Xanthate usually refers to a salt with the formula ROCS2−M+ (R = alkyl; M+ = Na+, K+). The name xanthates is derived from Greek ξανθός [ksantʰós], meaning “yellowish, golden”, and indeed most xanthate salts are yellow. These organosulfur compounds are important in two areas, the production of cellophane and related polymers from cellulose and secondly in mining for the extraction of certain ores. They are also versatile intermediates in organic synthesis. Xanthates also refer to esters of xanthic acid. These esters have the structure ROC(=S)SR'.
Formation and structure
- ROH + CS2 + KOH → ROCS2K + H2O
The reaction involves the attack of the alkoxide salt. For example, sodium ethoxide gives sodium ethyl xanthate. Virtually any alcohol can be used in this reaction. Technical grade xanthate salts are usually of 90–95% purity. Impurities include alkali-metal sulfide, sulfate, trithiocarbonates, thiosulfate, sulfite, or carbonate as well as residual raw material such as alcohol and alkali hydroxide. These salts are available commercially as powder, granules, flakes, sticks, and solutions are available. China is a major exporter of granules.
Some commercially important xanthate salts include:
- sodium ethyl xanthate CH3CH2OCS2Na,
- potassium ethyl xanthate, CH3CH2OCS2K,
- sodium isopropyl xanthate
- sodium isobutyl xanthate
- potassium amyl xanthate
The OCS2 core of xanthate salts and esters is characteristically planar. The central carbon is sp2-hybridized.
Xanthate salts characteristically decompose in acid:
- ROCS2K + HCl → ROH + CS2 + KCl
This reaction is the reverse of the method for the preparation of the xanthate salts. The intermediate in the decomposition is the xanthic acid, ROC(S)SH, which can be isolated in certain cases.
- ROCS2K + R'X → ROC(S)SR' + KX
The C-O bond in these compounds are susceptible to cleavage by the Barton–McCombie deoxygenation, which provides a means for deoxygenation of alcohols.
They can be oxidized to the so-called dixanthogens:
- 2 ROCS2Na + Cl2 → ROC(S)S2C(S)OR + 2 NaCl
Cellulose reacts with carbon disulfide (CS2) in presence of sodium hydroxide (NaOH) to produces sodium cellulose xanthate, which upon neutralization with sulfuric acid (H2SO4) gives viscose rayon or cellophane paper (Sellotape or Scotch Tape).
Xanthate salts are used as flotation agents in mineral processing. They are intermediates in the Chugaev elimination process and are used to control radical polymerisation under the RAFT process, also termed MADIX (macromolecular design via interchange of xanthates).
Rarely encountered, thioxanthates arise by the reaction of CS2 with thiolate salts. For example, sodium ethylthioxanthate has the formula C2H5SCS2Na. Dithiocarbamates are also related compounds, and are more useful. They arise from the reaction of the amine with CS2. For example, sodium diethyldithiocarbamate has the formula (C2H5)2NCS2Na.
- IUPAC does not recommend the use of the term xanthate, although it is in current use in the scientific literature: "IUPAC definition".
- Kathrin-Maria Roy "Xanthates" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a28 423
- This report gives a detailed procedure for the potassium ethyl xanthate: Charles C. Price and Gardner W. Stacy (1948). "p-nitrophenyl sulfide". Org. Synth. 28: 82.; Coll. Vol. 3, p. 667
- Fabien Gagosz and Samir Z. Zard (1948). "A Xanthate-Transfer Approach to α-Trifluoromethylamines". Org. Synth. 84: 32.; Coll. Vol. 11, p. 212
- Galsbøl, F.; Schãffer, C. E. (1967). "Inorganic Syntheses". Inorganic Syntheses 10. p. 42. doi:10.1002/9780470132418.ch6. ISBN 9780470132418.
- Olav Foss “Xanthates and Dithiocarbamates of Selenium(II) and Tellurium(II)”, 1953 vol. 4,, Pages: 91–93. doi:10.1002/9780470132357.ch32
- Besser, J.; Brumbaugh, W.; Allert, A.; Poulton, B.; Schmitt, C.; Ingersoll, C. (2009). "Ecological impacts of lead mining on Ozark streams: toxicity of sediment and pore water". Ecotoxicology and environmental safety 72 (2): 516–526. doi:10.1016/j.ecoenv.2008.05.013. PMID 18603298.
- Xu, Y.; Lay, J. P.; Korte, F. (1988). "Fate and effects of xanthates in laboratory freshwater systems". Bulletin of Environmental Contamination and Toxicology 41 (5): 683–689. doi:10.1007/BF02021019. PMID 3233367.