Радиоактивті нуклидтер: тұрақсыздық және ыдырау процесі

Atom that has excess nuclear energy, making it unstable

A radionuclide (radioactive nuclide, radioisotope or radioactive isotope) is a nuclide that has excess numbers of either neutrons or protons, giving it excess nuclear energy, and 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. 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. 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. Radionuclides are produced in stellar nucleosynthesis and supernova explosions along with stable nuclides. Most decay quickly but can still be observed astronomically and can play a part in understanding astronomic processes. Primordial radionuclides, such as uranium and thorium, exist in the present time because their half lives are so long (>100 million years) that they have not yet completely decayed. Some radionuclides have half lives so long (many times the age of the universe) that decay has only recently been detected, and for most practical purposes they can be considered stable, most notably bismuth 209: detection of this decay meant that bismuth was no longer considered stable. It is possible decay may be observed in other nuclides, adding to this list of primordial radionuclides. Secondary radionuclides are radiogenic isotopes derived from the decay of primordial radionuclides. They have shorter half lives than primordial radionuclides. They arise in the decay chain of the primordial isotopes thorium 232, uranium 238, and uranium 235. Examples include the natural isotopes of polonium and radium. Cosmogenic isotopes, such as carbon 14, are present because they are continually being formed in the atmosphere due to cosmic rays. 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.

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). In biology, radionuclides of carbon can serve as radioactive tracers because they are chemically very similar to the nonradioactive nuclides, so most chemical, biological, and ecological processes treat them in a nearly identical way. One can then examine the result with a radiation detector, such as a Geiger counter, to determine where the provided atoms were incorporated. For example, one might culture plants in an environment in which the carbon dioxide contained radioactive carbon; then the parts of the plant that incorporate atmospheric carbon would be radioactive. Radionuclides can be used to monitor processes such as DNA replication or amino acid transport. in physics and biology radionuclide X ray fluorescence spectrometry is used to determine chemical composition of the compound. Radiation from a radionuclide source hits the sample and excites characteristic X rays in the sample. This radiation is registered and the chemical composition of the sample can be determined from the analysis of the measured spectrum. By measuring the energy of the characteristic radiation lines, it is possible to determine the proton number of the chemical element that emits the radiation, and by measuring the number of emitted photons, it is possible to determine the concentration of individual chemical elements. In nuclear medicine, radioisotopes are used for diagnosis, treatment, and research. Radioactive chemical tracers emitting gamma rays or positrons can provide diagnostic information about internal anatomy and the functioning of specific organs, including the human brain. This is used in some forms of tomography: single photon emission computed tomography and positron emission tomography (PET) scanning and Cherenkov luminescence imaging. Radioisotopes are also a method of treatment in hemopoietic forms of tumors; the success for treatment of solid tumors has been limited. More powerful gamma sources sterilise syringes and other medical equipment. In food preservation, radiation is used to stop the sprouting of root crops after harvesting, to kill parasites and pests, and to control the ripening of stored fruit and vegetables. Food irradiation usually uses beta decaying nuclides with strong gamma emissions like cobalt 60 or caesium 137. In industry, and in mining, radionuclides are used to examine welds, to detect leaks, to study the rate of wear, erosion and corrosion of metals, and for on stream analysis of a wide range of minerals and fuels. In spacecraft, radionuclides are used to provide power and heat, notably through radioisotope thermoelectric generators (RTGs) and radioisotope heater units (RHUs). In astronomy and cosmology, radionuclides play a role in understanding stellar and planetary process. In particle physics, radionuclides help discover new physics (physics beyond the Standard Model) by measuring the energy and momentum of their beta decay products (for example, neutrinoless double beta decay and the search for weakly interacting massive particles). In ecology, radionuclides are used to trace and analyze pollutants, to study the movement of surface water, and to measure water runoffs from rain and snow, as well as the flow rates of streams and rivers. In geology, archaeology, and paleontology, natural radionuclides are used to measure ages of rocks, minerals, and fossil materials.

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. This is a summary table for the 989 nuclides with half lives longer than one hour (including those that are stable), given in list of nuclides. 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.

Isotope Activity Half life Energies (keV) 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 TBq/kg (5.27 × 105 Ci/g) 6 hours 140

Isotope Activity Half life Energies (keV) 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)

Isotope Activity Half life Energies (keV) 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