Synthetic radioisotope

A synthetic radioisotope is a radionuclide that is not found in nature: no natural process or mechanism exists which produces it, or it is so unstable that it decays away in a very short period of time. Examples include technetium-95 and promethium-146. Many of these are found in, and harvested from, spent nuclear fuel assemblies. Some must be manufactured in particle accelerators.

Production

Some synthetic radioisotopes are extracted from spent nuclear reactor fuel rods, which contain various fission products. For example, it is estimated that up to 1994, about 49,000 terabecquerels (78 metric ton) of technetium was produced in nuclear reactors, which is by far the dominant source of terrestrial technetium.[1]

Some synthetic isotopes are produced in significant quantities by fission but are not yet being reclaimed. Other isotopes are manufactured by neutron irradiation of parent isotopes in a nuclear reactor (for example, Tc-97 can be made by neutron irradiation of Ru-96) or by bombarding parent isotopes with high energy particles from a particle accelerator.[2][3]

Many isotopes are produced in cyclotrons, for example fluorine-18 and oxygen-15 which are widely used for positron emission tomography.[4]

Uses

Most synthetic radioisotopes have a short half-life. Though a health hazard, radioactive materials have many medical and industrial uses.

Nuclear medicine

The field of nuclear medicine covers use of radioisotopes for diagnosis or treatment.

Diagnosis

Radioactive tracer compounds, radiopharmaceuticals, are used to observe the function of various organs and body systems. These compounds use a chemical tracer which is attracted to or concentrated by the activity which is being studied. That chemical tracer incorporates a short lived radioactive isotope, usually one which emits a gamma ray which is energetic enough to travel through the body and be captured outside by a gamma camera to map the concentrations. Gamma cameras and other similar detectors are highly efficient, and the tracer compounds are generally very effective at concentrating at the areas of interest, so the total amounts of radioactive material needed are very small.

The metastable nuclear isomer Tc-99m is a gamma-ray emitter widely used for medical diagnostics because it has a short half-life of 6 hours, but can be easily made in the hospital using a technetium-99m generator. Weekly global demand for the parent isotope molybdenum-99 was 440 TBq (12,000 Ci) in 2010, overwhelmingly provided by fission of uranium-235.[5]

Treatment

Several radioisotopes and compounds are used for medical treatment, usually by bringing the radioactive isotope to a high concentration in the body near a particular organ. For example, iodine-131 is used for treating some disorders and tumors of the thyroid gland.

Industrial radiation sources

Alpha particle, beta particle, and gamma ray radioactive emissions are industrially useful. Most sources of these are synthetic radioisotopes. Areas of use include the petroleum industry, industrial radiography, homeland security, process control and food irradiation.[6][7][8]

Footnotes

  1. ^ Yoshihara, K (1996). "Technetium in the environment". In Yoshihara, K; Omori, T (eds.). Technetium and Rhenium Their Chemistry and Its Applications. Topics in Current Chemistry. 176. Springer. doi:10.1007/3-540-59469-8_2. ISBN 978-3-540-59469-7.
  2. ^ "Radioisotope Production". Brookhaven National Laboratory. 2009. Archived from the original on 6 January 2010.CS1 maint: BOT: original-url status unknown (link)
  3. ^ Manual for reactor produced radioisotopes. Vienna: IAEA. 2003. ISBN 92-0-101103-2.
  4. ^ Cyclotron Produced Radionuclides: Physical Characteristics and Production Methods. Vienna: IAEA. 2009. ISBN 978-92-0-106908-5.
  5. ^ "Production and Supply of Molybdenum-99" (PDF). IAEA. 2010. Retrieved 4 March 2018.
  6. ^ Greenblatt, Jack A. (2009). "Stable and Radioactive Isotopes: Industry & Trade Summary" (PDF). Office of Industries. United States International Trade Commission.
  7. ^ Rivard, Mark J.; Bobek, Leo M.; Butler, Ralph A.; Garland, Marc A.; Hill, David J.; Krieger, Jeanne K.; Muckerheide, James B.; Patton, Brad D.; Silberstein, Edward B. (August 2005). "The US national isotope program: Current status and strategy for future success" (PDF). Applied Radiation and Isotopes. 63 (2): 157–178. doi:10.1016/j.apradiso.2005.03.004.
  8. ^ Branch, Doug (2012). "Radioactive Isotopes in Process Measurement" (PDF). VEGA Controls. Retrieved 4 March 2018.

External links

Gallium

Gallium is a chemical element with symbol Ga and atomic number 31. Gallium in its solid state is slightly blue; however in its liquid state it becomes silvery white. Gallium is soft enough to be cut with shears however; if too much force is applied Gallium may fracture conchoidally. It is in group 13 of the periodic table, and thus has similarities to the other metals of the group, aluminium, indium, and thallium. Gallium does not occur as a free element in nature, but as gallium(III) compounds in trace amounts in zinc ores and in bauxite. Elemental gallium is a liquid at temperatures greater than 29.76 °C (85.57 °F) (above room temperature, but below the normal human body temperature of 37 °C (99 °F), hence, the metal will melt in a person's hands).

The melting point of gallium is used as a temperature reference point. Gallium alloys are used in thermometers as a non-toxic and environmentally friendly alternative to mercury, and can withstand higher temperatures than mercury. The alloy galinstan (70% gallium, 21.5% indium, and 10% tin) has an even lower melting point of −19 °C (−2 °F), well below the freezing point of water.

Since its discovery in 1875, gallium has been used to make alloys with low melting points. It is also used in semiconductors as a dopant in semiconductor substrates.

Gallium is predominantly used in electronics. Gallium arsenide, the primary chemical compound of gallium in electronics, is used in microwave circuits, high-speed switching circuits, and infrared circuits. Semiconducting gallium nitride and indium gallium nitride produce blue and violet light-emitting diodes (LEDs) and diode lasers. Gallium is also used in the production of artificial gadolinium gallium garnet for jewelry. Gallium is considered a technology-critical element.

Gallium has no known natural role in biology. Gallium(III) behaves in a similar manner to ferric salts in biological systems and has been used in some medical applications, including pharmaceuticals and radiopharmaceuticals.

Index of chemistry articles

Chemistry (from Egyptian kēme (chem), meaning "earth") is the physical science concerned with the composition, structure, and properties of matter, as well as the changes it undergoes during chemical reactions.Below is a list of chemistry-related articles. Chemical compounds are listed separately at list of organic compounds, list of inorganic compounds or list of biomolecules.

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