Isotopes of neptunium
Neptunium (93Np) is usually considered an artificial element, although trace quantities are found in nature, so a standard atomic weight cannot be given. Like all trace or artificial elements, it has no stable isotopes. The first isotope to be synthesized and identified was 239Np in 1940, produced by bombarding 238U with neutrons to produce 239U, which then underwent beta decay to 239Np.
Twenty-five neptunium radioisotopes have been characterized, with the most stable being 237
with a half-life of 2.14 million years, 236
with a half-life of 154,000 years, and 235
with a half-life of 396.1 days. All of the remaining radioactive isotopes have half-lives that are less than 4.5 days, and the majority of these have half-lives that are less than 50 minutes. This element also has 4 meta states, with the most stable being 236m
(t1/2 22.5 hours).
The isotopes of neptunium range from 219
, though the intermediate isotope 221
has not yet been observed. The primary decay mode before the most stable isotope, 237
, is electron capture (with a good deal of alpha emission), and the primary mode after is beta emission. The primary decay products before 237
are isotopes of uranium and protactinium, and the primary products after are isotopes of plutonium. Uranium-237 and neptunium-239 are regarded as the leading hazardous radioisotopes in the first hour-to-week period following nuclear fallout from a nuclear detonation, with 239Np dominating "the spectrum for several days."
List of isotopes
|Z||N||Isotopic mass (Da)
[n 2][n 3]
[n 6][n 7]
|Excitation energy[n 7]|
|93||131||224.03422(21)#||38(+26-11) μs||α (83%)||220m1Pa||1-#|
|93||134||227.03496(8)||510(60) ms||α (99.95%)||223Pa||5/2−#|
|93||135||228.03618(21)#||61.4(14) s||β+ (59%)||228U|
|β+, SF (.012%)||(various)|
|93||136||229.03626(9)||4.0(2) min||α (51%)||225Pa||5/2+#|
|93||137||230.03783(6)||4.6(3) min||β+ (97%)||230U|
|93||138||231.03825(5)||48.8(2) min||β+ (98%)||231U||(5/2)(+#)|
|93||139||232.04011(11)#||14.7(3) min||β+ (99.99%)||232U||(4+)|
|93||140||233.04074(5)||36.2(1) min||β+ (99.99%)||233U||(5/2+)|
|93||143||236.04657(5)||1.54(6)×105 y||EC (87.3%)||236U||(6−)|
|60(50) keV||22.5(4) h||EC (52%)||236U||1|
[n 8][n 9]
|93||144||237.0481734(20)||2.144(7)×106 y||α||233Pa||5/2+||Trace[n 10]|
|2300(200)# keV||112(39) ns|
|93||146||239.0529390(22)||2.356(3) d||β−||239Pu||5/2+||Trace[n 10]|
|93||147||240.056162(16)||61.9(2) min||β−||240Pu||(5+)||Trace[n 11]|
|20(15) keV||7.22(2) min||β− (99.89%)||240Pu||1(+)|
|0(50)# keV||5.5(1) min||6+#|
|This table header & footer:|
- mNp – Excited nuclear isomer.
- ( ) – Uncertainty (1σ) is given in concise form in parentheses after the corresponding last digits.
- # – Atomic mass marked #: value and uncertainty derived not from purely experimental data, but at least partly from trends from the Mass Surface (TMS).
Modes of decay:
CD: Cluster decay EC: Electron capture IT: Isomeric transition SF: Spontaneous fission
- Bold italics symbol as daughter – Daughter product is nearly stable.
- ( ) spin value – Indicates spin with weak assignment arguments.
- # – Values marked # are not purely derived from experimental data, but at least partly from trends of neighboring nuclides (TNN).
- Fissile nuclide
- Most common nuclide
- Produced by neutron capture in uranium ore
- Intermediate decay product of 244Pu
Actinides vs fission products
|Actinides by decay chain||Half-life
|Fission products of 235U by yield|
No fission products
... nor beyond 15.7 Ma
Legend for superscript symbols
Neptunium-235 has 142 neutrons and a half-life of 396.1 days. This isotope decays by:
- Alpha emission: the decay energy is 5.2 MeV and the decay product is protactinium-231.
- Electron capture: the decay energy is 0.125 MeV and the decay product is uranium-235
This isotope of neptunium has a weight of 235.044 063 3 u.
Neptunium-236 has 143 neutrons and a half-life of 154,000 years. It can decay by the following methods:
- Electron capture: the decay energy is 0.93 MeV and the decay product is uranium-236. This usually decays (with a half-life of 23 million years) to thorium-232.
- Beta emission: the decay energy is 0.48 MeV and the decay product is plutonium-236. This usually decays (half-life 2.8 years) to uranium-232, which usually decays (half-life 69 years) to thorium-228, which decays in a few years to lead-208.
- Alpha emission: the decay energy is 5.007 MeV and the decay product is protactinium-232. This decays with a half-life of 1.3 days to uranium-232.
is produced in small quantities via the (n,2n) and (γ,n) capture reactions of 237
, however, it is nearly impossible to separate in any significant quantities from its parent 237
. It is for this reason that despite its low critical mass and high neutron cross section, it has not been researched as a nuclear fuel in weapons or reactors. Nevertheless, 236
has been considered for use in mass spectrometry and as a radioactive tracer, because it decays predominantly by beta emission with a long half-life. Several alternative production routes for this isotope have been investigated, namely those that reduce isotopic separation from 237
or the isomer 236m
. The most favorable reactions to accumulate 236
were shown to be proton and deuteron irradiation of uranium-238.
In 2002, 237
was shown to be capable of sustaining a chain reaction with fast neutrons, as in a nuclear weapon, with a critical mass of around 60 kg. However, it has a low probability of fission on bombardment with thermal neutrons, which makes it unsuitable as a fuel for light water nuclear power plants (as opposed to fast reactor or accelerator-driven systems, for example).
is the only neptunium isotope produced in significant quantity in the nuclear fuel cycle, both by successive neutron capture by uranium-235 (which fissions most but not all of the time) and uranium-236, or (n,2n) reactions where a fast neutron occasionally knocks a neutron loose from uranium-238 or isotopes of plutonium. Over the long term, 237
also forms in spent nuclear fuel as the decay product of americium-241.
Use in plutonium-238 production
When exposed to neutron bombardment 237
can capture a neutron, undergo beta decay, and become 238
, this product being useful as an thermal energy source in a radio-isotope thermoelectric generator for the production of electricity and heat in deep space probes (such as the New Horizons and Voyager probes) and, of recent note, the Mars Science Laboratory (Curiosity rover). These applications are economically practical where photovoltaic power sources are weak or inconsistent due to probes being too far from the sun or rovers facing climate events that may obstruct sunlight for long periods. Space probes and rovers also make use of the heat output of the generator to keep their instruments and internals warm.
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- Plus radium (element 88). While actually a sub-actinide, it immediately precedes actinium (89) and follows a three-element gap of instability after polonium (84) where no nuclides have half-lives of at least four years (the longest-lived nuclide in the gap is radon-222 with a half life of less than four days). Radium's longest lived isotope, at 1,600 years, thus merits the element's inclusion here.
- Specifically from thermal neutron fission of uranium-235, e.g. in a typical nuclear reactor.
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"The isotopic analyses disclosed a species of mass 248 in constant abundance in three samples analysed over a period of about 10 months. This was ascribed to an isomer of Bk248 with a half-life greater than 9 [years]. No growth of Cf248 was detected, and a lower limit for the β− half-life can be set at about 104 [years]. No alpha activity attributable to the new isomer has been detected; the alpha half-life is probably greater than 300 [years]."
- This is the heaviest nuclide with a half-life of at least four years before the "Sea of Instability".
- Excluding those "classically stable" nuclides with half-lives significantly in excess of 232Th; e.g., while 113mCd has a half-life of only fourteen years, that of 113Cd is nearly eight quadrillion years.
- Final Report, Evaluation of nuclear criticality safety data and limits for actinides in transport Archived 2011-05-19 at the Wayback Machine, Republic of France, Institut de Radioprotection et de Sûreté Nucléaire, Département de Prévention et d'étude des Accidents.
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- Isotope masses from:
- Isotopic compositions and standard atomic masses from:
- de Laeter, John Robert; Böhlke, John Karl; De Bièvre, Paul; Hidaka, Hiroshi; Peiser, H. Steffen; Rosman, Kevin J. R.; Taylor, Philip D. P. (2003). "Atomic weights of the elements. Review 2000 (IUPAC Technical Report)". Pure and Applied Chemistry. 75 (6): 683–800. doi:10.1351/pac200375060683.
- Wieser, Michael E. (2006). "Atomic weights of the elements 2005 (IUPAC Technical Report)". Pure and Applied Chemistry. 78 (11): 2051–2066. doi:10.1351/pac200678112051. Lay summary.
- Half-life, spin, and isomer data selected from the following sources.
- Audi, Georges; Bersillon, Olivier; Blachot, Jean; Wapstra, Aaldert Hendrik (2003), "The NUBASE evaluation of nuclear and decay properties", Nuclear Physics A, 729: 3–128, Bibcode:2003NuPhA.729....3A, doi:10.1016/j.nuclphysa.2003.11.001
- National Nuclear Data Center. "NuDat 2.x database". Brookhaven National Laboratory.
- Holden, Norman E. (2004). "11. Table of the Isotopes". In Lide, David R. (ed.). CRC Handbook of Chemistry and Physics (85th ed.). Boca Raton, Florida: CRC Press. ISBN 978-0-8493-0485-9.