Boiling point of caesium11/13/2023 Long exposure can even cause coma or death. Due to this, nausea, vomiting, and bleeding may occur. Radioactivity: If a person comes in contact with a radioactive isotope of caesium then cell-damage may occur. Its advantages are that it has a half-life of 30 years and it has barium-137 as a stable end product. Nuclear application: Caesium-137 is used as a gamma emitter in industrial applications.Molecular Biology: High density caesium compound solutions such as caesium chloride, caesium sulfate, etc are used in density gradient ultracentrifugation.Atomic-clocks: They use the electromagnetic transition in the hyperfine structure of caesium-133 atoms as the reference point.It also helps bring rock cuttings to the surface and to maintain pressure on the formation during drilling of the well. The main function of drilling fluids is to lubricate drill bits. Petroleum exploration: The largest use of caesium is as a drilling fluid for extractive oil and petroleum industry. Relevance in Chemical and Related Industries This precipitated double salt is then decomposed and the water is evaporated to obtain pure caesium chloride. The grounded ore is dissolved in strong acids which leads to formation of caesium double salts. The caesium is extracted from pollucite mainly by acid digestion. The ore is crushed, hand-sorted, and then grounded. Caesium forms variety of compounds including variety of halides and oxides.įrom Pollucite: The mining and refining of pollucite is a selective process hence it is done on a smaller scale.Caesium can only be handled under inert atmosphere.It even reacts with ice whose temperature is as low as -116☌. It reacts explosively with water even at low temperatures. Caesium is pyrophyric in nature, which means that it spontaneously ignites in air.Among them, the only stable isotope is caesium-139. Caesium is softest among all metals which are solid at room temperature.The density of caesium is 1900 in S.I.Caesium is a soft metal which shines in gold colour.It is a relatively rare element and makes up 3 ppm of Earth’s crust. Also, throw light on the applications of Cs-137 in today’s world.Caesium is found in minerals pollucite and lepidolite. Due to its long half-life, Caesium-137 is most significant nuclide for the radiation exposure of the population after a nuclear accident. This may occur after nuclear accidents or detonation of atomic bombs. High levels of radioactive cesium in body can cause nausea, vomiting, diarrhea, bleeding, coma, and even death.Exposure to Cs-137 can increase the risk for cancer because of exposure to high-energy gamma radiation.External exposure to large amounts of Cs-137 can cause burns, acute radiation sickness.In larger amounts, Cs-137 is used in medical radiation therapy devices for treating cancer in industrial gauges that detect the flow of liquid through pipes and in other industrial devices to measure the thickness of materials, such as paper, photographic film, or sheets of metal. Cs-137 is produced by nuclear fission for use in medical devices and gauges.Caesium-137 has a half-life of approximately 30 years, which means that after a period of 30 years, the amount of Cs-137 will have halved due to radioactive decay.A Cs-137 atom emits radiation in the form of medium-energy gamma rays, and to a lesser extent, high-energy beta particles.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.With atomic explosions, it can travel very long distances in the air. Caesium-137 has a relatively low boiling pointof 671 ☌ and is volatilized easily when released suddenly at high temperature, as in the case of the Chernobyl Nuclear Accident.Caesium-137 was discovered by Glenn T.Cs- 137 is also one of the byproducts of nuclear fission processes in nuclear reactors and nuclear weapons testing.The most common radioactive form of cesium is Cesium-137 (Cs-137). Atomic Mass: Atomic mass number given for longest lived isotope.
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