Aluminium chloride

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Aluminium chloride
Names
IUPAC name
aluminium chloride
Other names
aluminium(III) chloride
aluminum trichloride
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.028.371
Gmelin Reference 1876
PubChem {{{value}}}
RTECS number BD0530000
UNII
SMILES {{{value}}}
Properties
AlCl3
Molar mass 133.341 g/mol (anhydrous)
241.432 g/mol (hexahydrate)[1]
Appearance white or pale yellow solid,
hygroscopic
Density 2.48 g/cm3 (anhydrous)
2.398 g/cm3 (hexahydrate)[1]
Melting point 192.6 °C (378.7 °F; 465.8 K)
(anhydrous)[1]
100 °C (212 °F; 373 K)
(hexahydrate, dec.)[1]
Boiling point 180 °C (356 °F; 453 K) (sublimes)[1]
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
Monoclinic, mS16
C12/m1, No. 12[3]
a = 0.591 nm, b = 0.591 nm, c = 1.752 nm[3]
0.52996 nm3
6
Octahedral (solid)
Tetrahedral (liquid)
Trigonal planar
(monomeric vapour)
Thermochemistry
Std enthalpy of
formation
ΔfHo298
−704.2 kJ/mol[4]
Standard molar
entropy
So298
109.3 J/mol·K[4]
Specific heat capacity, C 91.1 J/mol·K[4]
Pharmacology
D10AX01 (WHO)
Hazards
NFPA 704

NFPA 704.svg

0
3
2
 
U.S. Permissible
exposure limit (PEL)
none
Related compounds
Other anions Aluminium fluoride
Aluminium bromide
Aluminium iodide
Other cations Boron trichloride
Gallium trichloride
Indium(III) chloride
Magnesium chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references

Aluminium chloride (AlCl3), is a chemical compound. It is a white or yellow crystalline solid. It melts at a low temperature. It is made by reacting aluminium oxide with hydrochloric acid. The anhydrous (without water) form may be made by reacting aluminium and chlorine. It is used in the making of chemicals. It is also used in deodorants. It can cause slight irritation.

Related pages[change | change source]

Sources[change | change source]

  1. 1.0 1.1 1.2 1.3 1.4 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.45. ISBN 1439855110.
  2. 2.0 2.1 Aluminum chloride Archived 2014-05-05 at the Wayback Machine. Chemister.ru (2007-03-19). Retrieved on 2017-03-17.
  3. 3.0 3.1 Ketelaar, J.Α.A. (1935). "Die Kristallstruktur der Aluminiumhalogenide II". Zeitschrift für Kristallographie – Crystalline Materials 90. doi:10.1524/zkri.1935.90.1.237. 
  4. 4.0 4.1 4.2 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.5. ISBN 1439855110.