Final answer:
The given reaction demonstrates a Lewis acid-base reaction, where a base donates and an acid accepts an electron pair to form a new covalent bond C) Bronsted-Lowry acid-base reactions.
Step-by-step explanation:
The reaction H-A + :B ↔ :A⁻ + H-B⁺ demonstrates the concept of a Lewis acid-base reaction. In this reaction, a Lewis base (:B) donates an electron pair to the Lewis acid (H-A) to form a covalent bond, resulting in the products :A⁻, which is the base with one less proton, and H-B⁺, which now has an additional proton.
Key distinctions can be made among the three theories of acids and bases:
- Arrhenius theory predicts acids and bases as species that produce H+ and OH⁻ ions respectively in aqueous solution.
- Brønsted-Lowry theory defines acids as proton donors and bases as proton acceptors, which can occur in any medium.
- Lewis theory, which is demonstrated in the provided reaction, focuses on the transfer of electron pairs rather than protons, defining acids as electron pair acceptors and bases as electron pair donors.