Why do boron and aluminium halides behave as Lewis acids?

Question

Why do boron and aluminium halides behave as Lewis acids? (A) Both halides (MX3) can accept electrons from a donor to complete their octet (B) Both halides (MX3) can donate a pair of electrons (C) Both halides (MX3) are covalent polymeric structures (D) Both halides (MX3) react with water to give hydroxides and HCl

Tardigrade Admin · Accepted Answer

Both boron and aluminium in their trihalides (MX3) possess six electrons in their valence shell. To complete the octet they can accept a lone pair of electrons acting as Lewis acids.

Q. Why do boron and aluminium halides behave as Lewis acids?

Both halides $(M X_{3})$ can accept electrons from a donor to complete their octet

Both halides $(M X_{3})$ can donate a pair of electrons

Both halides $(M X_{3})$ are covalent polymeric structures

Both halides $(M X_{3})$ react with water to give hydroxides and $H Cl$

Both boron and aluminium in their trihalides $(M X_{3})$ possess six electrons in their valence shell. To complete the octet they can accept a lone pair of electrons acting as Lewis acids.

Q. Why do boron and aluminium halides behave as Lewis acids?

Both halides (MX3​) can accept electrons from a donor to complete their octet

Both halides (MX3​) can donate a pair of electrons

Both halides (MX3​) are covalent polymeric structures

Both halides (MX3​) react with water to give hydroxides and HCl

Both boron and aluminium in their trihalides (MX3​) possess six electrons in their valence shell. To complete the octet they can accept a lone pair of electrons acting as Lewis acids.

Both halides $(M X_{3})$ can accept electrons from a donor to complete their octet

Both halides $(M X_{3})$ can donate a pair of electrons

Both halides $(M X_{3})$ are covalent polymeric structures

Both halides $(M X_{3})$ react with water to give hydroxides and $H Cl$

Both boron and aluminium in their trihalides $(M X_{3})$ possess six electrons in their valence shell. To complete the octet they can accept a lone pair of electrons acting as Lewis acids.