What is the difference between a Bronsted acid/base and a Lewis acid/base?

Ammonia is a Bronsted base: $NH_3(aq) + H_2O(l) rightleftharpoons NH_4^+ + OH^-$ $pK_b = 4.75$ I am not going to solve this equation using $pK_b$, but most of the ammonia...

So first of all, what is Bronsted-Lowry theory of ? Well in 1923, two people with their last names Bronsted and Lowry defined acid as a substance which can...

$HONH_2(aq) + H_2O(l) rightleftharpoonsHONH_3^+ + HO^-$ And then we write the equilibrium expression: $K_b=10^-8=([HONH_3^+][HO^-])/([HONH_2])$, And we make the usual approximations, and invoke $x$ as the moles of hydroxylamine that associate,...

Well, for... $"NH"_4^(+)(aq) + "H"_2"O"(l) -> "NH"_3(aq) + "H"_3"O"^(+)(aq)$, the conjugate base has one less $"H"^(+)$. What has one less $"H"^(+)$ than $"H"_3"O"^(+)$? $"H"_3"O"^(+) - "H"^(+) =...

A Brønsted-Lowry base is a substance that behaves as a proton acceptor. For example, $underbrace("NH"_3)_color(red)("proton acceptor") + "H-Cl" → "NH"_4^"+" + "Cl"^"-"$ The $"NH"_3$ is accepting a proton from the...

(i) Arrhenius defined the acidium ion as $H^+$. (ii) Bronsted and Lowry defined the acid base reaction on the basis of proton transfer between .... $"Acid + Base "rightleftharpoons"...

$c.$, you got $"bisulfate ion"$; in aqueous solution this is a moderately strong acid. Certainly we treat $H_2SO_4$ as a diacid in aqueous solution. $e.$, you got $"ammonium ion"$; in...

According to Bronsted-Lowry, an acid is a substance that donates a proton ($H^+$) and a base is a substance that accepts the donated proton

Chemistry is still an experimental science. Notions of Lewis acidity/Lewis basicity are all very well. These notions are generalizations that account for observed chemical behaviour. So does the given species...

$NCl_3$, $NH_3$, and $PCl_3$ are all electron donors. $AlCl_3$ is an electron pair acceptor, and may thus be classified as a Lewis acid. In fact much of the chemistry of...