Metallic Bonding

• Metals consist of a giant structure of atoms arranged in a regular pattern.
• The electrons in the outer shell of the metal atoms are delocalised, so they can move freely around the metal atoms.
• There are strong forces of electrostatic attraction between the lattice of positive metal ions and the shared sea of negative electrons.
• The forces of attraction in metallic bonding are held together in a regular structure.
• Metallic elements and alloys are examples of metallic bonding.
• The electrostatic forces between the metal atoms and the delocalised sea of electrons are very strong, so need lots of energy to be broken. So most compounds with metallic bonding have very high melting and boiling points, so they're generally solid at room temperature.
• Ions with higher charges have more delocalised electrons, so have stronger forces of electrostatic attraction. This means they have higher melting and boiling points.
• The delocalised electrons carry electrical current and thermal (heat) energy, so metals are good conductors of electricity and heat.
• The layers of atoms in a metal can slide over each other- making metals malleable.
• The layers of atoms within metals also make them ductile- they can be drawn out into wires.