Question

Distinguish Lewis acids and bases from Brønsted-Lowry acids and bases. Give an example of each.

Short answer

The differences between Bronsted-Lowry acid and bases and Lewis acids and bases are given below:

Bronsted –Lowry concept	Lewis concept
The Bronsted-Lowry acid dissociates in aqueous solution to give ions.	The Lewis acid can accept a pair of electrons.
The Bronsted-Lowry base dissociates in aqueous solution to give ions.	The Lewis acid can donate a pair of electron.

Step-by-step solution

Bronsted-Lowry acid and bases.

The Bronsted-Lowry acid is a chemical species which is capable of donating a proton in an aqueous solution.

An example of Bronsted-Lowry acid is HCI.

$\mathrm{HCI}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{CI}}^{+}+{\mathrm{H}}_3{\mathrm{O}}^{+}$

The Bronsted-Lowry base is a chemical species which can liberate OH ions in aqueous solution.

An example of Bronsted-Lowry base is NaOH.

$\mathrm{NaOH}\left(\mathrm{aq}\right)\to {\mathrm{Na}}^{+}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)$

Lewis Acid and Base.

The chemical species which is able to accept a pair of an electron called Lewis acid. Lewis acids have vacant orbitals where they can accept electron pairs.

An example of a Lewis acid is ${\mathrm{BF}}_3$.

The chemical species which can donate a pair of electrons is called a Lewis base.

An example of a Lewis base is ${\mathrm{NH}}_3$