Ionic compound ...........

1. Ionic Compounds have high boiling and melting points as they’re very strong and require a lot of energy to break.

2. Theelectrostaticforces of attraction between oppositely charged ions lead to the formation of ions.

3. Ionic compounds form crystals.

4. These compounds are brittle and break into small pieces easily.

5. Electrovalent compounds usually dissolve in water and are insoluble in solvents like oil, petrol, kerosene, etc.

6. Ionic compounds do not conduct electricity in a solid state but they do conduct electricity in the molten state.

7. In comparison to molecular compounds, ionic compounds have higher enthalpies of fusion and vaporization.

1. Covalent compounds usually have low melting points. An exception to this include molecules of silica and diamonds that have a high melting point.

2. These compounds have low boiling points. This can be attributed to their weak force of attraction between the various bonded atoms. Van Der Waals forces bind these atoms.

3. These compounds are usually gases and liquids with low boiling and melting points.

4. The solid covalent compounds have soft structures like graphite. This is because of the presence of a cloud of electrons in between each layer of carbons atoms.

5. These compounds are non-conductors of electrical charge. The absence of charged ions is the main reason behind this. An exception to this is graphite, where we see a cloud of electrons. These make graphite a good conductor.

6. They are bad conductors of heat also. Their molecules lack free electrons and that obstructs the flow of heat energy.