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Thiol

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Thiol

Thiol with a blue-highlighted sulfhydryl group.

In organic chemistry, a thiol (, )[1] is an alcohols (that is, sulfur takes the place of oxygen in the hydroxyl group of an alcohol), and the word is a portmanteau of "thion" + "alcohol," with the first word deriving from Greek θεῖον ("thion") = "sulfur."[note 1] The –SH functional group itself is referred to as either a thiol group or a sulfhydryl group.

Many thiols have strong odors resembling that of garlic. Thiols are used as odorants to assist in the detection of natural gas (which in pure form is odorless), and the "smell of natural gas" is due to the smell of the thiol used as the odorant.

Thiols are often referred to as mercaptans.[3][4] The term mercaptan [5] was introduced in 1832 by William Christopher Zeise and is derived from the Latin mercurium captans (capturing mercury)[6] because the thiolate group bonds very strongly with mercury compounds.[7] Thiols react with mercury to form mercaptides.[8]

Contents

  • Structure and bonding 1
  • Nomenclature 2
  • Physical properties 3
    • Odor 3.1
    • Boiling points and solubility 3.2
  • Characterization 4
  • Preparation 5
    • Laboratory methods 5.1
  • Reactions 6
    • S-alkylation 6.1
    • Acidity 6.2
    • Redox 6.3
    • Metal ion complexation 6.4
  • Thiyl radicals 7
  • Biological importance 8
    • Cysteine and cystine 8.1
    • Cofactors 8.2
  • Examples of thiols 9
  • See also 10
  • Footnotes 11
  • References 12
  • External links 13

Structure and bonding

Thiols and alcohols have similar molecular structure. The major difference is the size of the chalcogenide, C–S bond lengths being around 180 picometers in length and C-O bond lengths being around 143 picometers in length. The C–S–H angles approach 90°. In the solid or molten liquids, the hydrogen-bonding between individual thiol groups is weak, the main cohesive force being van der Waals interactions between the highly polarizable divalent sulfur centers.

Due to the lesser electronegativity difference between sulfur and hydrogen compared to oxygen and hydrogen, an S–H bond is less polar than the hydroxyl group. Thiols have a lower dipole moment relative to the corresponding alcohol

Nomenclature

There are several ways to name the alkylthiols:

  • The suffix -thiol is added to the name of the alkane. This method is nearly identical to naming an alcohol and is used by the IUPAC. Example: CH3SH would be methanethiol.
  • The word mercaptan replaces alcohol in the name of the equivalent alcohol compound. Example: CH3SH would be methyl mercaptan, just as CH3OH is called methyl alcohol.
  • The term sulfanyl or mercapto is used as a prefix. Example: mercaptopurine.

Physical properties

Odor

Many thiols have strong odors resembling that of garlic. The odors of thiols are often strong and repulsive, in particular for those of low molecular weight. The spray of skunks consists mainly of low-molecular-weight thiols and derivatives.[9][10][11][12][13] These compounds are detectable by the human nose at concentrations of only 10 parts per billion.[14] Human sweat contains (R)/(S)-3-methyl-3-sulfanylhexan-1-ol (MSH), detectable at 2 parts per billion and having a fruity, onion-like odor. Women emit significantly more MSH than men.[15] (Methylthio)methanethiol (MeSCH2SH; MTMT) is a strong-smelling volatile thiol, also detectable at parts per billion levels, found in male mouse urine. Lawrence C. Katz and co-workers showed that MTMT functioned as a semiochemical, activating certain mouse olfactory sensory neurons, attracting female mice.[16] Copper has been shown to be required by a specific mouse olfactory receptor, MOR244-3, which is highly responsive to MTMT as well as to various other thiols and related compounds.[17]

Thiols are also responsible for a class of wine faults caused by an unintended reaction between sulfur and yeast and the "skunky" odor of beer that has been exposed to ultraviolet light.

Not all thiols have unpleasant odors. For example, furan-2-ylmethanethiol contributes to the aroma of roasted coffee, whereas grapefruit mercaptan, a monoterpenoid thiol, is responsible for the characteristic scent of grapefruit. The effect of the latter compound is present only at low concentrations. The pure mercaptan has an unpleasant odor.

Natural gas distributors were required to add thiols, originally ethanethiol, to natural gas (which is naturally odorless) after the deadly New London School explosion in New London, Texas, in 1937. Many gas distributors were odorizing gas prior to this event. Most gas odorants utilized currently contain mixtures of mercaptans and sulfides, with t-butyl mercaptan as the main odor constituent. In situations where thiols are used in commercial industry, such as liquid petroleum gas tankers and bulk handling systems, an oxidizing catalyst is used to destroy the odor. A copper-based oxidation catalyst neutralizes the volatile thiols and transforms them into inert products.

Boiling points and solubility

Thiols show little association by hydrogen bonding, with both water molecules and among themselves. Hence, they have lower boiling points and are less soluble in water and other polar solvents than alcohols of similar molecular weight. For this reason also, thiols and corresponding thioether functional group isomers have similar solubility characteristics and boiling points, whereas the same is not true of alcohols and their corresponding isomeric ethers.

Characterization

Volatile thiols are easily and almost unerringly detected by their distinctive odor. S-specific analyzers for gas chromatographs are useful. Spectroscopic indicators are the D2O-exchangeable SH signal in the 1H NMR spectrum (33S is NMR active but signals for divalent sulfur are very broad and of little utility[18]). The νSH band appears near 2400 cm−1 in the IR spectrum.[3] In the nitroprusside reaction, free thiol groups react with sodium nitroprusside and ammonium hydroxide to give a red colour.

Preparation

In industry, methanethiol is prepared by the reaction of hydrogen sulfide with methanol. This method is employed for the industrial synthesis of methanethiol:

CH3OH + H2S → CH3SH + H2O

Such reactions are conducted in the presence of acidic catalysts. The other principal route to thiols involves the addition of hydrogen sulfide to alkenes. Such reactions are usually conducted in the presence of an acid

  • Mercaptans (or Thiols) at The Periodic Table of Videos (University of Nottingham)
  • Applications, Properties, and Synthesis of w-Functionalized n-Alkanethiols and Disulfides – the Building Blocks of Self-Assembled Monolayers by D. Witt, R. Klajn, P. Barski, B.A. Grzybowski at Northwestern University.
  • Mercaptan, by The Columbia Electronic Encyclopedia.
  • What is Mercaptan?, by Columbia Gas of Pennsylvania and Maryland.
  • What Is the Worst Smelling Chemical?, by About Chemistry.

External links

  1. ^ Dictionary Reference: thiol
  2. ^ θεῖος. Scott, Robert; A Greek–English Lexicon at the Perseus Project
  3. ^ a b Patai, Saul “The chemistry of the thiol group” Saul Patai, Ed. Wiley, London, 1974. ISBN 0-471-66949-0.
  4. ^ a b R. J. Cremlyn “An Introduction to Organosulfur Chemistry” John Wiley and Sons: Chichester (1996). ISBN 0-471-95512-4.
  5. ^ Dictionary Reference: mercaptan
  6. ^ a b Oxford American Dictionaries (Mac OS X Leopard).
  7. ^ "Mercaptan" (ethyl thiol) was discovered in 1834 by the Danish professor of chemistry William Christopher Zeise (1789–1847). He called it "mercaptan", a contraction of "corpus mercurium captans" (mercury-capturing substance) [p. 88], because it reacted violently with mercury (II) oxide ("deutoxide de mercure") [p. 92]. See:
    • Zeise, William Christopher (1834) "Sur le mercaptan; avec des observations sur d'autres produits resultant de l'action des sulfovinates ainsi que de l'huile de vin, sur des sulfures metalliques" (On mercaptan; with observations on other products resulting from the action of sulfovinates [typically, ethyl hydrogen sulfate] and oil of wine [a mixture of diethylsufate and ethylene polymers] on metal sulfides), Annales de Chimie et de Physique, 56 : 87–97.
    • The article in Annales de Chimie et de Physique (1834) was translated from the German article: W. C. Zeise, "Das Mercaptan, nebst Bemerkungen über einige neue Producte aus der Einwirkung der Sulfurete auf weinschwefelsaure Salze und auf das Weinöl," Annalen der Physik und Chemie, 107 (27) : 369–431.
    • The article in Annalen der Physik und Chemie (1834) was translated from the original Danish article in: Zeise (1834) "Mercaptanet med Bemaerkninger over nogle andre nye Producter af Svovelvinsyre saltene, som og af den tunge Vinolle, ved Sulfureter," Saertskilt aftrykt af det Kongelige Danske Videnskabers Selskabs Skrifter (Special issue of the Journal of the Royal Danish Society of Science), 70 pages.
    • German translation is reprinted in: W. C. Zeise (1834) "Das Mercaptan, nebst Bemerkungen über einige andere neue Erzeugnisse der Wirkung schwefelweinsaurer Salze, wie auch des schweren Weinöls auf Sulphurete," Journal für praktische Chemie, 1 (1) : 257–268, 345–356, 396–413, 457–475.
    • Summarized in: Zeise , W. C. (1834), Ueber das Mercaptan (On mercaptan), Annalen der Pharmacie, 11 (1) : 1–10.
  8. ^ Vibrant Life Magazine, Loren K. "Sulfer & Mercury". 
  9. ^ Andersen K. K., Bernstein D. T. (1978). "Some Chemical Constituents of the Scent of the Striped Skunk (Mephitis mephitis)". Journal of Chemical Ecology 1 (4): 493–499.  
  10. ^ Andersen K. K., Bernstein D. T.; Bernstein (1978). "1-Butanethiol and the Striped Skunk". Journal of Chemical Education 55 (3): 159–160.  
  11. ^ Andersen K. K., Bernstein D. T., Caret R. L., Romanczyk L. J., Jr. (1982). "Chemical Constituents of the Defensive Secretion of the Striped Skunk (Mephitis mephitis)". Tetrahedron 38 (13): 1965–1970.  
  12. ^ Wood W. F., Sollers B. G., Dragoo G. A., Dragoo J. W. (2002). "Volatile Components in Defensive Spray of the Hooded Skunk, Mephitis macroura". Journal of Chemical Ecology 28 (9): 1865–70.  
  13. ^ William F. Wood. "Chemistry of Skunk Spray". Dept. of Chemistry,  
  14. ^ Aldrich, T.B. (1896). "A CHEMICAL STUDY OF THE SECRETION OF THE ANAL GLANDS OF MEPHITIS MEPHITIGA (COMMON SKUNK), WITH REMARKS ON THE PHYSIOLOGICAL PROPERTIES OF THIS SECRETION". J. Exp. Med. 1 (2): 323–340.  
  15. ^ Troccaz, Myriam; Borchard, Gerrit; Vuilleumier, Christine; Raviot-Derrien, Sophie; Niclass, Yvan; Beccucci, Sabine; Starkenmann, Christian (2009). "Gender-Specific Differences between the Concentrations of Nonvolatile (R)/(S)-3-Methyl-3-sulfanylhexan-1-ol and (R)/(S)-3-Hydroxy-3-methylhexanoic Acid Odor Precursors in Axillary Secretions". Chem. Senses 34 (3): 203–210.  
  16. ^ Lin, DaYu; Zhang, Shaozhong; Block, Eric; Katz, Lawrence C (2005). "Encoding social signals in the mouse main olfactory bulb". Nature 2005 (434): 470–477.  
  17. ^ Duan, Xufang; Block, Eric; Li, Zhen; Connelly, Timothy; Zhang, Jian; Huang, Zhimin; Su, Xubo; Pan, Yi; et al. (2012). "Crucial role of copper in detection of metal-coordinating odorants". Proc. Natl. Acad. Sci. U.S.A 2012 (109): 3492–3497.  
  18. ^ http://www.pascal-man.com/periodic-table/sulfur.shtml
  19. ^ John S Roberts, "Thiols", in Kirk-Othmer Encyclopedia of Chemical Technology, 1997, Wiley-VCH, Weinheim. doi:10.1002/0471238961.2008091518150205.a01
  20. ^ Speziale, A. J. (1963). "Ethanedithiol".  .
  21. ^ S. R. Wilson, G. M. Georgiadis (1990). "Mecaptans from Thioketals: Cyclododecyl Mercaptan".  .
  22. ^ E. Jones and I. M. Moodie (1990). "2-Thiophenethiol".  .
  23. ^ Melvin S. Newman and Frederick W. Hetzel (1990). "Thiophenols from Phenols: 2-Naphthalenethiol".  .
  24. ^ Ernest L. Eliel, Joseph E. Lynch, Fumitaka Kume, and Stephen V. Frye (1993). "Chiral 1,3-oxathiane from (+)-Pulegone: Hexahydro-4,4,7-trimethyl-4H-1,3-benzoxathiin".  
  25. ^ Heterogeneous catalytic demercaptization of light hydrocarbon feedstock. A. G. Akhmadullina, B. V. Kizhaev, G. M. Nurgalieva, I. K. Khrushcheva and A. S. Shabaeva, et al. Chemistry and Technology of Fuels and Oils, 1993, Volume 29, Number 3, Pages 108–109
  26. ^ Kathrin-Maria Roy "Thiols and Organic sulphides" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH Verlag, Weinheim. doi:10.1002/14356007.a26_767
  27. ^ JoAnne Stubbe, Daniel G. Nocera, Cyril S. Yee, Michelle C. Y. Chang "Radical Initiation in the Class I Ribonucleotide Reductase:  Long-Range Proton-Coupled Electron Transfer?" Chem. Rev 2003, 103 (6), pp 2167–2202. doi:10.1021/cr020421u
  28. ^ Dustin Hofstetter, Thomas Nauser, and Willem H. Koppenol "Hydrogen Exchange Equilibria in Glutathione Radicals: Rate Constants" Chem. Res. Toxicol. 2010; 23 (10), pp 1596–1600, doi:10.1021/tx100185k
  29. ^ Reece, Urry, et al. Campbell Biology, Ninth Edition. Pearson Benjamin Cummings, New York. 2011. Print. Pg 65, 83.

References

  1. ^ The Greek adjective theios, a, on (θεῖος, α, ον) means "divine",[2] but appears as a noun to mean "brimstone" in the Bible (c.f. Luke 17:29 "ἔβρεξεν πῦρ καὶ θεῖον ἀπ' οὐρανοῦ καὶ ἀπώλεσεν πάντας." ("it rained fire and sulfur from the sky, and destroyed them all."), brimstone being an alternative name for sulfur.

Footnotes

See also

Examples of thiols

Many cofactors (non-protein-based helper molecules) feature thiols. The biosynthesis and degradation of fatty acids and related long-chain hydrocarbons is conducted on a scaffold that anchors the growing chain through a thioester derived from the thiol Coenzyme A. The biosynthesis of methane, the principal hydrocarbon on Earth, arises from the reaction mediated by coenzyme M, 2-mercaptoethyl sulfonic acid. Thiolates, the conjugate bases derived from thiols, form strong complexes with many metal ions, especially those classified as soft. The stability of metal thiolates parallels that of the corresponding sulfide minerals.

Cofactors

Sulfhydryl groups in the active site of an enzyme can form noncovalent bonds with the enzyme's substrate as well, contributing to covalent catalytic activity in catalytic triads. Active site cysteine residues are the functional unit in cysteine protease catalytic triads. Cysteine residues may also react with heavy metal ions (Zn2+, Cd2+, Pb2+, Hg2+, Ag+) because of the high affinity between the soft sulfide and the soft metal (see hard and soft acids and bases). This can deform and inactivate the protein, and is one mechanism of heavy metal poisoning.

As the functional group of the amino acid cysteine, the thiol group plays a very important role in biology. When the thiol groups of two cysteine residues (as in monomers or constituent units) are brought near each other in the course of protein folding, an oxidation reaction can generate a cystine unit with a disulfide bond (-S-S-). Disulfide bonds can contribute to a protein's tertiary structure if the cysteines are part of the same peptide chain, or contribute to the quaternary structure of multi-unit proteins by forming fairly strong covalent bonds between different peptide chains. A physical manifestation of cysteine-cystine equilibrium is provided by hair straightening technologies.[29]

Cysteine and cystine

Biological importance

[28]—C bonds or backbone fragmentation.C-centred radicals could lead to protein damage via the formation of carbon. The formation of equilibria atom exchange hydrogen via. Thiyl radicals (sulfur-centred) can transform to carbon-centred radicals crosslinks polysulfide results when mercapto radicals couple forming disulfide and polyisoprene process. For example, the vulcanization of vulcanization, an antioxidant in biology. Thiyl radicals are also intermediates in the glutathione Thiyl intermediates also are produced by the oxidation of [27] (see figure).ribonucleotide reductase. This conversion is catalysed by DNA In biology thiyl radicals are responsible for the formation of the deoxyribonucleic acids, building blocks for [26]

The catalytic cycle for ribonucleotide reductase, demonstrating the role of thiyl radicals in producing the genetic machinery of life.

Thiyl radicals

With metal ions, thiolates behave as ligands to form transition metal thiolate complexes. The term mercaptan is derived from the Latin mercurium captans (capturing mercury)[6] because the thiolate group bonds so strongly with mercury compounds. According to Hard/Soft Acid/Base (HSAB) theory, sulfur is a relatively soft (polarizable) atom. This explains the tendency of thiols to bind to soft elements/ions such as mercury, lead, or cadmium. The stability of metal thiolates parallels that of the corresponding sulfide minerals.

Metal ion complexation

This reaction is important in nature.

RS–SR + 2 R'SH → 2 RSH + R'S–SR'

Thiols participate in thiol-disulfide exchange:

2R–SH + 1/2O2 → RS–SR + H2O

Oxidation can also be affected by oxygen in the presence of catalysts:[25]

R–SH + 3H2O2 → RSO3H + 3H2O

Oxidation by more powerful reagents such as sodium hypochlorite or hydrogen peroxide can also yield sulfonic acids (RSO3H).

2 R–SH + Br2 → R–S–S–R + 2 HBr

Thiols, especially in the presence of base, are readily disulfide (R–S–S–R).

Redox

Synthesis of thiophenolate from thiophenol

Relative to the alcohols, thiols are more acidic. The conjugate base of a thiol is called a thiolate. Butanethiol has a pKa of 10.5 vs 15 for butanol. Thiophenol has a pKa of 6 vs 10 for phenol. Thus, thiolates can be obtained from thiols by treatment with alkali metal hydroxides.

Acidity

RSH + R'Br + base → RSR' + [Hbase]Br

Thiols, or more specific their conjugate bases, are readily alkylated to give thioethers:

S-alkylation

Akin to the chemistry of alcohols, thiols form thioethers, thioacetals, and thioesters, which are analogous to ethers, acetals, and esters respectively. Thiols and alcohols are also very different in their reactivity, thiols being more easily oxidized than alcohols. Thiolates are more potent nucleophiles than the corresponding alkoxides.

Reactions

Many thiols are prepared by reductive dealkylation of thioethers, especially benzyl derivatives and thioacetals.[24]

Phenols can be converted to the thiophenols via rearrangement of their O-aryl dialkylthiocarbamates.[23]

RLi + S → RSLi
RSLi + HCl → RSH + LiCl

Grignard reagents react with sulfur to give the thiolates, which are readily hydrolyzed:[22]

Na[O3S2CH2CO2H] + H2O → HSCH2CO2H + NaHSO4
ClCH2CO2H + Na2S2O3 → Na[O3S2CH2CO2H] + NaCl

The thiourea route works well with primary halides, especially activated ones. Secondary and tertiary thiols are less easily prepared. Secondary thiols can be prepared from the ketone via the corresponding dithioketals.[21] A related two-step process involves alkylation of thiosulfate to give the thiosulfonate ("Bunte salt"), followed by hydrolysis. The method is illustrated by one synthesis of thioglycolic acid:

CH3CH2Br + SC(NH2)2 → [CH3CH2SC(NH2)2]Br
[CH3CH2SC(NH2)2]Br + NaOH → CH3CH2SH + OC(NH2)2 + NaBr

In general, on the typical laboratory scale, the direct reaction of a halogenoalkane with sodium hydrosulfide is inefficient owing to the competing formation of thioethers Instead, alkyl halides are converted to thiols via a S-alkylation of thiourea. This multistep, one-pot process proceeds via the intermediacy of the isothiouronium salt, which is hydrolyzed in a separate step:[20]

Laboratory methods

This method is used for the production of thioglycolic acid from chloroacetic acid.

RX + NaSH → RSH + NaX (X = Cl, Br, I)

Another method entails the alkylation of sodium hydrosulfide.

[19]

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