Search results
Results From The WOW.Com Content Network
This is a list of radioactive nuclides (sometimes also called isotopes), ordered by half-life from shortest to longest, in seconds, minutes, hours, days and years. Current methods make it difficult to measure half-lives between approximately 10 −19 and 10 −10 seconds.
The biological half-life of curium is about 20 years in the liver and 50 years in the bones. [52] [54] Curium is absorbed in the body much more strongly via inhalation, and the allowed total dose of 244 Cm in soluble form is 0.3 μCi. [13]
The longest-lived isotope is 247 Cm, with half-life 15.6 million years – orders of magnitude longer than that of any known isotope beyond curium, and long enough to study as a possible extinct radionuclide that would be produced by the r-process. [2] [3] The longest-lived known isomer is 246m Cm with a half-life of 1.12 seconds.
Plutonium-238, curium-242, curium-244 and strontium-90 have been used. [31] Besides the nuclear properties of the used isotope, there are also the issues of chemical properties and availability. A product deliberately produced via neutron irradiation or in a particle accelerator is more difficult to obtain than a fission product easily ...
Curium-250 is the isotope with the lowest atomic number that primarily decays by spontaneous fission, a process that releases many times more energy than alpha decay. Compared to plutonium-238, curium-250 provides about a quarter of the power density, but 95 times the half-life (~8300 years vs. ~87 years).
The isobar forming 132 Te/ 132 I is: Tin-132 (half-life 40 s) decaying to antimony-132 (half-life 2.8 minutes) decaying to tellurium-132 (half-life 3.2 days) decaying to iodine-132 (half-life 2.3 hours) which decays to stable xenon-132. The creation of tellurium-126 is delayed by the long half-life (230 k years) of tin-126.
Global shortages of nuclear chemical needed for cancer scans will see patients’ appointments cancelled, minister warns
The resulting complexes show strong yellow-orange emission under UV light excitation, which is convenient not only for their detection, but also for studying interactions between the Cm 3+ ion and the ligands via changes in the half-life (of the order ~0.1 ms) and spectrum of the fluorescence.