or dissolved in a liquid, the molecules don’t have charges and so make poor conductors.