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ALUMINIUM CHLORIDE

CAS NUMBER: 7446-70-0

EC NUMBER: 231-208-1


Aluminum chloride is a chemical compound with the chemical formula AlCl3. 
When contaminated with iron chloride, Aluminum chloride often displays a yellow color compared to the white pure compound. 

Aluminum chloride is used in various chemical applications as a Lewis base, with anhydrous aluminium trichloride being the most commonly used Lewis acid. 
Aluminum chloride may also be found in over-the-counter as an antiperspirant or prescription products as an antihemorrhagic agent. 

In antiperspirant products, FDA approves the use of aluminum chloride as an active ingredient up to 15%, calculated on the hexahydrate form, in an aqueous solution nonaerosol dosage form.
Aluminum chloride, solution appears as a straw-colored liquid. 

Denser than water. 
Contact may cause severe irritation to skin, eyes, and mucous membranes. 

May be toxic by ingestion.
Aluminum chloride, anhydrous appears as a white to gray powder with a pungent odor. 

Corrosive to tissue and toxic by ingestion.
Aluminium chloride (AlCl3), also known as aluminium trichloride, describe compounds with the formula AlCl3(H2O)n (n = 0 or 6). 

They consist of aluminium and chlorine atoms in a 1:3 ratio, and one form also contains six waters of hydration. 
Both are white solids, but samples are often contaminated with iron(III) chloride, giving a yellow color.

Aluminum chloride is important commercially. 
Aluminum chloride has a low melting and boiling point. 

Aluminum chloride is mainly produced and consumed in the production of aluminium metal, but large amounts are also used in other areas of the chemical industry.
The compound is often cited as a Lewis acid. 

Aluminum chloride is an example of an inorganic compound that reversibly changes from a polymer to a monomer at mild temperature.
Aluminum chloride is a chemical compound that is used primarily in making aluminum metal, but it has other uses, as well. 

The compound reacts strongly in the presence of water, so it’s important to take care when handling it.
Aluminium chloride (AlCl3) is a compound of aluminium and chlorine. 

The solid has a low melting and boiling point, and is covalently bonded. 
Aluminum chloride sublimes at 178 ° C. 

Aluminum chloride conducts electricity poorly, unlike more ionic halides such as sodium chloride. 
Aluminum chloride exists in the solid state as a six-coordinate layer lattice.

Aluminum chloride adopts the "YCl3" structure, featuring Al3+ cubic close packed layered structure. 
In contrast, AlBr3 has a more molecular structure, with the Al3+ centers occupying adjacent tetrahedral holes of the close-packed framework of Br− ions. 

Upon melting Aluminum chloride gives the dimer Al2Cl6, which can vaporise. 
At higher temperatures this Al2Cl6 dimer dissociates into trigonal planar AlCl3, which is structurally analogous to BF3.

Aluminium chloride is highly deliquescent, and it can explode in contact with water because of the high heat of hydration. 
Aluminum chloride partially hydrolyses with H2O, forming some hydrogen chloride and/or hydrochloric acid. 

Aqueous solutions of Aluminum chloride are fully ionized, and thus conduct electricity well. 
Such solutions are found to be acidic, indicating that partial hydrolysis of the Al3+ ion is occurring. 

Aluminum chloride is probably the most commonly used non-Bronsted Lewis acid and also one of the most powerful. 
Aluminum chloride finds widespread application in the chemical industry as a catalyst for Friedel-Crafts reactions, both acylations and alkylations. 

Aluminum chloride also finds use in polymerization and isomerization reactions of hydrocarbons. 
Aluminium chloride, like similar compounds such as Aluminium chlorohydrate, is also commonly used as an antiperspirant.

Aluminium also forms a lower chloride, aluminium(I) chloride (AlCl), but this is very unstable and only known in the vapour phase.
Aluminium chloride is an odorless inorganic solid, which is usually white to gray in color or sometimes yellow due to traces of iron chloride. 

Aluminum chloride is primarily used as a catalyst during Friedel Crafts reaction and as a Lewis Acid, making it a widely used compound in the chemical industry.
Aluminum chloride is an anhydrous white (when pure) salt compound formed by the reaction of aluminum and chlorine solutions. 

Aluminum chlorides chemical formula is AlCl3.
In cosmetics Aluminum chloride is used in its neutral form as an additive in deodorants and antiperspirants. 

Aluminum chloride is also used in therapies to treat auxiliary sweating.
Aluminum chloride is a major product of corrosion in the petrochemical industry.

Aluminum chloride is also known as trichloroalumane.
Although aluminum chloride is white in color in its pure state, it appears yellow when contaminated with other compounds, such as iron trichloride. 

Aluminum chlorides color may also change to yellow or gray when exposed to moisture.
Aluminum chloride salt is non-toxic; hence Aluminum chloride is used in many common preparations.

The corrosion rate of this salt under air-saturated solutions is high and it is unstable at high temperatures. 
The passivity of aluminum does not prevent the penetration of chloride molecules.

Aluminum chloride is produced in pitting corrosion or anodic corrosion when the aluminum ion is stabilized during the oxidation and reduction of the aluminum substrate.
Aluminium chloride is also sometimes referred to as aluminium trichloride or aluminium (III) chloride. 

The compound is formed when aluminium and chlorine are reacted together. 
Aluminum chlorides chemical formula is written as AlCl3. 

As for physical appearance, Aluminium chloride is usually white. 
However, due to the presence of contaminants (iron(III) chloride), it acquires a yellowish colour.

Industrially, aluminium chloride is used in the production of aluminium metal, but Aluminum chloride also has a wide number of uses in the chemical industry particularly as a Lewis acid. Solid aluminium chloride (AlCl3) is covalently bonded with low melting as well as boiling point.
Aluminum chloride is important industrial chemical. 

Aluminum chloride is used as the catalyst in variety of Friedel-Crafts type of reactions. 
Large amounts of ethylbenzene are prepared in this way and are used to make styrene.

Aluminum chloride is also used in the manufacture of anthraquinone (used in dyestuffs industry) and dodecylbenzene (used to make detergents) and in the isomerisation of hydrocarbons (petroleum industry).
Aluminum chloride reacts vigorously with water and fumes in air. 
Aluminum chloride is used as a catalyst in cracking petroleum and in organic synthesis.

 

 

USES OF ALUMINIUM CHLORIDE:


A use that may come closer to home for most people is that there’s a tiny bit of aluminum chloride in many antiperspirants. 
In fact, larger amounts of Aluminum chloride are in prescription antiperspirants. 

Aluminum chloride works in deodorant by combining with electrolytes in the skin to create a gel plug in the sweat glands. 
Aluminum chloride also has a slightly astringent effect on the pores, causing them to contract, which keeps the pores from releasing sweat. 

Because of this ability to contract pores, it’s also an ingredient in cosmetic astringents.
Aluminum chloride is a common Lewis-acid catalyst for Friedel–Crafts reactions, both acylations and alkylations.

Important products are detergents and ethylbenzene. 
These types of reactions are the major use for aluminium chloride, for example, in the preparation of anthraquinone (used in the dyestuffs industry) from benzene and phosgene.

For both reactions, the aluminium chloride, as well as other materials and the equipment, should be dry, although a trace of moisture is necessary for the reaction to proceed. 
A general problem with the Friedel–Crafts reaction is that the aluminium chloride catalyst sometimes is required in full stoichiometric quantities, because it complexes strongly with the products. 

This complication sometimes generates a large amount of corrosive waste. 
For these and similar reasons, the use of aluminium chloride has often been displaced by zeolites.

Aluminium chloride can also be used to introduce aldehyde groups onto aromatic rings, for example via the Gattermann-Koch reaction which uses carbon monoxide, hydrogen chloride and a copper(I) chloride co-catalyst.
The primary uses of aluminum chloride are in manufacturing and industry. 

First and foremost, Aluminum chloride’s a component in the production of aluminum, in metallurgy, and as an ingredient in aluminum smelting. 
Aluminum chloride’s also used in manufacturing petrochemicals like ethylbenzene and alkylbenzene. 

Certain kinds of pharmaceuticals require aluminum chloride as an ingredient. 
Aluminum chlorides many other applications include the production of paint, synthetic rubber, lubricants, wood preservatives, and some organic chemicals. 

Aluminum chloride is a versatile compound.
Aluminum chloride is a chemical compound with the chemical formula AlCl3. 

When contaminated with iron chloride, Aluminum chloride often displays a yellow color compared to the white pure compound. 
Aluminum chloride is used in various chemical applications as a Lewis base, with anhydrous aluminium trichloride being the most commonly used Lewis acid. 

Aluminum chloride may also be found in over-the-counter as an antiperspirant or prescription products as an antihemorrhagic agent. 
In antiperspirant products, FDA approves the use of aluminum chloride as an active ingredient up to 15%, calculated on the hexahydrate form, in an aqueous solution nonaerosol dosage form.

Aluminum chloride is also widely used for polymerization and isomerization reactions of hydrocarbons. 
Important examples include the manufacture of ethylbenzene, which used to make styrene and thus polystyrene, and also production of dodecylbenzene, which is used for making detergents.

Aluminum chloride combined with aluminium in the presence of an arene can be used to synthesize bis(arene) metal complexes, e.g. bis(benzene)chromium, from certain metal halides via the so-called Fischer-Hafner synthesis.
Aluminium Chloride is often regarded as a versatile chemical compound and therefore finds application in many areas, especially in chemical reactions and synthesis. 

Aluminum chloride is used mainly as a catalyst for different chemical reactions. 
Aluminum chloride is used extensively in Friedel-Crafts reaction including both acylations and alkylations. 

Aluminum chloride is used during the preparation of anthraquinone from phosgene and benzene.
Aluminium chloride can be used to bring in or attach aldehyde groups on aromatic series or rings. 

For instance, we can look at the Gatterman-Koch reaction, the Lewis acid (aluminium chloride) is used to remove a chloride ion from the species.
Aluminum chloride is also used in polymerization and isomerization reactions of light molecular weight hydrocarbons. 

Some common examples include the production of dodecylbenzene for detergents.
Aluminium chloride can be mixed with aluminium along with arene to synthesize bis(arene) metal complexes.

Aluminium chloride also has a variety of other applications, especially in organic chemistry. 
For example, Aluminum chloride is used to catalyse the “ene reaction”.We can take the case of the addition of (methyl vinyl ketone) 3-buten-2-one to carvone.

Aluminium chloride is used to induce a variety of hydrocarbon couplings and rearrangements.
Aluminum chloride has extensive commercial applications. 

Aluminum chloride is used primarily in the electrolytic production of aluminum. 
Another major use involves its catalytic applications in many organic reactions, including Friedel-Crafts alkylation, polymerization, isomerization, hydrocracking, oxidation, decarboxylation, and dehydrogenation. 

Aluminum chloride is also used in the production of rare earth chlorides, electroplating of aluminum and in many metal finishing and metallurgical operations.
Aluminum chloride was occasionally used in gold and platinum toning baths.

 

 

INDUSTRIAL USES OF ALUMINIUM CHLORIDE:


Aluminium chloride is used widely in manufacturing rubber, lubricants, wood preservatives, and paints.
Aluminum chloride is used in pesticides and pharmaceuticals.

As a flux in Aluminium melting.
Aluminum chloride is used as an antiperspirant.
Aluminum chloride’s also used in manufacturing petrochemicals like ethylbenzene and alkylbenzene.

 

 

APPLICATION OF ALUMINIUM CHLORIDE:


-Hydrocarbon Resins: 

Primary catalyst for Friedel-Crafts reactions (Alkylation and Acylation), also used in polymerization and isomerization of hydrocarbons (e.g. ethylbenzene which used in styrene)

-Inorganic Chemicals: 

Used as direct raw material for manufacturing Fumed Alumina and Titanium Dioxide

-Dyes & Pigments: 

Used as a catalyst in the production of pigments (primarily CPC green) and anthraquinone and its derivatives

-Pharmaceuticals: 

An intermediate in manufacturing of various pharmaceuticals including Ibuprofen (analgesic) which is used for treating pain, fever and inflammation

-Flavours & Fragrances: 

Aluminum chloride is used to produce hexamethyltetraline that has usage in soaps and cosmetics.

-Others: 

Used in components of dental cement, antacid, and food additives

 

 

PROPERTIES OF ALUMINIUM CHLORIDE:


-Density: 2.44 g/cm3 (20 °C) liquid

-Melting Point: 262 °C (sublimed)

-pH value: 2.4 (100 g/l, H₂O, 20 °C)

-Vapor pressure:    1 hPa (20 °C)

-Bulk density: 1200 kg/m3

-Solubility: 450 g/l (decomposition)

 

 

CHEMICAL PROPERTIES OF ALUMINIUM CHLORIDE:


Aluminum chloride is a white compound of aluminum and chloride. 
Aluminum chloride can often contaminate samples of this compound, which may give it a yellow color. 

Aluminum chlorides solid form has very low melting and boiling points. 
In Aluminum chlorides anhydrous (without water) form, aluminum chloride reacts strongly with both water and bases (they can bind with hydrogen), so it’s important to keep the compound away from substances that contain either of them. 

Even trace bits of moisture can cause a reaction with dry aluminum chloride. 
The chemical formula for aluminum chloride is AlCl₃.

Aluminium chloride is a powerful Lewis acid, capable of forming stable Lewis acid-base adducts with even weak Lewis bases such as benzophenone or mesitylene. 
Not surprisingly Aluminum chloride forms AlCl4− in the presence of chloride ion.

Aluminium chloride is a powerful Lewis acid.
Aluminum chloride is a major industrial catalyst.

Aluminum chloride is anhydrous, non-explosive, non-flammable but a corrosive solid.
Aluminum chloride reacts violently when Aluminum chloride comes in contact with water or bases.

Aluminum chloride is a noncombustible but highly reactive whitish-gray, yellow, or green powder or liquid. 
Strong, acidic, irritating odor like hydrochloric acid.

The vapor consists of double molecules Al2Cl6 . 
Soluble in water.

 

 

PHYSICAL PROPERTIES OF ALUMINIUM CHLORIDE:


Aluminium chloride has a very low melting and boiling point.
Aluminum chloride sublimes at a temperature of 180°C.

Aluminum chloride in a molten state is a poor conductor of electricity.
The colour of aluminium chloride is white, but often Aluminum chloride is contaminated with iron trichloride, which makes it yellow.
Aluminum chloride is in a liquid state only at pressures above 2.5 atm and temperature above 190°C.

 

 

MECHANISM OF ACTION OF ALUMINIUM CHLORIDE:


Aluminum chloride is commonly used topical antiperspirant. 
Aluminum chloride is proposed that aluminum chloride works by causing an obstruction of the distal sweat gland ducts, where the metal ions precipitate with mucopolysaccharides, damaging epithelial cells along the lumen of the duct and forming a plug that blocks sweat output. 

Aluminum chloride is also an astringent that promotes hemostasis; Aluminum chloride precipitates proteins on the superficial layer of mucosa and make it mechanically stronger. 
Aluminum chloride creates superficial and local coagulation in minor hemorrhages.

 

 

STRUCTURE OF ALUMINIUM CHLORIDE:


Aluminum chloride adopts three structures, depending on the temperature and the state (solid, liquid, gas). 
Aluminum chloride is a sheet-like layered cubic close packed layers. 

In this framework, the Aluminum chloride centres exhibit octahedral coordination geometry.
Aluminum chloride adopts the same structure, as do a range of other compounds. 

When Aluminum chloride is in its melted state, Aluminum chloride exists as the dimer Al2Cl6, with tetracoordinate aluminium. 
This change in structure is related to the lower density of the liquid phase (1.78 g/cm3) versus solid aluminium trichloride (2.48 g/cm3). 

Aluminum chloride dimers are also found in the vapour phase. 
At higher temperatures, the Al2Cl6 dimers dissociate into trigonal planar AlCl3, which is structurally analogous to BF3. 
The melt conducts electricity poorly, unlike more-ionic halides such as sodium chloride.

 

 

REACTION OF ALUMINIUM CHLORIDE:


Anhydrous aluminium chloride is a powerful Lewis acid, capable of forming Lewis acid-base adducts with even weak Lewis bases such as benzophenone and mesitylene.
Aluminum chloride forms tetrachloroaluminate (AlCl4−) in the presence of chloride ions.
Aluminium chloride reacts with calcium and magnesium hydrides in tetrahydrofuran forming tetrahydroaluminates.

 

ABSORPTION OF ALUMINIUM CHLORIDE:


Aluminum chloride is reported that about 17-30 % of aluminum chloride formed from the reaction between orally ingested aluminum hydroxide and hydrochloric acid of the stomach is absorbed. 
In rabbits, administration of a single maximum safe oral dose aluminum chloride (333 mg Al/kg) resulted in aluminum absorption of 0.57 %. 
Aluminum chloride may be absorbed via dermal route, with the uptake increasing in the microgram range but with an upper limit.

 

STORAGE OF ALUMINIUM CHLORIDE:

Separated from food and feedstuffs. 
Dry. 
Well closed. 
Store in an area without drain or sewer access. 

 

SYNONYM:

Aluminum trichloride
Aluminium trichloride
trichloroalumane
Aluminum chloride (AlCl3)
AlCl3
Trichloroaluminum
Aluminiumchlorid
Aluminum chloride anhydrous
Aluminum chloride (1:3)
Aluminum chloride, anhydrous
Chlorure d'aluminium
Alluminio(cloruro di)
Aluminium, (chlorure d')
Aluminum chloride, anhydrous, powder
MFCD00003422
NSC-143015

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