Isotopes of sodium

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Isotopes of sodium  (11Na)
Main isotopes [1] Decay
abun­dance half-life (t1/2) mode pro­duct
22Na trace 2.6019 y β+ 22Ne
23Na100% stable
24Natrace14.9560 h β− 24Mg
Standard atomic weight Ar°(Na)

There are 20 isotopes of sodium (11Na), ranging from 17
Na to 39
Na (except for the still-unknown 36Na and 38Na), [4] and five isomers (two for 22
Na, and one each for 24
Na, 26
Na, and 32
Na). 23
Na is the only stable (and the only primordial) isotope. It is considered a monoisotopic element and it has a standard atomic weight of 22.98976928(2). Sodium has two radioactive cosmogenic isotopes (22
Na, with a half-life of 2.6019(6) years; [nb 1] and 24
Na , with a half-life of 14.9560(15) h). With the exception of those two isotopes, all other isotopes have half-lives under a minute, most under a second. The shortest-lived is the unbound 18
Na, with a half-life of 1.3(4)×10−21 seconds (although the half-life of the similarly unbound 17Na is not measured).

Contents

Acute neutron radiation exposure (e.g., from a nuclear criticality accident) converts some of the stable 23
Na (in the form of Na+ ion) in human blood plasma to 24
Na. By measuring the concentration of this isotope, the neutron radiation dosage to the victim can be computed.

22
Na is a positron-emitting isotope with a remarkably long half-life. It is used to create test-objects and point-sources for positron emission tomography.

List of isotopes


Nuclide
[n 1] 		Z N Isotopic mass (Da) [5]
[n 2] [n 3] 		Half-life [1]
[n 4] 		Decay
mode [1]
[n 5] 		Daughter
isotope
[n 6] 		Spin and
parity [1]
[n 7] [n 4] 		Isotopic
abundance
Excitation energy
17
Na
11617.037270(60) p 16
Ne
(1/2+)
18
Na
11718.02688(10)1.3(4) zsp=? [n 8] 17
Ne
1−#
19
Na
11819.013880(11)> 1 asp18
Ne
(5/2+)
20
Na
11920.0073543(12)447.9(2.3) msβ+ (75.0(4)%)20
Ne
2+
β+α (25.0(4)%)16
O
21
Na
111020.99765446(5)22.4550(54) sβ+21
Ne
3/2+
22
Na
 		111121.99443742(18)2.6019(6) y [nb 1] β+ (90.57(8)%)22
Ne
3+Trace [n 9]
ε (9.43(6)%)22
Ne
22m1
Na
583.05(10) keV243(2) ns IT 22
Na
1+
22m2
Na
657.00(14) keV19.6(7) psIT22
Na
0+
23
Na
111222.9897692820(19)Stable3/2+1
24
Na
 		111323.990963012(18)14.9560(15) hβ−24
Mg
4+Trace [n 9]
24m
Na
472.2074(8) keV20.18(10) msIT (99.95%)24
Na
1+
β− (0.05%)24
Mg
25
Na
111424.9899540(13)59.1(6) sβ−25
Mg
5/2+
26
Na
111525.992635(4)1.07128(25) sβ−26
Mg
3+
26m
Na
82.4(4) keV4.35(16) μsIT26
Na
1+
27
Na
111626.994076(4)301(6) msβ− (99.902(24)%)27
Mg
5/2+
β−n (0.098(24)%)26
Mg
28
Na
111727.998939(11)33.1(1.3) msβ− (99.42(12)%)28
Mg
1+
β−n (0.58(12)%)27
Mg
29
Na
111829.002877(8)43.2(4) msβ− (78%)29
Mg
3/2+
β−n (22(3)%)28
Mg
β−2n ? [n 10] 27
Mg
 ?
30
Na
111930.009098(5)45.9(7) msβ− (70.2(2.2)%)30
Mg
2+
β−n (28.6(2.2)%)29
Mg
β−2n (1.24(19)%)28
Mg
β−α (5.5(2)%×10−5)26
Ne
31
Na
112031.013147(15)16.8(3) msβ− (> 63.2(3.5)%)31
Mg
3/2+
β−n (36.0(3.5)%)30
Mg
β−2n (0.73(9)%)29
Mg
β−3n (< 0.05%)28
Mg
32
Na
112132.020010(40)12.9(3) msβ− (66.4(6.2)%)32
Mg
(3−)
β−n (26(6)%)31
Mg
β−2n (7.6(1.5)%)30
Mg
32m
Na
 [6] 		625 keV24(2) μsIT32
Na
(0+,6−)
33
Na
112233.02553(48)8.2(4) msβ−n (47(6)%)32
Mg
(3/2+)
β− (40.0(6.7)%)33
Mg
β−2n (13(3)%)31
Mg
34
Na
112334.03401(64)5.5(1.0) msβ−2n (~50%)32
Mg
1+
β− (~35%)34
Mg
β−n (~15%)33
Mg
35
Na
112435.04061(72)#1.5(5) msβ−35
Mg
3/2+#
β−n ? [n 10] 34
Mg
 ?
β−2n ? [n 10] 33
Mg
 ?
37
Na
112637.05704(74)#1# ms [> 1.5 μs]β− ? [n 10] 37
Mg
 ?		3/2+#
β−n ? [n 10] 36
Mg
 ?
β−2n ? [n 10] 35
Mg
 ?
39
Na
 [4] 		112839.07512(80)#1# ms [> 400 ns]β− ? [n 10] 39
Mg
 ?		3/2+#
β−n ? [n 10] 38
Mg
 ?
β−2n ? [n 10] 37
Mg
 ?
This table header & footer:
  1. ↑ mNa – Excited nuclear isomer.
  2. ↑ ( ) – Uncertainty (1σ) is given in concise form in parentheses after the corresponding last digits.
  3. ↑ # – Atomic mass marked #: value and uncertainty derived not from purely experimental data, but at least partly from trends from the Mass Surface (TMS).
  4. 1 2 # – Values marked # are not purely derived from experimental data, but at least partly from trends of neighboring nuclides (TNN).
  5. ↑ Modes of decay:
    IT: Isomeric transition
    n: Neutron emission
    p: Proton emission
  6. ↑ Bold symbol as daughter – Daughter product is stable.
  7. ↑ ( ) spin value – Indicates spin with weak assignment arguments.
  8. ↑ Decay mode shown has been observed, but its intensity is not known experimentally.
  9. 1 2 Cosmogenic nuclide
  10. 1 2 3 4 5 6 7 8 9 Decay mode shown is energetically allowed, but has not been experimentally observed to occur in this nuclide.

Sodium-22

Disk containing 1 mCi of sodium-22 Sodium-22, 1-microcurie disk.jpg
Disk containing 1 μCi of sodium-22

Sodium-22 is a radioactive isotope of sodium, undergoing positron emission to 22
Ne with a half-life of 2.6019(6) years. 22
Na is being investigated as an efficient generator of "cold positrons" (antimatter) to produce muons for catalyzing fusion of deuterium.[ citation needed ] It is also commonly used as a positron source in positron annihilation spectroscopy. [7]

Sodium-23

Sodium-23 is an isotope of sodium with an atomic mass of 22.98976928. It is the only stable isotope of sodium and also the only primordial isotope. Because of its abundance, sodium-23 is used in nuclear magnetic resonance in various research fields, including materials science and battery research. [8] Sodium-23 relaxation has applications in studying cation-biomolecule interactions, intracellular and extracellular sodium, ion transport in batteries, and quantum information processing. [9]

Sodium-24

Sodium-24 is radioactive and can be created from common sodium-23 by neutron activation. With a half-life of 14.9560(15) h, 24
Na decays to 24
Mg by emission of an electron and two gamma rays. [10] [11]

Exposure of the human body to intense neutron radiation creates 24
Na in the blood plasma. Measurements of its quantity can be done to determine the absorbed radiation dose of a patient. [11] This can be used to determine the type of medical treatment required.

When sodium is used as coolant in fast breeder reactors, 24
Na is created, which makes the coolant radioactive. When the 24
Na decays, it causes a buildup of magnesium in the coolant. Since the half-life is short, the 24
Na portion of the coolant ceases to be radioactive within a few days after removal from the reactor. Leakage of the hot sodium from the primary loop may cause radioactive fires, [12] as it can ignite in contact with air (and explodes in contact with water). For this reason the primary cooling loop is within a containment vessel.

Sodium has been proposed as a casing for a salted bomb, as it would convert to 24
Na and produce intense gamma-ray emissions for a few days. [13] [14]

Notes

  1. 1 2 Note that NUBASE2020 uses the tropical year to convert between years and other units of time, not the Gregorian year. The relationship between years and other time units in NUBASE2020 is as follows: 1 y = 365.2422 d = 31 556 926 s

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Hydrogen (1H) has three naturally occurring isotopes: 1H, 2H, and 3H. 1H and 2H are stable, while 3H has a half-life of 12.32(2) years. Heavier isotopes also exist; all are synthetic and have a half-life of less than 1 zeptosecond (10−21 s). Of these, 5H is the least stable, while 7H is the most.

Fluorine (9F) has 19 known isotopes ranging from 13
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 to 31
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 and two isomers. Only fluorine-19 is stable and naturally occurring in more than trace quantities; therefore, fluorine is a monoisotopic and mononuclidic element.

Astatine (85At) has 41 known isotopes, all of which are radioactive; their mass numbers range from 188 to 229. There are also 24 known metastable excited states. The longest-lived isotope is 210At, which has a half-life of 8.1 hours; the longest-lived isotope existing in naturally occurring decay chains is 219At with a half-life of 56 seconds.

<span class="mw-page-title-main">Isotopes of thallium</span>

Thallium (81Tl) has 41 isotopes with atomic masses that range from 176 to 216. 203Tl and 205Tl are the only stable isotopes and 204Tl is the most stable radioisotope with a half-life of 3.78 years. 207Tl, with a half-life of 4.77 minutes, has the longest half-life of naturally occurring Tl radioisotopes. All isotopes of thallium are either radioactive or observationally stable, meaning that they are predicted to be radioactive but no actual decay has been observed.

There are two natural isotopes of iridium (77Ir), and 37 radioisotopes, the most stable radioisotope being 192Ir with a half-life of 73.83 days, and many nuclear isomers, the most stable of which is 192m2Ir with a half-life of 241 years. All other isomers have half-lives under a year, most under a day. All isotopes of iridium are either radioactive or observationally stable, meaning that they are predicted to be radioactive but no actual decay has been observed.

Natural tantalum (73Ta) consists of two stable isotopes: 181Ta (99.988%) and 180m
Ta
 (0.012%).

Naturally occurring erbium (68Er) is composed of six stable isotopes, with 166Er being the most abundant. Thirty-nine radioisotopes have been characterized with between 74 and 112 neutrons, or 142 to 180 nucleons, with the most stable being 169Er with a half-life of 9.4 days, 172Er with a half-life of 49.3 hours, 160Er with a half-life of 28.58 hours, 165Er with a half-life of 10.36 hours, and 171Er with a half-life of 7.516 hours. All of the remaining radioactive isotopes have half-lives that are less than 3.5 hours, and the majority of these have half-lives that are less than 4 minutes. This element also has numerous meta states, with the most stable being 167mEr.

Caesium (55Cs) has 41 known isotopes, the atomic masses of these isotopes range from 112 to 152. Only one isotope, 133Cs, is stable. The longest-lived radioisotopes are 135Cs with a half-life of 1.33 million years, 137
Cs
 with a half-life of 30.1671 years and 134Cs with a half-life of 2.0652 years. All other isotopes have half-lives less than 2 weeks, most under an hour.

Tin (50Sn) is the element with the greatest number of stable isotopes. This is probably related to the fact that 50 is a "magic number" of protons. In addition, twenty-nine unstable tin isotopes are known, including tin-100 (100Sn) and tin-132 (132Sn), which are both "doubly magic". The longest-lived tin radioisotope is tin-126 (126Sn), with a half-life of 230,000 years. The other 28 radioisotopes have half-lives of less than a year.

Naturally occurring zirconium (40Zr) is composed of four stable isotopes (of which one may in the future be found radioactive), and one very long-lived radioisotope (96Zr), a primordial nuclide that decays via double beta decay with an observed half-life of 2.0×1019 years; it can also undergo single beta decay, which is not yet observed, but the theoretically predicted value of t1/2 is 2.4×1020 years. The second most stable radioisotope is 93Zr, which has a half-life of 1.53 million years. Thirty other radioisotopes have been observed. All have half-lives less than a day except for 95Zr (64.02 days), 88Zr (83.4 days), and 89Zr (78.41 hours). The primary decay mode is electron capture for isotopes lighter than 92Zr, and the primary mode for heavier isotopes is beta decay.

Bromine (35Br) has two stable isotopes, 79Br and 81Br, and 35 known radioisotopes, the most stable of which is 77Br, with a half-life of 57.036 hours.

Germanium (32Ge) has five naturally occurring isotopes, 70Ge, 72Ge, 73Ge, 74Ge, and 76Ge. Of these, 76Ge is very slightly radioactive, decaying by double beta decay with a half-life of 1.78 × 1021 years (130 billion times the age of the universe).

Natural gallium (31Ga) consists of a mixture of two stable isotopes: gallium-69 and gallium-71. Twenty-nine radioisotopes are known, all synthetic, with atomic masses ranging from 60 to 89; along with three nuclear isomers, 64mGa, 72mGa and 74mGa. Most of the isotopes with atomic mass numbers below 69 decay to isotopes of zinc, while most of the isotopes with masses above 71 decay to isotopes of germanium. Among them, the most commercially important radioisotopes are gallium-67 and gallium-68.

Potassium has 25 known isotopes from 34
K to 57
K as well as 31
K, as well as an unconfirmed report of 59
K. Three of those isotopes occur naturally: the two stable forms 39
K (93.3%) and 41
K (6.7%), and a very long-lived radioisotope 40
K (0.012%)

Argon (18Ar) has 26 known isotopes, from 29Ar to 54Ar, of which three are stable. On the Earth, 40Ar makes up 99.6% of natural argon. The longest-lived radioactive isotopes are 39Ar with a half-life of 268 years, 42Ar with a half-life of 32.9 years, and 37Ar with a half-life of 35.04 days. All other isotopes have half-lives of less than two hours, and most less than one minute.

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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 238
U
 with neutrons to produce 239
U
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Np
.

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References

  1. 1 2 3 4 Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  2. ↑ "Standard Atomic Weights: Sodium". CIAAW. 2005.
  3. ↑ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN   1365-3075.
  4. 1 2 Ahn, D.S.; et al. (2022-11-14). "Discovery of 39Na". Physical Review Letters . 129 (21) 212502: 212502. Bibcode:2022PhRvL.129u2502A. doi: 10.1103/PhysRevLett.129.212502 . PMID   36461972. S2CID   253591660.
  5. ↑ Wang, Meng; Huang, W.J.; Kondev, F.G.; Audi, G.; Naimi, S. (2021). "The AME 2020 atomic mass evaluation (II). Tables, graphs and references*". Chinese Physics C. 45 (3): 030003. doi:10.1088/1674-1137/abddaf.
  6. ↑ Gray, T. J.; Allmond, J. M.; Xu, Z.; King, T. T.; Lubna, R. S.; Crawford, H. L.; Tripathi, V.; Crider, B. P.; Grzywacz, R.; Liddick, S. N.; Macchiavelli, A. O.; Miyagi, T.; Poves, A.; Andalib, A.; Argo, E.; Benetti, C.; Bhattacharya, S.; Campbell, C. M.; Carpenter, M. P.; Chan, J.; Chester, A.; Christie, J.; Clark, B. R.; Cox, I.; Doetsch, A. A.; Dopfer, J.; Duarte, J. G.; Fallon, P.; Frotscher, A.; Gaballah, T.; Harke, J. T.; Heideman, J.; Huegen, H.; Holt, J. D.; Jain, R.; Kitamura, N.; Kolos, K.; Kondev, F. G.; Laminack, A.; Longfellow, B.; Luitel, S.; Madurga, M.; Mahajan, R.; Mogannam, M. J.; Morse, C.; Neupane, S.; Nowicki, A.; Ogunbeku, T. H.; Ong, W.-J.; Porzio, C.; Prokop, C. J.; Rasco, B. C.; Ronning, E. K.; Rubino, E.; Ruland, T. J.; Rykaczewski, K. P.; Schaedig, L.; Seweryniak, D.; Siegl, K.; Singh, M.; Stuchbery, A. E.; Tabor, S. L.; Tang, T. L.; Wheeler, T.; Winger, J. A.; Wood, J. L. (13 June 2023). "Microsecond Isomer at the N = 20 Island of Shape Inversion Observed at FRIB". Physical Review Letters. 130 (24). arXiv: 2302.11607 . doi:10.1103/PhysRevLett.130.242501.
  7. ↑ Saro, Matúš; Kršjak, Vladimír; Petriska, Martin; Slugeň, Vladimír (2019-07-29). "Sodium-22 source contribution determination in positron annihilation measurements using GEANT4". AIP Conference Proceedings. 2131 (1): 020039. Bibcode:2019AIPC.2131b0039S. doi:10.1063/1.5119492. ISSN   0094-243X. S2CID   201349680.
  8. ↑ Gotoh, Kazuma (8 February 2021). "23Na Solid-State NMR Analyses for Na-Ion Batteries and Materials". Batteries & Supercaps. 4 (8): 1267–127. doi:10.1002/batt.202000295. S2CID   233827472.
  9. ↑ Song, Yifan; Yin, Yu; Chen, Qinlong; Marchetti, Alessandro; Kong, Xueqian (2023). "23Na relaxometry: An overview of theory and applications". Magnetic Resonance Letters. 3 (2): 150–174. doi: 10.1016/j.mrl.2023.04.001 .
  10. ↑ "sodium-24". Encyclopædia Britannica.
  11. 1 2 Ekendahl, Daniela; Rubovič, Peter; Žlebčík, Pavel; Hupka, Ivan; Huml, Ondřej; Bečková, Věra; Malá, Helena (7 November 2019). "Neutron dose assessment using samples of human blood and hair". Radiation Protection Dosimetry. 186 (2–3): 202–205. doi:10.1093/rpd/ncz202. PMID   31702764.
  12. ↑ Unusual occurrences during LMFR operation, Proceedings of a Technical Committee meeting held in Vienna, 9–13 November 1998, IAEA. Pages 84, 122.
  13. ↑ "Science: fy for Doomsday" . Time . November 24, 1961. Archived from the original on March 14, 2016.
  14. ↑ Clark, W. H. (1961). "Chemical and Thermonuclear Explosives". Bulletin of the Atomic Scientists . 17 (9): 356–360. Bibcode:1961BuAtS..17i.356C. doi:10.1080/00963402.1961.11454268.
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