Aluminium chloride
From Wikipedia, the free encyclopedia
| Aluminium chloride | |
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| IUPAC name | aluminium chloride |
| Other names | aluminium(III) chloride |
| Identifiers | |
| CAS number | , 10124-27-3 (hydrate), 7784-13-6 (hexahydrate) |
| PubChem | |
| ChEBI | CHEBI:30114 |
| RTECS number | BD0530000 |
| ATC code | D10 |
| SMILES | Cl[Al](Cl)Cl |
| Properties | |
| Molecular formula | AlCl3 |
| Molar mass | 133.34 g/mol (anhydrous) 241.43 g/mol (hexahydrate) |
| Appearance | white or pale yellow solid, hygroscopic |
| Density | 2.48 g/cm3 (anhydrous) 1.3 g/cm3 (hexahydrate) |
| Melting point |
192.4 °C *(anhydrous) |
| Boiling point |
120 °C (hexahydrate) |
| Solubility in water | 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 g/100 ml (100 °C) |
| Solubility | soluble in hydrogen chloride, ethanol, chloroform, carbon tetrachloride slightly soluble in benzene |
| Structure | |
| Crystal structure | Monoclinic, mS16 |
| Space group | C12/m1, No. 12 |
| Coordination geometry |
Octahedral (solid) Tetrahedral (liquid) |
| Molecular shape | Trigonal planar (monomeric vapour) |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
−704 kJ·mol−1[1] |
| Standard molar entropy S |
111 J·mol−1·K−1[1] |
| Hazards | |
| EU classification | Corrosive (C) |
| R-phrases | R34 |
| S-phrases | (S1/2), S7/8, S28, S45 |
| 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 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
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]
Sources [change]
- ↑ 1.0 1.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. ISBN 0-618-94690-X.
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