Ionic bonding typically involves metals and non-metals. In this type of bond, a metal atom donates one or more of its electrons to a non-metal atom, resulting in the formation of charged ions. The metal, which loses electrons, becomes a positively charged cation, while the non-metal, which gains electrons, becomes a negatively charged anion. This transfer of electrons creates an electrostatic attraction between the oppositely charged ions, resulting in the formation of an ionic compound.
Covalent bonding usually involves non-metals. In a covalent bond, atoms share pairs of electrons in order to achieve a full outer shell of electrons, which is a more stable state. This sharing can occur between two non-metal atoms, leading to the formation of a molecule. The bonds can be single (one pair of electrons shared), double (two pairs), or triple (three pairs) depending on how many electrons are shared between the atoms. This type of bonding allows both atoms to attain a full valence shell, resulting in a more stable molecular structure.