Using diagrams, describe the difference between Ionic, Covalent and Metallic Bonding.

Ionic bonding is the electrostatic forces of attraction between a metallic and non-metallic ion. The metallic ion has a positive charge because it loses an electron. For example, with KCl (Potassium Chloride), the potassium element becomes K+ when it loses an electron. The non-metallic ion has a negative charge because it gains an electron, hence becoming Cl-. The oppositely charged ions are attracted to each other, hence the strong electrostatic force of attraction. They are arranged in the form of a giant ionic lattice.Covalent bonding occurs when pairs of electrons are shared by atoms. Atoms will covalently bond with other atoms in order to gain more stability, which is gained by forming a full electron shell. For example, if we have two Fluorine atoms, both of which are one electron away from having a full outer shell, they can fill their outer shell by sharing their last unpaired electron. This forms a F2 molecule, with both F atoms bound together by a covalent bond.Metallic bonding is the electrostatic force of attraction between positive metal ions and a delocalised sea of electrons. For example, if we have a sample of magnesium, then each atom will lose its 2 outer electrons, to become Fe2+ ions, and the electrons will go into the delocalised sea of electrons. The electrostatic forces of attraction between the Fe2+ ions and the electrons constitute metallic bonding.