Question

Is $ AlC{l_3} $ a lewis base?

Answer 1

Hint :Lewis acids and bases are electron-pair acceptors and electron-pair donors, respectively, according to the Lewis theory of acid-base reactions. Lewis acids are chemical compounds with empty orbitals that can accept electron pairs from Lewis bases. Lewis bases are atomic or molecular chemical species with a highly localised HOMO (Highest Occupied Molecular Orbital).

Complete Step By Step Answer:
Since the aluminium atom has an open valence shell, aluminium chloride ( $ AlC{l_3} $ ) is a Lewis acid. Lewis acid (e.g., $ B{F_3} $ , $ Al{F_3} $ ) is an atom, ion, or molecule with an incomplete electron octet (e.g., $ SiB{r_4} $ , $ Si{F_4} $ ). Lewis bases donate a pair of electrons. A Lewis base is an atom, ion, or molecule with a single electron pair.
Aluminium chloride is a chemical compound with the formula $ AlC{l_3} $ . In comparison to the white, pure compound, it takes on a yellow hue when contaminated with iron chloride. It's used as a Lewis base in a variety of chemical reactions, with anhydrous aluminium trichloride being the most common Lewis acid.
Depending on the temperature and state, $ AlC{l_3} $ takes on one of three structures (solid, liquid, gas). Solid $ AlC{l_3} $ is layered cubic close packed layers in a sheet-like structure. When melted, aluminium trichloride exists as the dimer $ A{l_2}C{l_6} $ , which contains tetracoordinate aluminium.

Note :
In the Friedel-Crafts alkylation process, Lewis acids play an important role as a catalyst in the Friedel-Crafts reaction – $ AlC{l_3} $ accepts a lone pair of electrons from the chloride ion, resulting in the formation of $ AlC{l_4} $ –. This also results in the formation of the highly electrophilic carbonium ion, which functions as a powerful Lewis acid. The following is an example of a chemical reaction.
 $ RCl + AlC{l_3} \to {R^ + } + AlC{l_4}^ - $ Lewis acids are commonly used in organic chemistry to promote cationic or pseudo-cationic chemical reactions.