Perrhenate

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The perrhenate ion is the anion with the formula ReO
4
, or a compound containing this ion. The perrhenate anion is tetrahedral, being similar in size and shape to perchlorate and the valence isoelectronic permanganate. The perrhenate anion is stable over a broad pH range and can be precipitated from solutions with the use of organic cations. At normal pH, perrhenate exists as metaperrhenate (ReO
4
), but at high pH mesoperrhenate (ReO3−
5
) forms. Perrhenate, like its conjugate acid perrhenic acid, features rhenium in the oxidation state of +7 with a d0 configuration. Solid perrhenate salts takes on the color of the cation.[1]

Typical perrhenate salts are the alkali metal derivatives and ammonium perrhenate. These salts are prepared by oxidation of rhenium compounds with nitric acid followed by neutralization of the resulting perrhenic acid.[2][3][4]

Basicity of the anion[edit]

In inorganic chemistry, perrhenate anion is also used as a weakly coordinating anion. It is a weaker base than Cl or Br but stronger than ClO4 or BF4. Unlike the related permanganate, perrhenate is nonoxidising. Silver perrhenate reacts with trimethylsilyl chloride to give the silyl "ester" (CH3)3SiOReO3.[5]

Reactions of perrhenates[edit]

The perrhenate ion reacts with the cyanide to give trans-[ReO2(CN)4]3−. With sulfide sources such as hydrogen sulfide, one obtains black ReS2 and Re2S7. These species form via the intermediacy of ReO3S. Heating ammonium perrhenate gives Re2O7 and then ReO2.[2]

The chemistry of the perrhenate ion is similar to that of the pertechnetate ion TcO4. For this reason, perrhenate is sometimes used as a carrier for trace levels of pertechnetate, for instance in nuclear medicine scanning procedures.

References[edit]

  1. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419. 
  2. ^ a b O. Glemser "Rhenium" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1476-85.
  3. ^ Richard J. Thompson (1966). "Ammonium Perrhenate". Inorganic Syntheses 8: 171–173. doi:10.1002/9780470132395.ch44. 
  4. ^ Wm. T. Smith, S. Harmon Long (1948). "The Salts of Perrhenic Acid. I. The Alkali Metals and Ammonium". Journal of the American Chemical Society 70 (1): 354–356. doi:10.1021/ja01181a110. 
  5. ^ US patent 2008262256, Wolfgang A. Herrmann, Fritz E. Kuhn, Richard Fischer, "Method for efficiently producing methyltrioxorhenium(vii) (mto) and organorhenium(vii) oxides", issued 2005-08-30 

See also[edit]