Chemistry – Metals - Properties of metals | e-Consult

Metals generally have higher melting and boiling points than non-metals. This is primarily due to the nature of the metallic bonding present in metals. Metallic bonding involves a "sea" of delocalised electrons, which are strongly attracted to the positively charged metal ions. A significant amount of energy is required to overcome these strong attractions and separate the atoms, hence the high melting and boiling points.

Non-metals, on the other hand, exhibit various types of bonding, including covalent and ionic. Covalent bonding involves sharing of electrons between atoms, and ionic bonding involves the transfer of electrons between atoms, resulting in electrostatic attraction. While these bonds are strong, they are generally weaker than metallic bonds. Therefore, less energy is required to break these bonds and transition from solid to liquid (melting) or liquid to gas (boiling), leading to lower melting and boiling points compared to metals.

Comparison of Bonding Types: