Как пишется хлорид алюминия

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

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

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.

Хлорид алюминия
Общие
Систематическое наименование (b)	трихлоралюмин, трихлоралюминий, алюминия трихлорид
Традиционные названия	хлористый алюминий
Хим. формула (b)	AlCl₃
Физические свойства
Состояние (b)	белые или бледно-желтые гигроскопичные твердые кристаллы
Молярная масса (b)	(ангидрид) 133.34 г/моль (b) (гексагидрат) 241,43
Плотность (b)	(ангидрид) 2,48 г/см³ (гексагидрат) 1,3 г/см³
Термические свойства
Т. плав. (b)	(ангидрид) 192,4 ℃
Т. кип. (b)	(гексагидрат) 120 ℃
Химические свойства
Растворимость (b) 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 (b) в остальных веществах	растворим в хлороводороде (b) , этиловом спирте (b) , хлороформе (b) слабо растворим в бензоле (b)
Структура
Координационная геометрия (b)	октаэдрическая (линейные) четырехгранная (жидкость)
Кристаллическая структура (b)	моноклинная сингония (b)
Классификация
Номер CAS (b)	7446-70-0
PubChem (b)	24012
ChemSpider (b)	22445
Номер EINECS	231-208-1
RTECS (b)	BD0530000
ChEBI	30114
DrugBank (b)	DB11081
Номер ООН (b)	3264
SMILES (b)
[Al](Cl)(Cl)Cl
InChI (b)
InChI=1S/Al.3ClH/h;3*1H/q+3;;;/p-3
Безопасность
ЛД50 (b)	ангидрид крысы, перорально: 380 мг/кг гексагидрат крысы, орально: 3,311 г/кг
Токсичность (b)	0 3 2 COR
Приводятся данные для стандартных условий (25 ℃, 100 кПа), если не указано иное.

Хлори́д алюми́ния (хлористый алюминий) — неорганическое соединение (b) , соль (b) алюминия (b) и соляной кислоты (b) с химической формулой AlCl₃.

Свойства

В безводном виде бесцветные кристаллы, дымящие вследствие гидролиза (b) во влажном воздухе, выделяя HCl (b) ^[1]. 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). Из водных растворов выпадает виде кристаллогидрата (b)  — желтовато-белые расплывающиеся на воздухе кристаллы. Хорошо растворим во многих органических соединениях (в этаноле (b)  — 100 г в 100 г спирта при 25 °C, в ацетоне (b) , 1,2-дихлорэтане (b) , этиленгликоле (b) , нитробензоле (b) , тетрахлоруглероде (b) и др.); практически не растворяется в бензоле (b) и толуоле (b) .

Быстро гидролизуется в горячей воде:

Получение

Важнейший способ получения хлорида алюминия в промышленности — действие смеси Cl₂ (b) и CO (b) на обезвоженный каолин (b) или боксит (b) в шахтных печах^[1]:

При температуре в 900 °C трихлорид бора (b) и фосфид алюминия (b) образуют фосфид бора (b) и хлорид алюминия:

Также есть и другие способы получения хлорида алюминия:

Применение

Безводный хлорид алюминия образует аддукты (b) со многими неорганическими (например, NH₃ (b) , H₂S (b) , SO₂ (b) ) и органическими (хлорангидриды кислот, эфиры (b) и др.) веществами, с чем связано важнейшее техническое применение AlCl₃ как катализатора (b) при переработке нефти (b) и при органических синтезах (b) (например, реакция Фриделя — Крафтса (b) )^[1].

Хлорид алюминия и его растворы используются при очистке сточных вод, обработке древесины, производстве антиперспирантов (b) и пр.^[1]

Токсичность и безопасность

Хлорид алюминия токсичен при попадании в организм, а также обладает коррозионной активностью.

Примечания

1. 1 2 3 4 Данилов, 1988.

Литература

• Данилов В. П. Алюминия хлорид // Химическая энциклопедия (b)  : в 5 т. / Гл. ред. И. Л. Кнунянц (b) . — М.: Советская энциклопедия (b) , 1988. — Т. 1: А — Дарзана. — С. 122. — 623 с. — 100 000 экз. — ISBN 5-85270-008-8.

Соединения алюминия (b) *
Интерметаллиды	Алюминийнеодим (b) (NdAl) Алюминийдинеодим (b) (AlNd2) Алюминийтринеодим (b) (AlNd3) Алюминийникель (b) (NiAl) Алюминийдиниобий (b) (Nb2Al) Алюминийтриниобий (b) (Nb3Al) Алюминийпалладий (b) (AlPd) Алюминийдипалладий (b) (AlPd2)
Оксиды, гидроксиды	Гидроксид алюминия (b) (Al(OH)3) Метагидроксид алюминия (b) (AlO(OH)) Монооксид алюминия (b) (AlO) Оксид алюминия (b) (Al2O3) Оксинитрид алюминия (b) (AlON)
Соли	Арсенат алюминия (b) (AlAsO4) Ацетат алюминия (b) (Al(CH3COO)3) Молибдат алюминия (b) (Al2(MoO4)3) Нитрат алюминия (b) (Al(NO3)3) Силикат алюминия (b) (Al2O3·SiO2) Сульфат алюминия (b) (Al2(SO4)3) Сульфат алюминия-аммония (b) (NH4Al(SO4)2) Сульфат алюминия-калия (b) (KAl(SO4)2) Сульфат алюминия-натрия (b) (NaAl(SO4)2) Сульфат алюминия-рубидия (b) (RbAl(SO4)2) Сульфат алюминия-таллия (b) (TlAl(SO4)2) Сульфат алюминия-цезия (b) (CsAl(SO4)2) Фосфат алюминия (b) (AlPO4) Хлорат алюминия (b) (Al(ClO3)3)
Алюминаты	Алюминаты кальция (b) (mCaO·nAl2O3) Алюминат лития (b) (LiAlO2) Алюминат натрия (b) (NaAlO2) Гексафтороалюминат аммония (b) ((NH3)3[AlF6]) Гексафтороалюминат натрия (b) (Na3[AlF6]) Тетрагидридоалюминат натрия (b) (Na[AlH4]) Тетрагидридоалюминат калия (b) (K[AlH4]) Тетрагидридоалюминат цезия (b) (Cs[AlH4])
Галогениды	Бромид алюминия (b) (AlBr3) Иодид алюминия (b) (AlI3) Монофторид алюминия (b) (AlF) Монохлорид алюминия (b) (AlCl) Трифторид алюминия (b) (AlF3) Хлорид алюминия (b) (AlCl3)
Металлоорганические соединения	Триизобутилалюминий (b) (Al(C4H9)3) Триметилалюминий (b) (Al(CH3)3) Трифенилалюминий (b) (Al(C6H5)3) Триэтилалюминий (b) (Al(C2H5)3)
Соединения с неметаллами	Антимонид алюминия (b) (AlSb) Арсенид алюминия (b) (AlAs) Диборид алюминия (b) (AlB2) Додекаборид алюминия (b) (AlB12) Карбид алюминия (b) (Al4C3) Нитрид алюминия (b) (AlN) Селенид алюминия (b) (Al2Se3) Сульфид алюминия (b) (Al2S3) Фосфид алюминия (b) (AlP)
Гидриды	Алюмогидрид кальция (b) (Ca[AlH4]2) Алюмогидрид лития (b) (LiAlH4) Гидрид алюминия (b) (AlH3)
Другие	Алюмосиликаты (b)

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

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