isotopes of lithium

{{Anchor|Lithium-9}}

{{Isotopes table

|symbol=Li

|refs=NUBASE2020, AME2020 II

|notes=m, resonance, unc(), mass#, spin(), spin#, daughter-st, p, n, IT

}}

|-

| {{SimpleNuclide|Lithium|3}}Discovery of this isotope is unconfirmed

| style="text-align:right" | 3

| style="text-align:right" | 0

| {{val|3.03078|(215)}}#

|

| p ?Decay mode shown is energetically allowed, but has not been experimentally observed to occur in this nuclide.

| {{SimpleNuclide|Helium|2}} ?

| 3/2−#

|

|

|-

| {{SimpleNuclide|Lithium|4}}

| style="text-align:right" | 3

| style="text-align:right" | 1

| {{val|4.02719|(23)}}

| {{val|91|(9)|u=ys}}
[{{val|5.06|(52)|u=MeV}}]

| p

| Helium-3

| 2−

|

|

|-id=Lithium-5

| {{SimpleNuclide|Lithium|5}}

| style="text-align:right" | 3

| style="text-align:right" | 2

| {{val|5.012540|(50)}}

| {{val|370|(30)|u=ys}}
[{{val|1.24|(10)|u=MeV}}]

| p

| Helium-4

| 3/2−

|

|

|-

| {{SimpleNuclide|Lithium|6}}One of the few stable odd-odd nuclei

| style="text-align:right" | 3

| style="text-align:right" | 3

| {{val|6.0151228874|(15)}}

| colspan="3" style="text-align:center;"|Stable

| 1+

| style="text-align:center" colspan="2"|[{{val|0.019}}, {{val|0.078}}]{{Cite web|title=Atomic Weight of Lithium|url=https://ciaaw.org/lithium.htm|access-date=21 October 2021|website=ciaaw.org}}

|-id=Lithium-6m

| style="text-indent:1em" | {{SimpleNuclide|Lithium|6|m}}

| colspan="3" style="text-indent:2em" | {{val|3562.88|(10)|u=keV}}

| {{val|56|(14)|u=as}}

| IT

| {{SimpleNuclide|Lithium|6}}

| 0+

|

|

|-

| {{SimpleNuclide|Lithium|7}}Produced in Big Bang nucleosynthesis and by cosmic ray spallation

| style="text-align:right" | 3

| style="text-align:right" | 4

| {{val|7.016003434|(4)}}

| colspan="3" style="text-align:center;"|Stable

| 3/2−

| colspan="2" style="text-align:center"|[{{val|0.922}}, {{val|0.981}}]

|-

| {{SimpleNuclide|Lithium|8}}

| style="text-align:right" | 3

| style="text-align:right" | 5

| {{val|8.02248624|(5)}}

| {{val|838.7|(3)|u=ms}}

| β⁻

| {{SimpleNuclide|Beryllium|8|link=yes}}Immediately decays into two α-particles for a net reaction of ⁸Li → 2⁴He + e⁻

| 2+

|

|

|-

| rowspan="2"|{{SimpleNuclide|Lithium|9}}

| rowspan="2" style="text-align:right" | 3

| rowspan="2" style="text-align:right" | 6

| rowspan="2"|{{val|9.02679019|(20)}}

| rowspan="2"|{{val|178.2|(4)|u=ms}}

| β⁻n ({{val|50.5|(1.0)|u=%}})

| {{SimpleNuclide|Beryllium|8}}Immediately decays into two α-particles for a net reaction of ⁹Li → 2⁴He + ¹n + e⁻

| rowspan="2"|3/2−

| rowspan="2"|

| rowspan="2"|

|-

| β⁻ ({{val|49.5|(1.0)|u=%}})

| {{SimpleNuclide|Beryllium|9}}

|-id=Lithium-10

| {{SimpleNuclide|Lithium|10}}

| style="text-align:right" | 3

| style="text-align:right" | 7

| {{val|10.035483|(14)}}

| {{val|2.0|(5)|u=zs}}
[{{val|0.2|(1.2)|u=MeV}}]

| n

| {{SimpleNuclide|Lithium|9}}

| (1−, 2−)

|

|

|-id=Lithium-10m1

| style="text-indent:1em" | {{SimpleNuclide|Lithium|10|m1}}

| colspan="3" style="text-indent:2em" | {{val|200|(40)|u=keV}}

| {{val|3.7|(1.5)|u=zs}}

| IT

| {{SimpleNuclide|Lithium|10}}

| 1+

|

|

|-id=Lithium-10m2

| style="text-indent:1em" | {{SimpleNuclide|Lithium|10|m2}}

| colspan="3" style="text-indent:2em" | {{val|480|(40)|u=keV}}

| {{val|1.35|(24)|u=zs}}
[{{val|0.350|(70)|u=MeV}}]

| IT

| {{SimpleNuclide|Lithium|10}}

| 2+

|

|

|-

| rowspan=7|{{SimpleNuclide|Lithium|11}}Has 2 halo neutrons

| rowspan=7 style="text-align:right" | 3

| rowspan=7 style="text-align:right" | 8

| rowspan=7|{{val|11.0437236|(7)}}

| rowspan=7|{{val|8.75|(6)|u=ms}}

| β⁻n ({{val|86.3|(9)|u=%}})

| Beryllium-10

| rowspan=7|3/2−

| rowspan=7|

| rowspan=7|

|-

| β⁻ ({{val|6.0|(1.0)|u=%}})

| {{SimpleNuclide|Beryllium|11}}

|-

| β⁻2n ({{val|4.1|(4)|u=%}})

| {{SimpleNuclide|Beryllium|9}}

|-

| β⁻3n ({{val|1.9|(2)|u=%}})

| {{SimpleNuclide|Beryllium|8}}Immediately decays into two ⁴He atoms for a net reaction of ¹¹Li → 2⁴He + 3¹n + e⁻

|-

| β⁻α ({{val|1.7|(3)|u=%}})

| {{SimpleNuclide|Helium|7}}

|-

| β⁻d ({{val|0.0130|(13)|u=%}})

| {{SimpleNuclide|Lithium|9}}

|-

| β⁻t ({{val|0.0093|(8)|u=%}})

| {{SimpleNuclide|Lithium|8}}

|-

| {{SimpleNuclide|Lithium|12}}

| style="text-align:right" | 3

| style="text-align:right" | 9

| {{val|12.05378|(107)}}#

| < 10 ns

| n ?

| {{SimpleNuclide|Lithium|11}} ?

| (1−, 2−)

|

|

|-id=Lithium-13

| {{SimpleNuclide|Lithium|13}}

| style="text-align:right" | 3

| style="text-align:right" | 10

| {{val|13.061170|(80)}}

| {{val|3.3|(1.2)|u=zs}}
[{{val|0.2|(9.2)|u=MeV}}]

| 2n

| {{SimpleNuclide|Lithium|11}}

| 3/2−#

|

|

{{Isotopes table/footer}}

{{Main|COLEX process}}Lithium-6 has a greater affinity than lithium-7 for the element mercury. When an amalgam of lithium and mercury is added to solutions containing lithium hydroxide, the lithium-6 becomes more concentrated in the amalgam and the lithium-7 more in the hydroxide solution.

The colex (column exchange) separation method makes use of this by passing a counter-flow of amalgam and hydroxide through a cascade of stages. The fraction of lithium-6 is preferentially drained by the mercury, but the lithium-7 flows mostly with the hydroxide.

At the bottom of the column, the lithium (enriched with lithium-6) is separated from the amalgam, and the mercury is recovered to be reused with fresh raw material. At the top, the lithium hydroxide solution is electrolyzed to liberate the lithium-7 fraction. The enrichment obtained with this method varies with the column length and the flow speed.

In the vacuum distillation technique, lithium is heated to a temperature of about {{val|550|ul=degC}} in a vacuum. Lithium atoms evaporate from the liquid surface and are collected on a cold surface positioned a few centimetres above the liquid surface.{{Cite journal |last1=Katal'nikov |first1=S. G. |last2=Andreev |first2=B. M. |date=1 March 1962 |title=The separation factor of lithium isotopes during vacuum distillation |url=https://doi.org/10.1007/BF01491187 |journal=The Soviet Journal of Atomic Energy |language=en |volume=11 |issue=3 |pages=889–893 |doi=10.1007/BF01491187 |s2cid=96799991 |issn=1573-8205|url-access=subscription }} Since lithium-6 atoms have a greater mean free path, they are collected preferentially. The theoretical separation efficiency of this method is about 8.0 percent. A multistage process may be used to obtain higher degrees of separation.

The isotopes of lithium, in principle, can also be separated through electrochemical method and distillation chromatography, which are currently in development.{{Cite journal |last1=Badea |first1=Silviu-Laurentiu |last2=Niculescu |first2=Violeta-Carolina |last3=Iordache |first3=Andreea-Maria |date=April 2023 |title=New Trends in Separation Techniques of Lithium Isotopes: A Review of Chemical Separation Methods |journal=Materials |language=en |volume=16 |issue=10 |pages=3817 |doi=10.3390/ma16103817 |pmid=37241444 |pmc=10222844 |bibcode=2023Mate...16.3817B |issn=1996-1944 |doi-access=free }}

Lithium-3, also known as the triproton, would consist of three protons and zero neutrons. It was reported as proton unbound in 1969, but this result was not accepted and its existence is thus unproven.{{NUBASE2016|ref|page=030001–21}} No other resonances attributable to {{SimpleNuclide|Lithium|3}} have been reported, and it is expected to decay by prompt proton emission (much like the diproton, {{SimpleNuclide|Helium|2}}).{{cite journal |last1=Purcell |first1=J. E. |last2=Kelley |first2=J. H. |last3=Kwan |first3=E. |last4=Sheu |first4=C. G. |last5=Weller |first5=H. R. |title=Energy Levels of Light Nuclei (A = 3) |journal=Nuclear Physics A |volume=848 |date=2010 |issue=1 |page=1 |doi=10.1016/j.nuclphysa.2010.08.012 |bibcode=2010NuPhA.848....1P |url=http://www.tunl.duke.edu/nucldata/ourpubs/03_2010.pdf |access-date=3 January 2020 |archive-date=1 February 2018 |archive-url=https://web.archive.org/web/20180201093026/http://www.tunl.duke.edu/nucldata/ourpubs/03_2010.pdf |url-status=dead }}

Lithium-4 contains three protons and one neutron. It is the shortest-lived known isotope of lithium, with a half-life of {{val|91|(9)|u=yoctoseconds}} ({{val|9.1|e=-23|(9)|u=s}}) and decays by proton emission to helium-3.{{cite web| url=http://periodictable.com/Isotopes/003.4/index2.full.dm.html| title=Isotopes of Lithium| access-date=20 October 2013}} Lithium-4 can be formed as an intermediate in some nuclear fusion reactions.

File:Cross_Section_for_Fusion_reactions.png

Lithium-5 is very short-lived with a half-life of 370(30) yoctoseconds, decaying via proton emission to helium-4. It is formed as an intermediate in the fusion of deuterium and helium-3:

$\{\}^2\backslash mathrm\{D\}\; +\; \{\}^3\backslash mathrm\{He\}\; \backslash longrightarrow\; \{\}^5\backslash mathrm\{Li\}^\{*\}\; \backslash longrightarrow\; \{\}^4\backslash mathrm\{He\}\; +\; p\; +\; 18.4\backslash \; \backslash mathrm\{MeV\}$

The reaction is greatly enhanced by the existence of a resonance. Lithium-5, which has a natural spin state of −3/2 at the 0 MeV ground state, has a +3/2 excited spin state at 16.66 MeV. Because the reaction creates lithium-5 nuclei with an energy level close to this state, it happens more frequently. A symmetrical resonance in the helium-5 nucleus makes the deuterium–tritium fusion reaction the most favourable known.{{cite journal |last=Barker |first=FC |last2=Woods |first2=CL |year=1985 |title=States of 5He and 5Li |url=https://www.publish.csiro.au/ph/pdf/ph850563 |journal=Australian Journal of Physics |publisher=CSIRO Publishing |volume=38 |issue=4 |page=563 |doi=10.1071/ph850563 |issn=0004-9506 |access-date=2025-04-10 |doi-access=free}}

Lithium-6 is valuable as the source material for the production of tritium (hydrogen-3) and as an absorber of neutrons in nuclear fusion reactions. Between 1.9% and 7.8% of terrestrial lithium in normal materials consists of lithium-6, with the rest being lithium-7. Large amounts of lithium-6 have been separated out for placing into thermonuclear weapons. The separation of lithium-6 has by now ceased in the large thermonuclear powers{{Citation needed|reason=Uncited claim, China is known to officially practise isotopic lithium separation via the COLEX process. Russia is also known to isotopically separate lithium, as well as possibly the DPRK.|date=April 2018}}, but stockpiles of it remain in these countries.

The deuterium–tritium fusion reaction has been investigated as a possible energy source, as it is currently the only fusion reaction with sufficient energy output for feasible implementation. In this scenario, lithium enriched in lithium-6 would be required to generate the necessary quantities of tritium. Mineral and brine lithium resources are a potential limiting factor in this scenario, but seawater can eventually also be used.{{cite journal |last1=Bradshaw |first1=A.M. |last2=Hamacher |first2=T. |last3=Fischer |first3=U. |date=2010 |title=Is nuclear fusion a sustainable energy form? |journal=Fusion Engineering and Design |volume=86 |issue=9 |pages=2770–2773 |doi=10.1016/j.fusengdes.2010.11.040 |hdl=11858/00-001M-0000-0026-E9D2-6 |s2cid=54674085 |url=https://th.fhi-berlin.mpg.de/th/publications/FusionEngDesign-2011-2770-2011.pdf|hdl-access=free }} Pressurized heavy-water reactors such as the CANDU produce small quantities of tritium in their coolant/moderator from neutron absorption and this is sometimes extracted as an alternative to the use of lithium-6.

Lithium-6 is one of only four stable isotopes with a spin of 1, the others being deuterium, boron-10, and nitrogen-14,{{cite book | last= Chandrakumar | first= N. | date= 2012 | title= Spin-1 NMR | publisher= Springer Science & Business Media | page= 5 | isbn= 9783642610899 | url= https://books.google.com/books?id=gVHmCAAAQBAJ&pg=PA5}} and has the smallest nonzero nuclear electric quadrupole moment of any stable nucleus.

In 2025, researchers from ETH Zürich and Texas A&M University introduced a mercury-free method for isolating lithium-6, providing an alternative to the COLEX process, which uses toxic liquid mercury. This technique was discovered by accident during water purification research and utilized zeta-vanadium oxide (ζ-V2O5) to selectively trap lithium-6 ions, which could be a crucial step in scaling up the production of fusion-grade lithium-6, potentially unlocking more cost-effective and safer ways to isolate lithium for nuclear fusion reactors.{{cite journal |last=Luis Carrillo |first=J. |display-authors=et al. |title=Electrochemical 6Li isotope enrichment based on selective insertion in 1D tunnel-structured V2O5 |journal=Cell |date=20 March 2025 |doi=10.1016/j.chempr.2025.102486 }}

Lithium-7 is by far the most abundant isotope of lithium, making up between 92.2% and 98.1% of all terrestrial lithium. A lithium-7 atom contains three protons, four neutrons, and three electrons. Because of its nuclear properties, lithium-7 is less common than helium, carbon, nitrogen, or oxygen in the Universe, even though the latter three all have heavier nuclei. The Castle Bravo thermonuclear test greatly exceeded its expected yield due to incorrect assumptions about the nuclear properties of lithium-7.

The industrial production of lithium-6 results in a waste product which is enriched in lithium-7 and depleted in lithium-6. This material has been sold commercially, and some of it has been released into the environment. A relative abundance of lithium-7, as high as 35 percent greater than the natural value, has been measured in the ground water in a carbonate aquifer underneath the West Valley Creek in Pennsylvania, which is downstream from a lithium processing plant. The isotopic composition of lithium in normal materials can vary somewhat depending on its origin, which determines its relative atomic mass in the source material. An accurate relative atomic mass for samples of lithium cannot be measured for all sources of lithium.Coplen, Tyler B.; Hopple, J. A.; Böhlke, John Karl; Peiser, H. Steffen; Rieder, S. E.; Krouse, H. R.; Rosman, Kevin J. R.; Ding, T.; Vocke, R. D., Jr.; Révész, K. M.; Lamberty, A.; Taylor, Philip D. P.; De Bièvre, Paul; "Compilation of minimum and maximum isotope ratios of selected elements in naturally occurring terrestrial materials and reagents", U.S. Geological Survey Water-Resources Investigations Report 01-4222 (2002). As quoted in {{cite journal |title=Isotope-Abundance Variations of Selected Elements (IUPAC technical report) |author=T. B. Coplen |s2cid=97223816 |journal=Pure and Applied Chemistry |volume=74 |issue=10 |pages=1987–2017 |year=2002 |url=http://pac.iupac.org/publications/pac/pdf/2002/pdf/7410x1987.pdf |display-authors=etal |doi=10.1351/pac200274101987 |access-date=29 October 2012 |archive-date=3 March 2016 |archive-url=https://web.archive.org/web/20160303202428/http://pac.iupac.org/publications/pac/pdf/2002/pdf/7410x1987.pdf |url-status=dead }}

Lithium-7 is used as a part of the molten lithium fluoride in molten-salt reactors: liquid-fluoride nuclear reactors. The large neutron absorption cross section of lithium-6 (about 940 barns

{{cite journal

| first= Norman E.

| last= Holden

| title= The Impact of Depleted ⁶Li on the Standard Atomic Weight of Lithium

| date= January–February 2010

| journal=Chemistry International

| publisher= International Union of Pure and Applied Chemistry

| url= http://www.iupac.org/publications/ci/2010/3201/3_holden.html

| access-date= 6 May 2014

}}

)

as compared with the very small neutron cross section of lithium-7 (about 45 millibarns) makes high separation of lithium-7 from natural lithium a strong requirement for the possible use in lithium fluoride reactors.

Lithium-7 hydroxide is used for alkalizing of the coolant in pressurized water reactors.[http://www.gao.gov/products/GAO-13-716 Managing Critical Isotopes: Stewardship of Lithium-7 Is Needed to Ensure a Stable Supply, GAO-13-716] // U.S. Government Accountability Office, 19 September 2013; [http://www.gao.gov/assets/660/657964.pdf pdf]

Some lithium-7 has been produced, for a few picoseconds, which contains a lambda particle in its nucleus, whereas an atomic nucleus is generally thought to contain only neutrons and protons.{{cite book |first=John |last=Emsley |title=Nature's Building Blocks: An A-Z Guide to the Elements |year=2001 |publisher=Oxford University Press |isbn=978-0-19-850340-8 |pages=234–239 |url=https://books.google.com/books?id=j-Xu07p3cKwC&pg=PA239 }}{{cite magazine |first=Geoff |last=Brumfiel |title=The Incredible Shrinking Nucleus |magazine=Physical Review Focus |date=1 March 2001 |volume=7 |doi=10.1103/PhysRevFocus.7.11 }}

Lithium-8 has been proposed as a source of 6.4 MeV electron antineutrinos generated by the inverse beta decay to beryllium-8. The ISODAR particle physics collaboration describes a scheme to generate lithium-8 for immediate decay by bombarding stable lithium-7 with 60 MeV protons created by a cyclotron particle accelerator.{{Cite journal |last1=Bungau |first1=Adriana |last2=Alonso |first2=Jose |last3=Bartoszek |first3=Larry |last4=Conrad |first4=Janet |date=May 2018 |title=Optimizing the ⁸Li yield for the IsoDAR Neutrino Experiment |journal=Journal of Instrumentation |volume=14 |issue=3 |pages=03001 |doi=10.1088/1748-0221/14/03/P03001 |arxiv=1805.00410|s2cid=55756525 }}

Lithium-11 is a halo nucleus consisting of a lithium-9 core surrounded by two loosely-bound neutrons; both neutrons must be present in order for this system to be bound, which has led to the description as a "Borromean nucleus".{{cite web | url=https://www.sciencenews.org/article/rare-isotope-elements-new-particle-accelerator-atom-nucleus | title=A new particle accelerator aims to unlock secrets of bizarre atomic nuclei | date=15 November 2021 }} While the proton root-mean-square radius of ¹¹Li is {{val|2.18|0.16|0.21|u=fm}}, its neutron radius is much larger at {{val|3.34|0.02|0.08|u=fm}}; for comparison, the corresponding figures for ⁹Li are {{val|2.076|0.037|u=fm}} for the protons and {{val|2.4|0.03|u=fm}} for the neutrons.{{cite journal |last1=Moriguchi |first1=T. |last2=Ozawa |first2=A. |last3=Ishimoto |first3=S. |last4=Abe |first4=Y. |last5=Fukuda |first5=M. |last6=Hachiuma |first6=I. |last7=Ishibashi |first7=Y. |last8=Ito |first8=Y. |last9=Kuboki |first9=T. |last10=Lantz |first10=M. |last11=Nagae |first11=D. |last12=Namihira |first12=K. |last13=Nishimura |first13=D. |last14=Ohtsubo |first14=T. |last15=Ooishi |first15=H. |last16=Suda |first16=T. |last17=Suzuki |first17=H. |last18=Suzuki |first18=T. |last19=Takechi |first19=M. |last20=Tanaka |first20=K. |last21=Yamaguchi |first21=T. |title=Density distributions of 11 Li deduced from reaction cross-section measurements |journal=Physical Review C |date=16 August 2013 |volume=88 |issue=2 |page=024610 |doi=10.1103/PhysRevC.88.024610 |bibcode=2013PhRvC..88b4610M |url=https://www.researchgate.net/publication/258026116}} It decays by beta emission and neutron emission to beryllium-10, Isotopes of beryllium, or Isotopes of beryllium (see tables above and below). Having a magic number of 8 neutrons, lithium-11 sits on the first of five known islands of inversion, which explains its longer half-life compared to adjacent nuclei.{{cite journal |last1=Brown |first1=B. Alex |title=Islands of insight in the nuclear chart |url=https://physics.aps.org/articles/v3/104 |journal=Physics |pages=104 |language=en |doi=10.1103/PhysRevLett.105.252501 |date=13 December 2010|volume=3 |issue=25 |pmid=21231582 |arxiv=1010.3999 |s2cid=43334780 }}

Lithium-12 has a considerably shorter half-life. It decays by neutron emission into {{SimpleNuclide|Lithium|11}}, which decays as mentioned above.

While β⁻ decay into isotopes of beryllium (often combined with single- or multiple-neutron emission) is predominant in heavier isotopes of lithium, {{SimpleNuclide|Lithium|10}} and {{SimpleNuclide|Lithium|12}} decay via neutron emission into {{SimpleNuclide|Lithium|9}} and {{SimpleNuclide|Lithium|11}} respectively due to their positions beyond the neutron drip line. Lithium-11 has also been observed to decay via multiple forms of fission. Isotopes lighter than {{SimpleNuclide|Lithium|6}} decay exclusively by proton emission, as they are beyond the proton drip line. The decay modes of the two isomers of {{SimpleNuclide|Lithium|10}} are unknown.

:$\backslash begin\{array\}\{l\}\{\}\backslash \backslash$

\ce{^4_3Li ->[91~\ce{ys}] {^3_2He} + {^1_1H}} \\

\ce{^5_3Li ->[370~\ce{ys}] {^4_2He} + {^1_1H}} \\

\ce{^8_3Li ->[838.7~\ce{ms}] {^8_4Be} + e^-} \\

\ce{^9_3Li ->[178.2~\ce{ms}] {^8_4Be} + {^1_0n} + e^-} \\

\ce{^9_3Li ->[178.2~\ce{ms}] {^9_4Be} + e^-} \\

\ce{^{10}_3Li ->[2~\ce{zs}] {^9_3Li} + {^1_0n}} \\

\ce{^{11}_3Li ->[8.75~\ce{ms}] {^{10}_4Be} + {^1_0n} + e^-} \\

\ce{^{11}_3Li ->[8.75~\ce{ms}] {^{11}_4Be} + e^-} \\

\ce{^{11}_3Li ->[8.75~\ce{ms}] {^9_4Be} + 2{^1_0n} + e^-} \\

\ce{^{11}_3Li ->[8.75~\ce{ms}] {^8_4Be} + 3{^1_0n} + e^-} \\

\ce{^{11}_3Li ->[8.75~\ce{ms}] {^7_2He} + {^4_2He} + e^-} \\

\ce{^{11}_3Li ->[8.75~\ce{ms}] {^8_3Li} + {^3_1H} + e^-} \\

\ce{^{11}_3Li ->[8.75~\ce{ms}] {^9_3Li} + {^2_1H} + e^-} \\

\ce{^{12}_3Li -> {^{11}_3Li} + {^1_0n}} \\{}

\end{array}

• Cosmological lithium problem
• {{annotated link|Dilithium}}
• Halo nucleus
• {{annotated link|Lithium burning}}

Daughter products other than lithium

• Isotopes of beryllium
• Isotopes of helium

{{Reflist}}

{{Cite journal |last1=Lewis |first1=G. N. |last2=MacDonald |first2=R. T. |doi=10.1021/ja01303a045 |title=The Separation of Lithium Isotopes |journal=Journal of the American Chemical Society |volume=58 |issue=12 |pages=2519–2524 |year=1936 |bibcode=1936JAChS..58.2519L }}

{{Navbox element isotopes}}

Category:Lithium

Lithium