A xanthate is a salt or ester of a xanthic acid. The formula of the salt of xanthic acid is [R−O−CS₂]⁻M⁺ (where R is organyl group and M is usually Na or K).^[1] Xanthate also refers to the anion [R−O−CS₂]⁻. The formula of a xanthic acid is R−O−C(=S)−S−H, such as ethyl xanthic acid, while the formula of a xanthate ester is R−O−C(=S)−S−R', where R and R' are organyl groups. The salts of xanthates are sometimes called O-organyl dithioates. The esters of xanthic acid are sometimes called O,S-diorganyl esters of dithiocarbonic acid. The name xanthate is derived from Ancient Greek ξανθός (xanthos) meaning 'yellowish' or 'golden', and indeed most xanthate salts are yellow. They were discovered and named in 1823 by Danish chemist William Christopher Zeise. These organosulfur compounds are important in two areas: the production of cellophane and related polymers from cellulose and (in mining) for extraction of certain sulphide bearing ores.^[2] They are also versatile intermediates in organic synthesis.

Formation and structure

Xanthate salts of alkali metals are produced by the treatment of an alcohol, alkali, and carbon disulfide. The process is called xanthation.^[2] In chemical terminology, the alkali reacts with the alcohol to produce an alkoxide, which is the nucleophile that adds to the electrophilic carbon atom in CS₂.^[3] Often the alkoxide is generated in situ by treating the alcohol with sodium hydroxide or potassium hydroxide:

ROH + CS₂ + KOH → ROCS₂K + H₂O

For example, sodium ethoxide gives sodium ethyl xanthate. Many alcohols can be used in this reaction. Technical grade xanthate salts are usually of 90–95% purity. Impurities include alkali metal sulfides, sulfates, trithiocarbonates, thiosulfates, sulfites, or carbonates 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.

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 and esters, like that of the carbonates and the esters has trigonal planar molecular geometry. The central carbon atom is sp²-hybridized. The potassium salt of the amyl xanthate (KS₂COC₅H₁₁) has been characterized by X-ray crystallography. The COCS₂ portion of the anion is planar. The C-S bond lengths are both 1.65 Å, and the C-O distance is 1.38 Å.^[5]

Reactions

Reactions with electrophiles

Xanthate anions undergo alkylation to give xanthate esters, which are generally stable:^[9]

ROCS₂K + R′X → ROC(S)SR′ + KX

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.^[10]

Industrial applications

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 (e.g. sodium alkyl xanthates, dixanthogen) are widely used as flotation agents in mineral processing.

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.^[13] Water downstream of mining operations is often contaminated with xanthates.^[14]

References