Question

What is the difference between Arrhenius, Bronsted-lowry and Lewis acids and bases\[?\]

Answer 1

Hint: First we know Arrhenius, Bronsted-lowry and Lewis acids and bases. Then mention the difference between Arrhenius, Bronsted-lowry and Lewis acids and bases. Also give some examples.

Complete answer:
An Arrhenius base increases the concentration of OH- ions. A Bronsted-Lowry acid is any species that donates a proton to another molecule. A Bronsted-Lowry base is any species that accepts a proton from another molecule. A Lewis acid is an electron pair acceptor.
In Arrhenius, we are limited to cases in which water is the solvent. An acid will dissolve in water to produce H+ ions, while a base will dissolve in water to produce \[O{H^ - }\] ions.
Bronsted and Lowry state that an acid is any substance that will donate a proton (meaning an \[{H^ + }\] ion). This includes the case where the donation of the proton is made to a water molecule (which therefore includes everything Arrhenius would have considered), but allows for donation of protons to many other substances, opening the door for proton-transfer reactions such as
\[HCl + N{H_3} \to NH_4^ + + C{l^ - }\]
The Lewis definition goes this one further in stating that an acid is a substance that can receive an electron pair (meaning the lone pair of a particle) and that a base is a substance that can donate a lone pair.
Again, this definition includes all cases that fit into the B-L scheme, because the \[{H^ + }\] proton Bronsted and Lowry refer to is a proton with an empty orbital. This orbital can bond with the lone pair of a particle such as the ammonia molecule (the \[N\] atom has a full orbital not used to bond to the three \[H\] atoms, hence a lone pair).
However, Lewis also includes cases in which the \[{H^ + }\] proton is not the particle being transferred, and so broadens the concept of acids and bases to include many more cases. For example
\[B{F_3} + {F^ - } \to BF_4^ - \]
would not be an acid-base reaction according to Bronsted-Lowry, but does qualify in the Lewis sense.

Note:
Note the Bronsted and Lowry also change our thinking of what makes a substance a base. All that is required is that a particle (atom, molecule or ion) be able to acquire a proton, and that particle is a base. Check out the role of \[N{H_3}\] above.