Aluminium Chloride Structure

Aluminium chloride is a chemical compound of aluminium and chlorine. In a chemical formula, it is depicted as AICI3. In the liquid or molten form, it is a poor conductor of electricity. It is present in solid states in lattice layers, unlike ionic halides like sodium chloride.

The chlorides of aluminium are deliquescent. They can explode when mixed with water. Aluminium chlorides explode when coming in contact with water due to the high heat of hydration. Aluminium chloride is generally manufactured through exothermic reactions of chemical elements like aluminium and chlorine. It is manufactured in huge quantities for commercial uses. 

Chemical Structure of Aluminium Chloride

Studies depict that aluminium chloride is a potent form of Lewis acid, making it capable of forming stable acid-base adducts. Even if aluminium chloride is composed of a weak Lewis base like mesitylene, it can still form a stable Lewis base. 

The chloride ions help in the formation of AICI4. The contact with water results in the formation of different acid-base solutions. In fluids, like water, partial hydrolysis is formed through HCI gases or H3O+. 

The aqueous solutions in the water behave identically like aluminium salts, which contain hydrated AI3+ ions. Examples of aluminium chloride would include precipitation of gelation aluminium hydroxide that reacts only on equal quantities of sodium hydroxides. The chemical formula for aluminium chloride is given below: 

AICI3 (aq) + 3 Na OH (aq) → AI (OH)3 (s) + 3 NaCl (aq)

 The chemical properties for aluminium chlorides are mentioned below:

• The chlorides of aluminium are not explosive or flammable 
• It is solids of corrosive materials.
• The lewis acid in aluminium chlorides is used as a catalyst for industrial products. 

The physical properties for aluminium chlorides are mentioned below:

• Not a good electricity conductor if it is in a liquid state. 
• The colour of aluminium chloride is generally white as it contains a high amount of iron trichloride. However, it turns yellow.
• Aluminium chloride has low melting and boiling points.
• The chlorides of aluminium are in a molten state only at a temperature of 190 degrees Celsius. The pressure should be at 2.5 atm. 

Aluminium Chloride for Commercial Use

Aluminium chlorides are used in Friedel-Crafts reactions in dyestuff industries. In dyestuff industries, anthraquinone is prepared from the Friedel-Craft reaction. Friedel-Crafts react with acyl chlorides, which result in aromatic systems. With the use of benzene, the end product will contain para isomer. The alkyl halides react in the presence of anhydrous aluminium chloride to form homologues of benzene, for which the use of benzene for Friedel-Crafts reaction is comparatively low. As a result, acyl chloride reaction is mainly preferred for this. 

In acyl or alkyl reactions, aluminium chlorides must be dry with very little moisture, which acts as a catalyst for reactions. Issues might occur if aluminium chloride is not present in stoichiometric quantity as it will increase the complexity of the products. 

The complex reaction will lead to issues in recycling. It becomes essential to destroy the remaining residues as they generate substantial corrosive wastes. To reduce residues or corrosive wastes, chemists are researching environmentally benign catalysts: ytterbium, triflate, and recyclable products. 

Aluminium chlorides can be introduced within aldehyde groups onto aromatic rings. For instance, the use of the Gatterman Koch reaction in treating benzene with carbon monoxides and hydrogen chlorides in the presence of anhydrous aluminium chloride.

Preparation of aluminium chloride

Aluminium chloride is produced on a large scale by an exothermic reaction of chlorine or hydrogen chloride along with aluminium metal at temperatures ranging from 650°C to 750 °C (1,202°F to 1,382 °F). Aluminium chloride may be created by combining copper chloride with aluminium metal in a single displacement process.

Hence, aluminium chloride can be produced through:

• Exothermic reactions in aluminium and chlorine 
• Reactions of aluminium metal and chlorides of hydrogen

Uses of Aluminium Chlorides 

Aluminium chlorides are extensively used in:

• Manufacturing pesticides and other pharmaceutical products.
• Manufacturing rubber, lubricants, paints, and other products. 
• Lightweight hydrocarbon reactions that help in polymerisation and isomerisation.
• As a flux for melting minerals. 
• Because of its chemical properties, it acts as a catalyst for different reactions using synthetic materials. 
• Preparing anthraquinone. 
• Chlorides are mixed with compounds of aluminium to synthesise the metal complex.
•  Produce dodecylbenzene, which is a component of detergent. 

Conclusion 

Aluminium chloride is composed of both aluminium and chlorine components. Its chemical formula is AlCl3. It is generally formed through exothermic reactions in aluminium and chlorine. 

The presence of iron trichloride makes aluminium chloride appear white while it turns yellow when it comes in contact with oxides. It is not a good conductor of electricity when it is in a molten state. It is soluble in water, chloroform, ethanol, hydrogen chloride, etc.