Which isotope of hydrogen with a half-life of 12.32 years has a nucleus that contains one proton and two neutrons?
"deuterium, another isotope of hydrogen, by Ernest Rutherford, Mark Oliphant, and Paul Harteck. However, their experiment could not isolate tritium, which was later accomplished by Luis Alvarez and Robert Cornog, who also realized tritium's radioactivity. Willard F. Libby recognized that tritium could be used for radiometric dating of water and wine. Tritium Tritium ( or ; symbol ' or ', also known as hydrogen-3) is a radioactive isotope of hydrogen. The nucleus of tritium (sometimes called a triton) contains one proton and two neutrons, whereas the nucleus of protium (by far the most abundant hydrogen isotope) contains one proton and"
"observed to decay, and hydrogen-1 is therefore considered a stable isotope. Some grand unified theories proposed in the 1970s predict that proton decay can occur with a half-life between 10 and 10 years. If this prediction is found to be true, then hydrogen-1 (and indeed all nuclei now believed to be stable) are only observationally stable. To date, however, experiments have shown that the minimum proton half-life is in excess of 10 years. H (atomic mass u), the other stable hydrogen isotope, is known as ""deuterium"" and contains one proton and one neutron in its nucleus. The nucleus of deuterium"
"Deuterium Deuterium (or hydrogen-2, symbol ' or ', also known as heavy hydrogen) is one of two stable isotopes of hydrogen (the other being protium, or hydrogen-1). The nucleus of deuterium, called a deuteron, contains one proton and one neutron, whereas the far more common protium has no neutron in the nucleus. Deuterium has a natural abundance in Earth's oceans of about one atom in of hydrogen. Thus deuterium accounts for approximately 0.0156% (or, on a mass basis, 0.0312%) of all the naturally occurring hydrogen in the oceans, while protium accounts for more than 99.98%. The abundance of deuterium changes"
"Deuterium Deuterium (or hydrogen-2, symbol ' or ', also known as heavy hydrogen) is one of two stable isotopes of hydrogen (the other being protium, or hydrogen-1). The nucleus of deuterium, called a deuteron, contains one proton and one neutron, whereas the far more common protium has no neutron in the nucleus. Deuterium has a natural abundance in Earth's oceans of about one atom in of hydrogen. Thus deuterium accounts for approximately 0.0156% (or, on a mass basis, 0.0312%) of all the naturally occurring hydrogen in the oceans, while protium accounts for more than 99.98%. The abundance of deuterium changes"
"unstable, and gradually undergo radioactive decay to become another element. The hydrogen nucleus contain just one proton, Its isotope deuterium, or heavy hydrogen, contains a proton and a neutron. Helium contains two protons and two neutrons, and carbon, nitrogen and oxygen - six, seven and eight of each particle, respectively. However, a helium nucleus weighs less than the sum of the weights of the two hydrogen nuclei which combine to make it. The same is true for carbon, nitrogen and oxygen. For example, the carbon nucleus is slightly lighter than three helium nuclei, which can combine to make a carbon"
"Phosphorus-32 Phosphorus-32 is a radioactive isotope of phosphorus. The nucleus of phosphorus-32 contains 15 protons and 17 neutrons, one more neutron than the most common isotope of phosphorus, phosphorus-31. Phosphorus-32 only exists in small quantities on Earth as it has a short half-life of 14.29 days and so decays rapidly. Phosphorus is found in many organic molecules and so phosphorus-32 has many applications in medicine, biochemistry and molecular biology where it can be used to trace phosphorylated molecules, e.g. in elucidating metabolic pathways, and radioactively label DNA. Phosphorus has a short half-life of 14.29 days and decays into sulfur-32 by"
"contains a lambda particle in its nucleus, whereas an atomic nucleus is generally thought to contain only neutrons and protons. Lithium-11 is thought to possess a halo nucleus consisting of a core of three protons and eight neutrons, two of which are in a nuclear halo. It has an exceptionally large cross-section of 3.16 fm, comparable to that of Pb. It decays by beta emission to Be, which then decays in several ways (see table below). Lithium-12 has a considerably shorter half-life of around 10 nanoseconds. It decays by neutron emission into Li, which decays as mentioned above. While β"
"and French scientists at RIKEN's Radioactive Isotope Beam Factory by bombarding hydrogen with helium-8 atoms. In the resulting reaction, all six of the helium-8's neutrons were donated to the hydrogen's nucleus. The two remaining protons were detected by the ""RIKEN telescope"", a device composed of several layers of sensors, positioned behind the target of the RI Beam cyclotron. Hydrogen-7 has a half life of 23 yoctoseconds (2.3×10 seconds). The majority of heavy hydrogen isotopes decay directly to H, which then decays to the stable isotope He. However, H has occasionally been observed to decay directly to stable H. \ce{^3_1H} &\ce{->[12.32\"
"half-life of 8 seconds. The isotope Nh, as well as the unconfirmed Nh and Nh, have also been reported to have half-lives of over a second. The isotopes Nh and Nh have half-lives of 1 and 0.1 seconds respectively. The remaining two isotopes have half-lives between 0.1 and 100 milliseconds: Nh has a half-life of 70 milliseconds, and Nh, the lightest known nihonium isotope, is also the shortest-lived, with a half-life of 1.4 milliseconds. This rapid increase in the half-lives near the closed neutron shell at ""N"" = 184 is seen in roentgenium, copernicium, and nihonium (elements 111 through 113),"
"Because it has 84 neutrons (two more than 82, which is a magic number which corresponds to a stable neutron configuration), it may emit an alpha particle (which has 2 neutrons) to form praseodymium-141 with 82 neutrons. Thus it is the only promethium isotope with an experimentally observed alpha decay. Its partial half-life for alpha decay is about 6.3 years, and the relative probability for a Pm nucleus to decay in this way is 2.8 %. Several other promethium isotopes (Pm, Pm, Pm etc.) also have a positive energy release for alpha decay; their alpha decays are predicted to occur"
"in ice and sediment. Nickel-78's half-life was recently measured at 110 milliseconds, and is believed an important isotope in supernova nucleosynthesis of elements heavier than iron. The nuclide Ni, discovered in 1999, is the most proton-rich heavy element isotope known. With 28 protons and 20 neutrons Ni is ""double magic"", as is with 28 protons and 50 neutrons. Both are therefore unusually stable for nuclides with so large a proton-neutron imbalance. On Earth, nickel occurs most often in combination with sulfur and iron in pentlandite, with sulfur in millerite, with arsenic in the mineral nickeline, and with arsenic and sulfur"
"In total, only five isotopes have half-lives exceeding one hour (astatine-207 to -211). The least stable ground state isotope is astatine-213, with a half-life of 125 nanoseconds. It undergoes alpha decay to the extremely long-lived bismuth-209. Astatine has 24 known nuclear isomers, which are nuclei with one or more nucleons (protons or neutrons) in an excited state. A nuclear isomer may also be called a ""meta-state"", meaning the system has more internal energy than the ""ground state"" (the state with the lowest possible internal energy), making the former likely to decay into the latter. There may be more than one"
"isotope, because it has a nucleus with 126 neutrons, and 126 is a magic number corresponding to a filled neutron shell. Despite having a similar half-life to the previous isotope (8.1 hours for astatine-210 and 7.2 hours for astatine-211), the alpha decay probability is much higher for the latter: 41.81% against only 0.18%. The two following isotopes release even more energy, with astatine-213 releasing the most energy. For this reason, it is the shortest-lived astatine isotope. Even though heavier astatine isotopes release less energy, no long-lived astatine isotope exists, because of the increasing role of beta decay (electron emission). This"
"nuclear isomers. For example, there are two stable isotopes of chlorine: with 35 − 17 = 18 neutrons and with 37 − 17 = 20 neutrons. In chemistry, the term proton refers to the hydrogen ion, . Since the atomic number of hydrogen is 1, a hydrogen ion has no electrons and corresponds to a bare nucleus, consisting of a proton (and 0 neutrons for the most abundant isotope ""protium"" ). The proton is a ""bare charge"" with only about 1/64,000 of the radius of a hydrogen atom, and so is extremely reactive chemically. The free proton, thus, has an"
"emitting a beta particle and has a half-life of 0.8 seconds. Helium-7 also emits a beta particle as well as a gamma ray. The most widely studied heavy helium isotope is helium-8. This isotope, as well as helium-6, are thought to consist of a normal helium-4 nucleus surrounded by a neutron ""halo"" (containing two neutrons in and four neutrons in ). Halo nuclei have become an area of intense research. Isotopes up to helium-10, with two protons and eight neutrons, have been confirmed. Helium-7 and helium-8 are hyperfragments that are created in certain nuclear reactions. , despite being a doubly"
"isotope of thorium with 138 neutrons. It was once named Radiothorium, due to its occurrence in the disintegration chain of thorium-232. It has a half-life of 1.9116 years. It undergoes alpha decay to Ra. Occasionally it decays by the unusual route of cluster decay, emitting a nucleus of O and producing stable Pb. It is a daughter isotope of U. Th-228 has an atomic weight of 228.0287411 grams/mole. Uranium-232 decays to this nuclide by alpha emission. Th is a radioactive isotope of thorium that decays by alpha emission with a half-life of 7340 years. Th is produced by the decay"
"Bismuth-209 Bismuth-209 is the isotope of bismuth with the longest known half-life of any radioisotope that undergoes α-decay (alpha decay). It has 83 protons and a magic number of 126 neutrons, and an atomic mass of 208.9803987 amu (atomic mass units). All of the primordial bismuth is of this isotope. It is also the β daughter of lead-209. Bismuth-209 was long thought to have the heaviest stable nucleus of any element, but in 2003, Noël Coron and his colleagues at the Institut d’Astrophysique Spatiale in Orsay, France, discovered that Bi undergoes alpha decay with a half-life of approximately 19 exayears"
"36.345 days. All other isotopes have half-lives less than 12 days, most less than 20 hours. The shortest-lived isotope, Xe, has a half-life of 58 µs, and is the heaviest known nuclide with equal numbers of protons and neutrons. Of known isomers, the longest-lived is Xe with a half-life of 11.934 days. Xe is produced by beta decay of I (half-life: 16 million years); Xe, Xe, Xe, and Xe are some of the fission products of both U and Pu, so are used as indicators of nuclear explosions. The artificial isotope Xe is of considerable significance in the operation of"
"protons and electrons, and 5 neutrons. It has a spin of 3/2-, and a half-life of 8.58 ms. Its atomic mass is 13.0248 Da. It decays to nitrogen-13 by electron capture, and has a decay energy of 17.765 MeV. Its parent nuclide is fluorine-14. Oxygen-15 is an isotope of oxygen, frequently used in positron emission tomography, or PET imaging. It can be used, amongst other applications, in water for PET myocardial perfusion imaging and for brain imaging. It has 8 protons, 7 neutrons, and 8 electrons. The total atomic mass is 15.0030654 amu. It has a half-life of 122.24 seconds."
"upon equally by the strong interaction, which is invariant under rotation in isospin space. According to the Noether theorem, isospin is conserved with respect to the strong interaction. Protons and neutrons are best known in their role as nucleons, i.e., as the components of atomic nuclei, but they also exist as free particles. Free neutrons are unstable, with a half-life of around 13 minutes, but they are common in nature and have important applications (see neutron radiation and neutron scattering). Singular protons, not bound to other nucleons, are usually regarded as the nuclei of hydrogen atoms or ions, but in"
"(with the chemical symbol H) is a lone proton. The nuclei of the heavy hydrogen isotopes deuterium (D or H) and tritium (T or H) contain one proton bound to one and two neutrons, respectively. All other types of atomic nuclei are composed of two or more protons and various numbers of neutrons. The most common nuclide of the common chemical element lead, Pb, has 82 protons and 126 neutrons, for example. The table of nuclides comprises all the known nuclides. Even though it is not a chemical element, the neutron is included in this table. The free neutron has"
"Nickel-62 Nickel-62 is an isotope of nickel having 28 protons and 34 neutrons. It is a stable isotope, with the highest binding energy per nucleon of any known nuclide (8.7945 MeV). It is often stated that Fe is the ""most stable nucleus"", but only because Fe has the lowest ""mass"" per nucleon (not binding energy per nucleon) of all nuclides. The lower mass per nucleon of Fe-56 is possible because Fe has 26/56 = 46.43% protons, while Ni has only 28/62 = 45.16% protons; and the larger fraction of lighter protons in Fe lowers its mean mass-per-nucleon ratio, despite having"
"Atomic nuclei with an odd number of protons are less stable than those with even numbers, even when the total number of nucleons (protons + neutrons) is even, and odd numbered elements have fewer stable isotopes. The most stable radioactive isotopes are technetium-98 with a half-life of 4.2 million years (Ma), technetium-97 with 2.6 Ma, and technetium-99 with 211,000 years. Thirty other radioisotopes have been characterized with mass numbers ranging from 85 to 118. Most of these have half-lives that are less than an hour, the exceptions being technetium-93 (half-life: 2.73 hours), technetium-94 (half-life: 4.88 hours), technetium-95 (half-life: 20 hours),"
"found to be 100 pm to two significant figures. The enthalpy of hydration of No has been calculated as 1486 kJ/mol. Twelve isotopes of nobelium are known, with mass numbers 250–260 and 262; all are radioactive. Additionally, nuclear isomers are known for mass numbers 251, 253, and 254. Of these, the longest-lived isotope is No with a half-life of 58 minutes, and the longest-lived isomer is No with a half-life of 1.7 seconds. However, the still undiscovered isotope No is predicted to have a still longer half-life of 170 min. Additionally, the shorter-lived No (half-life 3.1 minutes) is more often"
"nuclei. It is prevented from having a stable isotope with 4 protons and 6 neutrons by the very large mismatch in proton/neutron ratio for such a light element. (Nevertheless, beryllium-10 has a half-life of 1.36 million years, which is too short to be primordial, but still indicates unusual stability for a light isotope with such an imbalance.) The set of monoisotopic elements overlap but are not the same as the set of 22 mononuclidic elements, which are characterized as having essentially only one isotope (nuclide) found in nature. The reason for this is the occurrence of certain long-lived radioactive primordial"
"129, 131, 132 and 136, have half-lives between a day and two weeks, while most of the other isotopes have half-lives from a few seconds to fractions of a second. At least 21 metastable nuclear isomers exist. Other than Cs (with a half-life of just under 3 hours), all are very unstable and decay with half-lives of a few minutes or less. The isotope Cs is one of the long-lived fission products of uranium produced in nuclear reactors. However, this fission product yield is reduced in most reactors because the predecessor, Xe, is a potent neutron poison and frequently transmutes"
"contain an excess of neutrons is also possible, but is hindered because positrons are repelled by the positive nucleus, and quickly annihilate when they encounter electrons. Three types of beta decay in competition are illustrated by the single isotope copper-64 (29 protons, 35 neutrons), which has a half-life of about 12.7 hours. This isotope has one unpaired proton and one unpaired neutron, so either the proton or the neutron can decay. This particular nuclide is almost equally likely to undergo proton decay (by positron emission, 18% or by electron capture, 43%) or neutron decay (by electron emission, 39%). The mass"
"than and including Pa are isotopes of actinium and the primary decay products for the heavier isotopes of protactinium are isotopes of uranium. Protactinium-230 has 139 neutrons and a half-life of 17.4 days. It undergoes beta-minus decay to U. It is not found in nature because its half-life is so short and it is not found in the decay chains of U, U, or Th. It has a mass of 230.034541 u. Protactinium-231 is the longest-lived isotope of protactinium, with a half-life of 32,760 years. In nature, it is found in trace amounts as part of the actinium series, which"
"appearing to have an even longer half-life of about 690 s. The unknown isotopes Bh and Bh are predicted to have even longer half-lives of around 90 minutes and 40 minutes respectively. Before its discovery, Bh was also predicted to have a half-life of 90 minutes, but it was found to have a half-life of only about 40 seconds. The proton-rich isotopes with masses 260, 261, and 262 were directly produced by cold fusion, those with mass 262 and 264 were reported in the decay chains of meitnerium and roentgenium, while the neutron-rich isotopes with masses 265, 266, 267 were"
"isotopes of carbon, while most of the isotopes with masses above 15 decay to isotopes of oxygen. The shortest-lived known isotope is nitrogen-10, with a half-life of about 2.3 microseconds. Nitrogen-14 is one of two stable (non-radioactive) isotopes of the chemical element nitrogen, which makes about 99.636% of natural nitrogen. Nitrogen-14 is one of the very few stable nuclides with both an odd number of protons and of neutrons (seven each) and is the only one to make up a majority of its element. Each of proton or neutron contributes a nuclear spin of plus or minus spin 1/2, giving"
"quantum shells correspond to a set of energy levels within the shell model of the nucleus; filled shells, such as the filled shell of 50 protons for tin, confers unusual stability on the nuclide. Of the 254 known stable nuclides, only four have both an odd number of protons ""and"" odd number of neutrons: hydrogen-2 (deuterium), lithium-6, boron-10 and nitrogen-14. Also, only four naturally occurring, radioactive odd–odd nuclides have a half-life over a billion years: potassium-40, vanadium-50, lanthanum-138 and tantalum-180m. Most odd–odd nuclei are highly unstable with respect to beta decay, because the decay products are even–even, and are therefore"
"Isotone Two nuclides are isotones if they have the same neutron number ""N"", but different proton number ""Z"". For example, boron-12 and carbon-13 nuclei both contain 7 neutrons, and so are isotones. Similarly, S, Cl, Ar, K, and Ca nuclei are all isotones of 20 because they all contain 20 neutrons. Despite its similarity to the Greek for ""same stretching"", the term was formed by the German physicist K. Guggenheimer by changing the ""p"" in ""isotope"" from ""p"" for ""proton"" to ""n"" for ""neutron"". The largest numbers of observationally stable nuclides exist for isotones 50 (five: Kr, Sr, Y, Zr,"
"Plutonium-244 Plutonium-244 (Pu) is an isotope of plutonium that has a half-life of 80 million years. This is longer than any of the other isotopes of plutonium and longer than any other actinide isotope except for the three naturally abundant ones: uranium-235 (704 million years), uranium-238 (4.468 billion years), and thorium-232 (14.05 billion years). Accurate measurements, beginning in the early 1970s, have detected primordial plutonium-244, making it the shortest-lived primordial nuclide. The amount of Pu in the pre-Solar nebula (4.57×10 years ago) was estimated as 0.008 of amount of U. As the age of the Earth is about 57 half-lives"