Final answer:
The statement is true; a Lewis acid is indeed an electron-pair acceptor and a Lewis base is an electron-pair donor, which expands upon the Brønsted-Lowry definition to include a wider range of substances.
Step-by-step explanation:
The statement that a Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor is true. In chemistry, the idea of acid and base interactions is a fundamental concept, and the Lewis definition broadens the scope beyond the Brønsted-Lowry definition of acids and bases, which are limited to proton donors and acceptors. Lewis acids include species like H+, metal cations such as Mg2+ and Zn2+, and neutral species such as boron trifluoride (BF3) and carbon dioxide (CO2). Lewis bases, also known as nucleophiles, are electron-pair donors that use unshared electrons to form new bonds with other atoms and are often involved in organic and inorganic reactions, including many biological processes.