What is Lewis theory of acids
Answers
Explanation:
Lewis' theory used electrons instead of proton transfer and specifically stated that an acid is a species that accepts an electron pair while a base donates an electron pair.
Answer:
by the Lewis theory of acid-base reactions as electron-pair acceptors and electron pair donors respectively. Therefore, a Lewis base can donate a pair of electrons to a Lewis acid to form a product containing a coordinate covalent bond. This product is also referred to as a Lewis adduct. An illustration detailing the reaction between a Lewis acid and base leading to the formation of a coordinate covalent bond between them
Lewis Acid
Lewis Acids are the chemical species which have empty orbitals and are able to accept electron pairs from Lewis bases. This term was classically used to describe chemical species with a trigonal planar structure and an empty p-orbital. An example of such a Lewis acid would be BR3 (where R can be a halide or an organic substituent).
Water and some other compounds are considered as both Lewis acids and bases since they can accept and donate electron pairs based on the reaction.
Examples of Lewis Acids
Some common examples of Lewis acids which can accept electron pairs include:
H+ ions (or protons) can be considered as Lewis acids along with onium ions like H3O+.
The cations of d block elements which display high oxidation states can act as electron pair acceptors.