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The Bronsted definitions of acids and bases relate to the protons. So a Bronsted acid is a proton donor and a Bronsted base is a proton acceptor. The Lewis definitions of acids and bases relate to the electrons. A Lewis acid is an electron acceptor and a Lewis base is an electron donor.
Bases and acids can be considered to fit in the Lewis and bronsted definition but not all fall in to this category. For example, "the HF molecule as a whole cannot be considered an electron acceptor as there is no room for more electrons,so HF first dissociates and then the H accepts the electron. But the Bronsted base is OH-, which is the Lewis base. It donates electrons".
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