Sodium thiocyanate (sometimes called sodium sulphocyanide) is the chemical compound with the formula NaSCN. This colorless deliquescent salt is one of the main sources of the thiocyanate anion. As such, it is used as a precursor for the synthesis of pharmaceuticals and other specialty chemicals.[2] Thiocyanate salts are typically prepared by the reaction of cyanide with elemental sulfur:
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| Names | |||
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| IUPAC name
Sodium thiocyanate
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| Other names
Sodium rhodanide
Sodium sulfocyanate Sodium rhodanate Thiocyanic acid, sodium salt | |||
| Identifiers | |||
3D model (JSmol)
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| 3863965 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| ECHA InfoCard | 100.007.960 | ||
| EC Number |
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| 1249825 | |||
PubChem CID
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| RTECS number |
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| UNII | |||
CompTox Dashboard (EPA)
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| Properties | |||
| NaSCN | |||
| Molar mass | 81.072 g/mol | ||
| Appearance | deliquescent colorless crystals | ||
| Density | 1.735 g/cm3 | ||
| Melting point | 287 °C (549 °F; 560 K) | ||
| Boiling point | 307 °C (585 °F; 580 K) decomposes | ||
| 139 g/100 mL (21 °C) 225 g/100 mL (100 °C) | |||
| Solubility | soluble in acetone, alcohols, ammonia, SO2 | ||
| Acidity (pKa) | −1.28 | ||
Refractive index (nD)
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1.545 | ||
| Structure | |||
| orthorhombic | |||
| Hazards | |||
| GHS labelling: | |||
 
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| Danger | |||
| H302, H312, H332, H412 | |||
| P261, P264, P270, P271, P273, P280, P301 P312, P302 P352, P304 P312, P304 P340, P305 P351 P338, P310, P312, P322, P330, P337 P313, P363, P501 | |||
| NFPA 704 (fire diamond) | |||
| Lethal dose or concentration (LD, LC): | |||
LD50 (median dose)
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764 mg/kg (oral, rat)[1] | ||
| Safety data sheet (SDS) | ICSC 0675 | ||
| Related compounds | |||
Other anions
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Sodium cyanate Sodium cyanide | ||
Other cations
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Lithium thiocyanate Potassium thiocyanate Ammonium thiocyanate | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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- 8 NaCN S8 → 8 NaSCN
Sodium thiocyanate crystallizes in an orthorhombic cell. Each Na center is surrounded by three sulfur and three nitrogen ligands provided by the triatomic thiocyanate anion.[3] It is commonly used in the laboratory as a test for the presence of Fe3 ions.
Applications in chemical synthesis
editSodium thiocyanate is employed to convert alkyl halides into the corresponding alkylthiocyanates. Closely related reagents include ammonium thiocyanate and potassium thiocyanate, which has twice the solubility in water. Silver thiocyanate may be used as well; the precipitation of insoluble silver halides help simplify workup. Treatment of isopropyl bromide with sodium thiocyanate in a hot ethanolic solution affords isopropyl thiocyanate.[4] Protonation of sodium thiocyanate affords isothiocyanic acid, S=C=NH (pKa = −1.28).[5] This species is generated in situ from sodium thiocyanate; it adds to organic amines to afford derivatives of thiourea.[6]
References
edit- ^ Sodium thiocyanate, chemicalland21.com
- ^ Schwan, A. L. (2001). Encyclopedia of Reagents for Organic Synthesis. New York: John Wiley & Sons. doi:10.1002/047084289X.rs109.
- ^ van Rooyen, P. H.; Boeyens, J. C. A. (1975). "Sodium thiocyanate". Acta Crystallographica. B31 (12): 2933–2934. Bibcode:1975AcCrB..31.2933V. doi:10.1107/S0567740875009326.
- ^ R. L. Shriner (1931). "Isopropyl Thiocyanate". Organic Syntheses. 11: 92. doi:10.15227/orgsyn.011.0092.
- ^ Chiang, Y.; Kresge, A. J. (2000). "Determination of the Acidity Constant of Isothiocyanic Acid in Aqueous Solution". Canadian Journal of Chemistry. 78 (12): 1627–1628. doi:10.1139/cjc-78-12-1627.
- ^ Allen, C. F. H.; VanAllan, J. (1955). "2-Amino-6-Methylbenzothiazole". Organic Syntheses
{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 3, p. 76.