Organoastatine chemistry : Further reading Wikipedia, the free encyclopedia

Organoastatine chemistry

Study of the carbon-astatine bond

Organoastatine chemistry describes the synthesis and properties of organoastatine compounds, chemical compounds containing a carbon to astatine chemical bond.

Astatine is extremely radioactive, with the longest-lived isotope (²¹⁰At) having a half-life of only 8.1 hours. Consequently, organoastatine chemistry can only be studied by tracer techniques on extremely small quantities. The problems caused by radiation damage as well as difficulties in separation and identification are worse for organic astatine derivatives than for inorganic compounds. Most studies of organoastatine chemistry focus on ²¹¹At (half-life 7.21 hours), which is the subject of ongoing studies in nuclear medicine: it is better than ¹³¹I at destroying abnormal thyroid tissue.^[1]

Astatine-labelled iodine reagents have been used to synthesise RAt, RAtCl₂, R₂AtCl, and RAtO₂ (R = phenyl or p-tolyl).^[1] Alkyl and aryl astatides are relatively stable and have been analysed at high temperatures (120 °C) with radio gas chromatography.^[2] Demercuration reactions have produced with good yields trace quantities of ²¹¹At-containing aromatic amino acids, steroids, and imidazoles, among other compounds.^[1]

Astatine has both halogen-like and metallic properties, so that analogies with iodine sometimes hold, but sometimes do not. Astatine can be incorporated into organic molecules via halogen exchange, halodediazotation (replacing a diazonium group), halodeprotonation, or halodemetallation. Initial attempts to radiolabel proteins with ²¹¹At exemplify its intermediate behaviour, as astatination (analogous to radioiodination) produces unstable results and it is instead AtO⁺ (or a hydrolysed species) that probably bonds to proteins. Two-step procedures are used today, first synthesising stable astatoaryl prosthetic groups before incorporating them into the protein.^[3] Not only is the C–At bond the weakest of all carbon–halogen bonds (following periodic trends), but also the bond easily breaks as the astatine is oxidised back to free astatine.^[3]

References

^ ^a ^b ^c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 885–887. ISBN 978-0-08-037941-8.
^ Coenen, H. H.; Moerlein, S. M.; Stöcklin, G. (1983). "No-Carrier-Added Radiohalogenation Methods with Heavy Halogens". Radiochimica Acta. 34 (1–2): 47–68. doi:10.1524/ract.1983.34.12.47. S2CID 99845370.
^ ^a ^b Guérard, François; Maingueneau, Clémence; Liu, Lu; Eychenne, Romain; Gestin, Jean-François; Montavon, Gilles; Galland, Nicolas (2021). "Advances in the Chemistry of Astatine and Implications for the Development of Radiopharmaceuticals" (PDF). Accounts of Chemical Research. 54 (16): 3264–3275. doi:10.1021/acs.accounts.1c00327. PMID 34350753. S2CID 236926712.