1. Ionic Bonding: This occurs when one atom donates an electron to another atom. This results in one atom becoming positively charged (a cation) and the other becoming negatively charged (an anion). The electrostatic attraction between these oppositely charged ions holds them together.

2. Covalent Bonding: In covalent bonding, atoms share electrons. This sharing can be equal (nonpolar covalent bond) or unequal (polar covalent bond), where one atom has a stronger pull on the shared electrons. The shared electrons create a strong attraction between the atoms.

3. Metallic Bonding: This type of bonding occurs only between metal atoms. It involves a "sea" of delocalized electrons that are not bound to any particular atom. This sea of electrons allows metals to conduct electricity and heat well, and gives them their characteristic luster and malleability.

4. Hydrogen Bonding: While not a "true" bond in the same way as the others, hydrogen bonding is a strong type of intermolecular attraction. It occurs between a hydrogen atom covalently bonded to a highly electronegative atom (like oxygen, nitrogen, or fluorine) and a lone pair of electrons on an adjacent electronegative atom. This attraction plays a vital role in the properties of water and other biological molecules.