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{{more footnotes needed|date=August 2017}}
{{more footnotes needed|date=August 2017}}
{{infobox sodium isotopes}}
{{infobox sodium isotopes}}
There are 21 isotopes of [[sodium]] (<sub>11</sub>Na), ranging from {{chem|17|Na}} to {{chem|39|Na}},<ref name="RikenNa39">{{cite journal |last=Ahn |first=D.S. |display-authors=etal |title=Discovery of <sup>39</sup>Na |journal=[[Physical Review Letters]] |volume=129 |issue=21 |article-number=212502 |date=2022-11-14 |page=212502 |url=https://physics.aps.org/featured-article-pdf/10.1103/PhysRevLett.129.212502 |doi=10.1103/PhysRevLett.129.212502|pmid=36461972 |s2cid=253591660 }}</ref> and two [[nuclear isomer|isomers]] ({{chem|22m|Na}} and {{chem|24m|Na}}). {{chem|23|Na}} is the only [[stable nuclide|stable]] (and the only [[primordial nuclide|primordial]]) isotope. It is considered a [[monoisotopic element]] and it has a [[standard atomic weight]] of {{val|22.98976928|(2)}}. Sodium has two [[radioactive]] [[cosmogenic]] isotopes ({{chem|22|Na}}, with a [[half-life]] of {{val|2.6019|(6)|u=years}};{{refn|group=nb|name=NUBASE2020 tropical year|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: {{nowrap|1=1 y = 365.2422 d = 31 556 926 s}} }} and {{chem|link=Sodium-24|24|Na}}, with a half-life of {{val|14.9560|(15)|u=hours}}). With the exception of those two isotopes, all other isotopes have [[half-lives]] under a minute, most under a second. The shortest-lived is {{chem|18|Na}}, with a half-life of {{val|1.3|(4)|e=−21}} seconds.
There are 21 isotopes of [[sodium]] (<sub>11</sub>Na), ranging from {{chem|17|Na}} to {{chem|39|Na}},<ref name="RikenNa39">{{cite journal |last=Ahn |first=D.S. |display-authors=etal |title=Discovery of <sup>39</sup>Na |journal=[[Physical Review Letters]] |volume=129 |issue=21 |article-number=212502 |date=2022-11-14 |page=212502 |url=https://physics.aps.org/featured-article-pdf/10.1103/PhysRevLett.129.212502 |doi=10.1103/PhysRevLett.129.212502|pmid=36461972 |bibcode=2022PhRvL.129u2502A |s2cid=253591660 }}</ref> and two [[nuclear isomer|isomers]] ({{chem|22m|Na}} and {{chem|24m|Na}}). {{chem|23|Na}} is the only [[stable nuclide|stable]] (and the only [[primordial nuclide|primordial]]) isotope. It is considered a [[monoisotopic element]] and it has a [[standard atomic weight]] of {{val|22.98976928|(2)}}. Sodium has two [[radioactive]] [[cosmogenic]] isotopes ({{chem|22|Na}}, with a [[half-life]] of {{val|2.6019|(6)|u=years}};{{refn|group=nb|name=NUBASE2020 tropical year|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: {{nowrap|1=1 y = 365.2422 d = 31 556 926 s}} }} and {{chem|link=Sodium-24|24|Na}}, with a half-life of {{val|14.9560|(15)|u=hours}}). With the exception of those two isotopes, all other isotopes have [[half-lives]] under a minute, most under a second. The shortest-lived is {{chem|18|Na}}, with a half-life of {{val|1.3|(4)|e=−21}} seconds.


Acute neutron radiation exposure (e.g., from a nuclear [[criticality accident]]) converts some of the stable {{chem|23|Na}} in human blood plasma to {{chem|24|Na}}. By measuring the concentration of this isotope, the neutron radiation dosage to the victim can be computed.
Acute neutron radiation exposure (e.g., from a nuclear [[criticality accident]]) converts some of the stable {{chem|23|Na}} in human blood plasma to {{chem|24|Na}}. By measuring the concentration of this isotope, the neutron radiation dosage to the victim can be computed.
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==Sodium-22==
==Sodium-22==
Sodium-22 is a [[radioactive]] isotope of sodium, undergoing [[positron emission]] to {{chem|link=Isotopes of neon|22|Ne}} with a half-life of {{val|2.6019|(6)|u=years}}. {{chem|22|Na}} is being investigated as an efficient generator of "cold [[positron]]s" ([[antimatter]]) to produce [[muon]]s for [[Muon-catalyzed fusion|catalyzing fusion of deuterium]].{{Citation needed|date=February 2023}} It is also commonly used as a positron source in [[positron annihilation spectroscopy]].<ref>{{Cite journal|last1=Saro|first1=Matúš|last2=Kršjak|first2=Vladimír|last3=Petriska|first3=Martin|last4=Slugeň|first4=Vladimír|date=2019-07-29|title=Sodium-22 source contribution determination in positron annihilation measurements using GEANT4|url=https://aip.scitation.org/doi/abs/10.1063/1.5119492|journal=AIP Conference Proceedings|volume=2131|issue=1|pages=020039|doi=10.1063/1.5119492|s2cid=201349680 |issn=0094-243X}}</ref>
Sodium-22 is a [[radioactive]] isotope of sodium, undergoing [[positron emission]] to {{chem|link=Isotopes of neon|22|Ne}} with a half-life of {{val|2.6019|(6)|u=years}}. {{chem|22|Na}} is being investigated as an efficient generator of "cold [[positron]]s" ([[antimatter]]) to produce [[muon]]s for [[Muon-catalyzed fusion|catalyzing fusion of deuterium]].{{Citation needed|date=February 2023}} It is also commonly used as a positron source in [[positron annihilation spectroscopy]].<ref>{{Cite journal|last1=Saro|first1=Matúš|last2=Kršjak|first2=Vladimír|last3=Petriska|first3=Martin|last4=Slugeň|first4=Vladimír|date=2019-07-29|title=Sodium-22 source contribution determination in positron annihilation measurements using GEANT4|url=https://aip.scitation.org/doi/abs/10.1063/1.5119492|journal=AIP Conference Proceedings|volume=2131|issue=1|pages=020039|doi=10.1063/1.5119492|bibcode=2019AIPC.2131b0039S |s2cid=201349680 |issn=0094-243X}}</ref>


==Sodium-23==
==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 because of its abundance, it has been used for [[nuclear magnetic resonance]] in various research fields, including materials science and battery research.<ref>{{cite journal| last = Gotoh| first = Kazuma |title = 23Na Solid-State NMR Analyses for Na-Ion Batteries and Materials| date = 8 February 2021 | url = https://chemistry-europe.onlinelibrary.wiley.com/doi/10.1002/batt.202000295 | journal = Batteries & Supercaps
Sodium-23 is an isotope of sodium with an atomic mass of 22.98976928. It is the only stable isotope of sodium, and because of its abundance, it has been used for [[nuclear magnetic resonance]] in various research fields, including materials science and battery research.<ref>{{cite journal| last = Gotoh| first = Kazuma |title = 23Na Solid-State NMR Analyses for Na-Ion Batteries and Materials| date = 8 February 2021 | url = https://chemistry-europe.onlinelibrary.wiley.com/doi/10.1002/batt.202000295 | journal = Batteries & Supercaps
| volume = 4 |issue =8 | pages = 1267–127| doi = 10.1002/batt.202000295 }}</ref> Sodium-23 relaxation has applications in studying cation-biomolecule interactions, intracellular and extracellular sodium, ion transport in batteries, and quantum information processing.<ref>{{Cite journal| last1 = Song| first1 = Yifan| last2 = Yin | first2 = Yu| last3 = Chen| first3 = Qinlong| last4 = Marchetti| first4 = Alessandro | last5 = Kong| first5 = Xueqian| title = 23Na relaxometry: An overview of theory and applications| journal = Magnetic Resonance Letters| year = 2023 | volume =3| issue =2 |pages =150–174 | doi = 10.1016/j.mrl.2023.04.001| doi-access = free}}</ref>
| volume = 4 |issue =8 | pages = 1267–127| doi = 10.1002/batt.202000295 | s2cid = 233827472 }}</ref> Sodium-23 relaxation has applications in studying cation-biomolecule interactions, intracellular and extracellular sodium, ion transport in batteries, and quantum information processing.<ref>{{Cite journal| last1 = Song| first1 = Yifan| last2 = Yin | first2 = Yu| last3 = Chen| first3 = Qinlong| last4 = Marchetti| first4 = Alessandro | last5 = Kong| first5 = Xueqian| title = 23Na relaxometry: An overview of theory and applications| journal = Magnetic Resonance Letters| year = 2023 | volume =3| issue =2 |pages =150–174 | doi = 10.1016/j.mrl.2023.04.001| doi-access = free}}</ref>


==Sodium-24==
==Sodium-24==
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When sodium is used as coolant in [[fast breeder reactor]]s, {{chem|24|Na}} is created, which makes the coolant radioactive. When the {{chem|24|Na}} decays, it causes a buildup of magnesium in the coolant. Since the half-life is short, the {{chem|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,<ref>[https://www-pub.iaea.org/MTCD/Publications/PDF/te_1180_prn.pdf Unusual occurrences during LMFR operation], Proceedings of a Technical Committee meeting held in Vienna, 9–13 November 1998, [[International Atomic Energy Agency|IAEA]]. Pages 84, 122.</ref> 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.
When sodium is used as coolant in [[fast breeder reactor]]s, {{chem|24|Na}} is created, which makes the coolant radioactive. When the {{chem|24|Na}} decays, it causes a buildup of magnesium in the coolant. Since the half-life is short, the {{chem|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,<ref>[https://www-pub.iaea.org/MTCD/Publications/PDF/te_1180_prn.pdf Unusual occurrences during LMFR operation], Proceedings of a Technical Committee meeting held in Vienna, 9–13 November 1998, [[International Atomic Energy Agency|IAEA]]. Pages 84, 122.</ref> 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 {{chem|24|Na}} and produce intense gamma-ray emissions for a few days.<ref>{{cite magazine|magazine = [[Time (magazine)|Time]]|url = http://content.time.com/time/magazine/article/0,9171,828877,00.html|title = Science: fy for Doomsday|date = November 24, 1961|archive-url = https://web.archive.org/web/20160314102436/http://content.time.com/time/magazine/article/0,9171,828877,00.html|url-status = live|url-access = subscription|archive-date = March 14, 2016}}</ref><ref>{{cite journal | first=W. H. | last=Clark | title=Chemical and Thermonuclear Explosives | journal=[[Bulletin of the Atomic Scientists]] | year=1961 | volume=17 | issue=9 | pages=356–360 | doi=10.1080/00963402.1961.11454268}}</ref>
Sodium has been proposed as a casing for a [[salted bomb]], as it would convert to {{chem|24|Na}} and produce intense gamma-ray emissions for a few days.<ref>{{cite magazine|magazine = [[Time (magazine)|Time]]|url = http://content.time.com/time/magazine/article/0,9171,828877,00.html|title = Science: fy for Doomsday|date = November 24, 1961|archive-url = https://web.archive.org/web/20160314102436/http://content.time.com/time/magazine/article/0,9171,828877,00.html|url-status = live|url-access = subscription|archive-date = March 14, 2016}}</ref><ref>{{cite journal | first=W. H. | last=Clark | title=Chemical and Thermonuclear Explosives | journal=[[Bulletin of the Atomic Scientists]] | year=1961 | volume=17 | issue=9 | pages=356–360 | doi=10.1080/00963402.1961.11454268| bibcode=1961BuAtS..17i.356C }}</ref>


==Notes==
==Notes==

Revision as of 18:55, 26 August 2023

Isotopes of sodium (11Na)
Main isotopes[1] Decay
abun­dance half-life (t1/2) mode pro­duct
22Na trace 2.6019 y β+ 22Ne
23Na 100% stable
24Na trace 14.9560 h β− 24Mg
Standard atomic weight Ar°(Na)

There are 21 isotopes of sodium (11Na), ranging from 17
Na to 39
Na,[4] and two isomers (22m
Na and 24m
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 18
Na, with a half-life of 1.3(4)×10−21 seconds.

Acute neutron radiation exposure (e.g., from a nuclear criticality accident) converts some of the stable 23
Na 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
 		11 6 17.037270(60) p 16
Ne
 		(1/2+)
18
Na
 		11 7 18.02688(10) 1.3(4) zs p=?[n 8] 17
Ne
 		1−#
19
Na
 		11 8 19.013880(11) > 1 as p 18
Ne
 		(5/2+)
20
Na
 		11 9 20.0073543(12) 447.9(2.3) ms β+ (75.0(4)%) 20
Ne
 		2+
β+α (25.0(4)%) 16
O
21
Na
 		11 10 20.99765446(5) 22.4550(54) s β+ 21
Ne
 		3/2+
22
Na
 		11 11 21.99443742(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) keV 243(2) ns IT 22
Na
 		1+
22m2
Na
 		657.00(14) keV 19.6(7) ps IT 22
Na
 		0+
23
Na
 		11 12 22.9897692820(19) Stable 3/2+ 1
24
Na
 		11 13 23.990963012(18) 14.9560(15) h β− 24
Mg
 		4+ Trace[n 9]
24m
Na
 		472.2074(8) keV 20.18(10) ms IT (99.95%) 24
Na
 		1+
β− (0.05%) 24
Mg
25
Na
 		11 14 24.9899540(13) 59.1(6) s β− 25
Mg
 		5/2+
26
Na
 		11 15 25.992635(4) 1.07128(25) s β− 26
Mg
 		3+
26m
Na
 		82.4(4) keV 4.35(16) μs IT 26
Na
 		1+
27
Na
 		11 16 26.994076(4) 301(6) ms β− (99.902(24)%) 27
Mg
 		5/2+
β−n (0.098(24)%) 26
Mg
28
Na
 		11 17 27.998939(11) 33.1(1.3) ms β− (99.42(12)%) 28
Mg
 		1+
β−n (0.58(12)%) 27
Mg
29
Na
 		11 18 29.002877(8) 43.2(4) ms β− (78%) 29
Mg
 		3/2+
β−n (22(3)%) 28
Mg
β−2n ?[n 10] 27
Mg
 ?
30
Na
 		11 19 30.009098(5) 45.9(7) ms β− (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
 		11 20 31.013147(15) 16.8(3) ms β− (> 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
 		11 21 32.020010(40) 12.9(3) ms β− (66.4(6.2)%) 32
Mg
 		(3−)
β−n (26(6)%) 31
Mg
β−2n (7.6(1.5)%) 30
Mg
33
Na
 		11 22 33.02553(48) 8.2(4) ms β−n (47(6)%) 32
Mg
 		(3/2+)
β− (40.0(6.7)%) 33
Mg
β−2n (13(3)%) 31
Mg
34
Na
 		11 23 34.03401(64) 5.5(1.0) ms β−2n (~50%) 32
Mg
 		1+
β− (~35%) 34
Mg
β−n (~15%) 33
Mg
35
Na
 		11 24 35.04061(72)# 1.5(5) ms β− 35
Mg
 		3/2+#
β−n ?[n 10] 34
Mg
 ?
β−2n ?[n 10] 33
Mg
 ?
37
Na
 		11 26 37.05704(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] 		11 28 39.07512(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. ^ a b # – 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. ^ a b Cosmogenic nuclide
  10. ^ a b c d e f g h i Decay mode shown is energetically allowed, but has not been experimentally observed to occur in this nuclide.

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.[6]

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 because of its abundance, it has been used for nuclear magnetic resonance in various research fields, including materials science and battery research.[7] Sodium-23 relaxation has applications in studying cation-biomolecule interactions, intracellular and extracellular sodium, ion transport in batteries, and quantum information processing.[8]

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.[9][10]

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.[10] 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,[11] 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.[12][13]

Notes

  1. ^ a b 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

References

  1. ^ a b c d 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. ^ a b 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. ^ 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.
  7. ^ 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.
  8. ^ 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.
  9. ^ "sodium-24". Encyclopædia Britannica.
  10. ^ a b 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.
  11. ^ Unusual occurrences during LMFR operation, Proceedings of a Technical Committee meeting held in Vienna, 9–13 November 1998, IAEA. Pages 84, 122.
  12. ^ "Science: fy for Doomsday". Time. November 24, 1961. Archived from the original on March 14, 2016.
  13. ^ 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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