Как пишется формула хлорид алюминия

From Wikipedia, the free encyclopedia

Aluminium chloride

Aluminium trichloride hexahydrate, pure (top), and contaminated with iron(III) chloride (bottom)
Names
IUPAC name Aluminium chloride
Other names Aluminium(III) chloride Aluminium trichloride
Identifiers
CAS Number	7446-70-0 (anhydrous)  10124-27-3 (hydrate)  7784-13-6 (hexahydrate)
3D model (JSmol)	monomer: Interactive image dimer: Interactive image
ChEBI	CHEBI:30114
ChemSpider	22445
ECHA InfoCard	100.028.371
EC Number	231-208-1
Gmelin Reference	1876
PubChem CID	24012
RTECS number	BD0530000
UNII	LIF1N9568Y  3CYT62D3GA (hexahydrate)
CompTox Dashboard (EPA)	DTXSID6029674
InChI InChI=1S/Al.3ClH/h;3*1H/q+3;;;/p-3  Key: VSCWAEJMTAWNJL-UHFFFAOYSA-K  InChI=1/Al.3ClH/h;3*1H/q+3;;;/p-3 Key: VSCWAEJMTAWNJL-DFZHHIFOAR
SMILES monomer: Cl[Al](Cl)Cl dimer: Cl[Al-]1(Cl)[Cl+][Al-]([Cl+]1)(Cl)Cl
Properties
Chemical formula	AlCl3
Molar mass	133.341 g/mol (anhydrous) 241.432 g/mol (hexahydrate) [1]
Appearance	Colourless crystals, hygroscopic
Density	2.48 g/cm3 (anhydrous) 2.398 g/cm3 (hexahydrate) [1]
Melting point	180 °C (356 °F; 453 K) (anhydrous, sublimes)[1] 100 °C (212 °F; 373 K) (hexahydrate, decomposes)[1]
Solubility in water	439 g/L (0 °C) 449 g/L (10 °C) 458 g/L (20 °C) 466 g/L (30 °C) 473 g/L (40 °C) 481 g/L (60 °C) 486 g/L (80 °C) 490 g/L (100 °C)
Solubility	Soluble in hydrogen chloride, ethanol, chloroform, carbon tetrachloride Slightly soluble in benzene
Vapor pressure	133.3 Pa (99 °C) 13.3 kPa (151 °C) [2]
Viscosity	0.35 cP (197 °C) 0.26 cP (237 °C) [2]
Structure
Crystal structure	Monoclinic, mS16
Space group	C12/m1, No. 12[3]
Lattice constant	a = 0.591 nm, b = 0.591 nm, c = 1.752 nm[3]
Lattice volume (V)	0.52996 nm3
Formula units (Z)	6
Coordination geometry	Octahedral (solid) Tetrahedral (liquid)
Molecular shape	Trigonal planar (monomeric vapour)
Thermochemistry
Heat capacity (C)	91.1 J/(mol·K)[4]
Std molar entropy (S⦵298)	109.3 J/(mol·K)[4]
Std enthalpy of formation (ΔfH⦵298)	−704.2 kJ/mol[4]
Gibbs free energy (ΔfG⦵)	−628.8 kJ/mol[4]
Pharmacology
ATC code	D10AX01 (WHO)
Hazards
GHS labelling:[6]
Pictograms
Signal word	Danger
Hazard statements	H314
Precautionary statements	P260, P280, P301+P330+P331, P303+P361+P353, P305+P351+P338+P310, P310
NFPA 704 (fire diamond)	3 0 2
Lethal dose or concentration (LD, LC):
LD50 (median dose)	380 mg/kg, rat (oral, anhydrous) 3311 mg/kg, rat (oral, hexahydrate)
NIOSH (US health exposure limits):
PEL (Permissible)	None[5]
REL (Recommended)	2 mg/m3[5]
IDLH (Immediate danger)	N.D.[5]
Related compounds
Other anions	Aluminium fluoride Aluminium bromide Aluminium iodide
Other cations	Boron trichloride Gallium trichloride Indium(III) chloride Magnesium chloride
Related Lewis acids	Iron(III) chloride Boron trifluoride
Supplementary data page
Aluminium chloride (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).  verify (what is  ?) Infobox references

Aluminium chloride, also known as aluminium trichloride, is an inorganic compound with the formula AlCl₃. It forms hexahydrate with the formula [Al(H₂O)₆]Cl₃, containing six water molecules of hydration. Both are colourless crystals, but samples are often contaminated with iron(III) chloride, giving a yellow color.

The anhydrous material is important commercially. It has a low melting and boiling point. It is mainly produced and consumed in the production of aluminium metal, but large amounts are also used in other areas of the chemical industry.^[7] The compound is often cited as a Lewis acid. It is an example of an inorganic compound that reversibly changes from a polymer to a monomer at mild temperature.

Structure[edit]

Anhydrous[edit]

AlCl₃ adopts three structures, depending on the temperature and the state (solid, liquid, gas). Solid AlCl₃ has a sheet-like layered structure with cubic close-packed chloride ions. In this framework, the Al centres exhibit octahedral coordination geometry.^[8] Yttrium(III) chloride adopts the same structure, as do a range of other compounds. When aluminium trichloride is in its melted state, it 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). Al₂Cl₆ dimers are also found in the vapour phase. At higher temperatures, the Al₂Cl₆ dimers dissociate into trigonal planar AlCl₃ monomer, which is structurally analogous to BF₃. The melt conducts electricity poorly,^[9] unlike more ionic halides such as sodium chloride.

Aluminium chloride monomer belongs to the point group D_3h in its monomeric form and D_2h in its dimeric form.

Hexahydrate[edit]

The hexahydrate consists of octahedral [Al(H₂O)₆]³⁺ cation centers and chloride anions (Cl⁻) as counterions. Hydrogen bonds link the cation and anions.^[10]
The hydrated form of aluminium chloride has an octahedral molecular geometry, with the central aluminium ion surrounded by six water ligand molecules. Being coordinatively saturated, the hydrate is of little value as a catalyst in Friedel-Crafts alkylation and related reactions.

Uses[edit]

Alkylation and acylation of arenes[edit]

AlCl₃ is a common Lewis-acid catalyst for Friedel-Crafts reactions, both acylations and alkylations.^[11] 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.^[9] In the general Friedel-Crafts reaction, an acyl chloride or alkyl halide reacts with an aromatic system as shown:^[11]

The alkylation reaction is more widely used than the acylation reaction, although its practice is more technically demanding. 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.^[12] Detailed procedures are available for alkylation^[13] and acylation^[14][15] of arenes.

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.^[7]

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.^[16]

Other applications in organic and organometallic synthesis[edit]

Aluminium chloride finds a wide variety of other applications in organic chemistry.^[17] For example, it can catalyse the «ene reaction», such as the addition of 3-buten-2-one (methyl vinyl ketone) to carvone:^[18]

It is used to induce a variety of hydrocarbon couplings and rearrangements.^[19][20]

Aluminium 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. Dichlorophenylphosphine is prepared by reaction of benzene and phosphorus trichloride catalyzed by aluminium chloride.^[21]

Reactions[edit]

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.^[11] It forms tetrachloroaluminate ([AlCl₄]⁻) in the presence of chloride ions.

Aluminium chloride reacts with calcium and magnesium hydrides in tetrahydrofuran forming tetrahydroaluminates.

Reactions with water[edit]

Anhydrous aluminium chloride is hygroscopic, having a very pronounced affinity for water. It fumes in moist air and hisses when mixed with liquid water as the Cl⁻ ligands are displaced with H₂O molecules to form the hexahydrate [Al(H₂O)₆]Cl₃. The anhydrous phase cannot be regained on heating the hexahydrate. Instead HCl is lost leaving aluminium hydroxide or alumina (aluminium oxide):

[Al(H₂O)₆]Cl₃ → Al(OH)₃ + 3 HCl + 3 H₂O

Like metal aquo complexes, aqueous AlCl₃ is acidic owing to the ionization of the aquo ligands:

[Al(H₂O)₆]³⁺ ⇌ [Al(OH)(H₂O)₅]²⁺ + H⁺

Aqueous solutions behave similarly to other aluminium salts containing hydrated Al³⁺ ions, giving a gelatinous precipitate of aluminium hydroxide upon reaction with dilute sodium hydroxide:

AlCl₃ + 3 NaOH → Al(OH)₃ + 3 NaCl

Synthesis[edit]

Aluminium chloride is manufactured on a large scale by the exothermic reaction of aluminium metal with chlorine or hydrogen chloride at temperatures between 650 to 750 °C (1,202 to 1,382 °F).^[9]

2 Al + 3 Cl₂ → 2 AlCl₃

2 Al + 6 HCl → 2 AlCl₃ + 3 H₂

Aluminium chloride may be formed via a single displacement reaction between copper(II) chloride and aluminium metal.

2 Al + 3 CuCl₂ → 2 AlCl₃ + 3 Cu

In the US in 1993, approximately 21,000 tons were produced, not counting the amounts consumed in the production of aluminium.^[7]

Hydrated aluminium trichloride is prepared by dissolving aluminium oxides in hydrochloric acid. Metallic aluminium also readily dissolves in hydrochloric acid ─ releasing hydrogen gas and generating considerable heat. Heating this solid does not produce anhydrous aluminium trichloride, the hexahydrate decomposes to aluminium hydroxide when heated:

[Al(H₂O)₆]Cl₃ → Al(OH)₃ + 3 HCl + 3 H₂O

Aluminium also forms a lower chloride, aluminium(I) chloride (AlCl), but this is very unstable and only known in the vapour phase.^[9]

Natural occurrence[edit]

Anhydrous aluminium chloride is not found as a mineral. The hexahydrate, however, is known as the rare mineral chloraluminite.^[22] A more complex, basic and hydrated aluminium chloride mineral is cadwaladerite.^[23][22]

Safety[edit]

Anhydrous AlCl₃ reacts vigorously with bases, so suitable precautions are required.
It can cause irritation to the eyes, skin, and the respiratory system if inhaled or on contact.^[24]

See also[edit]

• Aluminium monochloride

References[edit]

External links[edit]

• International Chemical Safety Card 1125
• Index of Organic Synthesis procedures that utilize AlCl₃
• The period 3 chlorides
• MSDS Archived 2011-07-22 at the Wayback Machine
• Government of Canada Fact Sheets and Frequently Asked Questions: Aluminum Salts

From Wikipedia, the free encyclopedia

Aluminium chloride

Aluminium trichloride hexahydrate, pure (top), and contaminated with iron(III) chloride (bottom)
Names
IUPAC name Aluminium chloride
Other names Aluminium(III) chloride Aluminium trichloride
Identifiers
CAS Number	7446-70-0 (anhydrous)  10124-27-3 (hydrate)  7784-13-6 (hexahydrate)
3D model (JSmol)	monomer: Interactive image dimer: Interactive image
ChEBI	CHEBI:30114
ChemSpider	22445
ECHA InfoCard	100.028.371
EC Number	231-208-1
Gmelin Reference	1876
PubChem CID	24012
RTECS number	BD0530000
UNII	LIF1N9568Y  3CYT62D3GA (hexahydrate)
CompTox Dashboard (EPA)	DTXSID6029674
InChI InChI=1S/Al.3ClH/h;3*1H/q+3;;;/p-3  Key: VSCWAEJMTAWNJL-UHFFFAOYSA-K  InChI=1/Al.3ClH/h;3*1H/q+3;;;/p-3 Key: VSCWAEJMTAWNJL-DFZHHIFOAR
SMILES monomer: Cl[Al](Cl)Cl dimer: Cl[Al-]1(Cl)[Cl+][Al-]([Cl+]1)(Cl)Cl
Properties
Chemical formula	AlCl3
Molar mass	133.341 g/mol (anhydrous) 241.432 g/mol (hexahydrate) [1]
Appearance	Colourless crystals, hygroscopic
Density	2.48 g/cm3 (anhydrous) 2.398 g/cm3 (hexahydrate) [1]
Melting point	180 °C (356 °F; 453 K) (anhydrous, sublimes)[1] 100 °C (212 °F; 373 K) (hexahydrate, decomposes)[1]
Solubility in water	439 g/L (0 °C) 449 g/L (10 °C) 458 g/L (20 °C) 466 g/L (30 °C) 473 g/L (40 °C) 481 g/L (60 °C) 486 g/L (80 °C) 490 g/L (100 °C)
Solubility	Soluble in hydrogen chloride, ethanol, chloroform, carbon tetrachloride Slightly soluble in benzene
Vapor pressure	133.3 Pa (99 °C) 13.3 kPa (151 °C) [2]
Viscosity	0.35 cP (197 °C) 0.26 cP (237 °C) [2]
Structure
Crystal structure	Monoclinic, mS16
Space group	C12/m1, No. 12[3]
Lattice constant	a = 0.591 nm, b = 0.591 nm, c = 1.752 nm[3]
Lattice volume (V)	0.52996 nm3
Formula units (Z)	6
Coordination geometry	Octahedral (solid) Tetrahedral (liquid)
Molecular shape	Trigonal planar (monomeric vapour)
Thermochemistry
Heat capacity (C)	91.1 J/(mol·K)[4]
Std molar entropy (S⦵298)	109.3 J/(mol·K)[4]
Std enthalpy of formation (ΔfH⦵298)	−704.2 kJ/mol[4]
Gibbs free energy (ΔfG⦵)	−628.8 kJ/mol[4]
Pharmacology
ATC code	D10AX01 (WHO)
Hazards
GHS labelling:[6]
Pictograms
Signal word	Danger
Hazard statements	H314
Precautionary statements	P260, P280, P301+P330+P331, P303+P361+P353, P305+P351+P338+P310, P310
NFPA 704 (fire diamond)	3 0 2
Lethal dose or concentration (LD, LC):
LD50 (median dose)	380 mg/kg, rat (oral, anhydrous) 3311 mg/kg, rat (oral, hexahydrate)
NIOSH (US health exposure limits):
PEL (Permissible)	None[5]
REL (Recommended)	2 mg/m3[5]
IDLH (Immediate danger)	N.D.[5]
Related compounds
Other anions	Aluminium fluoride Aluminium bromide Aluminium iodide
Other cations	Boron trichloride Gallium trichloride Indium(III) chloride Magnesium chloride
Related Lewis acids	Iron(III) chloride Boron trifluoride
Supplementary data page
Aluminium chloride (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).  verify (what is  ?) Infobox references

Aluminium chloride, also known as aluminium trichloride, is an inorganic compound with the formula AlCl₃. It forms hexahydrate with the formula [Al(H₂O)₆]Cl₃, containing six water molecules of hydration. Both are colourless crystals, but samples are often contaminated with iron(III) chloride, giving a yellow color.

The anhydrous material is important commercially. It has a low melting and boiling point. It is mainly produced and consumed in the production of aluminium metal, but large amounts are also used in other areas of the chemical industry.^[7] The compound is often cited as a Lewis acid. It is an example of an inorganic compound that reversibly changes from a polymer to a monomer at mild temperature.

Structure[edit]

Anhydrous[edit]

AlCl₃ adopts three structures, depending on the temperature and the state (solid, liquid, gas). Solid AlCl₃ has a sheet-like layered structure with cubic close-packed chloride ions. In this framework, the Al centres exhibit octahedral coordination geometry.^[8] Yttrium(III) chloride adopts the same structure, as do a range of other compounds. When aluminium trichloride is in its melted state, it 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). Al₂Cl₆ dimers are also found in the vapour phase. At higher temperatures, the Al₂Cl₆ dimers dissociate into trigonal planar AlCl₃ monomer, which is structurally analogous to BF₃. The melt conducts electricity poorly,^[9] unlike more ionic halides such as sodium chloride.

Aluminium chloride monomer belongs to the point group D_3h in its monomeric form and D_2h in its dimeric form.

Hexahydrate[edit]

The hexahydrate consists of octahedral [Al(H₂O)₆]³⁺ cation centers and chloride anions (Cl⁻) as counterions. Hydrogen bonds link the cation and anions.^[10]
The hydrated form of aluminium chloride has an octahedral molecular geometry, with the central aluminium ion surrounded by six water ligand molecules. Being coordinatively saturated, the hydrate is of little value as a catalyst in Friedel-Crafts alkylation and related reactions.

Uses[edit]

Alkylation and acylation of arenes[edit]

AlCl₃ is a common Lewis-acid catalyst for Friedel-Crafts reactions, both acylations and alkylations.^[11] 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.^[9] In the general Friedel-Crafts reaction, an acyl chloride or alkyl halide reacts with an aromatic system as shown:^[11]

The alkylation reaction is more widely used than the acylation reaction, although its practice is more technically demanding. 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.^[12] Detailed procedures are available for alkylation^[13] and acylation^[14][15] of arenes.

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.^[7]

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.^[16]

Other applications in organic and organometallic synthesis[edit]

Aluminium chloride finds a wide variety of other applications in organic chemistry.^[17] For example, it can catalyse the «ene reaction», such as the addition of 3-buten-2-one (methyl vinyl ketone) to carvone:^[18]

It is used to induce a variety of hydrocarbon couplings and rearrangements.^[19][20]

Aluminium 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. Dichlorophenylphosphine is prepared by reaction of benzene and phosphorus trichloride catalyzed by aluminium chloride.^[21]

Reactions[edit]

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.^[11] It forms tetrachloroaluminate ([AlCl₄]⁻) in the presence of chloride ions.

Aluminium chloride reacts with calcium and magnesium hydrides in tetrahydrofuran forming tetrahydroaluminates.

Reactions with water[edit]

Anhydrous aluminium chloride is hygroscopic, having a very pronounced affinity for water. It fumes in moist air and hisses when mixed with liquid water as the Cl⁻ ligands are displaced with H₂O molecules to form the hexahydrate [Al(H₂O)₆]Cl₃. The anhydrous phase cannot be regained on heating the hexahydrate. Instead HCl is lost leaving aluminium hydroxide or alumina (aluminium oxide):

[Al(H₂O)₆]Cl₃ → Al(OH)₃ + 3 HCl + 3 H₂O

Like metal aquo complexes, aqueous AlCl₃ is acidic owing to the ionization of the aquo ligands:

[Al(H₂O)₆]³⁺ ⇌ [Al(OH)(H₂O)₅]²⁺ + H⁺

Aqueous solutions behave similarly to other aluminium salts containing hydrated Al³⁺ ions, giving a gelatinous precipitate of aluminium hydroxide upon reaction with dilute sodium hydroxide:

AlCl₃ + 3 NaOH → Al(OH)₃ + 3 NaCl

Synthesis[edit]

Aluminium chloride is manufactured on a large scale by the exothermic reaction of aluminium metal with chlorine or hydrogen chloride at temperatures between 650 to 750 °C (1,202 to 1,382 °F).^[9]

2 Al + 3 Cl₂ → 2 AlCl₃

2 Al + 6 HCl → 2 AlCl₃ + 3 H₂

Aluminium chloride may be formed via a single displacement reaction between copper(II) chloride and aluminium metal.

2 Al + 3 CuCl₂ → 2 AlCl₃ + 3 Cu

In the US in 1993, approximately 21,000 tons were produced, not counting the amounts consumed in the production of aluminium.^[7]

Hydrated aluminium trichloride is prepared by dissolving aluminium oxides in hydrochloric acid. Metallic aluminium also readily dissolves in hydrochloric acid ─ releasing hydrogen gas and generating considerable heat. Heating this solid does not produce anhydrous aluminium trichloride, the hexahydrate decomposes to aluminium hydroxide when heated:

[Al(H₂O)₆]Cl₃ → Al(OH)₃ + 3 HCl + 3 H₂O

Aluminium also forms a lower chloride, aluminium(I) chloride (AlCl), but this is very unstable and only known in the vapour phase.^[9]

Natural occurrence[edit]

Anhydrous aluminium chloride is not found as a mineral. The hexahydrate, however, is known as the rare mineral chloraluminite.^[22] A more complex, basic and hydrated aluminium chloride mineral is cadwaladerite.^[23][22]

Safety[edit]

Anhydrous AlCl₃ reacts vigorously with bases, so suitable precautions are required.
It can cause irritation to the eyes, skin, and the respiratory system if inhaled or on contact.^[24]

See also[edit]

• Aluminium monochloride

References[edit]

External links[edit]

• International Chemical Safety Card 1125
• Index of Organic Synthesis procedures that utilize AlCl₃
• The period 3 chlorides
• MSDS Archived 2011-07-22 at the Wayback Machine
• Government of Canada Fact Sheets and Frequently Asked Questions: Aluminum Salts

Aluminum Chloride is a combination of Aluminium and Chlorine elements. Aluminum is represented by Al. It is a lightweight silver metal that belongs to the boron family in the periodic table. Aluminum’s atomic number is 13. The density of it is lower than steel and had a greater affinity towards oxygen. So when aluminum is exposed to air, a thin protective layer of oxide is formed. On the other side Chlorine is a toxic, corrosive green-colored gas that causes irritation to the eyes and problems to the respiratory system. It is the second lightest member of the halogen family.

Aluminum Chloride is formed by an exothermic reaction between metallic aluminum and chlorine. Its chemical formula is AlCl₃. Aluminum Chloride is also called Aluminium trichloride. The physical form of aluminum chloride is silvery-white colored powder but due to the presence of contaminants (ferric chloride), it acquires yellow color. It is soluble in various solvents such as water, chloroform, ethanol, CCl₄, hydrogen chloride, and slightly soluble in benzene. It was corrosive and toxic.

Aluminum Chloride Preparation 

There are many ways of preparing AlCl₃. All those processes are listed below along with equations.

• Aluminum Chloride is mainly produced by the exothermic reaction between aluminum and chlorine.

2Al + 3Cl₂ —> 2AlCl₃ 

• Aluminum Chloride can be formed by reacting the aluminum metal with hydrogen chloride.

2Al + 6HCl → 2AlCl₃ +  H₂

• It was even prepared by conducting a single displacement reaction between copper chloride and aluminum metal.

2Al + 3CuCl₂ → 2AlCl₃ + 3Cu

Physical Properties  of Aluminium Chloride

• Aluminum Chloride is a poor conductor of electricity in a molten state.
• The actual color of Aluminium Chloride is white in color but due to the presence of contaminants of Iron trichloride, it turns into yellowish color.
• It has a very low melting point and boiling point.
• Aluminum Chloride is in a liquid state when the temperature is above 190^o C and pressure at above 2.5 atm.

Chemical Properties of Aluminium Chloride

• Aluminum Chloride is non-flammable, non-explosive.
• It is a corrosive solid.
• Aluminum chloride behaves violently when it reacts with water and bases.
• It is a lewis acid and an industrial catalyst.

Uses of Aluminium Chloride

• Used in pesticides & pharmaceuticals.
• Useful in manufacturing rubber, lubricants, paints, wood preservatives, and also petrochemicals like ethylbenzene.
• Aluminum Chloride is used in polymerization and isomerization reactions of light-weighted hydrocarbons like the production of ethylbenzene.
• Acts as a flux in melting aluminum.
• Aluminum Chloride is used as a catalyst for many chemical reactions. It is used in the preparation of anthraquinone from benzene and phosgene.
• It is used to attach aldehyde groups to aromatic series.
• Aluminum Chloride is mixed with aluminum, arene to synthesize arene metal complexes.

Sample Questions

Question 1: How does Aluminium Chloride react with water?

Answer:

Aluminium Chloride is hygroscopic which means it absorb moisture from air. Actually it fumes when in air containing moisture, creating a hissing sound when it comes contact with water. By this reaction Cl^– ions are replaced with H₂O and forms Hexahydrate i.e., Al(H₂O)₆Cl₃. When heat is applied, ammonium hydroxide is obtained as final product by dissipating HCl.

Al(H₂O)₆Cl₃  —> Al(OH)₃ + 3HCl + 3H₂O

Question 2: What are the melting and boiling points of Aluminium Chloride?

Answer:

The melting point of Aluminium Chloride is 192.6° C when it is anhydrous from. If it is a Hexahydrate then melting point is 100° C. The Boiling point of Aluminium Chloride is 180° C.

Question 3: Is Aluminium Chloride a Lewis Acid?

Answer:

Yes, Aluminium Chloride is a powerful Lewis acid. It forms Lewis Acid-base adducts even with bases that are weak in nature. 

Example 1: Aluminium Chloride forms tetrachloroaluminate (AlCl₄^–) when Chlorine ions are present.

Example 2: AlCl₃ react with magnesium and calcium hydride to form tetrahydridoaluminate.

Question 4: What is the molecular weight of Aluminium Chloride (AlCl₃)?

Solution:

Molecular weight can be calculated by finding the weight of each element.

Weight of Aluminium = 26.982

Weight of chlorine = 35.453

Here there are three chlorine atoms so the above weight can be multiplied with 3 to give weight of 3 chlorine atoms.

Weight of 3 chlorine atoms = 3 × 35.453 = 106.359

So molecular weight of Aluminium chloride (AlCl₃) = 26.982 + 106.359 = 133.341

Hence molecular weight of AlCl₃ is 133.341 gram/molecule.

Question 5: Aluminium Chloride is hazardous?

Answer:

• Aluminium Chloride can explode when it comes contact to water. So precautions need to be taken like wearing gloves, face guards etc. It should be stored in tightly sealed container to protect it from moisture.
• It corrode metals like stainless steel.
• Exposure to AlCl₃ for long period causes irritation to eyes and problem to respiratory organs.
• Aluminium Chloride is found to be neurotoxin and can destruct the nerve tissues. So from all these points, it can be concluded that AlCl₃ is hazardous if proper precautions are not taken.

Question 6: What is the structure of Aluminium Chloride?

Answer:

The structure of Aluminium Chloride varies based on the factors such as state of compound i.e., solid, liquid or gaseous state and also the temperature it is exposed. In solid state, The structure of AlCl₃ is Octahedral. In liquid/molten state, the structure is Tetrahedral. At higher temperature the structure is dissociates from tetrahedral to trigonal planar.

Aluminum Chloride is a combination of Aluminium and Chlorine elements. Aluminum is represented by Al. It is a lightweight silver metal that belongs to the boron family in the periodic table. Aluminum’s atomic number is 13. The density of it is lower than steel and had a greater affinity towards oxygen. So when aluminum is exposed to air, a thin protective layer of oxide is formed. On the other side Chlorine is a toxic, corrosive green-colored gas that causes irritation to the eyes and problems to the respiratory system. It is the second lightest member of the halogen family.

Aluminum Chloride is formed by an exothermic reaction between metallic aluminum and chlorine. Its chemical formula is AlCl₃. Aluminum Chloride is also called Aluminium trichloride. The physical form of aluminum chloride is silvery-white colored powder but due to the presence of contaminants (ferric chloride), it acquires yellow color. It is soluble in various solvents such as water, chloroform, ethanol, CCl₄, hydrogen chloride, and slightly soluble in benzene. It was corrosive and toxic.

Aluminum Chloride Preparation 

There are many ways of preparing AlCl₃. All those processes are listed below along with equations.

• Aluminum Chloride is mainly produced by the exothermic reaction between aluminum and chlorine.

2Al + 3Cl₂ —> 2AlCl₃ 

• Aluminum Chloride can be formed by reacting the aluminum metal with hydrogen chloride.

2Al + 6HCl → 2AlCl₃ +  H₂

• It was even prepared by conducting a single displacement reaction between copper chloride and aluminum metal.

2Al + 3CuCl₂ → 2AlCl₃ + 3Cu

Physical Properties  of Aluminium Chloride

• Aluminum Chloride is a poor conductor of electricity in a molten state.
• The actual color of Aluminium Chloride is white in color but due to the presence of contaminants of Iron trichloride, it turns into yellowish color.
• It has a very low melting point and boiling point.
• Aluminum Chloride is in a liquid state when the temperature is above 190^o C and pressure at above 2.5 atm.

Chemical Properties of Aluminium Chloride

• Aluminum Chloride is non-flammable, non-explosive.
• It is a corrosive solid.
• Aluminum chloride behaves violently when it reacts with water and bases.
• It is a lewis acid and an industrial catalyst.

Uses of Aluminium Chloride

• Used in pesticides & pharmaceuticals.
• Useful in manufacturing rubber, lubricants, paints, wood preservatives, and also petrochemicals like ethylbenzene.
• Aluminum Chloride is used in polymerization and isomerization reactions of light-weighted hydrocarbons like the production of ethylbenzene.
• Acts as a flux in melting aluminum.
• Aluminum Chloride is used as a catalyst for many chemical reactions. It is used in the preparation of anthraquinone from benzene and phosgene.
• It is used to attach aldehyde groups to aromatic series.
• Aluminum Chloride is mixed with aluminum, arene to synthesize arene metal complexes.

Sample Questions

Question 1: How does Aluminium Chloride react with water?

Answer:

Aluminium Chloride is hygroscopic which means it absorb moisture from air. Actually it fumes when in air containing moisture, creating a hissing sound when it comes contact with water. By this reaction Cl^– ions are replaced with H₂O and forms Hexahydrate i.e., Al(H₂O)₆Cl₃. When heat is applied, ammonium hydroxide is obtained as final product by dissipating HCl.

Al(H₂O)₆Cl₃  —> Al(OH)₃ + 3HCl + 3H₂O

Question 2: What are the melting and boiling points of Aluminium Chloride?

Answer:

The melting point of Aluminium Chloride is 192.6° C when it is anhydrous from. If it is a Hexahydrate then melting point is 100° C. The Boiling point of Aluminium Chloride is 180° C.

Question 3: Is Aluminium Chloride a Lewis Acid?

Answer:

Yes, Aluminium Chloride is a powerful Lewis acid. It forms Lewis Acid-base adducts even with bases that are weak in nature. 

Example 1: Aluminium Chloride forms tetrachloroaluminate (AlCl₄^–) when Chlorine ions are present.

Example 2: AlCl₃ react with magnesium and calcium hydride to form tetrahydridoaluminate.

Question 4: What is the molecular weight of Aluminium Chloride (AlCl₃)?

Solution:

Molecular weight can be calculated by finding the weight of each element.

Weight of Aluminium = 26.982

Weight of chlorine = 35.453

Here there are three chlorine atoms so the above weight can be multiplied with 3 to give weight of 3 chlorine atoms.

Weight of 3 chlorine atoms = 3 × 35.453 = 106.359

So molecular weight of Aluminium chloride (AlCl₃) = 26.982 + 106.359 = 133.341

Hence molecular weight of AlCl₃ is 133.341 gram/molecule.

Question 5: Aluminium Chloride is hazardous?

Answer:

• Aluminium Chloride can explode when it comes contact to water. So precautions need to be taken like wearing gloves, face guards etc. It should be stored in tightly sealed container to protect it from moisture.
• It corrode metals like stainless steel.
• Exposure to AlCl₃ for long period causes irritation to eyes and problem to respiratory organs.
• Aluminium Chloride is found to be neurotoxin and can destruct the nerve tissues. So from all these points, it can be concluded that AlCl₃ is hazardous if proper precautions are not taken.

Question 6: What is the structure of Aluminium Chloride?

Answer:

The structure of Aluminium Chloride varies based on the factors such as state of compound i.e., solid, liquid or gaseous state and also the temperature it is exposed. In solid state, The structure of AlCl₃ is Octahedral. In liquid/molten state, the structure is Tetrahedral. At higher temperature the structure is dissociates from tetrahedral to trigonal planar.

Хлорид алюминия
Общие
Систематическое наименование	трихлоралюмин, трихлоралюминий, алюминия трихлорид
Традиционные названия	хлористый алюминий
Химическая формула	AlCl3
Физические свойства
Состояние (ст. усл.)	белые или бледно-желтые гигроскопичные твердые тела
Молярная масса	(ангидрид) 133.34 г/моль (гексагидрат) 241.43 г/моль
Плотность	(ангидрид) 2.48 г/см³ (гексагидрат) 1.3 г/см³
Термические свойства
Температура плавления	(ангидрид) 192.4 °C
Температура кипения	(гексагидрат) 120 °C
Химические свойства
Растворимость в воде	(0 °C) 43.9 г/100 мл (10 °C) 44.9 г/100 мл (20 °C) 45.8 г/100 мл (30 °C) 46.6 г/100 мл (40 °C) 47.3 г/100 мл (60 °C) 48.1 г/100 мл (80 °C) 48.6 г/100 мл (100 °C) 49 г/100 мл
Растворимость в остальных веществах	растворим в хлороводороде, этиловом спирте, хлороформе; слабо растворим в бензоле г/100 мл
Структура
Координационная геометрия	октаэдрическая (линейные) четырехгранная (жидкость)
Кристаллическая структура	моноклинная
Классификация
Рег. номер CAS	7446-70-0, 10124-27-3 (гексагидрат)
SMILES	Cl[Al](Cl)Cl
RTECS	BD0530000
Безопасность
ЛД50	ангидрид; крысы, орально: 380 мг/кг гексагидрат; крысы, орально: 3311 мг/кг
Токсичность

Хлорид алюминия (хлористый алюминий) — соль алюминия и соляной кислоты. Химическая формула — AlCl₃.

Свойства

При обычном давлении возгоняется при 183 °C (под давлением плавится при 192,6 °C). В воде хорошо растворим (44,38 г в 100 г H₂O при 25 °C); вследствие гидролиза дымит во влажном воздухе, выделяя HCl. Из водных растворов выпадает кристаллогидрат AlCl₃· 6H₂O — желтовато-белые расплывающиеся кристаллы. Хорошо растворим во многих органических соединениях (в этаноле — 100 г в 100 г спирта при 25 °C, в ацетоне, дихлорэтане, диэтиленгликоле, нитробензоле, тетрахлоруглероде и др.); однако практически не растворяется в бензоле и толуоле.

Получение

Важнейший способ получения хлорида алюминия в промышленности — действие смеси Cl₂ и CO на обезвоженный каолин или боксит в шахтных печах:

Al₂O₃ + ЗСО + ЗСl₂ → 2AlCl₃ + 3CO₂

При температуре в 900 °C трихлорид бора и фосфид алюминия дают на выходе фосфид бора и хлорид алюминия:

Также есть и другие способы получения хлорида алюминия:

Al + FeCl₃ → AlCl₃ + Fe

Al(OH)₃ + 3HCl → AlCl₃ + 3H₂O

3CuCl₂ + 2Al → 2AlCl₃ + 3Cu↓

2Al + 6HCl → 2AlCl₃ + 3H₂↑

Применение

Безводный хлорид алюминия образует продукты присоединения со многими неорганическими (например, NH₃, H₂S, SO₂) и органическими (хлорангидриды кислот, эфиры и др.) веществами, с чем связано важнейшее техническое применение AlCl₃ как катализатора при переработке нефти и при органических синтезах (например, реакция Фриделя — Крафтса). Гексагидрат и его растворы используются при очистке сточных вод, обработке древесины, производстве антиперспирантов и пр.

Справочник содержит названия веществ и описания химических формул (в т.ч. структурные формулы и скелетные формулы).

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