Final answer:
Arrhenius and Brønsted-Lowry acid-base reactions are not synonymous with Lewis acid-base reactions because the latter involves electron-pair transfer, expanding the concept beyond proton transfer or hydroxide ion presence.
Step-by-step explanation:
Arrhenius and Brønsted-Lowry acid-base reactions are not the same as Lewis acid-base reactions. While all Arrhenius acids and bases are also Brønsted-Lowry acids and bases, not all Brønsted-Lowry acids and bases are Arrhenius acids and bases. This is because the Arrhenius definition is limited to aqueous solutions and requires the presence of hydroxide ions for bases, and the production of hydrogen ions for acids. In contrast, the Brønsted-Lowry definition is broader, encompassing acids and bases in non-aqueous media and does not require the presence of hydroxide ions.
The Lewis definition goes even further by not restricting to proton transfer, but instead focusing on the transfer of electron pairs, defining an acid as an electron-pair acceptor and a base as an electron-pair donor. This allows for a wider variety of acid-base reactions, such as those involving the formation of coordinate covalent bonds.