Arrhenius acid: [H+] ion donor Arrhenius base: [OH-] ion donor Bronsted-Lowry acid: proton [H+] donor Bronsted-Lowry base: proton [H+] acceptor Lewis acid: electron acceptor Lewis base: electron donor
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. H+ + OH- => H20. H+ has no electrons, so when it bonds to the Oxygen, it gains an electron pair. OH-"loses" an electron pair.
The Arrhenius model for acids and bases states that acids contain H+ ions and bases contain OH- ions. The Bronsted-Lowry acid base model states that acids are H+ donors and that bases are H+ acceptors. This might be more valid since not all bases have OH- ions, such as NH3. Finally, the Lewis acid base model focuses on the electrons and it states that acids are electron pair acceptors and bases are electron pair donors.
Arrhenius acid: [H+] ion donor
ReplyDeleteArrhenius base: [OH-] ion donor
Bronsted-Lowry acid: proton [H+] donor
Bronsted-Lowry base: proton [H+] acceptor
Lewis acid: electron acceptor
Lewis base: electron donor
The Arrhenius model says that acids always contain H+ and that bases always contain OH-.
ReplyDeleteThe 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. H+ + OH- => H20. H+ has no electrons, so when it bonds to the Oxygen, it gains an electron pair. OH-"loses" an electron pair.
The Arrhenius model for acids and bases states that acids contain H+ ions and bases contain OH- ions. The Bronsted-Lowry acid base model states that acids are H+ donors and that bases are H+ acceptors. This might be more valid since not all bases have OH- ions, such as NH3. Finally, the Lewis acid base model focuses on the electrons and it states that acids are electron pair acceptors and bases are electron pair donors.
ReplyDeleteArrhenius acid: produces H+ ions
ReplyDeleteArrhenius base: produces OH- ions
Bronsted-Lowry acid: proton [H+] donor
Bronsted-Lowry base: proton [H+] acceptor
Lewis acid: electron acceptor
Lewis base: electron donor