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Caesium-137 AI simulator
(@Caesium-137_simulator)
Hub AI
Caesium-137 AI simulator
(@Caesium-137_simulator)
Caesium-137
Caesium-137 (137
55Cs), cesium-137 (US), or radiocaesium, is a radioactive isotope of caesium that is formed as one of the more common fission products by the nuclear fission of uranium-235 and other fissionable isotopes in nuclear reactors and nuclear weapons. Trace quantities also originate from spontaneous fission of uranium-238. It is among the most problematic of the short-to-medium-lifetime fission products. Caesium has a relatively low boiling point of 671 °C (1,240 °F) and easily becomes volatile when released suddenly at high temperature, as in the case of the Chernobyl nuclear accident and with nuclear explosions, and can travel very long distances in the air. After being deposited onto the soil as radioactive fallout, it moves and spreads easily in the environment because of the high water solubility of caesium's most common chemical compounds, which are salts. Caesium-137 was discovered by Glenn T. Seaborg and Margaret Melhase.
Caesium-137 has a half-life of about 30.04 years, decaying by beta emission to stable barium-137. About 94.6% of the decays go to a metastable nuclear isomer of barium: barium-137m (137m
Ba) and the remainder directly to the ground state. Barium-137m has a half-life of about 153 seconds, its dropping to the ground state usually (85.1% of all Cs-137 decays) emitting photons having energy 0.6617 MeV. This is responsible for all of the gamma ray emissions in samples of 137
Cs.
Caesium-137 has a number of practical uses. In small amounts, it is used to calibrate radiation-detection equipment. In medicine, it is used in radiation therapy. In industry, it is used in flow meters, thickness gauges, moisture-density gauges (for density readings, with americium-241/beryllium providing the moisture reading), and in borehole logging devices.
Caesium-137 is not widely used for industrial radiography because it is hard to obtain a very high specific activity material with a well defined (and small) shape, as caesium from used nuclear fuel contains stable caesium-133 and also long-lived caesium-135. Isotope separation is too costly compared to cheaper alternatives. Also, the higher specific activity caesium sources tend to be made from highly soluble caesium chloride (CsCl); as a result, if a radiography source were to be damaged, the risk of radioactive contamination is high. It is possible to make water-insoluble caesium sources (with ferrocyanides, for example) but their specific activity will be lower. Other chemically inert caesium compounds include caesium-aluminosilicate-glasses akin to the natural mineral pollucite. The latter has been used in demonstrations of chemically stable water-insoluble forms of nuclear waste for disposal in deep geological repositories. A large emitting volume will harm the image quality in radiography. The isotopes 192
Ir and 60
Co are preferred for radiography, since iridium and cobalt are chemically non-reactive metals and can be obtained with much higher specific activities by the activation of stable 191
Ir and 59
Co in high-flux reactors. However, while 137
Cs is a waste product produced in great quantities in nuclear fission reactors, 192
Ir and 60
Co are specifically produced in commercial and research reactors and their life cycle entails the destruction of the involved high-value elements. Cobalt-60 decays to stable nickel, whereas iridium-192 can decay to either stable osmium or platinum. Due to the residual radioactivity and legal hurdles, the resulting material is not commonly recovered even from "spent" radioactive sources, meaning in essence that the entire mass is "lost" for non-radioactive uses.
As an almost purely synthetic isotope not existing in the environment before 1945, caesium-137 has been used to date wine and detect counterfeits and as a relative-dating material for assessing the age of sedimentation occurring after 1945.
Caesium-137 is also used as a radioactive tracer in geologic research to measure soil erosion and deposition; its affinity for fine sediments is useful in this application.
The biological behaviour of caesium is similar to that of potassium and rubidium. After entering the body, caesium gets more or less uniformly distributed throughout the body, with the highest concentrations in soft tissue. However, unlike group 2 radionuclides like radium and strontium-90, caesium does not bioaccumulate and is excreted relatively quickly. The biological half-life of caesium is about 70 days.
A 1961 experiment showed that mice dosed with 21.5 μCi/g of 137
Cs had a 50% fatality rate within 30 days, implying an LD50 of 245 μg/kg. A similar experiment in 1972 showed that when dogs are subjected to a whole body burden of 3800 μCi/g (140 MBq/kg, or approximately 44 μg/kg) of caesium-137 (and 950 to 1400 rad), they die within 33 days, while animals with half of that burden all survived for a year. A 1960 mouse study found there were high levels of Cs-137 for the first day after exposure in the mucus glands of the colon, the pancreas, cartilage, tendons, and skeletal muscle. After 24 hours, cartilage and skeletal muscle showed the highest activity.
Caesium-137
Caesium-137 (137
55Cs), cesium-137 (US), or radiocaesium, is a radioactive isotope of caesium that is formed as one of the more common fission products by the nuclear fission of uranium-235 and other fissionable isotopes in nuclear reactors and nuclear weapons. Trace quantities also originate from spontaneous fission of uranium-238. It is among the most problematic of the short-to-medium-lifetime fission products. Caesium has a relatively low boiling point of 671 °C (1,240 °F) and easily becomes volatile when released suddenly at high temperature, as in the case of the Chernobyl nuclear accident and with nuclear explosions, and can travel very long distances in the air. After being deposited onto the soil as radioactive fallout, it moves and spreads easily in the environment because of the high water solubility of caesium's most common chemical compounds, which are salts. Caesium-137 was discovered by Glenn T. Seaborg and Margaret Melhase.
Caesium-137 has a half-life of about 30.04 years, decaying by beta emission to stable barium-137. About 94.6% of the decays go to a metastable nuclear isomer of barium: barium-137m (137m
Ba) and the remainder directly to the ground state. Barium-137m has a half-life of about 153 seconds, its dropping to the ground state usually (85.1% of all Cs-137 decays) emitting photons having energy 0.6617 MeV. This is responsible for all of the gamma ray emissions in samples of 137
Cs.
Caesium-137 has a number of practical uses. In small amounts, it is used to calibrate radiation-detection equipment. In medicine, it is used in radiation therapy. In industry, it is used in flow meters, thickness gauges, moisture-density gauges (for density readings, with americium-241/beryllium providing the moisture reading), and in borehole logging devices.
Caesium-137 is not widely used for industrial radiography because it is hard to obtain a very high specific activity material with a well defined (and small) shape, as caesium from used nuclear fuel contains stable caesium-133 and also long-lived caesium-135. Isotope separation is too costly compared to cheaper alternatives. Also, the higher specific activity caesium sources tend to be made from highly soluble caesium chloride (CsCl); as a result, if a radiography source were to be damaged, the risk of radioactive contamination is high. It is possible to make water-insoluble caesium sources (with ferrocyanides, for example) but their specific activity will be lower. Other chemically inert caesium compounds include caesium-aluminosilicate-glasses akin to the natural mineral pollucite. The latter has been used in demonstrations of chemically stable water-insoluble forms of nuclear waste for disposal in deep geological repositories. A large emitting volume will harm the image quality in radiography. The isotopes 192
Ir and 60
Co are preferred for radiography, since iridium and cobalt are chemically non-reactive metals and can be obtained with much higher specific activities by the activation of stable 191
Ir and 59
Co in high-flux reactors. However, while 137
Cs is a waste product produced in great quantities in nuclear fission reactors, 192
Ir and 60
Co are specifically produced in commercial and research reactors and their life cycle entails the destruction of the involved high-value elements. Cobalt-60 decays to stable nickel, whereas iridium-192 can decay to either stable osmium or platinum. Due to the residual radioactivity and legal hurdles, the resulting material is not commonly recovered even from "spent" radioactive sources, meaning in essence that the entire mass is "lost" for non-radioactive uses.
As an almost purely synthetic isotope not existing in the environment before 1945, caesium-137 has been used to date wine and detect counterfeits and as a relative-dating material for assessing the age of sedimentation occurring after 1945.
Caesium-137 is also used as a radioactive tracer in geologic research to measure soil erosion and deposition; its affinity for fine sediments is useful in this application.
The biological behaviour of caesium is similar to that of potassium and rubidium. After entering the body, caesium gets more or less uniformly distributed throughout the body, with the highest concentrations in soft tissue. However, unlike group 2 radionuclides like radium and strontium-90, caesium does not bioaccumulate and is excreted relatively quickly. The biological half-life of caesium is about 70 days.
A 1961 experiment showed that mice dosed with 21.5 μCi/g of 137
Cs had a 50% fatality rate within 30 days, implying an LD50 of 245 μg/kg. A similar experiment in 1972 showed that when dogs are subjected to a whole body burden of 3800 μCi/g (140 MBq/kg, or approximately 44 μg/kg) of caesium-137 (and 950 to 1400 rad), they die within 33 days, while animals with half of that burden all survived for a year. A 1960 mouse study found there were high levels of Cs-137 for the first day after exposure in the mucus glands of the colon, the pancreas, cartilage, tendons, and skeletal muscle. After 24 hours, cartilage and skeletal muscle showed the highest activity.
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