 radioactivity

/ray'dee oh ak tiv"i tee/, n. Physics, Chem.the phenomenon, exhibited by and being a property of certain elements, of spontaneously emitting radiation resulting from changes in the nuclei of atoms of the element. Also called activity.[18951900; RADIO + ACTIVITY]
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Property exhibited by certain types of matter of emitting radiation spontaneously.The phenomenon was first reported in 1896 by Henri Becquerel for a uranium salt, and it was soon found that all uranium compounds are radioactive due to the uranium's radioactivity. In 1898 Marie Curie and her husband discovered two other naturally occurring, strongly radioactive elements, radium and polonium. The radiation is emitted by unstable atomic nuclei (see nucleus) as they attempt to become more stable. The main processes of radioactivity are alpha decay, beta decay, and gamma decay. In 1934 it was discovered that radioactivity could be induced in ordinary matter by artificial transmutation.* * *
Introductionproperty exhibited by certain types of matter of emitting energy and subatomic particles spontaneously. It is, in essence, an attribute of individual atomic nuclei.An unstable nucleus will decompose spontaneously, or decay, into a more stable configuration but will do so only in a few specific ways by emitting certain particles (subatomic particle) or certain forms of electromagnetic energy. Radioactive decay is a property of several naturally occurring elements as well as of artificially produced isotopes of the elements. The rate at which a radioactive element decays is expressed in terms of its halflife; i.e., the time required for onehalf of any given quantity of the isotope to decay. Halflives range from more than 1,000,000,000 years for some nuclei to less than 10^{−9} second (see below Rates of radioactive transitions (radioactivity)). The product of a radioactive decay process—called the daughter of the parent isotope—may itself be unstable, in which case it, too, will decay. The process continues until a stable nuclide has been formed.The nature of radioactive emissionsThe emissions of the most common forms of spontaneous radioactive decay are the alpha (alpha particle) (α) particle, the beta (beta particle) (β) particle, the gamma (gamma ray) (γ) ray, and the neutrino. The alpha particle is actually the nucleus of a helium4 atom, with two positive charges ^{4}/_{2}He. Such charged atoms are called ions (ion). The neutral helium atom has two electrons outside its nucleus balancing these two charges. Beta particles may be negatively charged (beta minus, symbol e^{−}), or positively charged (beta plus, symbol e^{+}). The beta minus [β^{−}] particle is actually an electron created in the nucleus during beta decay without any relationship to the orbital electron cloud of the atom. The beta plus particle, also called the positron, is the antiparticle of the electron; when brought together, two such particles will mutually annihilate each other. Gamma rays are electromagnetic radiations such as radio waves, light, and Xrays. Beta radioactivity also produces the neutrino and antineutrino, particles that have no charge and very little mass, symbolized by ν and ν, respectively.In the less common forms of radioactivity, fission fragments, neutrons, or protons may be emitted. Fission fragments are themselves complex nuclei with usually between onethird and twothirds the charge Z and mass A of the parent nucleus. Neutrons and protons are, of course, the basic building blocks of complex nuclei, having approximately unit mass on the atomic scale and having zero charge or unit positive charge, respectively. The neutron cannot long exist in the free state. It is rapidly captured by nuclei in matter; otherwise, in free space it will undergo betaminus decay to a proton, an electron, and an antineutrino with a halflife of 12.8 minutes. The proton is the nucleus of ordinary hydrogen and is stable.Types of radioactivityThe early work on natural radioactivity associated with uranium and thorium ores identified two distinct types of radioactivity: alpha and beta decay.In alpha decay, an energetic helium ion (alpha particle) is ejected, leaving a daughter nucleus of atomic number two less than the parent and of atomic mass number four less than the parent. An example is the decay (symbolized by an arrow) of the abundant isotope of uranium, ^{238}U, to a thorium daughter plus an alpha particle:Given for this and subsequent reactions are the energy released (Q) in millions of electron volts (MeV) and the halflife (t_{1⁄2}). It should be noted that in alpha decays the charges, or number of protons, shown in subscript are in balance on both sides of the arrow, as are the atomic masses, shown in superscript.Betaminus decayIn betaminus decay, an energetic negative electron is emitted, producing a daughter nucleus of one higher atomic number and the same mass number. An example is the decay of the uranium daughter product thorium234 into protactinium234:In the above reaction for beta decay, ν represents the antineutrino. Here, the number of protons is increased by one in the reaction, but the total charge remains the same, because an electron, with negative charge, is also created.A third type of radiation, gamma radiation, usually accompanies alpha or beta decay. Gamma rays are photons (photon) and are without rest mass or charge. Alpha or beta decay may simply proceed directly to the ground (lowest energy) state of the daughter nucleus without gamma emission, but the decay may also proceed wholly or partly to higher energy states (excited states) of the daughter. In the latter case, gamma emission may occur as the excited states transform to lower energy states of the same nucleus. (Alternatively to gamma emission, an excited nucleus may transform to a lower energy state by ejecting an electron from the cloud surrounding the nucleus. This orbital electron ejection is known as internal conversion and gives rise to an energetic electron and often an Xray as the atomic cloud fills in the empty orbital of the ejected electron. The ratio of internal conversion to the alternative gamma emission is called the internalconversion coefficient.)Isomeric transitionsThere is a wide range of rates of halflives for the gammaemission process. Usually dipole transitions (transition) (see below Gamma transition (radioactivity)), in which the gamma ray carries off one ℏ unit of angular momentum, are fast, less than nanoseconds (one nanosecond equals 10^{−9} second). The law of conservation of angular momentum requires that the sum of angular momenta of the radiation and daughter nucleus is equal to the angular momentum (spin) of the parent. If the spins of initial and final states differ by more than one, dipole radiation is forbidden, and gamma emission must proceed more slowly by a higher multipole (quadrupole, octupole, etc.) gamma transition. If the gammaemission halflife exceeds about one nanosecond, the excited nucleus is said to be in a metastable (metastable state), or isomeric, state (the names for a longlived excited state), and it is customary to classify the decay as another type of radioactivity, an isomeric transition. An example of isomerism is found in the protactinium234 nucleus of the uranium238 decay chain:The letter m following the mass number stands for metastable and indicates a nuclear isomer.Betaplus decayDuring the 1930s new types of radioactivity were found among the artificial products of nuclear reactions: betaplus decay, or positron emission, and electron capture. In betaplus decay an energetic positron is created and emitted, along with a neutrino, and the nucleus transforms to a daughter, lower by one in atomic number and the same in mass number. For instance, carbon11 (carbon) (Z = 6) decays to boron11 (Z = 5), plus one positron and one neutrino:Electron capture (EC) is a process in which decay follows the capture by the nucleus of an orbital electron. It is similar to positron decay in that the nucleus transforms to a daughter of one lower atomic number. It differs in that an orbital electron from the cloud is captured by the nucleus with subsequent emission of an atomic Xray as the orbital vacancy is filled by an electron from the cloud about the nucleus. An example is the nucleus of beryllium7 (beryllium) capturing one of its inner electrons to give lithium7:The main features of radioactive decay of a nuclear species are often displayed in a decay scheme. Figure 1—> shows the decay scheme of beryllium7. Indicated are the halflife of the parent and that of the excited daughter state, as well as its energy 0.4774 MeV. The spins and parities of all three states are provided on the upper lefthand side of the level. The multipolarity of the gamma ray (magnetic dipole, M1, plus 0.005 percent electric quadrupole, E2) is indicated above the vertical arrow symbolizing the gamma transition. The slanted arrows symbolize the electroncapture decay with labels giving the percentage of decay directly to ground state (89.7 percent) and the percentage of EC decay going via the excited state (10.3 percent). The boldface numbers following the percentages are socalled log ft values, to be encountered below in connection with betadecay rates. The overall energy release, Q_{EC}, is indicated below. The Q_{EC} is necessarily a calculated value because there is no general practical means of measuring the neutrino energies accompanying EC decay. With a few electroncapturing nuclides, it has been possible to measure directly the decay energy by measurement of a rare process called inner bremsstrahlung (braking radiation). In this process the energy release is shared between the neutrino and a gamma ray. The measured distribution of gammaray energies indicates the total energy release. Usually there is so much ordinary gamma radiation with radioactive decay that the inner bremsstrahlung is unobservable.Yet another type of radioactivity is spontaneous fission. In this process the nucleus splits into two fragment nuclei of roughly half the mass of the parent. This process is only barely detectable in competition with the more prevalent alpha decay for uranium, but for some of the heaviest artificial nuclei, such as fermium256 (fermium), spontaneous fission becomes the predominant mode of radioactive decay. Kineticenergy releases from 150 to 200 MeV may occur as the fragments are accelerated apart by the large electrical repulsion between their nuclear charges. The reaction is as follows:Only one of several product sets is shown. A few neutrons are always emitted in fission of this isotope, a feature essential to chain reactions. Spontaneous fission is not to be confused with induced fission, the process involved in nuclear reactors. Induced fisson is a property of uranium235, plutonium239, and other isotopes to undergo fission after absorption of a slow neutron. Other than the requirement of a neutron capture to initiate it, induced fission is quite similar to spontaneous fission regarding total energy release, numbers of secondary neutrons, and so on (see nuclear fission).Proton radioactivityProton radioactivity, discovered in 1970, is exhibited by an excited isomeric state of cobalt53, ^{53m}Co, 1.5 percent of which emits protons:Special betadecay (beta decay) processesIn addition to the above types of radioactivity, there is a special class of rare betadecay processes that gives rise to heavyparticle emission. In these processes the beta decay partly goes to a high excited state of the daughter nucleus, and this state rapidly emits a heavy particle.One such process is betadelayed neutron emission, which is exemplified by the following reaction:(Note: the asterisk denotes the shortlived intermediate excited states of oxygen17, and E_{max n} denotes the maximum energy observed for emitted neutrons.) There is a small production of delayed neutron emitters following nuclear fission, and these radioactivities are especially important in providing a reasonable response time to allow control of nuclear fission reactors by mechanically moved control rods.Among the positron emitters in the lightelement region, a number beta decay partly to excited states that are unstable with respect to emission of an alpha particle. Thus, these species exhibit alpha radiation with the halflife of the beta emission. Both the positron decay from boron8 and electron decay from lithium8 are betadelayed alpha emission, because ground as well as excited states of beryllium8 are unstable with respect to breakup into two alpha particles. Another example, sodium20 (^{2}^{0}Na) to give successively neon20 (^{2}^{0}Ne; the asterisk again indicating the shortlived intermediate state) and finally oxygen16 is listed below:In a few cases, positron decay leads to an excited nuclear state not able to bind a proton. In these cases, proton radiation appears with the halflife of the beta transition. The combination of high positrondecay energy and low protonbinding energy in the daughter ground state is required. In the example given below, tellurium111 (^{1}^{1}^{1}Te) yields antimony111 (^{1}^{1}^{1}Sb) and then tin110 (^{1}^{1}^{0}Sn) successively:Heavyion radioactivityIn 1980 A. Sandulescu, D.N. Poenaru, and W. Greiner described calculations indicating the possibility of a new type of decay of heavy (heavy ion) nuclei intermediate between alpha decay and spontaneous fission. The first observation of heavyion radioactivity was that of a 30MeV, carbon14 emission from radium223 by H.J. Rose and G.A. Jones in 1984. The ratio of carbon14 decay to alpha decay is about 5 × 10^{−10}. Observations also have been made of carbon14 from radium222, radium224, and radium226, as well as neon24 from thorium230, protactinium231, and uranium232. Such heavyion radioactivity, like alpha decay and spontaneous fission, involves quantummechanical tunneling through the potentialenergy barrier. Shell effects play a major role in this phenomenon, and in all cases observed to date the heavy partner of carbon14 or neon24 is close to doubly magic lead208 (see below Nuclear models (radioactivity)).Occurrence of radioactivitySome species of radioactivity occur naturally on Earth. A few species have halflives comparable to the age of the elements (about 6 × 10^{9} years), so that they have not decayed away after their formation in stars. Notable among these are uranium238, uranium235, and thorium232. Also, there is potassium40, the chief source of irradiation of the body through its presence in potassium of tissue. Of lesser significance are the beta emitters (beta decay) vanadium50, rubidium87, indium115, tellurium123, lanthanum138, lutetium176, and rhenium187, and the alpha emitters cerium142, neodymium144, samarium147, gadolinium152, dysprosium156, hafnium174, platinum190, and lead204. Besides these approximately 10^{9}year species, there are the shorterlived daughter activities fed by one or another of the above species; e.g., by various nuclei of the elements between lead (Z = 82) and thorium (Z = 90).Another category of natural radioactivity includes species produced in the upper atmosphere by cosmic ray bombardment. Notable are 5,720year carbon14 and 12.3year tritium (hydrogen3), 53day beryllium7, and 2,700,000year beryllium10. Meteorites (meteorite) are found to contain additional small amounts of radioactivity, the result of cosmic ray bombardments during their history outside the Earth's atmospheric shield. Activities as shortlived as 35day argon37 have been measured in fresh falls of meteorites. Nuclear explosions since 1945 have injected additional radioactivities into the environment, consisting of both nuclear fission products and secondary products formed by the action of neutrons from nuclear weapons on surrounding matter.The fission products encompass most of the known beta emitters in the mass region 75–160. They are formed in varying yields, rising to maxima of about 7 percent per fission in the mass region 92–102 (light peak of the fission yield versus atomic mass curve) and 134–144 (heavy peak). Two kinds of delayed hazards caused by radioactivity are recognized. First, the general radiation level is raised by fallout settling to Earth. Protection can be provided by concrete or earth shielding until the activity has decayed to a sufficiently low level. Second, ingestion or inhalation of even low levels of certain radioactive species can pose a special hazard, depending on the halflife, nature of radiations, and chemical behaviour within the body. For a detailed discussion on the biologic effects of radiation, see radiation: Biologic effects of ionizing radiation (radiation).Nuclear reactors (nuclear reactor) also produce fission products but under conditions in which the activities may be contained. Containment and wastedisposal practices should keep the activities confined and eliminate the possibility of leaching into groundwaters for times that are long compared to the halflives. A great advantage of thermonuclear fusion (nuclear fusion) power over fission power, if it can be practically realized, is not only that its fuel reserves, heavy hydrogen and lithium, are vastly greater than uranium, but also that the generation of radioactive fission product wastes can be largely avoided. In this connection, it may be noted that a major source of heat in the interior of both the Earth and the Moon is provided by radioactive decay. Theories about the formation and evolution of the Earth, Moon, and other planets must take into account these large heat production sources.Desired radioactivities other than natural activities and fission products may be produced either by irradiation of certain selected target materials by reactor neutrons or by charged particle beams or gamma ray beams of accelerators.Energetics and kinetics of radioactivityenergy release in radioactive transitionsConsideration of the energy release of various radioactive transitions leads to the fundamental question of nuclear binding energies (binding energy) and stabilities. A muchused method of displaying nuclearstability relationships is an isotope chart, those positions on the same horizontal row corresponding to a given proton number (Z) and those on the same vertical column to a given neutron number (N). Such a map is shown in Figure 2. The irregular bold line surrounds the region of presently known nuclei. The area encompassed by this is often referred to as the valley of stability because the chart may be considered a map of a binding energy surface, the lowest areas of which are the most stable. The most tightly bound nuclei of all are the abundant iron and nickel isotopes. Near the region of the valley containing the heaviest nuclei (largest mass number A; i.e., largest number of nucleons, N + Z), the processes of alpha decay and spontaneous fission are most prevalent; both these processes relieve the energetically unfavourable concentration of positive charge in the heavy nuclei.Along the region that borders on the valley of stability on the upper lefthand side are the positronemitting and electroncapturing radioactive nuclei, with the energy release and decay rates increasing the farther away the nucleus is from the stability line. Along the lower righthand border region, betaminus decay is the predominant process, with energy release and decay rates increasing the farther the nucleus is from the stability line.The grid lines of the graph are at the nucleon numbers corresponding to extra stability, the “magic numbers” (see below Nuclear models (radioactivity)). The circles labeled “deformed regions” enclose regions in which nuclei should exhibit cigar shapes; elsewhere the nuclei are spherical. Outside the dashed lines nuclei would be unbound with respect to neutron or proton loss and would be exceedingly shortlived (less than 10^{−19} second).Calculation and measurement of energyBy the method of closed energy cycles, it is possible to use measured radioactiveenergyrelease (Q) values for alpha (alpha decay) and beta decay to calculate the energy release for unmeasured transitions. An illustration is provided by the cycle of four nuclei below:In this cycle, energies from two of the alpha decays and one beta decay are measurable. The unmeasured betadecay energy for bismuth211, Q_{β−}(Bi), is readily calculated because conservation of energy requires the sum of Q values around the cycle to be zero. Thus, Q_{β−}(Bi) + 7.59 − 1.43 − 6.75 = 0. Solving this equation gives Q_{β−}(Bi) = 0.59 MeV. This calculation by closed energy cycles can be extended from stable lead207 back up the chain of alpha and beta decays to its natural precursor uranium235 and beyond. In this manner the nuclear binding energies of a series of nuclei can be linked together. Because alpha decay decreases the mass number A by 4, and beta decay does not change A, closed α−βcycle calculations based on lead207 can link up only those nuclei with mass numbers of the general type A = 4n + 3, in which n is an integer. Another, the 4n series, has as its natural precursor thorium232 and its stable end product lead208. Another, the 4n + 2 series, has uranium238 as its natural precursor and lead206 as its end product.In early research on natural radioactivity, the classification of isotopes (radioactive series) into the series cited above was of great significance because they were identified and studied as families. Newly discovered radioactivities were given symbols relating them to the family and order of occurrence therein. Thus, thorium234 was known as UX_{1}, the isomers of protactinium234 as UX_{2} and UZ, uranium234 as U_{II}, and so forth. These original symbols and names are occasionally encountered in more recent literature but are mainly of historical interest. The remaining 4n + 1 series is not naturally occurring but comprises wellknown artificial activities decaying down to stable thallium205.To extend the knowledge of nuclear binding energies, it is clearly necessary to make measurements to supplement the radioactivedecay energy cycles. In part, this extension can be made by measurement of Q values of artificial nuclear reactions. For example, the neutronbinding energies of the lead isotopes needed to link the energies of the four radioactive families together can be measured by determining the threshold gammaray energy to remove a neutron (photonuclear reaction); or the energies of incoming deuteron and outgoing proton in the reaction can be measured to provide this information.Further extensions of nuclearbindingenergy measurements rely on precision mass spectroscopy (mass spectrometry) (see spectroscopy). By ionizing, accelerating, and magnetically deflecting various nuclides (nuclide), their masses can be measured with great precision. A precise measurement of the masses of atoms involved in radioactive decay is equivalent to direct measurement of the energy release in the decay process. The atomic mass of naturally occurring but radioactive potassium40 is measured to be 39.964008 amu. Potassium40 decays predominantly by βemission to calcium40, having a measured mass 39.962589. Through Einstein's equation, energy is equal to mass (m) times velocity of light (c) squared, or E = mc^{2}, the energy release (Q) and the mass difference, Δm, are related, the conversion factor being one amu, equal to 931.478 MeV. Thus, the excess mass of potassium40 over calcium40 appears as the total energy release Q_{β} in the radioactive decay Q_{β−} = (39.964008 − 39.962589) × 931.478 MeV = 1.31 MeV. The other neighbouring isobar (same mass number, different atomic number) to argon40 is also of lower mass, 39.962384, than potassium40. This mass difference converted to energy units gives an energy release of 1.5 MeV, this being the energy release for EC decay to argon40. The maximum energy release for positron emission is always less than that for electron capture by twice the rest mass energy of an electron (2m_{0}c^{2} = 1.022 MeV); thus, the maximum positron energy for this reaction is 1.5 − 1.02, or 0.48 MeV.To connect alphadecay energies and nuclear mass differences requires a precise knowledge of the alphaparticle (helium4) atomic mass. The mass of the parent minus the sum of the masses of the decay products gives the energy release. Thus, for alpha decay of plutonium239 to uranium235 and helium4 the calculation goes as follows:By combining radioactivedecayenergy information with nuclearreaction Q values and precision mass spectroscopy, extensive tables of nuclear masses have been prepared. From them the Q values of unmeasured reactions or decay may be calculated.Alternative to the full mass, the atomic masses may be expressed as mass defect, symbolized by the Greek letter delta, Δ (the difference between the exact mass M and the integer A, the mass number), either in energy units or atomic mass units.Absolute nuclear binding energyThe absolute nuclear binding energy is the hypothetical energy release if a given nuclide were synthesized from Z separate hydrogen atoms and N (equal to A − Z) separate neutrons. An example is the calculation giving the absolute binding energy of the stablest of all nuclei, iron56 (iron):A general survey of the average binding energy per nucleon (for nuclei of all elements grouped according to ascending mass) shows a maximum at iron56 falling off gradually on both sides to about 7 MeV at helium4 and to about 7.4 MeV for the most massive nuclei known. Most of the naturally occurring nuclei are thus not stable in an absolute nuclear sense. Nuclei heavier than iron would gain energy by degrading into nuclear products closer to iron, but it is only for the elements of greatest mass that the rates of degradation processes such as alpha decay and spontaneous fission attain observable rates. In a similar manner, nuclear energy is to be gained by fusion of most elements lighter than iron. The coulombic repulsion between nuclei, however, keeps the rates of fusion reactions unobservably low unless the nuclei are subjected to temperatures of greater than 10^{7} K. Only in the hot cores of the Sun and other stars or in thermonuclear bombs or controlled fusion plasmas are these temperatures attained and nuclearfusion energy released.Nuclear models (nuclear model)The average behaviour of the nuclear binding energy can be understood with the model of a charged liquid drop. In this model, the aggregate of nucleons has the same properties of a liquid drop, such as surface tension, cohesion, and deformation. There is a dominant attractivebindingenergy term proportional to the number of nucleons A. From this must be subtracted a surfaceenergy term proportional to surface area and a coulombic repulsion energy proportional to the square of the number of protons and inversely proportional to the nuclear radius. Furthermore, there is a symmetryenergy term of quantummechanical (quantum mechanics) origin favouring equal numbers of protons and neutrons. Finally, there is a pairing term that gives slight extra binding to nuclei with even numbers of neutrons or protons.The pairingenergy term accounts for the great rarity of odd–odd nuclei (the terms odd–odd, even–even, even–odd, and odd–even refer to the evenness or oddness of proton number, Z, and neutron number, N, respectively) that are stable against beta decay. The sole examples are deuterium, lithium6, boron10, and nitrogen14. A few other odd–odd nuclei, such as potassium40, occur in nature, but they are unstable with respect to beta decay. Furthermore, the pairingenergy term makes for the larger number of stable isotopes of evenZ elements, compared to oddZ, and for the lack of stable isotopes altogether in element 43, technetium, and element 61, promethium.The betadecay energies of socalled mirror nuclei (mirror nucleus) afford one means of estimating nuclear sizes. For example, the neon and fluorine nuclei, ^{19}/_{10}Ne_{9} and ^{19}/_{9}F_{10}, are mirror nuclei because the proton and neutron numbers of one of them equal the respective neutron and proton numbers of the other. Thus, all bindingenergy terms are the same in each except for the coulombic term, which is inversely proportional to the nuclear radius. Such calculations along with more direct determinations by highenergy electron scattering and energy measurements of Xrays from muonic atoms (hydrogen atoms in which the electrons are replaced by negative muons) establish the nuclear charge as roughly uniformly distributed in a sphere of radius 1.2 A^{1⁄3} × 10^{−13} centimetre. That the radius is proportional to the cube root of the mass number has the great significance that the average density of all nuclei is nearly constant.Careful examination of nuclearbinding energies reveals periodic deviations from the smooth average behaviour of the chargedliquiddrop model. An extra binding energy arises in the neighbourhood of certain numbers of neutrons or protons, the socalled magic numbers (2, 8, 20, 28, 50, 82, and 126). Nuclei such as ^{4}/_{2}He_{2}, ^{16}/_{8}O_{8}, ^{40}/_{20}Ca_{20}, ^{48}/_{20}Ca_{28}, and ^{208}/_{82}Pb_{126} are especially stable species, doubly magic, in view of their having both proton and neutron numbers magic. These doubly magic nuclei are situated at the intersections of grid lines on Figure 2 above.The shell model (shell nuclear model)In the preceding section, the overall trends of nuclear binding energies were described in terms of a chargedliquiddrop model. Yet there were noted periodic bindingenergy irregularities at the magic numbers (magic number). The periodic occurrence of magic numbers of extra stability is strongly analogous to the extra electronic stabilities occurring at the atomic numbers of the noblegas atoms. The explanations of these stabilities are quite analogous in atomic and nuclear cases as arising from filling of particles into quantized orbitals of motion. The completion of filling of a shell of orbitals is accompanied by an extra stability. The nuclear model accounting for the magic numbers is, as previously noted, the shell model. In its simplest form, this model can account for the occurrence of spin zero for all even–even nuclear ground states; the nucleons fill pairwise into orbitals with angular momenta canceling. The shell model also readily accounts for the observed nuclear spins of the oddmass nuclei adjacent to doubly magic nuclei, such as ^{208}/_{82}Pb. Here, the spins of 1/2 for neighbouring ^{207}/_{81}Tl and ^{207}/_{82}Pb are accounted for by having all nucleons fill pairwise into the lowest energy orbits and putting the odd nucleon into the last available orbital before reaching the doubly magic configuration (the Pauli exclusion principle dictates that no more than two nucleons may occupy a given orbital, and their spins must be oppositely directed); calculations show the last available orbitals below lead208 to have angular momentum 1/2. Likewise, the spins of 9/2 for ^{209}/_{82}Pb and ^{209}/_{83}Bi are understandable because spin9/2 orbitals are the next available orbitals beyond doubly magic lead208. Even the associated magnetization, as expressed by the magnetic dipole moment, is rather well explained by the simple sphericalshell model.The orbitals of the sphericalshell model are labeled in a notation close to that for electronic orbitals in atoms. The orbital configuration of calcium40 has protons and neutrons filling the following orbitals: 1s_{1/2}, 1p_{3/2}, 1p_{1/2}, 1d_{5/2}, and 1d_{3/2}. The letter denotes the orbital angular momentum in usual spectroscopic notation, in which the letters s, p, d, f, g, h, i, etc., represent integer values of l running from zero for s (not to be confused with spins) through six for i. The fractional subscript gives the total angular momentum j with values of l + 1/2 and l − 1/2 allowed, as the intrinsic spin of a nucleon is 1/2. The first integer is a radial quantum number taking successive values 1, 2, 3, etc., for successively higher energy values of an orbital of given l and j. Each orbital can accommodate a maximum of 2j + 1 nucleons. The Table—> lists the orbitals comprising each shell, the exact order of various orbitals within a shell differing somewhat for neutrons and protons. The parity associated with an orbital is even (+) if l is even (s, d, g, i) and odd (−) if l is odd (p, f, h).An example of a sphericalshellmodel interpretation is provided by the betadecay scheme of 2.2minute thallium209 shown below, in which spin and parity are given for each state. The ground and lowest excited states of lead209 are to be associated with occupation by the 127th neutron of the lowest available orbitals above the closed shell of 126. From the last line of the Table—>, it is to be notedthat there are available g_{9/2}, d_{5/2}, and s_{1/2} orbitals with which to explain the ground and first two excited states. Lowlying states associated with the i_{11/2} and j_{15/2} orbitals are known from nuclearreaction studies, but they are not populated in the beta decay.The 2.13MeV state that receives the primary beta decay is not so simply interpreted as the other states. It is to be associated with the promotion of a neutron from the 3p_{1/2} orbital below the 126 shell closure. The density (number per MeV) of states increases rapidly above this excitation, and the interpretations become more complex and less certain.By suitable refinements, the sphericalshell model can be extended further from the doubly magic region. Primarily, it is necessary to drop the approximation that nucleons move independently in orbitals and to invoke a residual force, mainly shortrange and attractive, between the nucleons. The sphericalshell model augmented by residual interactions can explain and correlate around the magic regions a large amount of data on binding energies, spins, magnetic moments, and the spectra of excited states.The collective modelFor nuclei more removed from the doubly magic regions, the sphericalshell model encounters difficulty in explaining the large observed electric quadrupole moments indicating cigarshaped nuclei. For these nuclei a hybrid of liquiddrop and shell models, the collective model, has been proposed. (See the circular regions of Figure 2 for occurrence of cigarshaped nuclei.)Nucleons can interact with one another in a collective fashion to deform the nuclear shape to a cigar shape. Such large spheroidal distortions are usual for nuclei far from magic, notably with 150 ≲ A ≲ 190, and 224 ≲ A (the symbol < denotes less than, and ∼ means that the number is approximate). In these deformed regions the collective model prescribes that orbitals be computed in a cigarshaped potential and that the relatively lowenergy rotational excitations of the tumbling motion of the cigar shape be taken into account. The collective model has been highly successful in correlating and predicting nuclear properties in deformed regions. An example of a nuclear rotational band (a series of adjacent states) is provided by the decay of the isomer hafnium180m, in Figure 3—>, through a cascade of gamma rays down the ground rotational band (see below Gamma transition (radioactivity) for explanation of M2, E1, E2, and E3).Rates of radioactive transitionsThere is a vast range (activity) of the rates of radioactive decay, from undetectably slow to unmeasurably short. Before considering the factors governing particular decay rates in detail, it seems appropriate to review the mathematical equations governing radioactive decay and the general methods of rate measurement in different ranges of halflife.Exponentialdecay lawRadioactive decay occurs as a statistical exponential rate process. That is to say, the number of atoms likely to decay in a given infinitesimal time interval (dN/dt) is proportional to the number (N) of atoms present. The proportionality constant, symbolized by the Greek letter lambda, λ, is called the decay constant. Mathematically, this statement is expressed by the firstorder differential equation,This equation is readily integrated to givein which N_{0} is the number of atoms present when time equals zero. From the above two equations it may be seen that a disintegration rate, as well as the number of parent nuclei, falls exponentially with time. An equivalent expression in terms of halflife t_{1⁄2} isIt can readily be shown that the decay constant λ and halflife (t_{1⁄2}) are related as follows: λ = log_{e}2/t_{1⁄2} = 0.693/t_{1⁄2}. The reciprocal of the decay constant λ is the mean life, symbolized by the Greek letter tau, τ.For a radioactive nucleus such as potassium40 that decays by more than one process (89 percent β− , 11 percent electron capture), the total decay constant is the sum of partial decay constants for each decay mode. (The partial halflife for a particular mode is the reciprocal of the partial decay constant times 0.693.) It is helpful to consider a radioactive chain in which the parent (generation 1) of decay constant λ_{1} decays into a radioactive daughter (generation 2) of decay constant λ_{2}. The case in which none of the daughter isotope (2) is originally present yields an initial growth of daughter nuclei followed by its decay. The equation giving the number (N_{2}) of daughter nuclei existing at time t in terms of the number N_{1}(0) of parent nuclei present when time equals zero isin which e represents the logarithmic constant 2.71828.The general equation for a chain of n generations with only the parent initially present (when time equals zero) is as follows:in which e represents the logarithmic constant 2.71828.These equations can readily be modified to the case of production of isotopes in the steady neutron flux of a reactor or in a star. In such cases, the chain of transformations might be mixed with some steps occurring by neutron capture and some by radioactive decay. The neutroncapture probability for a nucleus is expressed in terms of an effective crosssectional (cross section) area. If one imagines the nuclei replaced by spheres of the same crosssectional area, the rate of reaction in a neutron flux would be given by the rate at which neutrons strike the spheres. The cross section is usually symbolized by the Greek letter sigma, σ, with the units of barns (barn) (10^{−24} cm^{2}) or millibarns (10^{−3} b) or microbarns (10^{−6} b). Neutron flux is often symbolized by the letters nv (neutron density, n, or number per cubic centimetre, times average speed, v) and given in neutrons per square centimetre per second.The modification of the transformation equations merely involves substituting the product nvσ_{i} in place of λ_{i} for any step involving neutron capture rather than radioactive decay. Reactor fluxes nv even higher than 10^{1}^{5} neutrons per square centimetre per second are available in several research reactors, but usual fluxes are somewhat lower by a factor of 1,000 or so. Tables of neutroncapture cross sections of the naturally occurring nuclei and some radioactive nuclei can be used for calculation of isotope production rates in reactors.Measurement of halflifeThe measurement of halflives of radioactivity in the range of seconds to a few years commonly involves measuring the intensity of radiation (radiation measurement) at successive times over a time range comparable to the halflife. The logarithm of the decay rate is plotted against time, and a straight line is fitted to the points. The time interval for this straightline decay curve to fall by a factor of 2 is read from the graph as the halflife, by virtue of equations (1—>) and (2—>). If there is more than one activity present in the sample, the decay curve will not be a straight line over its entire length, but it should be resolvable graphically (or by more sophisticated statistical analysis) into sums and differences of straightline exponential terms. The general equations (4—>) for chain decays show a time dependence given by sums and differences of exponential terms, though special modified equations are required in the unlikely case that two or more decay constants are identically equal.For halflives longer than several years it is often not feasible to measure accurately the decrease in counting rate over a reasonable length of time. In such cases, a measurement of specific activity may be resorted to; i.e., a carefully weighed amount of the radioactive isotope is taken for counting measurements to determine the disintegration rate, D. Then by equation (1) the decay constant λ_{i} may be calculated. Alternately, it may be possible to produce the activity of interest in such a way that the number of nuclei, N, is known, and again with a measurement of D equation (1) may be used. The number of nuclei, N, might be known from counting the decay of a parent activity or from knowledge of the production rate by a nuclear reaction in a reactor or accelerator beam.Halflives from 100 microseconds to one nanosecond are measured electronically in coincidence experiments. The radiation yielding the species of interest is detected to provide a start pulse for an electronic clock, and the radiation by which the species decays is detected in another device to provide a stop pulse. The distribution of these time intervals is plotted semilogarithmically, as discussed for the decayrate treatment, and the halflife is determined from the slope of the straight line.Halflives in the range of 100 microseconds to one second must often be determined by special techniques. For example, the activities produced may be deposited on rapidly rotating drums or moving tapes, with detectors positioned along the travel path. The activity may be produced so as to travel through a vacuum at a known velocity and the disintegration rate measured as a function of distance; however, this method usually applies to shorter halflives in or beyond the range of the electronic circuit.Species with halflives shorter than the electronic measurement limit are not considered as separate radioactivities, and the various techniques of determining their halflives will hence not be cited here.Decayrate considerations for various types of radioactivity are given here in the same order as listed above in Types of radioactivity (radioactivity).Alpha decay, the emission of helium ions, exhibits sharp line spectra when spectroscopic measurements of the alphaparticle energies are made. For even–even alpha emitters the most intense alpha group or line is always that leading to the ground state of the daughter. Weaker lines of lower energy go to excited states, and there are frequently numerous lines observable.The main decay group of even–even alpha emitters exhibits a highly regular dependence on the atomic number, Z, and the energy release, Q_{α}. (Total alpha energy release, Q_{α}, is equal to alphaparticle energy, E_{α}, plus daughter recoil energy needed for conservation of momentum; E_{recoil} = (m_{α}/[m_{α} + M_{d}])E_{α}, with m_{α} equal to the mass of the alpha particle and M_{d} the mass of the daughter product.) As early as 1911 the German physicist Johannes Wilhelm Geiger (Geiger, Hans), together with the British physicist John Mitchell Nuttall, noted the regularities of rates for even–even nuclei and proposed a remarkably successful equation for the decay constant, log λ = a + b log r, in which r is the range in air, b is a constant, and a is given different values for the different radioactive series. The decay constants of odd alpha emitters (odd A or odd Z or both) are not quite so regular and may be much smaller. The values of the constant b that were used by Geiger and Nuttall implied a roughly 90thpower dependence of λ on Q_{α}. There is a tremendous range of known halflives from the 2 × 10^{1}^{5} years of ^{144}/_{60}Nd (neodymium) with its 1.83MeV alphaparticle energy (E_{α}) to the 0.3 microsecond of ^{212}/_{84}Po (polonium) with E_{α} = 8.78 MeV.The theoretical basis for the Geiger–Nuttall empirical rate law remained unknown until the formulation of wave mechanics. A dramatic early success of wave mechanics was the quantitative theory of alphadecay rates. One curious feature of wave mechanics is that particles may have a nonvanishing probability of being in regions of negative kinetic energy. In classical mechanics a ball that is tossed to roll up a hill will slow down until its gravitational potential energy equals its total energy, and then it will roll back toward its starting point. In quantum mechanics the ball has a certain probability of tunneling through the hill and popping out on the other side. For objects large enough to be visible to the eye, the probability of tunneling through energetically forbidden regions is unobservably small. For submicroscopic objects such as alpha particles, nucleons, or electrons, however, quantum mechanical tunneling can be an important process—as in alpha decay.The logarithm of tunneling probability on a single collision with an energy barrier of height B and thickness D is a negative number proportional to thickness D, to the square root of the product of B and particle mass m. The size of the proportionality constant will depend on the shape of the barrier and will depend inversely on Planck's constant h.In the case of alpha decay, the electrostatic repulsive potential between alpha particle and nucleus generates an energetically forbidden region, or potential barrier, from the nuclear radius out to several times this distance. The maximum height (B) of this alpha barrier is given approximately by the expression B = 2Ze^{2}/R, in which Z is the charge of the daughter nucleus, e is the elementary charge in electrostatic units, and R is the nuclear radius. Numerically, B is roughly equal to 2Z/A^{1⁄3}, with A the mass number and B in energy units of MeV. Thus, although the height of the potential barrier for ^{212}/_{84}Po decay is nearly 28 MeV, the total energy released is Q_{α} = 8.95 MeV. The thickness of the barrier (i.e., distance of the alpha particle from the centre of the nucleus at the moment of recoil) is about twice the nuclear radius of 8.8 × 10^{−13} centimetre. The tunneling calculation for the transition probability (P) through the barrier gives approximatelyin which M is the mass of the alpha particle and ℏ is Planck's constant h divided by 2π. By making simple assumptions about the frequency of the alpha particle striking the barrier, the penetration formula (5—>) can be used to calculate an effective nuclear radius for alpha decay. This method was one of the early ways of estimating nuclear sizes. In more sophisticated modern techniques the radius value is taken from other experiments, and alphadecay data and penetrabilities are used to calculate the frequency factor.The form of equation (5—>) suggests the correlation of decay rates by an empirical expression relating the halflife (t_{1⁄2}) of decay in seconds to the release energy (Q_{α}) in MeV:Semiempirical constantsValues of the constants a and b that give best fits to experimental rates of even–even nuclei with neutron number greater than 126 are given in the Table (Semiempirical constants). The nuclei with 126 or fewer neutrons decay more slowly than the heavier nuclei, and constants a and b must be readjusted to fit their decay rates.The alphadecay rates to excited states of even–even nuclei and to ground and excited states of nuclei with odd numbers of neutrons, protons, or both may exhibit retardations from equation (6—>) rates ranging to factors of thousands or more. The factor by which the rate is slower than the rate formula (6—>) is the hindrance factor. The existence of uranium235 in nature rests on the fact that alpha decay to the ground and low excited states exhibits hindrance factors of over 1,000. Thus the uranium235 halflife is lengthened to 7 × 10^{8} years, a time barely long enough compared to the age of the elements in the solar system for uranium235 to exist in nature today.The alpha hindrance factors are fairly well understood in terms of the orbital motion of the individual protons and neutrons that make up the emitted alpha particle. The alphaemitting nuclei heavier than radium are considered to be cigarshaped, and alpha hindrance factor data have been used to infer the most probable zones of emission on the nuclear surface—whether polar, equatorial, or intermediate latitudes.The processes separately introduced at the beginning of this section as betaminus decay, betaplus decay, and orbital electron capture can be appropriately treated together. They all are processes whereby neutrons and protons may transform to one another by weak interaction (weak force). In striking contrast to alpha decay, the electrons (minus or plus charged) emitted in betaminus and betaplus decay do not exhibit sharp, discrete energy spectra but have distributions of electron energies ranging from zero up to the maximum energy release, Q_{β} . Furthermore, measurements of heat released by beta emitters (most radiation stopped in surrounding material is converted into heat energy) show a substantial fraction of the energy, Q_{β} , is missing. These observations, along with other considerations involving the spins or angular momenta of nuclei and electrons, led Wolfgang Pauli (Pauli, Wolfgang) to postulate the simultaneous emission of the neutrino (1931). The neutrino, as a light and uncharged particle with nearly no interaction with matter, was supposed to carry off the missing heat energy. Today, neutrino theory is well accepted with the elaboration that there are six kinds of neutrinos, the electron neutrino, mu neutrino, and tau neutrino and corresponding antineutrinos of each. The electron neutrinos are involved in nuclear betadecay transformations, the mu neutrinos are encountered in decay of muons to electrons, and the tau neutrinos are produced when a massive lepton called a tau breaks down.Although in general the more energetic the beta decay the shorter is its halflife, the rate relationships do not show the clear regularities of the alphadecay dependence on energy and atomic number.The first quantitative rate theory of beta decay was given by Enrico Fermi (Fermi, Enrico) in 1934, and the essentials of this theory form the basis of modern theory. As an example, in the simplest betadecay process, a free neutron decays into a proton, a negative electron, and an antineutrino: n → p + e^{−} + ν. The weak interaction responsible for this process, in which there is a change of species (n to p) by a nucleon with creation of electron and antineutrino, is characterized in Fermi theory by a universal constant, g. The sharing of energy between electron and antineutrino is governed by statistical probability laws giving a probability factor for each particle proportional to the square of its linear momentum (defined by mass times velocity for speeds much less than the speed of light and by a more complicated, relativistic relation for faster speeds). The overall probability law from Fermi theory gives the probability per unit time per unit electron energy interval, P(W), as follows:in which W is the electron energy in relativistic units (W = 1 + E/m_{0}c^{2}) and W_{0} is the maximum (W_{0} = 1 + Q_{β}/m_{0}c^{2}), m_{0} the rest mass of the electron, c the speed of light, and h Planck's constant. This rate law expresses the neutron betadecay spectrum in good agreement with experiment, the spectrum falling to zero at lowest energies by the factor W and falling to zero at the maximum energy by virtue of the factor (W_{0} − W)^{2}.In Fermi's original formulation, the spins of an emitted beta and neutrino are opposing and so cancel to zero. Later work showed that neutron beta decay partly proceeds with the ^{1}/_{2} ℏ spins of beta and neutrino adding to one unit of ℏ. The former process is known as Fermi decay (F) and the latter Gamow–Teller (GT) decay, after George Gamow and Edward Teller, the physicists who first proposed it. The interaction constants are determined to be in the ratio g_{GT}^{2}/g_{F}^{2} = 1.4. Thus, g^{2} in equation (7—>) should be replaced by (g_{F}^{2} + g_{GT}^{2}).The scientific world was shaken in 1957 by the measurement in beta decay of maximum violation of the law of conservation (energy, conservation of) of parity. The meaning of this nonconservation in the case of neutron beta decay considered above is that the preferred direction of electron emission is opposite to the direction of the neutron spin. By means of a magnetic field and low temperature it is possible to cause neutrons in cobalt60 and other nuclei, or free neutrons, to have their spins set preferentially in the up direction perpendicular to the plane of the coil generating the magnetic field. The fact that beta decay prefers the down direction for spin means that the reflection of the experiment as seen in a mirror parallel to the coil represents an unphysical situation: conservation of parity, obeyed by most physical processes, demands that experiments with positions reversed by mirror reflection should also occur. Further consequences of parity violation in beta decay are that spins of emitted neutrinos and electrons are directed along the direction of flight, totally so for neutrinos and partially so by the ratio of electron speed to the speed of light for electrons.The overall halflife for beta decay of the free neutron, measured as 12 minutes, may be related to the interaction constants g^{2} (equal to g_{F}^{2} + g_{GT}^{2}) by integrating (summing) probability expression (7—>) over all possible electron energies from zero to the maximum. The result for the decay constant isin which W_{0} is the maximum betaparticle energy in relativistic units (W_{0} = 1 + Q_{β}/m_{0}c^{2}), with m_{0} the rest mass of the electron, c the speed of light, and h Planck's constant. The best g value from decay rates is approximately 10^{−49} erg per cubic centimetre. As may be noted from equation (8—>), there is a limiting fifthpower energy dependence for highest decay energies.In the case of a decaying neutron not free but bound within a nucleus, the above formulas must be modified. First, as the nuclear charge Z increases, the relative probability of lowenergy electron emission increases by virtue of the coulombic attraction. For positron emission, which is energetically impossible for free protons but can occur for bound protons in protonrich nuclei, the nuclear coulomb charge suppresses lower energy positrons from the shape given by equation (7—>). This equation can be corrected by a factor F(Z,W) depending on the daughter atomic number Z and electron energy W. The factor can be calculated quantum mechanically. The coulomb charge also affects the overall rate expression (8—>) such that it can no longer be expressed as an algebraic function, but tables are available for analysis of beta decay rates. The rates are analyzed in terms of a function f(Z,Q_{β}) calculated by integration of equation (7—>) with correction factor F(Z,W).Approximate expressions for the f functions usable for decay energies Q between 0.1 MeV and 10 MeV, in which Q is measured in MeV, and Z is the atomic number of the daughter nucleus, are as follows (the symbol ≈ means approximately equal to):For electron capture, a much weaker dependence on energy is found:The basic beta decay rate expression obeyed by the class of socalled superallowed transitions, including decay of the neutron and several light nuclei isLike the groundtoground alpha transitions of even–even nuclei, the superallowed beta transitions obey the basic rate law, but most beta transitions go much more slowly. The extra retardation is explained in terms of mismatched orbitals of neutrons and protons involved in the transition. For the superallowed transitions the orbitals in initial and final states are almost the same. Most of them occur between mirror nuclei, with one more or less neutron than protons; i.e., betaminus decay of hydrogen3, electron capture of beryllium7 and positron emission of carbon11, oxygen15, neon19, . . . titanium43.The nuclear retardation of beta decay rates below those of the superallowed class may be expressed in a fundamental way by multiplying the right side of equation (9—>) by the square of a nuclear matrix element (a quantity of quantum mechanics), which may range from unity down to zero depending on the degree of mismatch of initial and final nuclear states of internal motion. A more usual way of expressing the nuclear factor of the beta rate is the log ft value, in which f refers to the function f(Z,Q_{β}). Because the halflife is inversely proportional to the decay constant λ, the product f_{β}t_{1⁄2} will be a measure of (inversely proportional to) the square of the nuclear matrix element. For the log ft value, the beta halflife is taken in seconds, and the ordinary logarithm to the base 10 is used. The superallowed transitions have log ft values in the range of 3 to 3.5. Beta log ft values are known up to as large as ∼ 23 in the case of indium115. There is some correlation of log ft values with spin changes between parent and daughter nucleons, the indium115 decay involving a spin change of four, whereas the superallowed transitions (transition) all have spin changes of zero or one.Gamma transition (gamma decay)The nuclear gamma transitions belong to the large class of electromagnetic transitions encompassing radiofrequency emission by antennas or rotating molecules, infrared emission by vibrating molecules or hot filaments, visible light, ultraviolet light, and Xray emission by electronic jumps in atoms or molecules. The usual relations apply for connecting frequency ν, wavelength λ, and photon quantum energy E with speed of light c and Planck's constant h; namely, λ = c/ν and E = hv. It is sometimes necessary to consider the momentum (p) of the photon given by p = E/c.Classically, radiation accompanies any acceleration of electric charge. Quantum (quantum mechanics) mechanically there is a probability of photon emission from higher to lower energy nuclear states, in which the internal state of motion involves acceleration of charge in the transition. Therefore, purely neutron orbital acceleration would carry no radiative contribution.A great simplification in nuclear gamma transition rate theory is brought about by the circumstance that the nuclear diameters are always much smaller than the shortest wavelengths of gamma radiation in radioactivity—i.e., the nucleus is too small to be a good antenna for the radiation. The simplification is that nuclear gamma transitions can be classified according to multipolarity, or amount of spin angular momentum carried off by the radiation. One unit of angular momentum in the radiation is associated with dipole (magnetic dipole) transitions (a dipole consists of two separated equal charges, plus and minus). If there is a change of nuclear parity, the transition is designated electric dipole (E1) and is analogous to the radiation of a linear halfwave dipole radio antenna. If there is no parity change, the transition is magnetic dipole (M1) and is analogous to the radiation of a fullwave loop antenna. With two units of angular momentum change, the transition is electric quadrupole (E2), analogous to a fullwave linear antenna of two dipoles outofphase, and magnetic quadrupole (M2), analogous to coaxial loop antennas driven outofphase. Higher multipolarity radiation also frequently occurs with radioactivity.Transition rates are usually compared to the singleproton theoretical rate, or Weisskopf formula, named after the American physicist Victor Frederick Weisskopf, who developed it. The Table—> gives the theoretical reference rate formulas in their dependence on nuclear mass number A and gammaray energy Eγ (in MeV).It is seen for the illustrative case of gamma energy 0.1 MeV and mass number 125 that there occurs an additional factor of 10^{7} retardation with each higher multipole order. For a given multipole, magnetic radiation should be a factor of 100 or so slower than electric. These rate factors ensure that nuclear gamma transitions are nearly purely one multipole, the lowest permitted by the nuclear spin change. There are many exceptions, however; mixed M1–E2 transitions are common, because E2 transitions are often much faster than the Weisskopf formula gives and M1 transitions are generally slower. All E1 transitions encountered in radioactivity are much slower than the Weisskopf formula. The other higher multipolarities show some scatter in rates, ranging from agreement to considerable retardation. In most cases the retardations are well understood in terms of nuclear model calculations.Though not literally a gamma transition, electric monopole (E0) transitions may appropriately be mentioned here. These may occur when there is no angular momentum change between initial and final nuclear states and no parity change. For spinzero to spinzero transitions, single gamma emission is strictly forbidden. The electric monopole transition occurs largely by the ejection of electrons from the orbital cloud in heavier elements and by positron–electron pair creation in the lighter elements.Applications of radioactivityIn medicineRadioisotopes have found extensive use in diagnosis and therapy, and this has given rise to a rapidly growing field called nuclear medicine. These radioactive isotopes have proven particularly effective as tracers (isotopic tracer) in certain diagnostic procedures. As radioisotopes are identical chemically with stable isotopes of the same element, they can take the place of the latter in physiological processes. Moreover, because of their radioactivity, they can be readily traced even in minute quantities with such detection devices as gammaray spectrometers and proportional counters. Though many radioisotopes are used as tracers, iodine131, phosphorus32, and technetium99m are among the most important. Physicians employ iodine131 to determine cardiac output, plasma volume, and fat metabolism and particularly to measure the activity of the thyroid gland where this isotope accumulates. Phosphorus32 is useful in the identification of malignant tumours because cancerous cells tend to accumulate phosphates more than normal cells do. Technetium99m, used with radiographic scanning devices, is valuable for studying the anatomic structure of organs.Such radioisotopes as cobalt60 and cesium137 are widely used to treat cancer. They can be administered selectively to malignant tumours and so minimize damage to adjacent healthy tissue.In industryForemost among industrial applications is power generation based on the release of the fission energy of uranium (see the articles nuclear fission and nuclear reactor: Nuclear fission reactors (nuclear reactor)). Other applications include the use of radioisotopes to measure (and control) the thickness or density of metal and plastic sheets, to stimulate the crosslinking of polymers, to induce mutations in plants in order to develop hardier species, and to preserve certain kinds of foods by killing microorganisms that cause spoilage. In tracer applications radioactive isotopes are employed, for example, to measure the effectiveness of motor oils on the wearability of alloys for piston rings and cylinder walls in automobile engines. For additional information about industrial uses, see radiation: Applications in science and industry (radiation).In scienceResearch in the Earth sciences has benefited greatly from the use of radiometricdating techniques, which are based on the principle that a particular radioisotope (radioactive parent) in geologic material decays at a constant known rate to daughter isotopes. Using such techniques, investigators have been able to determine the ages of various rocks and rock formations and thereby quantify the geologic time scale (see geochronology: Absolute dating (dating)). A special application of this type of radioactivity age method, carbon14 dating, has proved especially useful to physical anthropologists and archaeologists. It has helped them to better determine the chronological sequence of past events by enabling them to date more accurately fossils and artifacts from 500 to 50,000 years old.Radioisotopic tracers are employed in environmental studies, as, for instance, those of water pollution in rivers and lakes and of air pollution by smokestack effluents. They also have been used to measure deepwater currents in oceans and snowwater content in watersheds. Researchers in the biologic sciences, too, have made use of radioactive tracers to study complex processes. For example, thousands of plant metabolic studies have been conducted on amino acids and compounds of sulfur, phosphorus, and nitrogen.Additional ReadingBernard G. Harvey, Introduction to Nuclear Physics and Chemistry, 2nd ed. (1969), an excellent introductory text on nuclear phenomena; Aage Bohr and Ben R. Mottelson, Nuclear Structure, 2 vol. (1969); C. Michael Lederer and Virginia S. Shirley, Table of Isotopes, 7th ed. (1978), a comprehensive table that lists all the known radioactive and stable isotopes and their properties; and Alfred Romer, The Restless Atom: The Awakening of Nuclear Physics (1960, reprinted 1982), a popular account of the discovery of radioactivity and research in that field. Collections of articles and reports are Frederick Soddy, Radioactivity and Atomic Theory (1975); and Alfred Romer (ed.), The Discovery of Radioactivity and Transmutation (1964). Applications of radiation are discussed in International Atomic Energy Agency, Industrial Application of Radioisotopes and Radiation Technology (1982); and Howard J. Glenn (ed.), Biologic Applications of Radiotracers (1982), on the use of small animals in radiotracer research.Ellis P. Steinberg* * *
Universalium. 2010.