What is the difference between Arrhenius, bronsted-lowry and Lewis acids and bases?
The Arrhenius model says that acids always contain H+ and that bases always contain OH-. The Bronsted-Lowry model thinks of acids as being proton donors and proton acceptors, so bases no longer need to contain OH-, and acids donate a proton to water forming H3O+. Lewis acids are electron pair acceptors, and Lewis bases are electron pair donors. For instance, H+ + OH- => H20. H+ has no electrons, so when it bonds to the Oxygen, it gains an electron pair. OH- “loses” an electron pair. Sorry it’s not a great example.
