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Organothallium compounds are compounds that contain the carbon-thallium bond. The area is not well developed because of the lack of applications and the high toxicity of thallium. The behavior of rrganothallium compounds can be inferred from that of organogallium and organoindium compounds. Organothallium(III) compounds are more numerous than organothallium(I) compounds.[1]

Organothallium(I) Chemistry[edit]

Structure of trimeric Tl(C6H3-2,6-(C6H3-2,6-Me2)2.[2] Color code: magenta= Tl.

Organothallium(I) compounds remain obscure and limited scope. Attempts to generate the simple compound thallium methyl results in disproportionation, giving thallium(III) derivatives. With the bulky tris(trimethylsilyl)methyl substituent, a tetramer has been crystallized.[3]

Similarly, thallium(I) aryl compounds require steric bulk for their isolation.[4]

A well-known organothallium(I) species is thallium cyclopentadienide. It arises by treatment of thallium(I) salts, such as thallium sulfate, with cyclopentadiene. Thallium(I) cyclopentadienide adopts a zig-zag chain structure of cyclopentadienide and thallium.[5]

Organothallium(III) Chemistry[edit]

Trialkyl Organothallium Compounds[edit]

Structure[edit]

In the gas and liquid phase, trialkyl organothallium compounds are monomeric and planar. In the solid phase, there is significant intermolecular interactions between the monomers.[6]

Preparation[edit]

Trialkyl thallium compounds, like those of indium and gallium, can be prepared from thallium trihalides and Grignard reagents or organolithium reagents, though the former may yield the ether complex of the product.[6] However, unlike that of gallium and indium, trialkyl thallium compounds cannot be prepared from dialkyl mercury and thallium trihalides, in which case R2TlX will be obtained.[6]Trimethyl thallium can be prepared from methyl iodide, methyl lithium, and thallium(I) iodide.[6]Triethyl thallium can be similarly prepared.

Reactions[edit]

Trialkyl thallium compounds can undergo alkyl exchange with itself and some acidic hydrocarbons like alkynes and cyclopentadiene. Some trialkyl thallium compounds are photosensitive.[7]

Dialkyl Organothallium Compounds[edit]

Structure[edit]

R2TlX has ionic properties, such that they are water soluble and that R2TlOH is strongly basic. The structure of the dialkyl thallium anion resembles that of dialkyl mercury.[7][8][9]However, dimeric or polymeric structures may exist in inert solvents or crystalline structures.

Preparation[edit]

Dialkyl Organothallium Halides can be prepared from two equivalents of Grignard reagents and thallium trihalides, or the reaction of trialkylthallium compounds with protonic compounds.[7][9]Another preparation involves the oxidation of thallium metal with aryldiazonium tetrafluoroborate salts. They are formed from dialkyl mercury and thallium trihalides instead of trialkyl thallium compounds.

Reactions[edit]

Dialkyl Organothallium Compounds are mostly stable to air and moisture.[7] The halide atom can be substituted by nucleophiles, and the alkyl group can be abstracted by mercury acetate. (C5F6)2TlBr can act as alkyl donors for low-valent metal halides, performing oxidative alkyl insertions onto the metals with itself being reduced to thallium(I) bromide.

Monoalkyl Organothallium Compounds[edit]

Preparation[edit]

Arylthallium dichloride can be prepared from TlCl3 and aryl boronic acids.[10]Excess boronic acid will result in diarylthallium chloride formation. Thallium(III) trifluoroacetate can oxidize aromatic rings to form ArTl(OCOCF3)2.[11]Alkenes can also react with thallium(III) salts in a fashion analogous to oxymercuration to yield monoalkyl organothallium compounds.

Reactions[edit]

Phenylthallium dihalides are prone to eliminating halobenzene, with the tendency increasing from chlorine to iodine, to the point that the iodide derivative is unknown.[12]They are Lewis acidic in nature. Nucleophile treatment can displace the halide atom, and substituent self-exchange to form thallium(III) halides and diphenylthallium halides is also possible. The dichloride can undergo transmetallation with mercuric chloride.[12]

Applications[edit]

ArTl(OCOCF3)2 obtained from the oxidation of aromatic compounds by thallium(III) trifluoroacetate can be used to form a variety of aryl derivatives, as shown below, and has found applications in organic chemistry.[7]

History[edit]

The first organothallium compound, diethylthallium chloride, was prepared in 1870, shortly after the discovery of the element thallium.[13]

See also[edit]

References[edit]

  1. ^ C. Elschenbroich (2006). Organometallics. VCH. p. 126-128. ISBN 978-3-527-29390-2.
  2. ^ Wright, Robert J.; Phillips, Andrew D.; Hino, Shirley; Power, Philip P. (2005). "Synthesis and Reactivity of Dimeric Ar'TlTlAr' and Trimeric (Ar' 'Tl)3 (Ar', Ar' ' = Bulky Terphenyl Group) Thallium(I) Derivatives: Tl(I)−Tl(I) Bonding in Species Ligated by Monodentate Ligands". Journal of the American Chemical Society. 127 (13): 4794–4799. doi:10.1021/ja0432259. PMID 15796545.
  3. ^ Uhl, Werner; Keimling, Sven Uwe; Klinkhammer, Karl Wilhelm; Schwarz, Wolfgang (1997). "TlI[C(SiMe3)3]—An Alkylthallium(<SCP>I</SCP>) Compound with a Distorted Tetrahedron of Tl Atoms in the Solid State". Angewandte Chemie International Edition in English. 36 (1–2): 64–65. doi:10.1002/anie.199700641.
  4. ^ Niemeyer, Mark; Power, Philip P. (1998). "Synthesis and Solid-State Structure of 2,6-Trip2C6H3Tl (Trip=2,4,6-iPr3C6H2): A Monomeric Arylthallium(I) Compound with a Singly Coordinated Thallium Atom". Angewandte Chemie International Edition. 37 (9): 1277–1279. doi:10.1002/(SICI)1521-3773(19980518)37:9<1277::AID-ANIE1277>3.3.CO;2-T.
  5. ^ {{cite book|Organometallic Syntheses, Volume 2 Nontransition-Metal Compounds|editor=J. J. Eisch, R. B. King|publisher=Academic Press|year=1981
  6. ^ a b c d Housecroft, Catherine (2018). Inorganic Chemistry (5th ed.). Pearson. pp. 887–892. ISBN 978-1-292-13414-7.
  7. ^ a b c d e 无机化学丛书 第二卷 [Books of Inorganic Chemistry]. pp. 524–528. ISBN 978-7-03-056380-4.
  8. ^ Housecroft, Catherine (2018). Inorganic Chemistry (5th ed.). Pearson. pp. 887–892. ISBN 978-1-292-13414-7.
  9. ^ a b Greenwood (2001). Chemistry of the Elements (2nd ed.). Elsevier. pp. 262–265. ISBN 0-7506-3365-4.
  10. ^ Challenger, Frederick; Richards, Oswald V. (1934). "94. Organo-derivatives of bismuth and thallium". Journal of the Chemical Society (Resumed): 405–411. doi:10.1039/jr9340000405. ISSN 0368-1769.
  11. ^ 无机化学丛书 第二卷 [Books of Inorganic Chemistry]. pp. 524–528. ISBN 978-7-03-056380-4.
  12. ^ a b Challenger, Frederick; Richards, Oswald V. (1934). "94. Organo-derivatives of bismuth and thallium". Journal of the Chemical Society (Resumed): 405–411. doi:10.1039/jr9340000405. ISSN 0368-1769.
  13. ^ Lee, A. G. (1970-01-01). "Organothallium chemistry". Quarterly Reviews, Chemical Society. 24 (2): 310–329. doi:10.1039/QR9702400310. ISSN 0009-2681.
source: https://en.wikipedia.org/wiki/Organothallium_chemistry

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