Physical Properties of AlCl3

Aluminium Chloride, also known as Aluminum Trichloride, is a pure compound. It is obtained from the exothermic reaction of aluminium and chlorine. The chemical formula for the pure compound is AlCl3. Aluminium is generally white, but the presence of iron and chloride turns the pure compound into yellow. It is highly optimised for organic reactions. Aluminium chloride is soluble in hydrogen chloride, chloroform, ethanol, and water. However, the compound is toxic at times and causes harm to the skin, eyes and respiratory system if you breathe or touch it. Now, let’s learn more about the concept, AlCl3 physical properties, chemical properties and uses.

Formation of Aluminum Chloride 

Apart from the exothermic process of aluminium and chlorine, there are different ways to form aluminium chloride. They are as follows:

• Forming a reaction between aluminium metal and hydrogen chloride.
• Forming a reaction between copper chloride and aluminium metal by single displacement method.

After obtaining Aluminium Chloride from the above reactions, the final equations will be:

• 2Al + 3Cl₂ → 2AlCl₃
• 2Al + 6HCl → 2AlCl₃ + H₂
• Al is aluminium chloride, Cu is copper chloride, and H₂
• is hydrogen.

Equation is –

2Al + 3CuCl₂→ 2AlCl₂+ 3Cu

AlCl₃ Physical Properties:

• Aluminium Chloride is a poor conductor of electricity when in a molten state.
• Generally, the melting and boiling points of AlCl₃ are low.
• Boiling and melting points exceed 180°C.
• Usually, aluminium chloride is white; however, when it reacts with iron trichloride, it turns yellow. Eventually, it is an essential AlC₃ physical property.
• The liquid state of aluminium chloride remains at a 2.5 pressure point and temperature of more than 190°C.

Chemical properties of aluminium chloride (AlCl₃)

• Aluminium Chloride is a primary industrial catalyst.
• The pure corrosive solid is completely non-explosive, anhydrous and non-flammable.
• It is a strong Lewis acid, i.e., it can form a Lewis base with weak bases.
• Aluminium Chloride (AlCl₃) reacts aggressively when in contact with water (H₂O).

Industrial applications of aluminium chloride

Aluminium Chloride is a pure compound and has wide applications in many industries.

• Aluminium chloride (AlCl₃) is widely used in pesticides and pharmaceuticals.
• The compound benefits lubricants, manufacturing rubber, paints and wood preservatives.
• Aluminium chloride (AlCl₃) is functional for antiperspirants.
• Industries use the chemical compound as a flux in melting Aluminium.

The reaction between aluminium chloride and water

Aluminium chloride (AlCl₃) is a perfect absorbent that can engross moisture present in the air. Generally, the compound exhales in the air with moisture; it creates a buzzing sound in contact with water. When water and aluminium chloride react together, it displaces the chloride ions by water molecules and obtains hexahydrate. The formula will be Al(H₂O)6Cl₃.

• The anhydrous form of aluminium chloride is lost with the application of heat. After that, the hydrogen chloride disappears and obtains aluminium hydroxide as the final product.

Al(H₂O)6Cl₃→Al(OH)₃+ 3HCl + 3H₂O

• Likewise, with an increase in temperature at 400°C, the hydroxide molecules obtain aluminium oxide in the reaction.

2Al(OH)₃→Al2O₃ + 3H₂O

• The aqueous solution of AlCl3 is often ionic and thus comes as a good conductor of electricity. Also, an acidic solution sometimes results in alkylation in Al3+ions. The reaction will be defined as:

Al(H₂O)6Cl₃ (aq) ⇌(Al(OH)(H₂O)₅²+(aq) + H+(aq)

• The aqueous aluminium chloride solution is parallel to that of Aluminium salts containing hydrated Al₃+ ions.
• One should take necessary precautions to maintain a distance between water and aluminium chloride compounds. Often, the contact of both these molecules can lead to explosions, owing to a large amount of heat in hydration. Although the compound exhausts in the air, safety tools like gloves faceguards must be available.
• A tightly sealed storage container of the chemical compound is compulsory to prevent it from moisture.
• When the chemical compound is exposed to air, the AlCl₃ holds the moisture from air to turn acidic and stick simultaneously. Often the reaction can corrode rubber and stainless steel at exposure.
• Continuous contact with aluminium chloride can harm your skin, respiratory tract and eyes. Also, it can be dangerous for nerve tissues leading to permanent damage at times.

Conclusion

The structure of aluminium chloride relies upon its state if it is liquid, solid or gaseous. Generally, the chemical compound is white coloured but often turns yellow in contact with iron as defined by AlCl3 physical properties. The chemical compound is a poor conductor of electricity in a molten state but a good conductor at aqueous solutions. Following its metal synthesising property, the chemical is widely used for industrial purposes. On the one hand, the chemical property makes the chemical compound non-explosive.

On the other hand, its reaction with hydrogen turns aluminium chloride explosive. Consequently, prolonged contact with the chemical compound can sometimes be harmful to the skin, eyes, respiratory tract, and nervous system. The results are so hazardous that they can lead to deaths. Laboratories take precautions while forming various reactions of aluminium chloride in their space.