 | |
| General | |
|---|---|
| Symbol | 129I |
| Names | iodine-129, 129I, I-129 |
| Protons(Z) | 53 |
| Neutrons(N) | 76 |
| Nuclide data | |
| Natural abundance | Trace |
| Half-life(t1/2) | 1.614(12)×107 years[1] |
| Isotope mass | 128.9049836(34)[2]Da |
| Decay products | 129Xe |
| Decay modes | |
| Decay mode | Decay energy (MeV) |
| β− | 0.189 |
| Isotopes of iodine Complete table of nuclides | |
Iodine-129 (129I) is a long-livedradioisotope ofiodine that occurs naturally but is also of special interest in the monitoring and effects of man-made nuclearfission products, where it serves as both a tracer and a potential radiological contaminant.
| Nuclide | t1⁄2 | Yield | Q[a 1] | βγ |
|---|---|---|---|---|
| (Ma) | (%)[a 2] | (keV) | ||
| 99Tc | 0.211 | 6.1385 | 294 | β |
| 126Sn | 0.230 | 0.1084 | 4050[a 3] | βγ |
| 79Se | 0.327 | 0.0447 | 151 | β |
| 135Cs | 1.33 | 6.9110[a 4] | 269 | β |
| 93Zr | 1.53 | 5.4575 | 91 | βγ |
| 107Pd | 6.5 | 1.2499 | 33 | β |
| 129I | 16.14 | 0.8410 | 194 | βγ |
129I is one of sevenlong-lived fission products. It is primarily formed from thefission ofuranium andplutonium innuclear reactors. Significant amounts were released into theatmosphere bynuclear weapons testing in the 1950s and 1960s, bynuclear reactor accidents and by both military and civil reprocessing of spent nuclear fuel.[3]
It is also naturally produced in small quantities, due to thespontaneous fission ofnatural uranium, bycosmic ray spallation of trace levels ofxenon in the atmosphere, and bycosmic raymuons strikingtellurium-130.[4][5]
129I decays with ahalf-life of 16.14 million years, with low-energybeta andgamma emissions, to stablexenon-129 (129Xe).[6]
129I is one of the sevenlong-lived fission products that are produced in significant amounts. Its yield is 0.706% per fission of235U.[7] Larger proportions of other iodine isotopes such as131I are produced, but because these all have short half-lives, iodine in cooledspent nuclear fuel consists of about 5/6129I and 1/6 the only stable iodine isotope,127I.
Because129I is long-lived and relatively mobile in the environment, it is of particular importance in long-term management of spent nuclear fuel. In adeep geological repository for unreprocessed used fuel,129I is likely to be the radionuclide of most potential impact at long times.
Since129I has a modestneutron absorptioncross-section of 30 barns,[8] and is relatively undiluted by other isotopes of the same element, it is being studied for disposal bynuclear transmutation by re-irradiation withneutrons[9] or gamma irradiation.[10]
| Thermal | Fast | 14 MeV | |
|---|---|---|---|
| 232Th | notfissile | 0.431 ± 0.089 | 1.68 ± 0.33 |
| 233U | 1.63 ± 0.26 | 1.73 ± 0.24 | 3.01 ± 0.43 |
| 235U | 0.706 ± 0.032 | 1.03 ± 0.26 | 1.59 ± 0.18 |
| 238U | notfissile | 0.622 ± 0.034 | 1.66 ± 0.19 |
| 239Pu | 1.407 ± 0.086 | 1.31 ± 0.13 | ? |
| 241Pu | 1.28 ± 0.36 | 1.67 ± 0.36 | ? |
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A large fraction of the129I contained in spent fuel is released into the gas phase, when spent fuel is first chopped and then dissolved in boilingnitric acid during reprocessing.[3] At least for civil reprocessing plants, special scrubbers are supposed to withhold 99.5% (or more) of the Iodine by adsorption,[3] before exhaust air is released into the environment. However, the Northeastern Radiological Health Laboratory (NERHL) found, during their measurements at the first US civil reprocessing plant, which was operated byNuclear Fuel Services, Inc. (NFS) in Western New York, that "between 5 and 10% of the total129I available from the dissolved fuel" was released into the exhaust stack.[3] They further wrote that "these values are greater than predicted output (Table 1). This was expected since the iodine scrubbers were not operating during the dissolution cycles monitored."[3]
The Northeastern Radiological Health Laboratory further states that, due to limitations of their measuring systems, the actual release of129I may have even been higher, "since [129I] losses [by adsorption] probably occurred in the piping and ductwork between the stack and the sampler".[3] Furthermore, the sample taking system used by the NERHL had a bubbler trap for measuring thetritium content of the gas samples before the iodine trap. The NERHL found out only after taking the samples that "the bubbler trap retained 60 to 90% of the129I sampled".[3] NERHL concluded: "The bubblers located upstream of the ion exchangers removed a major portion of the gaseous129I before it reached the ion exchange sampler. The iodine removal ability of the bubbler was anticipated, but not in the magnitude that it occurred." The documented release of "between 5 and 10% of the total129I available from the dissolved fuel"[3] is not corrected for those two measurement deficiencies.
Military isolation of plutonium from spent fuel has also released129I to the atmosphere: "More than 685,000 curies of iodine 131 spewed from the stacks of Hanford's separation plants in the first three years of operation."[11] As129I and131I have very similar physical and chemical properties, and no isotope separation was performed at Hanford,129I must have also been released there in large quantities during the Manhattan project. As Hanford reprocessed "hot" fuel, that had been irradiated in a reactor only a few months earlier, the activity of the released short-lived131I, with a half-life time of just 8 days, was much higher than that of the long-lived129I. However, while all of the131I released during the times of the Manhattan project has decayed by now, over 99.999% of the129I is still in the environment.
Ice borehole data obtained from the university of Bern at the Fiescherhorn glacier in the Alpian mountains at a height of 3950 m show a somewhat steady increase in the129I deposit rate (shown in the image as a solid line) with time. In particular, the highest values obtained in 1983 and 1984 are about six times as high as the maximum that was measured during the period of the atmospheric bomb testing in 1961. This strong increase following the conclusion of the atmospheric bomb testing indicates that nuclear fuel reprocessing has been the primary source of atmospheric iodine-129 since then. These measurements lasted until 1986.[12]
129I is not deliberately produced for any practical purposes. However, its long half-life and its relative mobility in the environment have made it useful for a variety of dating applications. These include identifying older groundwaters based on the amount of natural129I (or its129Xe decay product) present, as well as identifying younger groundwaters by the increased anthropogenic129I levels since the 1960s.[13][14][15]
In 1960, physicistJohn H. Reynolds discovered that certainmeteorites contained an isotopic anomaly in the form of an overabundance of129Xe. He inferred that this must be adecay product of long-decayed radioactive129I. This isotope is produced in quantity in nature only insupernova explosions. As the half-life of129I is comparatively short in astronomical terms, this demonstrated that only a short time had passed between the supernova and the time the meteorites had solidified and trapped the129I. These two events (supernova and solidification of gas cloud) were inferred to have happened during the early history of theSolar System, as the129I isotope was likely generated before the Solar System was formed, but not long before, and seeded the solar gas cloud isotopes with isotopes from a second source. This supernova source may also have caused collapse of the solar gas cloud.[16][17]