How does Bronsted Lowry's definition of acids and bases work? I can understand Arrhenius' and Lewis' but I don't quite understand this one.. Could someone help me please?

Question

anonymous · Answer

Bronsted-Lowry bases are compounds that can accept hydronium ions(H+) Ammonia(NH3)  is an example of a Bronsted Lowry base.
             While Bronsted-Lowry acids are compounds that gives hydronium ions(H+) to another compound Hydrochloric acid(HCl) is an example of Bronsted Lowry Acid .Other examples of Bronsted Lowry Acids are B2H6, BF3, Al2Cl6, AlF3, SiF4, PCl5 and SF4.

anonymous · Answer

Simply,
Acording to Bronsted-Lowry
acid = a substance that donates an H+(e.g,NH3)
Base = a substance that accepts an H+(e.g,HCl)

vincent-lyon.fr · Answer

The examples should be the other way round.

"BF3, Al2Cl6, AlF3, SiF4, PCl5 and SF4" are 'extended' Bronsted-Lowry acids because they cannot give away H+ by themselves (they do not have hydrogen in their formulae).