Xanthate
A xanthate is a
Formation and structure
Xanthate salts of
- ROH + CS2 + KOH → ROCS2K + H2O
For example,
Some commercially or otherwise useful xanthate salts include:
- sodium ethyl xanthate CH3CH2OCS2Na
- potassium ethyl xanthate, CH3CH2OCS2K
- potassium isopropyl xanthate, (CH3)2CHOCS2K[4]
- sodium isobutyl xanthate, (CH3)2CHCH2OCS2Na
- potassium amyl xanthate, CH3(CH2)4OCS2K
The OCS2 core of xanthate salts, like that of the carbonates and the esters has trigonal planar molecular geometry. The central carbon atom is sp2-hybridized.
Reactions
Acid-base properties
Xanthatic acids, with the formula ROC(S)SH, can be prepared by treating alkali metal xanthates, e.g.
Xanthic acids characteristically decompose:
- 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.
Other reactions
Xanthate anions also undergo alkylation to give xanthate esters, which are generally stable:[7]
- 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 dixanthogen disulfides:
- 2 ROCS2Na + I2 → ROC(S)S2C(S)OR + 2 NaI
Acylation of xanthates gives alkyl xanthogen esters (ROC(S)SC(O)R') and related anhydrides.[2]
Xanthates bind to transition metal cations as bidentate ligands. The charge-neutral complexes are soluble in organic solvents.[8]
Xanthates are intermediates in the
Industrial applications
Cellulose reacts with
).Xanthate salts (e.g. sodium alkyl xanthates,
Related compounds
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. They arise from the reaction of a secondary amine with CS2. For example, sodium diethyldithiocarbamate has the formula (C2H5)2NCS2Na.
Environmental impacts
While biodegradable, this class of chemicals may be toxic to life in water at concentrations of less than 1 mg/L.[11] Water downstream of mining operations is often contaminated with xanthates.[12]
References
- ^ ISBN 978-3527306732.
- .
- .
- .
- ISBN 3135262014.
- ^ Gagosz, Fabien; Zard, Samir Z. (2007). "A Xanthate-Transfer Approach to α-Trifluoromethylamines". Organic Syntheses. 84: 32; Collected Volumes, vol. 11, p. 212.
- ^ Haiduc, I. (2004). "1,1-Dithiolato ligands". In McClevert, J. A.; Meyer, T. J. (eds.). Comprehensive Coordination Chemistry II. Vol. 1. pp. 349–376.
- ISBN 9780470132418.
- ISBN 3-342-00280-8.
- PMID 18603298.
- S2CID 2696850.