Topics: Radionuclide, Ionizing radiation, Radioactive decay Pages: 24 (9133 words) Published: April 1, 2013
adioisotopes: What Are They and How Are They Made?What are isotopes?The isotopes of an element are all the atoms that have in their nucleus the number of protons (atomic number) corresponding to the chemical behavior of that element. However, the isotopes of a single element vary in the number of neutrons in their nuclei. Since they still have the same number of protons, all these isotopes of an element have identical chemical behavior. But since they have different numbers of neutrons, these isotopes of the same element may have different radioactivity. An isotope that is radioactive is called a radioisotope or radionuclide. Two examples may help clarify this.The most stable isotope of uranium, U-238, has an atomic number of 92 (protons) and an atomic weight of 238 (92 protons plus 146 neutrons). The isotope of uranium of greatest importance in atomic bombs, U-235, though, has three fewer neutrons. Thus, it also has an atomic number of 92 (since the number of protons has not changed) but an atomic weight of 235 (92 protons plus only 143 neutrons). The chemical behavior of U-235 is identical to all other forms of uranium, but its nucleus is less stable, giving it higher radioactivity and greater susceptibility to the chain reactions that power both atomic bombs and nuclear fission reactors. Another example is iodine, an element essential for health; insufficient iodine in one's diet can lead to a goiter. Iodine also is one of the earliest elements whose radioisotopes were used in what is now called nuclear medicine. The most common, stable form of iodine has an atomic number of 53 (protons) and an atomic weight of 127 (53 protons plus 74 neutrons). Because its nucleus has the "correct" number of neutrons, it is stable and is not radioactive. A less stable form of iodine also has 53 protons (this is what makes it behave chemically as iodine) but four extra neutrons, for a total atomic weight of 131 (53 protons and 78 neutrons). With "too many" neutrons in its nucleus, it is unstable and radioactive, with a half-life of eight days. Because it behaves chemically as iodine, it travels throughout the body and localizes in the thyroid gland just like the stable form of iodine. But, because it is radioactive, its presence can be detected. Iodine 131 thus became one of the earliest radioactive tracers.How can different isotopes of an element be produced?How can isotopes be produced--especially radioisotopes, which can serve many useful purposes? There are two basic methods: separation and synthesis.Some isotopes occur in nature. If radioactive, these usually are radioisotopes with very long half-lives. Uranium 235, for example, makes up about 0.7 percent of the naturally occurring uranium on the earth.[89] The challenge is to separate this very small amount from the much larger bulk of other forms of uranium. The difficulty is that all these forms of uranium, because they all have the same number of electrons, will have identical chemical behavior: they will bind in identical fashion to other atoms. Chemical separation, developing a chemical reaction that will bind only uranium atoms, will separate out uranium atoms, but not distinguish among different isotopes of uranium. The only difference among the uranium isotopes is their atomic weight. A method had to be developed that would sort atoms according to weight. One initial proposal was to use a centrifuge. The basic idea is simple: spin the uranium atoms as if they were on a very fast merry-go-round. The heavier ones will drift toward the outside faster and can be drawn off. In practice the technique was an enormous challenge: the goal was to draw off that very small portion of uranium atoms that were lighter than their brethren. The difficulties were so enormous the plan was abandoned in 1942.[90] Instead, the technique of gaseous diffusion was developed. Again, the basic idea was very simple: the rate at which gas passed (diffused) through a filter depended on the weight of the...

References: Barium-133 | 9694 TBq/Kg (262 Ci/g) | 10.7 years | 81.0, 356.0 |
Cadmium-109 | 96200 TBq/Kg (2600 Ci/g) | 453 days | 88.0 |
Cobalt-57 | 312280 TBq/Kg (8440 Ci/g) | 270 days | 122.1 |
Cobalt-60 | 40700 TBq/Kg (1100 Ci/g) | 5.27 years | 1173.2, 1332.5 |
Europium-152 | 6660 TBq/Kg (180 Ci/g) | 13.5 years | 121.8, 344.3, 1408.0 |
Manganese-54 | 287120 TBq/Kg (7760 Ci/g) | 312 days | 834.8 |
Sodium-22 | 237540 Tbq/Kg (6240 Ci/g) | 2.6 years | 511.0, 1274.5 |
Zinc-65 | 304510 TBq/Kg (8230 Ci/g) | 244 days | 511.0, 1115.5 |
Tritium (Hydrogen-3) | 357050 TBq/Kg (9650 Ci/g) | 12.32 years | 5.7 (average) |
Alpha emission only
Isotope | Activity | Half-life | Energies (KeV) |
Polonium-210 | 166500 TBq/Kg (4500 Ci/g) | 138 days | 5304.5 |
Isotope | Activity | Half-life | Radiation types | Energies (KeV) |
Caesium-137 | 3256 TBq/Kg (88 Ci/g) | 30.1 years | Gamma & beta | G: 32, 661.6 B: 511.6, 1173.2 |
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