Difference between revisions of "Aluminium chloride"

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(Created page with "'''Aluminium chloride''',''' '''or '''aluminium trichloride''', is a chemical compound of aluminium and chlorine, with the formula AlCl<sub>3</sub>. ==Properties== ===Chemica...")
 
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'''Aluminium chloride''',''' '''or '''aluminium trichloride''', is a chemical compound of aluminium and chlorine, with the formula AlCl<sub>3</sub>.
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| Name = Aluminium chloride
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| Reference =
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| IUPACName = Aluminium chloride
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| PIN =
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| SystematicName =
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| OtherNames = Aluminium(III) chloride<br>Aluminum trichloride
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| ImageFile = Aluminium chloride anhydrous in Schlenk tube.jpg
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| ImageCaption = Anhydrous AlCl<sub>3</sub> purified via sublimation under vacuum
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| Section1 = {{Chembox Identifiers
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| 3DMet =
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| Abbreviations =
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| Section2 = {{Chembox Properties
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| AtmosphericOHRateConstant =
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| Appearance = White hygroscopic solid
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| BoilingPt =
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| BoilingPtC = 180
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| BoilingPt_ref =
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| BoilingPt_notes =
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| Density = 2.48 g/cm<sup>3</sup> (anhydrous)<br> 2.398 g/cm<sup>3</sup> (hexahydrate)
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| Formula = AlCl<sub>3</sub>
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| HenryConstant =
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| LogP =
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| MolarMass = 133.341 g/mol (anhydrous)<br>241.432 g/mol (hexahydrate)
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| MeltingPt =
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| MeltingPtC = 192.6
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| MeltingPt_ref =
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| MeltingPt_notes = (anhydrous)
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| pKa =
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| pKb =
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| Solubility = 43.9 g/100 ml (0 °C)<br>44.9 g/100 ml (10 °C)<br>45.8 g/100 ml (20 °C)<br>46.6 g/100 ml (30 °C)<br>47.3 g/100 ml (40 °C)<br>48.1 g/100 ml (60 °C)<br>48.6 g/100 ml (80 °C)<br>49.0 g/100 ml (100 °C)
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| SolubleOther = Soluble in [[carbon tetrachloride]], [[chloroform]], [[diethyl ether]], [[1,4-Dioxane|dioxane]], [[ethanol]], [[hydrogen chloride]], [[methanol]], [[Tetrahydrofuran|THF]]<br>Slightly soluble in [[benzene]], [[toluene]], [[xylene]]
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| Solvent =
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| VaporPressure = 133.3 Pa (99 °C)<br> 13.3 kPa (151 °C)
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| Section3 = {{Chembox Structure
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| Coordination = Octahedral (solid)<br>Tetrahedral (liquid)
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| CrystalStruct = Monoclinic, mS16
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| MolShape = Trigonal planar<br>(monomeric vapor)
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| Section4 = {{Chembox Thermochemistry
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| DeltaGf = -628.8 kJ/mol
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| DeltaHc =
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| DeltaHf = −704.2 kJ/mol
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| Entropy = 109.3 J·mol<sup>-1</sup>·K<sup>-1</sup>
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| HeatCapacity = 91.1 J·mol<sup>-1</sup>·K<sup>-1</sup>
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| Section5 = {{Chembox Explosive
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| Section6 = {{Chembox Hazards
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| AutoignitionPt =
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| ExternalMSDS = [https://www.docdroid.net/DAPm5qr/aluminium-chloride-anhydrous-sa.pdf.html Sigma-Aldrich] (anhydrous)<br>[https://www.docdroid.net/TbxPHI3/aluminium-chloride-hexahydrate-sa.pdf.html Sigma-Aldrich] (hexahydrate)
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| FlashPt =
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| LD50 = ''anhydrous''<br>380 mg/kg (rat, oral)<br>''hexahydrate''<br>3,311 mg/kg (rat, oral)
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| MainHazards = Corrosive
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| OtherCompounds = [[Aluminium bromide]]<br>[[Aluminium iodide]]<br>[[Boron trichloride]]
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  }}
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}}
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'''Aluminium chloride''',''' '''or '''aluminium trichloride''', is a chemical compound of aluminium and chlorine, with the formula '''AlCl<sub>3</sub>'''.
  
 
==Properties==
 
==Properties==
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==Availability==
 
==Availability==
 
Aluminium chloride, both anhydrous and hydrated can be purchased from chemical suppliers.
 
Aluminium chloride, both anhydrous and hydrated can be purchased from chemical suppliers.
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 +
Hydrated aluminium chloride is available as aqueous solution in may pool stores.
  
 
==Preparation==
 
==Preparation==
Aluminium chloride can be prepared by reacting [[aluminium]] metal with [[chlorine]] or [[hydrogen chloride]] gas in a water-free medium, at temperatures between 650 to 750 °C:
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Anhydrous aluminium chloride can be prepared by reacting [[aluminium]] metal with [[chlorine]] or [[hydrogen chloride]] gas in a water-free medium, at temperatures between 650 to 750 °C:
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:2 Al + 3 Cl<sub>2</sub> → 2 AlCl<sub>3</sub>
 
:2 Al + 3 Cl<sub>2</sub> → 2 AlCl<sub>3</sub>
 
:2 Al + 6 HCl → 2 AlCl<sub>3</sub> + 3 H<sub>2</sub>
 
:2 Al + 6 HCl → 2 AlCl<sub>3</sub> + 3 H<sub>2</sub>
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The resulting AlCl<sub>3</sub> vapors are condensed outside the reactor and then collected and stored in anhydrous conditions.
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Aqueous AlCl<sub>3</sub> can be prepared by reacting hydrochloric acid with aluminium metal. This reaction is very exothermic and the resulting hydrogen may ignite or explode if the reaction is done improperly.
  
 
==Projects==
 
==Projects==
 
*Friedel–Crafts reactions
 
*Friedel–Crafts reactions
 
*Organoaluminium compounds
 
*Organoaluminium compounds
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*Make [[aluminium nitrate]]
  
 
==Handling==
 
==Handling==
 
===Safety===
 
===Safety===
 
Aluminium chloride is irritant to skin, eyes and respiratory system. It is a known neurotoxin.
 
Aluminium chloride is irritant to skin, eyes and respiratory system. It is a known neurotoxin.
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===Storage===
 
===Storage===
Anhydrous AlCl<sub>3</sub> must be stored in sealed containers, to prevent it from hydrolyzing.
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Anhydrous AlCl<sub>3</sub> must be stored in airtight sealed containers, to prevent it from hydrolyzing. [[Schlenk flask]]s are often used or long term storage, and ampouling may also be used for small amounts.
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Hydrated aluminium chloride doesn't require special storage.
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===Disposal===
 
===Disposal===
 
Aluminium chloride will hydrolyze into aluminium hydroxide and hydrochloric acid. The acid is easy to neutralize and dispose of, but aluminium hydroxide is harmful to environment. Since is insoluble in water, it can easily be separated, purified and recovered.
 
Aluminium chloride will hydrolyze into aluminium hydroxide and hydrochloric acid. The acid is easy to neutralize and dispose of, but aluminium hydroxide is harmful to environment. Since is insoluble in water, it can easily be separated, purified and recovered.
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===Relevant Sciencemadness threads===
 
===Relevant Sciencemadness threads===
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=14224 Anhydrous Aluminum Chloride prepration]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=14224 Anhydrous Aluminum Chloride prepration]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=19772 Anhydrous AlCl3 handling and storage]
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=152523 Anhydrous AlCl3]
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[[Category:Chemical compounds]]
 
[[Category:Chemical compounds]]
 
[[Category:Inorganic compounds]]
 
[[Category:Inorganic compounds]]

Latest revision as of 18:37, 7 February 2024

Aluminium chloride
Aluminium chloride anhydrous in Schlenk tube.jpg
Anhydrous AlCl3 purified via sublimation under vacuum
Names
IUPAC name
Aluminium chloride
Other names
Aluminium(III) chloride
Aluminum trichloride
Properties
AlCl3
Molar mass 133.341 g/mol (anhydrous)
241.432 g/mol (hexahydrate)
Appearance White hygroscopic solid
Density 2.48 g/cm3 (anhydrous)
2.398 g/cm3 (hexahydrate)
Melting point 192.6 °C (378.7 °F; 465.8 K) (anhydrous)
Boiling point 180 °C (356 °F; 453 K)
43.9 g/100 ml (0 °C)
44.9 g/100 ml (10 °C)
45.8 g/100 ml (20 °C)
46.6 g/100 ml (30 °C)
47.3 g/100 ml (40 °C)
48.1 g/100 ml (60 °C)
48.6 g/100 ml (80 °C)
49.0 g/100 ml (100 °C)
Solubility Soluble in carbon tetrachloride, chloroform, diethyl ether, dioxane, ethanol, hydrogen chloride, methanol, THF
Slightly soluble in benzene, toluene, xylene
Vapor pressure 133.3 Pa (99 °C)
13.3 kPa (151 °C)
Thermochemistry
109.3 J·mol-1·K-1
−704.2 kJ/mol
Hazards
Safety data sheet Sigma-Aldrich (anhydrous)
Sigma-Aldrich (hexahydrate)
Lethal dose or concentration (LD, LC):
anhydrous
380 mg/kg (rat, oral)
hexahydrate
3,311 mg/kg (rat, oral)
Related compounds
Related compounds
Aluminium bromide
Aluminium iodide
Boron trichloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Aluminium chloride, or aluminium trichloride, is a chemical compound of aluminium and chlorine, with the formula AlCl3.

Properties

Chemical

Aluminium chloride has a high affinity for water. Hydrated aluminium chloride cannot be turned back anhydrous via heating heating as HCl is lost leaving aluminium hydroxide or alumina (aluminium oxide):

Al(H2O)6Cl3 → Al(OH)3 + 3 HCl + 3 H2O

Physical

Aluminium chloride is a white hygroscopic salt. It melts at 192.4 °C (anhydrous form). The hydrated form, which is much less useful as a reagent, appears as grainy, oily beads which are often yellow due to even the smallest of iron impurities.

Availability

Aluminium chloride, both anhydrous and hydrated can be purchased from chemical suppliers.

Hydrated aluminium chloride is available as aqueous solution in may pool stores.

Preparation

Anhydrous aluminium chloride can be prepared by reacting aluminium metal with chlorine or hydrogen chloride gas in a water-free medium, at temperatures between 650 to 750 °C:

2 Al + 3 Cl2 → 2 AlCl3
2 Al + 6 HCl → 2 AlCl3 + 3 H2

The resulting AlCl3 vapors are condensed outside the reactor and then collected and stored in anhydrous conditions.

Aqueous AlCl3 can be prepared by reacting hydrochloric acid with aluminium metal. This reaction is very exothermic and the resulting hydrogen may ignite or explode if the reaction is done improperly.

Projects

Handling

Safety

Aluminium chloride is irritant to skin, eyes and respiratory system. It is a known neurotoxin.

Storage

Anhydrous AlCl3 must be stored in airtight sealed containers, to prevent it from hydrolyzing. Schlenk flasks are often used or long term storage, and ampouling may also be used for small amounts.

Hydrated aluminium chloride doesn't require special storage.

Disposal

Aluminium chloride will hydrolyze into aluminium hydroxide and hydrochloric acid. The acid is easy to neutralize and dispose of, but aluminium hydroxide is harmful to environment. Since is insoluble in water, it can easily be separated, purified and recovered.

References

Relevant Sciencemadness threads