Bonding

• Metals are electron donors and hence become positive.
• Non metals are electron acceptors and hence become negative.
• Ionic bonding takes place between a metal and a non metal.
• Ionic compounds are soluble in H2O.
• Ionic compounds have high melting and boiling points because they have strong electrostatic forces between negative and positive ions and huge amounts of energy is required to break these forces.
• All ionic compounds conduct electricity in their molten or aqueous form as in that form, they have delocalized ions.
• Ionic compounds do not conduct electricity in their solid form.
• Covalent bonding takes place between non metals.
• In covalent bonding, a shared pair of electrons come in the overlapping region.
• Covalent compounds do not conduct electricity.
• Covalent compounds are insoluble in water but they are soluble in some organic solvents.
• In ionic compounds, electrostatic forces hold the compound together.
• In covalent compounds, intermolecular forces hold the compound together.
• Covalent compounds have low melting and boiling points because they have weak intermolecular forces between the atoms, and so less energy is required to overcome these forces.