How do Lewis acids and bases differ from other acids and bases?

Both definitions are correct. Neither definition is wrong. The definitions are related, but they refer to different phenomena. A Brønsted acid is a proton donor. A Brønsted base is a...

It came from his long interest in how electrons are involved in bonding. Early in his career, in 1902, Lewis had been interested in the role of the recently-discovered electron...

Lewis acids: $Fe^(3+)$ $BH_2$ Lewis bases: $NH_3$ $F^-$ Lewis acids(or electrophiles) are electron-deficient species. We can also say that they have a net positive charge. $BH_3$ is a lewis acid...

Which species in the equation has accepted an electron pair? Which species has donated an electron pair? Hydride anion is clearly the Lewis base. Why?

Ammonia has a formal lone pair of electrons on the nitrogen atom. This can donate to Lewis acids (including boron trichloride) in a Lewis base/Lewis acid interaction. On the other...

In Arrhenius, we are limited to cases in which water is the solvent (this is assumed by Arrhenius). An acid will dissolve in water to produce $H^+$ ions, while a...

And thus $"Lewis acids"$ include, $BX_3, OH_2, AlX_3, AlR_3, ""^(-):C-=O^+, ............$. And $"Lewis bases"$ are electron pair DONORS..........., and include, $HO^-, X^-, NR_3, ""^(-)CR_3, H^(-), PR_3, "ethers"$, and $"thioethers"$. This...

Know the definition Lewis acids- accept an electron pair Lewis base- donate an electron pair Now what you need to look for in the given compound, is whether...

.....and a $"Lewis acid"$ is an electron pair acceptor. Bronsted acids and bases fit this description. Hydroxide anion certainly tends to react as a nucleophile, and donate electron density.

The expansion from the Arrhenius acid-base theory to a more general understanding of proton transfer explained the acid/base behavior of many more compounds than the previous inorganic water-based systems....