Ionic bonds occur primarily between metals and non-metals. These bonds are formed through the transfer of electrons from one atom to another.
In this process, the metal loses electrons to become a positively charged cation, while the non-metal gains electrons to become a negatively charged anion. The resulting attraction between opposite charges holds the ionic compound together.
Despite the traditional view of strict electron transfer, we can see through Fajan's rules that ionic bonds also exhibit a degree of sharing, making them not purely ionic in nature. Factors such as electronegativity differences play a major role, but are not the only determinants.
- Ionic bonds typically have high melting and boiling points.
- They are often soluble in water.
- This type of bonding provides compounds with crystal lattice structures.
Therefore, while ionic bonds are characterized by the presence of charges, there's room for covalency, giving more depth and color to their nature.