Thiourea

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Thiourea
Thiourea.png
Thiourea-3D-vdW.png
Names
Preferred IUPAC name
Thiourea[1]
Other names
Thiocarbamide
Identifiers
3D model (JSmol)
605327
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.494
1604
KEGG
RTECS number YU2800000
UNII
UN number 2811
Properties
CH4N2S
Molar mass 76.12 g/mol
Appearance white solid
Density 1.405 g/ml
Melting point 182 °C (360 °F; 455 K)
142 g/l (25 °C)
−4.24×10−5 cm3/mol
Hazards
Carc. Cat. 3
Repr. Cat. 3
Harmful (Xn)
Dangerous for the environment (N)
R-phrases (outdated) R22, R40, R51/53, R63
S-phrases (outdated) (S2), S36/37, S61
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oilHealth code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
1
3
0
Related compounds
Related compounds
Urea
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

Thiourea (/ˌθjʊəˈrə/)[2][3] is an organosulfur compound with the formula SC(NH2)2. It is structurally similar to urea, except that the oxygen atom is replaced by a sulfur atom, but the properties of urea and thiourea differ significantly. Thiourea is a reagent in organic synthesis. "Thioureas" refers to a broad class of compounds with the general structure (R1R2N)(R3R4N)C=S. Thioureas are related to thioamides, e.g. RC(S)NR2, where R is methyl, ethyl, etc.

General chemical structure of a thiourea

Structure and bonding[edit]

Thiourea is a planar molecule. The C=S bond distance is 1.60±0.1 Å for thiourea (as well as many of its derivatives). The material has the unusual property of changing to ammonium thiocyanate upon heating above 130 °C. Upon cooling, the ammonium salt converts back to thiourea.

Thiourea occurs in two tautomeric forms, of which the thione form predominates in aqueous solutions. The equilibrium constant has been calculated as being Keq = 1.04×10−3.[4] The thiol form, which is also known as an isothiourea, can be encountered in substituted compounds such as isothiouronium salts.

Thiourea tautomers.png

Production[edit]

The global annual production of thiourea is around 10,000 tonnes. About 40% is produced in Germany, another 40% in China, and 20% in Japan. Thiourea can be produced from ammonium thiocyanate, but more commonly it is produced by the reaction of hydrogen sulfide with calcium cyanamide in the presence of carbon dioxide.[5]

Applications[edit]

The main application of thiourea is in textile processing.[5]

Organic synthesis[edit]

Thiourea reduces peroxides to the corresponding diols.[6] The intermediate of the reaction is an unstable endoperoxide.

reduction of cyclic peroxide

Thiourea is also used in the reductive workup of ozonolysis to give carbonyl compounds.[7] Dimethyl sulfide is also an effective reagent for this reaction, but it is highly volatile (boiling point 37 °C) and has an obnoxious odor whereas thiourea is odorless and conveniently non-volatile (reflecting its polarity).

reduction cleavage of product from ozonolysis

Source of sulfide[edit]

Thiourea is employed as a source of sulfide, such as for converting alkyl halides to thiols. The reaction capitalizes on the high nucleophilicity of the sulfur center and easy hydrolysis of the intermediate isothiouronium salt:

CS(NH2)2 + RX → RSC(NH
2
)+
2
X
RSC(NH
2
)+
2
X
+ 2 NaOH → RSNa + OC(NH2)2 + NaX
RSNa + HCl → RSH + NaCl

In this example, ethane-1,2-dithiol is prepared from 1,2-dibromoethane:[8]

C2H4Br2 + 2 SC(NH2)2 → [C2H4(SC(NH2)2)2]Br2
[C2H4(SC(NH2)2)2]Br2 + 2 KOH → C2H4(SH)2 + 2 OC(NH2)2 + 2 KBr

Like other thioamides, thiourea can serve as a source of sulfide upon reaction with metal ions. For example, mercury sulfide forms when mercuric salts in aqueous solution are treated with thiourea:

Hg2+ + SC(NH2)2 + H2O → HgS + OC(NH2)2 + 2 H+

These sulfiding reactions, which have been applied to the synthesis of many metal sulfides, require water and typically some heating.[9][10]

Precursor to heterocycles[edit]

Thioureas are building blocks to pyrimidine derivatives. Thus thioureas condense with β-dicarbonyl compounds.[11] The amino group on the thiourea initially condenses with a carbonyl, followed by cyclization and tautomerization. Desulfurization delivers the pyrimidine.

Pyrimidine.png

Similarly, aminothiazoles can be synthesized by the reaction of α-haloketones and thiourea.[12]

Aminothiazole.png

The pharmaceuticals thiobarbituric acid and sulfathiazole are prepared using thiourea.[5] 4-Amino-3-hydrazino-5-mercapto-1,2,4-triazole is prepared by the reaction of thiourea and hydrazine.

Silver polishing[edit]

According to the label on the consumer product, the liquid silver cleaning product TarnX contains thiourea, a detergent, and sulfamic acid. A lixiviant for gold and silver leaching can be created by selectively oxidizing thiourea, bypassing the steps of cyanide use and smelting.[13]

Other uses[edit]

Other industrial uses of thiourea include production of flame retardant resins, and vulcanization accelerators.

Thiourea is used as an auxiliary agent in diazo paper, light-sensitive photocopy paper and almost all other types of copy paper.

It is also used to tone silver-gelatin photographic prints.

Thiourea is used in the Clifton-Phillips and Beaver bright and semi-bright electroplating processes.[14] It is also used in a solution with tin(II) chloride as an electroless tin plating solution for copper printed circuit boards.

Safety[edit]

The LD50 for thiourea is 125 mg/kg for rats (oral).[15]

A goitrogenic effect (enlargement of the thyroid gland) has been reported for chronic exposure, reflecting the ability of thiourea to interfere with iodide uptake.[5]

See also[edit]

References[edit]

  1. ^ Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: Royal Society of Chemistry. 2014. pp. 98, 864. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
  2. ^ "Thiourea". Oxford Dictionaries. Oxford University Press. Retrieved 2016-01-21.
  3. ^ "Thiourea". Merriam-Webster Dictionary. Retrieved 2016-01-21.
  4. ^ Allegretti, P.E; Castro, E.A; Furlong, J.J.P (March 2000). "Tautomeric equilibrium of amides and related compounds: theoretical and spectral evidences". Journal of Molecular Structure: THEOCHEM. 499 (1–3): 121–126. doi:10.1016/S0166-1280(99)00294-8.
  5. ^ a b c d Bernd Mertschenk, Ferdinand Beck, Wolfgang Bauer (2002). "Thiourea and Thiourea Derivatives". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a26_803.
  6. ^ C. Kaneko; A. Sugimoro & S. Tanaka (1974). "A facile one-step synthesis of cis-2-cyclopentene and cis-2-cyclohexene-1,4-diols from the corresponding cyclodienes". Synthesis. 1974 (12): 876–877. doi:10.1055/s-1974-23462.
  7. ^ Gupta, D., Soman, G., and Dev, S. (1982). "Thiourea, a convenient reagent for the reductive cleavage of olefin ozonolysis products". Tetrahedron. 38 (20): 3013–3018. doi:10.1016/0040-4020(82)80187-7.
  8. ^ Speziale, A. J. (1963). "Ethanedithiol". Organic Syntheses.; Collective Volume, 4, p. 401
  9. ^ Liang, Y.; et, al. (2016). "An efficient precursor to synthesize various FeS2 nanostructures via a simple hydrothermal synthesis method". CrystEngComm. 18: 6262–6271.
  10. ^ Bao, N.; et al. (2007). "Facile Cd−Thiourea Complex Thermolysis Synthesis of Phase-Controlled CdS Nanocrystals for Photocatalytic Hydrogen Production under Visible Light". The Journal of Physical Chemistry C. 111: 17527–17534.
  11. ^ Foster, H. M., and Snyder, H. R. (1963). "4-Methyl-6-hydroxypyrimidine". Organic Syntheses.; Collective Volume, 4, p. 638
  12. ^ Dodson, R. M. & King, L. C. (1945). "The reaction of ketones with halogens and thiourea". J. Am. Chem. Soc. 67 (12): 2242–2243. doi:10.1021/ja01228a059. PMID 21005695.
  13. ^ Anthony Esposito. "Peñoles, UAM unveil pilot thiourea Au-Ag leaching plant - Mexico". Business News Americas (July 13, 2007).
  14. ^ 81st Universal Metal Finishing Guidebook. Metal Finishing Magazine. Fall 2013. p. 285. ISSN 0026-0576.
  15. ^ http://gis.dep.wv.gov/tri/cheminfo/msds1385.txt

Further reading[edit]

  • Patai, S., ed. (1977). The Chemistry of double-bonded functional groups. New York, NY: John Wiley & Sons. pp. 1355–1496. ISBN 0-471-92493-8.

External links[edit]