Thiocyanate

Thiocyanate
Names
IUPAC name
cyanosulfanide
Other names
sulfocyanate (sulphocyanate), thiocyanide
Identifiers
302-04-5 N
ChEBI CHEBI:18022 YesY
ChEMBL ChEMBL84336 N
ChemSpider 8961 YesY
4529
Jmol 3D model Interactive image
PubChem 9322
Properties
SCN-
Molar mass 58.0824
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Thiocyanate (also known as rhodanide) is the anion [SCN]−. It is the conjugate base of thiocyanic acid. Common derivatives include the colourless salts potassium thiocyanate and sodium thiocyanate. Organic compounds containing the functional group SCN are also called thiocyanates. Mercury(II) thiocyanate was formerly used in pyrotechnics.

Thiocyanate is analogous to the cyanate ion, [OCN]−, wherein oxygen is replaced by sulfur. [SCN]− is one of the pseudohalides, due to the similarity of its reactions to that of halide ions. Thiocyanate used to be known as rhodanide (from a Greek word for rose) because of the red colour of its complexes with iron. Thiocyanate is produced by the reaction of elemental sulfur or thiosulfate with cyanide:

8 CN− + S8 → 8 SCN−
CN− + S
2O2−
3 → SCN− + SO2−
3

The second reaction is catalyzed by the enzyme sulfotransferase known as rhodanase and may be relevant to detoxification of cyanide in the body.

Organic thiocyanates

Organic and transition metal derivatives of the thiocyanate ion can exist as "linkage isomers". In thiocyanates, the organic group (or metal ion) is attached to sulfur: R−S−C≡N has a S–C single bond and a C≡N triple bond.[1] In isothiocyanates, the substituent is attached to nitrogen: R−N=C=S has a S=C double bond and a C=N double bond:

Phenylthiocyanate and phenylisothiocyanate are linkage isomers and are bonded differently

Synthesis

Several synthesis routes exist, the most basic being the reaction between alkyl halides and alkali thiocyanate in aqueous media.[2] Organic thiocyanates are hydrolyzed to thiocarbamates in the Riemschneider thiocarbamate synthesis.

Biological chemistry of thiocyanate in medicine

Thiocyanate[3] is known to be an important part in the biosynthesis of hypothiocyanite by a lactoperoxidase.[4][5][6] Thus the complete absence of thiocyanate[7] or reduced thiocyanate[8] in the human body, (e.g., cystic fibrosis) is damaging to the human host defense system.[9][10]

Thiocyanate is a potent competitive inhibitor of the thyroid sodium-iodide symporter.[11] Iodine is an essential component of thyroxine. Since thiocyanates will decrease iodide transport into the thyroid follicular cell, they will decrease the amount of thyroxine produced by the thyroid gland. As such, foodstuffs containing thiocyanate are best avoided by hypothyroid patients.[12]

In the early 20th century, thiocyanate was used in the treatment of hypertension, but it is no longer used because of associated toxicity.[13] Sodium nitroprusside, a metabolite of which is thiocyanate, is however still used for the treatment of a hypertensive emergency. Rhodanese catalyzes the reaction of sodium nitroprusside with thiosulfate to form the metabolite thiocyanate.

Coordination chemistry

Resonance structures of the thiocyanate ion

Thiocyanate shares its negative charge approximately equally between sulfur and nitrogen. As a consequence, thiocyanate can act as a nucleophile at either sulfur or nitrogen — it is an ambidentate ligand. [SCN]− can also bridge two (M−SCN−M) or even three metals (>SCN− or −SCN<). Experimental evidence leads to the general conclusion that class A metals (hard acids) tend to form N-bonded thiocyanate complexes, whereas class B metals (soft acids) tend to form S-bonded thiocyanate complexes. Other factors, e.g. kinetics and solubility, are sometimes involved, and linkage isomerism can occur, for example [Co(NH3)5(NCS)]Cl2 and [Co(NH3)5(SCN)]Cl2.[14]

Structure of Pd(Me2N(CH2)3PPh2)(SCN)(NCS).[15]

Test for iron(III) and cobalt(II)

If [SCN]− is added to a solution containing iron(III) ions (Fe3+), a blood red solution is formed due to the formation of [Fe(NCS)(H2O)5]2+.

Similarly, Co2+ gives a blue complex with thiocyanate. Both the iron and cobalt complexes can be extracted into organic solvents like diethyl ether or amyl alcohol. This allows the determination of these ions even in strongly coloured solutions. The determination of Co(II) in the presence of Fe(III) is possible by adding KF (toxic!) to the solution, which forms uncoloured, very stable complexes with Fe(III), which no longer react with SCN−.

Phospholipids or some detergents aid the transfer of thiocyanatoiron into chlorinated solvents like chloroform and can be determined in this fashion.[16]

References

  1. ↑ Guy, R. G. (1977). "Syntheses and Preparative Applications of Thiocyanates". In Patai, S. Chemistry of Cyanates and Their Derivatives 2. New York: John Wiley.
  2. ↑ "Synthesis of thiocyanates".
  3. ↑ Pedemonte, N.; Caci, E.; Sondo, E.; Caputo, A.; Rhoden, K.; Pfeffer, U.; di Candia, M.; Bandettini, R.; Ravazzolo, R.; Zegarra-Moran, O.; Galietta, L. J. (2007). "Thiocyanate Transport in Resting and IL-4-Stimulated Human Bronchial Epithelial Cells: Role of Pendrin and Anion Channels" (pdf). Journal of Immunology 178 (8): 5144–5153. doi:10.4049/jimmunol.178.8.5144. PMID 17404297.
  4. ↑ Conner, G. E.; Wijkstrom-Frei, C.; Randell, S. H.; Fernandez, V. E.; Salathe, M. (2007). "The Lactoperoxidase System Links Anion Transport to Host Defense in Cystic Fibrosis" (pdf). FEBS Letters 581 (2): 271–278. doi:10.1016/j.febslet.2006.12.025. PMC 1851694. PMID 17204267.
  5. ↑ White, W. E.; Pruitt, K. M.; Mansson-Rahemtulla, B. (1983). "Peroxidase-Thiocyanate-Peroxide Antibacterial System Does not Damage DNA" (pdf). Antimicrobial Agents and Chemotherapy 23 (2): 267–272. doi:10.1128/aac.23.2.267. PMC 186035. PMID 6340603.
  6. ↑ Thomas, E. L.; Aune, T. M. (1978). "Lactoperoxidase, Peroxide, Thiocyanate Antimicrobial System: Correlation of Sulfhydryl Oxidation with Antimicrobial Action" (pdf). Infection and Immunity 20 (2): 456–463. PMC 421877. PMID 352945.
  7. ↑ Childers, M.; Eckel, G.; Himmel, A.; Caldwell, J. (2007). "A new Model of Cystic Fibrosis Pathology: Lack of Transport of Glutathione and its Thiocyanate Conjugates". Medical Hypotheses 68 (1): 101–112. doi:10.1016/j.mehy.2006.06.020. PMID 16934416.
  8. ↑ Minarowski, Ł.; Sands, D.; Minarowska, A.; Karwowska, A.; Sulewska, A.; Gacko, M.; Chyczewska, E. (2008). "Thiocyanate concentration in saliva of cystic fibrosis patients" (pdf). Folia Histochemica et Cytobiologica 46 (2): 245–246. doi:10.2478/v10042-008-0037-0. PMID 18519245.
  9. ↑ Moskwa, P.; Lorentzen, D.; Excoffon, K. J.; Zabner, J.; McCray, P. B. Jr.; Nauseef, W. M.; Dupuy, C.; Bánfi, B. (2007). "A Novel Host Defense System of Airways is Defective in Cystic Fibrosis" (pdf). American Journal of Respiratory and Critical Care Medicine 175 (2): 174–183. doi:10.1164/rccm.200607-1029OC. PMC 2720149. PMID 17082494.
  10. ↑ Xu, Y.; Szép, S.; Lu, Z.; Szep; Lu (2009). "The antioxidant role of thiocyanate in the pathogenesis of cystic fibrosis and other inflammation-related diseases" (pdf). Proceedings of the National Academy of Sciences of the United States of America 106 (48): 20515–20519. Bibcode:2009PNAS..10620515X. doi:10.1073/pnas.0911412106. PMC 2777967. PMID 19918082.
  11. ↑ Braverman L. E.; He X.; Pino S.; et al. (2005). "The effect of perchlorate, thiocyanate, and nitrate on thyroid function in workers exposed to perchlorate long-term". J Clin Endocrinol Metab. 90 (2): 700–706. doi:10.1210/jc.2004-1821. PMID 15572417.
  12. ↑ "Hypothyroidism". umm.edu. University of Maryland Medical Center. Retrieved 3 December 2014.
  13. ↑ Warren F. Gorman; Emanuel Messinger; And Morris Herman (1949). "Toxicity of Thiocyanates Used in Treatment of Hypertension". Ann Intern Med. 30 (5): 1054–1059. doi:10.7326/0003-4819-30-5-1054.
  14. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 326. ISBN 0-08-037941-9.
  15. ↑ Gus J. Palenik, George Raymond Clark "Crystal and Molecular Structure of Isothiocyanatothiocyanato-(1-diphenylphosphino-3-dimethylaminopropane)palladium(II)" Inorganic Chemistry, 1970, volume 9, pp 2754–2760. doi:10.1021/ic50094a028
  16. ↑ Stewart, J.C. (1980). "Colorimetric determination of phospholipids with ammonium ferrothiocyanate". Anal. Biochem. 104: 10–14. doi:10.1016/0003-2697(80)90269-9.
This article is issued from Wikipedia - version of the Friday, April 15, 2016. The text is available under the Creative Commons Attribution/Share Alike but additional terms may apply for the media files.