Lewis Acids

The Lewis theory of acid-base reactions define Lewis acids and bases as electron pair acceptors and donors, respectively. In order to create a product with a coordinate covalent bond, a Lewis base can give a pair of electrons to a Lewis acid. Lewis adduct is another name for this item. The chemical species known as Lewis Acids contain vacant orbitals and can take electron pairs from Lewis Bases. This phrase was historically used to refer to chemical species with a trigonal planar structure and an empty p-orbital. Such a Lewis acid would include BR3. Given that they may take and give electron pairs, water and several other substances are regarded as both Lewis acids and bases. Examples of Lewis acids that may receive electron pairs include the following:

Lewis acids include onium ions like H3O+ as well as H+ ions (or protons).

High oxidation stated block element cations can serve as acceptors for an electron pair. Fe3+ is an illustration of such a cation.

Metal cations like Mg2+ and Li+ can combine with water to generate coordination compounds. These aquo compounds exhibit Lewis acid behaviour and can receive electron pairs.

H3C+ and other trigonal planar species tend to provide carbocations that accept electron pairs.

Lewis acids can be created using the pentahalides of the following group 15 elements: antimony, arsenic, and phosphorus.