Difference between revisions of "Aluminium sulfide"
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| IUPACName = Aluminium sulfide | | IUPACName = Aluminium sulfide | ||
| PIN = | | PIN = | ||
| − | | SystematicName =Aluminium sulfide | + | | SystematicName = Aluminium sulfide |
| OtherNames = Aluminium sulphide | | OtherNames = Aluminium sulphide | ||
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| MeltingPt_ref = | | MeltingPt_ref = | ||
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| + | | Odor = Rotten-eggs | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| Solubility = Hydrolyses to release H<sub>2</sub>S | | Solubility = Hydrolyses to release H<sub>2</sub>S | ||
| − | | SolubleOther = Insoluble in organic solvents | + | | SolubleOther = Reacts with acids<br>Insoluble in organic solvents |
| Solvent = | | Solvent = | ||
| VaporPressure = | | VaporPressure = | ||
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===Disposal=== | ===Disposal=== | ||
| − | Aluminium sulfide can be neutralized with [[hydrogen peroxide]] or bleach. | + | Aluminium sulfide can be neutralized with [[hydrogen peroxide]] or bleach. This oxidizes the aluminium sulfide to aluminium sulfate. |
==References== | ==References== | ||
Latest revision as of 19:18, 19 July 2017
| Names | |
|---|---|
| IUPAC name
Aluminium sulfide
| |
| Systematic IUPAC name
Aluminium sulfide | |
| Other names
Aluminium sulphide
| |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| Al2S3 | |
| Molar mass | 150.158 g/mol |
| Appearance | Gray solid |
| Odor | Rotten-eggs |
| Density | 2.02 g/cm3 |
| Melting point | 1,100 °C (2,010 °F; 1,370 K) |
| Boiling point | 1,500 °C (2,730 °F; 1,770 K) |
| Hydrolyses to release H2S | |
| Solubility | Reacts with acids Insoluble in organic solvents |
| Thermochemistry | |
| Std molar
entropy (S |
116.9 J/mol K |
| Std enthalpy of
formation (ΔfH |
-724 kJ/mol |
| Hazards | |
| Safety data sheet | LTS Research Laboratories, Inc. |
| Related compounds | |
| Related compounds
|
Aluminium sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Aluminium sulfide or aluminium sulphide is a gray chemical compound, that readily hydrolyzes in air to release hydrogen sulfide gas. It has the chemical formula Al2S3.
Contents
Properties
Chemical
Aluminium sulfide reacts with water to release hydrogen sulfide:
- Al2S3 + 6 H2O → 2 Al(OH)3 + 3 H2S
This reaction is a cheap and accessible way to obtain hydrogen sulfide.
Aluminium sulfide will react with alcohols at high temperature to give their respective thiols. such as: With methanol, it forms methanethiol and dimethyl sulfide, the yield being 40-45 % and 15% for each product, at 300 °C; reaction with ethanol gives ethanethiol at temperatures between 310-360 °C, with a 39% yield. At 310 °C it reacts with propanol to give propanethiol, with a 32.5 % yield. Reaction with ethers gives thioethers.[1]
Aluminium sulfide will not react with aromatic hydrocarbons. It also tends to decompose slightly under vacuum.
Physical
Aluminium sulfide is a greyish solid, with a bad sulfide smell, especially in moist air. It reacts with water to release hydrogen sulfide, and is insoluble in most solvents. It melts at 1100 °C and sublimes at 1,500 °C. Aluminium sulfide has at least six crystalline forms, the more important ones being α, β, γ and δ.
Availability
Aluminium sulfide is sold by various chemical suppliers.
Preparation
Aluminium sulfide can be prepared through a thermite-like reaction between aluminium and sulfur powders.
- 2 Al + 3 S → Al2S3
The mixture is somewhat difficult to ignite and burns much slower than the classical thermite. The resulting sulfide results in a fused form and is very hard, requiring grinding. If it reaches temperatures greater than 1100 °C, it may melt its way through steel.
Another route involves the reaction of potassium thiocyanate with aluminium powder at temperatures over 600°C, in a 1:1 wight ratio. If the KSCN is present in excess, it will lower the yield.[2]
- 4 Al + 5 KSCN = 2 AlN + Al2S3 + 2 K2S + KCN + 4 C + N2
Burning aluminium powder in carbon disulfide also produces aluminium sulfide. However the yield is not very good.[3][4]
Projects
- Make hydrogen sulfide
- Make ethanethiol (ethyl mercaptane)
- Make aluminium metal, by reacting aluminium sulfide with alumina at high temperatures[5][6]
Handling
Safety
Aluminium sulfide releases hydrogen sulfide vapors in moist air, which has an extremely unpleasant smell and is very toxic. Given that the latter is detectable in minute quantities, sealing the container is mandatory, otherwise you will stink your lab.
Storage
Aluminium sulfide must be stored in air tight sealed containers or ampoules, as it will hydrolyze in the presence of moisture to release hydrogen sulfide, an extremely toxic and unpleasant gas.
Disposal
Aluminium sulfide can be neutralized with hydrogen peroxide or bleach. This oxidizes the aluminium sulfide to aluminium sulfate.
References
- ↑ Levi, G. R.; Natta, G.; Atti della Accademia Nazionale dei Lincei, Classe di Scienze Fisiche, Matematiche e Naturali, Rendiconti; vol. 33; (1924); p. 350
- ↑ "Z. Anorg. Chem.; vol. 156; (1926); p. 228".
- ↑ Cavazzi, A.; Mem. Accad. Bologna (4); vol. 7; (1887); p. 27 - 27; C.; (1887); p. 888
- ↑ Matignon, C.; Comptes Rendus Hebdomadaires des Seances de l'Academie des Sciences; vol. 130; (1900); p. 1392
- ↑ DE407927
- ↑ CA251381
Relevant Sciencemadness threads
- Chemical pages without CAS Registry Number
- Articles without EBI source
- Chemical pages without ChemSpiderID
- Chemical pages without DrugBank identifier
- Articles without KEGG source
- Articles without InChI source
- Articles without UNII source
- Articles containing unverified chemical infoboxes
- Chembox articles without image
- Chemical compounds
- Inorganic compounds
- Aluminium compounds
- Sulfur compounds
- Sulfides
- Materials unstable in basic solution
- Materials unstable in acidic solution
- Materials that react with water
- Foul smelling compounds
- Easily prepared chemicals
