Aluminum Chloride and Chloride Ion (Lewis Acid-Base)

AlCl3 + Cl− → AlCl4−

Overview

Aluminum chloride acts as a Lewis acid, accepting a lone pair from chloride ion to form the tetrachloroaluminate anion. AlCl₃ has an electron-deficient aluminum center that readily accepts electron pairs. This Lewis acidity makes AlCl₃ one of the most important catalysts in organic chemistry.

Participants

Role Substance Coefficient State
Reactant Aluminum Al 1 (s)
Reactant Chlorine Cl 1 (aq)

Everyday Example

Friedel-Crafts reactions used to produce polystyrene and other important materials rely on AlCl₃ acting as a Lewis acid catalyst.

Industrial Importance

Aluminum chloride is used as a catalyst in Friedel-Crafts alkylation and acylation, petroleum cracking, and in the production of detergent alkylates.

Properties

Type
Acid-Base
Reversible
Yes
Energy
Exothermic
ΔH
-55.0 kJ/mol

Related Reactions

Acetic Acid and Sodium Acetate Buffer System Acetic Acid and Sodium Hydroxide Neutralization Acetic Acid Dissociation in Water Aluminum Hydroxide as Amphoteric Acid with NaOH Aluminum Hydroxide as Amphoteric Base with HCl Ammonia and Ammonium Chloride Buffer System Ammonia and Hydrochloric Acid Ascorbic Acid and Sodium Hydroxide Barium Hydroxide and Ammonium Thiocyanate (Endothermic) Benzoic Acid and Sodium Hydroxide

Frequently Asked Questions

What is the equation for Aluminum Chloride and Chloride Ion (Lewis Acid-Base)?
The balanced equation is: AlCl₃ + Cl⁻ → AlCl₄⁻.
What type of reaction is Aluminum Chloride and Chloride Ion (Lewis Acid-Base)?
Aluminum Chloride and Chloride Ion (Lewis Acid-Base) is a acid-base reaction. It is reversible under certain conditions.
Is Aluminum Chloride and Chloride Ion (Lewis Acid-Base) exothermic or endothermic?
Aluminum Chloride and Chloride Ion (Lewis Acid-Base) is exothermic (releases energy). The enthalpy change (ΔH) is -55.0 kJ/mol.