A radionuclide (radioactive nuclide, radioisotope or radioactive isotope) is a nuclide that has excess nuclear energy, making it unstable. This excess energy can be used in one of three ways: emitted from the nucleus as gamma radiation; transferred to one of its electrons to release it as a conversion electron; or used to create and emit a new particle (alpha particle or beta particle) from the nucleus. During those processes, the radionuclide is said to undergo radioactive decay. These emissions are considered ionizing radiation because they are energetic enough to liberate an electron from another atom. The radioactive decay can produce a stable nuclide or will sometimes produce a new unstable radionuclide which may undergo further decay. Radioactive decay is a random process at the level of single atoms: it is impossible to predict when one particular atom will decay. However, for a collection of atoms of a single nuclide the decay rate, and thus the half-life (t1/2) for that collection, can be calculated from their measured decay constants. The range of the half-lives of radioactive atoms has no known limits and spans a time range of over 55 orders of magnitude.
Radionuclides occur naturally or are artificially produced in nuclear reactors, cyclotrons, particle accelerators or radionuclide generators. There are about 730 radionuclides with half-lives longer than 60 minutes (see list of nuclides). Thirty-two of those are primordial radionuclides that were created before the Earth was formed. At least another 60 radionuclides are detectable in nature, either as daughters of primordial radionuclides or as radionuclides produced through natural production on Earth by cosmic radiation. More than 2400 radionuclides have half-lives less than 60 minutes. Most of those are only produced artificially, and have very short half-lives. For comparison, there are about 251 stable nuclides. (In theory, only 146 of them are stable, and the other 105 are believed to decay via alpha decay, beta decay, double beta decay, electron capture, or double electron capture.)
All chemical elements can exist as radionuclides. Even the lightest element, hydrogen, has a well-known radionuclide, tritium. Elements heavier than lead, and the elements technetium and promethium, exist only as radionuclides. (In theory, elements heavier than dysprosium exist only as radionuclides, but some such elements, like gold and platinum, are observationally stable and their half-lives have not been determined).
Unplanned exposure to radionuclides generally has a harmful effect on living organisms including humans, although low levels of exposure occur naturally without harm. The degree of harm will depend on the nature and extent of the radiation produced, the amount and nature of exposure (close contact, inhalation or ingestion), and the biochemical properties of the element; with increased risk of cancer the most usual consequence. However, radionuclides with suitable properties are used in nuclear medicine for both diagnosis and treatment. An imaging tracer made with radionuclides is called a radioactive tracer. A pharmaceutical drug made with radionuclides is called a radiopharmaceutical.
On Earth, naturally occurring radionuclides fall into three categories: primordial radionuclides, secondary radionuclides, and cosmogenic radionuclides.
Many of these radionuclides exist only in trace amounts in nature, including all cosmogenic nuclides. Secondary radionuclides will occur in proportion to their half-lives, so short-lived ones will be very rare. For example, polonium can be found in uranium ores at about 0.1 mg per metric ton (1 part in 1010). Further radionuclides may occur in nature in virtually undetectable amounts as a result of rare events such as spontaneous fission or uncommon cosmic ray interactions.
Radionuclides are produced as an unavoidable result of nuclear fission and thermonuclear explosions. The process of nuclear fission creates a wide range of fission products, most of which are radionuclides. Further radionuclides can be created from irradiation of the nuclear fuel (creating a range of actinides) and of the surrounding structures, yielding activation products. This complex mixture of radionuclides with different chemistries and radioactivity makes handling nuclear waste and dealing with nuclear fallout particularly problematic.
Synthetic radionuclides are deliberately synthesised using nuclear reactors, particle accelerators or radionuclide generators:
Radionuclides are used in two major ways: either for their radiation alone (irradiation, nuclear batteries) or for the combination of chemical properties and their radiation (tracers, biopharmaceuticals).
The following table lists properties of selected radionuclides illustrating the range of properties and uses.
|Mode of formation||Comments|
|Tritium (3H)||1||2||12.3 y||β−||19||Cosmogenic||lightest radionuclide, used in artificial nuclear fusion, also used for radioluminescence and as oceanic transient tracer. Synthesized from neutron bombardment of lithium-6 or deuterium|
|Beryllium-10||4||6||1,387,000 y||β−||556||Cosmogenic||used to examine soil erosion, soil formation from regolith, and the age of ice cores|
|Carbon-14||6||8||5,700 y||β−||156||Cosmogenic||used for radiocarbon dating|
|Fluorine-18||9||9||110 min||β+, EC||633/1655||Cosmogenic||positron source, synthesised for use as a medical radiotracer in PET scans.|
|Aluminium-26||13||13||717,000 y||β+, EC||4004||Cosmogenic||exposure dating of rocks, sediment|
|Chlorine-36||17||19||301,000 y||β−, EC||709||Cosmogenic||exposure dating of rocks, groundwater tracer|
|Potassium-40||19||21||1.24×109 y||β−, EC||1330 /1505||Primordial||used for potassium-argon dating, source of atmospheric argon, source of radiogenic heat, largest source of natural radioactivity|
|Calcium-41||20||21||99,400 y||EC||Cosmogenic||exposure dating of carbonate rocks|
|Cobalt-60||27||33||5.3 y||β−||2824||Synthetic||produces high energy gamma rays, used for radiotherapy, equipment sterilisation, food irradiation|
|Krypton-81||36||45||229,000 y||β+||Cosmogenic||groundwater dating|
|Strontium-90||38||52||28.8 y||β−||546||Fission product||medium-lived fission product; probably most dangerous component of nuclear fallout|
|Technetium-99||43||56||210,000 y||β−||294||Fission product||most common isotope of the lightest unstable element, most significant of long-lived fission products|
|Technetium-99m||43||56||6 hr||γ,IC||141||Synthetic||most commonly used medical radioisotope, used as a radioactive tracer|
|Iodine-129||53||76||15,700,000 y||β−||194||Cosmogenic||longest lived fission product; groundwater tracer|
|Iodine-131||53||78||8 d||β−||971||Fission product||most significant short-term health hazard from nuclear fission, used in nuclear medicine, industrial tracer|
|Xenon-135||54||81||9.1 h||β−||1160||Fission product||strongest known "nuclear poison" (neutron-absorber), with a major effect on nuclear reactor operation.|
|Caesium-137||55||82||30.2 y||β−||1176||Fission product||other major medium-lived fission product of concern|
|Gadolinium-153||64||89||240 d||EC||Synthetic||Calibrating nuclear equipment, bone density screening|
|Bismuth-209||83||126||2.01×1019y||α||3137||Primordial||long considered stable, decay only detected in 2003|
|Polonium-210||84||126||138 d||α||5307||Decay product||Highly toxic, used in poisoning of Alexander Litvinenko|
|Radon-222||86||136||3.8 d||α||5590||Decay product||gas, responsible for the majority of public exposure to ionizing radiation, second most frequent cause of lung cancer|
|Thorium-232||90||142||1.4×1010 y||α||4083||Primordial||basis of thorium fuel cycle|
|Uranium-235||92||143||7×108y||α||4679||Primordial||fissile, main nuclear fuel|
|Uranium-238||92||146||4.5×109 y||α||4267||Primordial||Main Uranium isotope|
|Plutonium-238||94||144||87.7 y||α||5593||Synthetic||used in radioisotope thermoelectric generators (RTGs) and radioisotope heater units as an energy source for spacecraft|
|Plutonium-239||94||145||24,110 y||α||5245||Synthetic||used for most modern nuclear weapons|
|Americium-241||95||146||432 y||α||5486||Synthetic||used in household smoke detectors as an ionising agent|
|Californium-252||98||154||2.64 y||α/SF||6217||Synthetic||undergoes spontaneous fission (3% of decays), making it a powerful neutron source, used as a reactor initiator and for detection devices|
Radionuclides are present in many homes as they are used inside the most common household smoke detectors. The radionuclide used is americium-241, which is created by bombarding plutonium with neutrons in a nuclear reactor. It decays by emitting alpha particles and gamma radiation to become neptunium-237. Smoke detectors use a very small quantity of 241Am (about 0.29 micrograms per smoke detector) in the form of americium dioxide. 241Am is used as it emits alpha particles which ionize the air in the detector's ionization chamber. A small electric voltage is applied to the ionized air which gives rise to a small electric current. In the presence of smoke, some of the ions are neutralized, thereby decreasing the current, which activates the detector's alarm.
Radionuclides that find their way into the environment may cause harmful effects as radioactive contamination. They can also cause damage if they are excessively used during treatment or in other ways exposed to living beings, by radiation poisoning. Potential health damage from exposure to radionuclides depends on a number of factors, and "can damage the functions of healthy tissue/organs. Radiation exposure can produce effects ranging from skin redness and hair loss, to radiation burns and acute radiation syndrome. Prolonged exposure can lead to cells being damaged and in turn lead to cancer. Signs of cancerous cells might not show up until years, or even decades, after exposure."
Following is a summary table for the list of 989 nuclides with half-lives greater than one hour. A total of 251 nuclides have never been observed to decay, and are classically considered stable. Of these, 90 are believed to be absolutely stable except to proton decay (which has never been observed), while the rest are "observationally stable" and theoretically can undergo radioactive decay with extremely long half-lives.
The remaining tabulated radionuclides have half-lives longer than 1 hour, and are well-characterized (see list of nuclides for a complete tabulation). They include 30 nuclides with measured half-lives longer than the estimated age of the universe (13.8 billion years), and another four nuclides with half-lives long enough (> 100 million years) that they are radioactive primordial nuclides, and may be detected on Earth, having survived from their presence in interstellar dust since before the formation of the Solar System, about 4.6 billion years ago. Another 60+ short-lived nuclides can be detected naturally as daughters of longer-lived nuclides or cosmic-ray products. The remaining known nuclides are known solely from artificial nuclear transmutation.
Numbers are not exact, and may change slightly in the future, as "stable nuclides" are observed to be radioactive with very long half-lives.
|Stability class||Number of nuclides||Running total||Notes on running total|
|Theoretically stable to all but proton decay||90||90||Includes first 40 elements. Proton decay yet to be observed.|
|Theoretically stable to alpha decay, beta decay, isomeric transition, and double beta decay but not spontaneous fission, which is possible for "stable" nuclides ≥ niobium-93||56||146||All nuclides that are possibly completely stable (spontaneous fission has never been observed for nuclides with mass number < 232).|
|Energetically unstable to one or more known decay modes, but no decay yet seen. All considered "stable" until decay detected.||105||251||Total of classically stable nuclides.|
|Radioactive primordial nuclides.||35||286||Total primordial elements include uranium, thorium, bismuth, rubidium-87, potassium-40, tellurium-128 plus all stable nuclides.|
|Radioactive nonprimordial, but naturally occurring on Earth.||61||347||Carbon-14 (and other isotopes generated by cosmic rays) and daughters of radioactive primordial elements, such as radium, polonium, etc. 41 of these have a half life of greater than one hour.|
|Radioactive synthetic half-life ≥ 1.0 hour). Includes most useful radiotracers.||662||989||These 989 nuclides are listed in the article List of nuclides.|
|Radioactive synthetic (half-life < 1.0 hour).||>2400||>3300||Includes all well-characterized synthetic nuclides.|
This list covers common isotopes, most of which are available in very small quantities to the general public in most countries. Others that are not publicly accessible are traded commercially in industrial, medical, and scientific fields and are subject to government regulation.
|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|
|Technetium-99m||1.95×107 TBq/kg (5.27 × 105 Ci/g)||6 hours||140|
|Strontium-90||5180 TBq/kg (140 Ci/g)||28.5 years||546.0|
|Thallium-204||17057 TBq/kg (461 Ci/g)||3.78 years||763.4|
|Carbon-14||166.5 TBq/kg (4.5 Ci/g)||5730 years||49.5 (average)|
|Tritium (Hydrogen-3)||357050 TBq/kg (9650 Ci/g)||12.32 years||5.7 (average)|
|Polonium-210||166500 TBq/kg (4500 Ci/g)||138.376 days||5304.5|
|Uranium-238||12580 kBq/kg (0.00000034 Ci/g)||4.468 billion years||4267|
|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|
|Americium-241||129.5 TBq/kg (3.5 Ci/g)||432.2 years||Gamma & alpha||G: 59.5, 26.3, 13.9 A: 5485, 5443|