Sodium pertechnetate

From Wikipedia, the free encyclopedia

Sodium pertechnetate
IUPAC name Sodium technetate(VII)
Other names sodium tetraoxotechnetate (VII)
Properties
Molecular formula NaTcO4
Molar mass 169.89 g/mol
Appearance White or pale pink solid
Solubility in water Soluble
Related compounds
Other anions Sodium permanganate; sodium perrhenate
Other cations Ammonium pertechnetate
Related compounds Technetium heptoxide
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references

Sodium pertechnetate is the inorganic compound with the formula Na[TcO4]. This colourless salt consists of the anion [TcO4]−. The radioactive 99mTcO4− anion is an importantradiopharmaceutical for diagnostic use. The advantages to 99mTc include its short half-life of 6 hours and the low radiation exposure to the patient, which allow a patient to be injected with activities of more than 30 milliCuries.[1] Na[99mTcO4] is a precursor to a variety of derivatives that are used to image different parts of the body.

Contents

[edit] Chemistry

[TcO4]− is the starting material for most of the chemistry of technetium. Pertechnetate salts are usually colorless.[2] [TcO4]− is produced by oxidizing technetium with nitric acid or with hydrogen peroxide. The pertechnetate anion is similar to the permanganate anion but is a weaker oxidizing agent. It is tetrahedral and diamagnetic. The standard electrode potential for TcO4−/TcO2 is only +0.738 V in acidic solution, as compared to +1.695 V for MnO4−/MnO2.[1] Because of its diminished oxidizing power, [TcO4]− is stable in alkaline solution. [TcO4]− is more similar to ReO4−. Depending of the reducing agent, [TcO4]− can be converted to derivatives containing Tc(VI), Tc(V), and Tc(IV).[3] In the absence of strong complexing ligands, TcO4− is reduced to a +4 oxidation state via the formation of TcO2 hydrate.[1]

[edit] Pharmaceutical use

The half-life of 99mTc is long enough that labelling synthesis of the radiopharmaceutical and scintigraphic measurements can be performed without significant loss of radioactivity.[1] The energy emitted from 99mTc is 140 keV, which allows for the study of deep body organs. Radiopharmaceuticals have no intended pharmacologic effect and are used in very low concentrations. Radiopharmaceuticals containing 99mTc are currently being applied in the determining morphology of organs, testing of organ function, and scintigraphic and emission tomographic imaging. The gamma radiation emitted by the radionuclide allows organs to be imaged in vivo tomographically. Currently, over 80% of radiopharmaceuticals used clinically are labelled with 99mTc. A majority of radiopharmaceuticals labelled with 99mTc are synthesized by the reduction of the pertechnetate ion in the presence of ligands chosen to confer organ specificity of the drug. The resulting 99mTc compound is then injected into the body and a "gamma camera" is focused on sections or planes in order to image the spacial distribution of the 99mTc.

[edit] Specific imaging applications

99mTc is used primarily in the study of the thyroid gland - its morphology, vascularity, and function. [TcO4]− and iodide, due to their comparable charge/radius ratio, are similarly incorporated into the thyroid gland. The pertechnetate ion is not incorporated into the thyroglobulin. It is also used in the study of blood perfusion, regional accumulation, and cerebral lesions in the brain, as it accumulates primarily in the choroid plexus.

Sodium pertechnetate cannot pass through the blood-brain barrier. In addition to the salivary and thyroid glands, 99mTcO4− localizes in the stomach. 99mTcO4− is renally eliminated for the first three days after being injected. After a scanning is performed, it is recommended that a patient drink large amounts of water in order to expedite elimination of the radionuclide.[4] Other methods of 99mTcO4− administration include intraperitoneal, intramuscular, subcutaneous, as well as orally. The behavior of the 99mTcO4− ion is essentially the same, with small differences due to the difference in rate of absorption, regardless of the method of administration.[5]

Other examples of organ-specific radiopharmaceuticals include:

[edit] Preparation of 99mTcO4-

99mTc is conveniently available in high nuclidic purity from molybdenum-99, which decays with 87% probability to 99mTc. The subsequent decay of 99mTc leads to either 99Tc or 99Rb. 99Mo is obtained in a nuclear reactor via irradiation of either molybdenum-98 or naturally occurring molybdenum with thermal neutrons. 99mTc is also obtained by the fission of 235U or 239Pu,[6] but the isolation of 99mTc requires many steps due to the presence of other fission products and transuranium elements.[1]

Once 99mTc is formed, it can be separated from 99Mo by column chromatography on acidic aluminum oxide as the packing material. At the top of the column is bound 99MoO42−. 99mTcO4− is extracted from the column by washing with a 0.15 M NaCl (" saline solution"). The eluate from the column must be sterile and pyrogen free, so that the Tc drug can be used directly, usually within 12 h of elution.[1] In a few cases, sublimation or solvent extraction may be used.

[edit] Synthesis of 99mTcO4− radiopharmaceuticals

99mTcO4− is advantageous for the synthesis of a variety of radiopharmaceuticals because Tc can adopt a number of oxidation states.[1] The oxidation state and coligands dictate the specificity of the radiopharmaceutical. The starting material Na99mTcO4, made available after elution from the generator column, as mentioned above, can be reduced in the presence of complexing ligands. Many different reducing agents can be used, but transition metal reductants are avoided because they compete with 99mTc for ligands. Oxalates, formates, hydroxylamine, and hydrazine are also avoided because they form complexes with the technetium. Electrochemical reduction is impractical.

Ideally, the synthesis of the desired radiopharmaceutical from 99mTcO4−, a reducing agent, and desired ligands should occur in one container after elution, and the reaction must be performed in a solvent that can be injected intravenously, such as a saline solution. Kits are available that contain the reducing agent, usually tin(II) and ligands. These kits are sterile, pyrogen-free, easily purchased, and can be stored for long periods of time. The reaction with 99mTcO4− takes place directly after elution from the generator column and shortly before its intended use. A high organ specificity is important because the injected activity should accumulate in the organ under investigation, as there should be a high activity ratio of the target organ to nontarget organs. If there is a high activity in organs adjacent to the one under investigation, the image of the target organ can be obscured. Also, high organ specificity allows for the reduction of the injected activity, and thus the exposure to radiation, in the patient. The radiopharmaceutical must be kinetically inert, in that it must not change chemically in vivo en route to the target organ.

[edit] Examples

  • A complex that can penetrate the blood-brain barrier is generated by reduction of 99mTcO4− with tin(II) in the presence of the ligand "d,l-HM-PAO" to form TcO-d,l-HM-PAO (HM-PAO is hexamethylpropyleneamino oxime).
  • A complex that for imaging the lungs, "Tc-MAA," is generated by reduction of 99mTcO4- with SnCl2 in the presence of human serum albumin.
  • [99mTc(OH2)3(CO)3]+, which is both water and air stable, is generated by reduction of 99mTcO4− with carbon monoxide. This compound is a precursor to complexes that can be used in cancer diagnosis and therapy involving DNA-DNA pretargeting.[7]

[edit] Other reactions involving the pertechnetate ion

  • Radiolysis of TcO4− in nitrate solutions proceeds through the reduction to TcO42− which induces complex disproportionation processes:
TcO4− + eaq− → TcO42−
2 TcO42− → TcO4− + Tc(V)
2 Tc(V) → TcO42− + Tc(IV)
Tc(V) + TcO42− → Tc(IV) + TcO4−
  • Pertechnetate can be reduced by H2S to give Tc2S7.10
  • Pertechnetate is also be reduced to Tc(IV/V) compounds in alkaline solutions in nuclear waste tanks without adding catalytic metals, reducing agents, or external radiation. Reactions of mono- and disaccharides with 99mTcO4− yield Tc(IV) compounds that are water soluble.[8]

[edit] References

  1. ^ a b c d e f g Schwochau, K. (1994). "Technetium Radiopharmaceuticals-Fundamentals, Synthesis, Structure, and Development". Angew. Chem. Int. Ed. Engl. 33: 2258-2267. doi:10.1002/anie.199422581. 
  2. ^ Wells, A. F.; Structural Inorganic Chemistry; Clarendon Press: Oxford, Great Britain; 1984; p. 1050.
  3. ^ Encyclopedia Britannica: Technetium
  4. ^ Shukla, S. K., Manni, G. B., and Cipriani, C. (1977). "The Behaviour of the Pertechnetate Ion in Humans". Journal of Chromatography 143 (5): 522-526. PMID 893641. 
  5. ^ Razzak, M. A., Naguib, M., and El-Garhy, M. (1967) Fate of Sodium Pertechnetate-Technetium-99m. Journal of Nuclear Medicine, 8, 50-59.
  6. ^ Beasley, T. M., Palmer, H. E., and Nelp, W. B. (1966). "Distriubtion and Excretion of Technetium in Humans". Health Physics 12 (10): 1425-1435. 
  7. ^ R. Alberto, R. Schibli, A. Egli, A. P. Schubiger, U. Abram and T. A. Kaden (1998). "A Novel Organometallic Aqua Complex of Technetium for the Labeling of Biomolecules: Synthesis of [99mTc(OH2)3(CO)3]+ from [99mTcO4]− in Aqueous Solution and Its Reaction with a Bifunctional Ligand". J. Am. Chem. Soc. 120 (31): 7987-7988. doi:10.1021/ja980745t. 
  8. ^ D. E. Berning, N. C. Schroeder and R. M. Chamberlin (2005). "The autoreduction of pertechnetate in aqueous, alkaline solutions". Journal of Radioanalytical and Nuclear Chemistry 263: 613-618. doi:10.1007/s10967-005-0632-x.