Isotopes of lithium

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Isotopes of lithium  (3Li)
Main isotopes [1] Decay
abun­dance half-life (t1/2) mode pro­duct
6Li[1.9%, 7.8%] stable
7Li[92.2%, 98.1%]stable
Significant variation occurs in commercial samples because of the wide distribution of samples depleted in 6Li.
Standard atomic weight Ar°(Li)

Naturally occurring lithium (3Li) is composed of two stable isotopes, lithium-6 (6Li) and lithium-7 (7Li), with the latter being far more abundant on Earth. Both of the natural isotopes have an unexpectedly low nuclear binding energy per nucleon (5332.3312(3) keV for 6Li and 5606.4401(6) keV for 7Li) when compared with the adjacent lighter and heavier elements, helium (7073.9156(4) keV for helium-4) and beryllium (6462.6693(85) keV for beryllium-9). The longest-lived radioisotope of lithium is 8Li, which has a half-life of just 838.7(3)  milliseconds . 9Li has a half-life of 178.2(4) ms, and 11Li has a half-life of 8.75(6) ms. All of the remaining isotopes of lithium have half-lives that are shorter than 10 nanoseconds. The shortest-lived known isotope of lithium is 4Li, which decays by proton emission with a half-life of about 91(9) yoctoseconds (9.1(9)×10−23 s), although the half-life of 3Li is yet to be determined, and is likely to be much shorter, like 2He (helium-2, diproton) which undergoes proton emission within 10−9 s.

Contents

Both 7Li and 6Li are two of the primordial nuclides that were produced in the Big Bang, with 7Li to be 10−9 of all primordial nuclides, and 6Li around 10−13. [4] A small percentage of 6Li is also known to be produced by nuclear reactions in certain stars. The isotopes of lithium separate somewhat during a variety of geological processes, including mineral formation (chemical precipitation and ion exchange). Lithium ions replace magnesium or iron in certain octahedral locations in clays, and lithium-6 is sometimes preferred over 7Li. This results in some enrichment of 6Li in geological processes.

In nuclear physics, 6Li is an important isotope, because when it is bombarded with neutrons, tritium is produced.

Both 6Li and 7Li isotopes show nuclear magnetic resonance effect, despite being quadrupolar (with nuclear spins of 1+ and 3/2−). 6Li has sharper lines, but due to its lower abundance requires a more sensitive NMR-spectrometer. 7Li is more abundant, but has broader lines because of its larger nuclear spin. The range of chemical shifts is the same of both nuclei and lies within +10 (for LiNH2 in liquid NH3) and −12 (for Li+ in fulleride). [5]

List of isotopes


Nuclide
[n 1] 		Z N Isotopic mass (Da) [6]
[n 2] [n 3] 		Half-life [1]

[resonance width]		 Decay
mode [1]
[n 4] 		Daughter
isotope
[n 5] 		Spin and
parity [1]
[n 6] [n 7] 		Natural abundance (mole fraction)
Excitation energyNormal proportion [1] Range of variation
3
Li
 [n 8] 		303.03078(215)# p  ? [n 9] 2
He
 ?		3/2−#
4
Li
314.02719(23)91(9) ys
[5.06(52) MeV]		p 3
He
 		2−
5
Li
325.012540(50)370(30) ys
[1.24(10) MeV]		p 4
He
 		3/2−
6
Li
 [n 10] 		336.0151228874(15)Stable1+[0.019, 0.078] [7]
6m
Li
3562.88(10) keV56(14) as IT 6
Li
0+
7
Li
 [n 11] 		347.016003434(4)Stable3/2−[0.922, 0.981] [7]
8
Li
358.02248624(5)838.7(3) msβ− 8
Be
 [n 12] 		2+
9
Li
369.02679019(20)178.2(4) msβ−n (50.5(1.0)%)8
Be
 [n 13] 		3/2−
β− (49.5(1.0)%)9
Be
10
Li
3710.035483(14)2.0(5) zs
[0.2(1.2) MeV]		n9
Li
(1−, 2−)
10m1
Li
200(40) keV3.7(1.5) zsIT1+
10m2
Li
480(40) keV1.35(24) zs
[0.350(70) MeV]		IT2+
11
Li
 [n 14] 		3811.0437236(7)8.75(6) msβ−n (86.3(9)%) 10
Be
 		3/2−
β− (6.0(1.0)%)11
Be
β−2n (4.1(4)%)9
Be
β−3n (1.9(2)%)8
Be
 [n 15]
β−α (1.7(3)%)7
He
β−d (0.0130(13)%)9
Li
β−t (0.0093(8)%)8
Li
12
Li
3912.05378(107)#< 10 nsn ? [n 9] 11
Li
 ?		(1−, 2−)
13
Li
31013.061170(80)3.3(1.2) zs
[0.2(9.2) MeV]		2n11
Li
3/2−#
This table header & footer:
  1. ↑ mLi – 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. ↑ Modes of decay:
    IT: Isomeric transition
    n: Neutron emission
    p: Proton emission
  5. ↑ Bold symbol as daughter – Daughter product is stable.
  6. ↑ ( ) spin value – Indicates spin with weak assignment arguments.
  7. ↑ # – Values marked # are not purely derived from experimental data, but at least partly from trends of neighboring nuclides (TNN).
  8. ↑ Discovery of this isotope is unconfirmed
  9. 1 2 Decay mode shown is energetically allowed, but has not been experimentally observed to occur in this nuclide.
  10. ↑ One of the few stable odd-odd nuclei
  11. ↑ Produced in Big Bang nucleosynthesis and by cosmic ray spallation
  12. ↑ Immediately decays into two α-particles for a net reaction of 8Li → 24He + e−
  13. ↑ Immediately decays into two α-particles for a net reaction of 9Li → 24He + 1n + e−
  14. ↑ Has 2 halo neutrons
  15. ↑ Immediately decays into two 4He atoms for a net reaction of 11Li → 24He + 31n + e−

Isotope separation

Colex separation

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.

Other methods

In the vacuum distillation technique, lithium is heated to a temperature of about 550  °C 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. [8] 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. [9]

Lithium-3

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. [10] No other resonances attributable to 3
Li
 have been reported, and it is expected to decay by prompt proton emission (much like the diproton, 2
He
). [11]

Lithium-4

Lithium-4 contains three protons and one neutron. It is the shortest-lived known isotope of lithium, with a half-life of 91(9) yoctoseconds (9.1(9)×10−23 s) and decays by proton emission to helium-3. [12] Lithium-4 can be formed as an intermediate in some nuclear fusion reactions.

Lithium-6

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 ], 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. [13] 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, [14] and has the smallest nonzero nuclear electric quadrupole moment of any stable nucleus.

Lithium-7

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. [15]

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 [16] ) 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. [17]

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. [18] [19]

Lithium-8

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 generated Lithium-8 for immediate decay by bombarding stable Lithium-7 with 60 MeV protons created by a cyclotron particle accelerator. [20]

Lithium-11

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". [21] While the proton root-mean-square radius of 11Li is 2.18+0.16
−0.21 fm, its neutron radius is much larger at 3.34+0.02
−0.08 fm; for comparison, the corresponding figures for 9Li are 2.076±0.037 fm for the protons and 2.4±0.03 fm for the neutrons. [22] It decays by beta emission and neutron emission to 10
Be
, 11
Be
, or 9
Be
 (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. [23]

Lithium-12

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

Decay chains

While β− decay into isotopes of beryllium (often combined with single- or multiple-neutron emission) is predominant in heavier isotopes of lithium, 10
Li
 and 12
Li
 decay via neutron emission into 9
Li
 and 11
Li
 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 6
Li
 decay exclusively by proton emission, as they are beyond the proton drip line. The decay modes of the two isomers of 10
Li
 are unknown.

See also

Related Research Articles

<span class="mw-page-title-main">Atom</span> Smallest unit of a chemical element

Atoms are the basic particles of the chemical elements. An atom consists of a nucleus of protons and generally neutrons, surrounded by an electromagnetically bound swarm of electrons. The chemical elements are distinguished from each other by the number of protons that are in their atoms. For example, any atom that contains 11 protons is sodium, and any atom that contains 29 protons is copper. Atoms with the same number of protons but a different number of neutrons are called isotopes of the same element.

<span class="mw-page-title-main">Lithium</span> Chemical element with atomic number 3 (Li)

Lithium is a chemical element; it has symbol Li and atomic number 3. It is a soft, silvery-white alkali metal. Under standard conditions, it is the least dense metal and the least dense solid element. Like all alkali metals, lithium is highly reactive and flammable, and must be stored in vacuum, inert atmosphere, or inert liquid such as purified kerosene or mineral oil. It exhibits a metallic luster. It corrodes quickly in air to a dull silvery gray, then black tarnish. It does not occur freely in nature, but occurs mainly as pegmatitic minerals, which were once the main source of lithium. Due to its solubility as an ion, it is present in ocean water and is commonly obtained from brines. Lithium metal is isolated electrolytically from a mixture of lithium chloride and potassium chloride.

<span class="mw-page-title-main">Neutron</span> Subatomic particle with no charge

The neutron is a subatomic particle, symbol
n
 or
n0
, that has no electric charge, and a mass slightly greater than that of a proton. Protons and neutrons constitute the nuclei of atoms. Since protons and neutrons behave similarly within the nucleus, they are both referred to as nucleons. Nucleons have a mass of approximately one atomic mass unit, or dalton. Their properties and interactions are described by nuclear physics. Protons and neutrons are not elementary particles; each is composed of three quarks.

<span class="mw-page-title-main">Big Bang nucleosynthesis</span> Process during the early universe

In physical cosmology, Big Bang nucleosynthesis is the production of nuclei other than those of the lightest isotope of hydrogen during the early phases of the universe. This type of nucleosynthesis is thought by most cosmologists to have occurred from 10 seconds to 20 minutes after the Big Bang. It is thought to be responsible for the formation of most of the universe's helium, along with small fractions of the hydrogen isotope deuterium, the helium isotope helium-3 (3He), and a very small fraction of the lithium isotope lithium-7 (7Li). In addition to these stable nuclei, two unstable or radioactive isotopes were produced: the heavy hydrogen isotope tritium and the beryllium isotope beryllium-7 (7Be). These unstable isotopes later decayed into 3He and 7Li, respectively, as above.

<span class="mw-page-title-main">Nucleosynthesis</span> Process that creates new atomic nuclei from pre-existing nucleons, primarily protons and neutrons

Nucleosynthesis is the process that creates new atomic nuclei from pre-existing nucleons and nuclei. According to current theories, the first nuclei were formed a few minutes after the Big Bang, through nuclear reactions in a process called Big Bang nucleosynthesis. After about 20 minutes, the universe had expanded and cooled to a point at which these high-energy collisions among nucleons ended, so only the fastest and simplest reactions occurred, leaving our universe containing hydrogen and helium. The rest is traces of other elements such as lithium and the hydrogen isotope deuterium. Nucleosynthesis in stars and their explosions later produced the variety of elements and isotopes that we have today, in a process called cosmic chemical evolution. The amounts of total mass in elements heavier than hydrogen and helium remains small, so that the universe still has approximately the same composition.

<span class="mw-page-title-main">Positron emission</span> Type of radioactive decay

Positron emission, beta plus decay, or β+ decay is a subtype of radioactive decay called beta decay, in which a proton inside a radionuclide nucleus is converted into a neutron while releasing a positron and an electron neutrino. Positron emission is mediated by the weak force. The positron is a type of beta particle (β+), the other beta particle being the electron (β−) emitted from the β− decay of a nucleus.

A radioactive tracer, radiotracer, or radioactive label is a synthetic derivative of a natural compound in which one or more atoms have been replaced by a radionuclide. By virtue of its radioactive decay, it can be used to explore the mechanism of chemical reactions by tracing the path that the radioisotope follows from reactants to products. Radiolabeling or radiotracing is thus the radioactive form of isotopic labeling. In biological contexts, experiments that use radioisotope tracers are sometimes called radioisotope feeding experiments.

<span class="mw-page-title-main">Nuclear reaction</span> Transformation of a nuclide to another

In nuclear physics and nuclear chemistry, a nuclear reaction is a process in which two nuclei, or a nucleus and an external subatomic particle, collide to produce one or more new nuclides. Thus, a nuclear reaction must cause a transformation of at least one nuclide to another. If a nucleus interacts with another nucleus or particle, they then separate without changing the nature of any nuclide, the process is simply referred to as a type of nuclear scattering, rather than a nuclear reaction.

<span class="mw-page-title-main">Mass number</span> Number of heavy particles in the atomic nucleus

The mass number (symbol A, from the German word: Atomgewicht, "atomic weight"), also called atomic mass number or nucleon number, is the total number of protons and neutrons (together known as nucleons) in an atomic nucleus. It is approximately equal to the atomic (also known as isotopic) mass of the atom expressed in atomic mass units. Since protons and neutrons are both baryons, the mass number A is identical with the baryon number B of the nucleus (and also of the whole atom or ion). The mass number is different for each isotope of a given chemical element, and the difference between the mass number and the atomic number Z gives the number of neutrons (N) in the nucleus: N = A − Z.

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

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.

<span class="mw-page-title-main">Lithium hydride</span> Chemical compound

Lithium hydride is an inorganic compound with the formula LiH. This alkali metal hydride is a colorless solid, although commercial samples are grey. Characteristic of a salt-like (ionic) hydride, it has a high melting point, and it is not soluble but reactive with all protic organic solvents. It is soluble and nonreactive with certain molten salts such as lithium fluoride, lithium borohydride, and sodium hydride. With a molar mass of 7.95 g/mol, it is the lightest ionic compound.

Technetium (43Tc) is one of the two elements with Z < 83 that have no stable isotopes; the other such element is promethium. It is primarily artificial, with only trace quantities existing in nature produced by spontaneous fission or neutron capture by molybdenum. The first isotopes to be synthesized were 97Tc and 99Tc in 1936, the first artificial element to be produced. The most stable radioisotopes are 97Tc, 98Tc, and 99Tc.

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

Boron (5B) naturally occurs as isotopes 10
B
 and 11
B
, the latter of which makes up about 80% of natural boron. There are 13 radioisotopes that have been discovered, with mass numbers from 7 to 21, all with short half-lives, the longest being that of 8
B
, with a half-life of only 771.9(9) ms and 12
B
 with a half-life of 20.20(2) ms. All other isotopes have half-lives shorter than 17.35 ms. Those isotopes with mass below 10 decay into helium while those with mass above 11 mostly become carbon.

Beryllium (4Be) has 11 known isotopes and 3 known isomers, but only one of these isotopes is stable and a primordial nuclide. As such, beryllium is considered a monoisotopic element. It is also a mononuclidic element, because its other isotopes have such short half-lives that none are primordial and their abundance is very low. Beryllium is unique as being the only monoisotopic element with both an even number of protons and an odd number of neutrons. There are 25 other monoisotopic elements but all have odd atomic numbers, and even numbers of neutrons.

Helium (2He) has nine known isotopes, but only helium-3 (3He) and helium-4 (4He) are stable. All radioisotopes are short-lived; the longest-lived is 6He with half-life 806.92(24) milliseconds. The least stable is 10He, with half-life 260(40) yoctoseconds, though 2He may have an even shorter half-life.

<span class="mw-page-title-main">Valley of stability</span> Characterization of nuclide stability

In nuclear physics, the valley of stability is a characterization of the stability of nuclides to radioactivity based on their binding energy. Nuclides are composed of protons and neutrons. The shape of the valley refers to the profile of binding energy as a function of the numbers of neutrons and protons, with the lowest part of the valley corresponding to the region of most stable nuclei. The line of stable nuclides down the center of the valley of stability is known as the line of beta stability. The sides of the valley correspond to increasing instability to beta decay. The decay of a nuclide becomes more energetically favorable the further it is from the line of beta stability. The boundaries of the valley correspond to the nuclear drip lines, where nuclides become so unstable they emit single protons or single neutrons. Regions of instability within the valley at high atomic number also include radioactive decay by alpha radiation or spontaneous fission. The shape of the valley is roughly an elongated paraboloid corresponding to the nuclide binding energies as a function of neutron and atomic numbers.

<span class="mw-page-title-main">Isotope</span> Different atoms of the same element

Isotopes are distinct nuclear species of the same chemical element. They have the same atomic number and position in the periodic table, but different nucleon numbers due to different numbers of neutrons in their nuclei. While all isotopes of a given element have similar chemical properties, they have different atomic masses and physical properties.

<span class="mw-page-title-main">Nuclear drip line</span> Atomic nuclei decay delimiter

The nuclear drip line is the boundary beyond which atomic nuclei are unbound with respect to the emission of a proton or neutron.

Lithium helide is a compound of helium and lithium with the formula LiHe. The substance is a cold low-density gas made of Van der Waals molecules, each composed of a helium atom and lithium atom bound by van der Waals force. The preparation of LiHe opens up the possibility to prepare other helium dimers, and beyond that multi-atom clusters that could be used to investigate Efimov states and Casimir retardation effects.

The COLEX process is a chemical method of isotopic separation of lithium-6 and lithium-7, based on the use of mercury. COLEX stands for column exchange.

References

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  20. ↑ Bungau, Adriana; Alonso, Jose; Bartoszek, Larry; Conrad, Janet (May 2018). "Optimizing the 8Li yield for the IsoDAR Neutrino Experiment". Journal of Instrumentation. 14 (3): 03001. arXiv: 1805.00410 . doi:10.1088/1748-0221/14/03/P03001. S2CID   55756525.
  21. ↑ "A new particle accelerator aims to unlock secrets of bizarre atomic nuclei". 15 November 2021.
  22. ↑ Moriguchi, T.; Ozawa, A.; Ishimoto, S.; Abe, Y.; Fukuda, M.; Hachiuma, I.; Ishibashi, Y.; Ito, Y.; Kuboki, T.; Lantz, M.; Nagae, D.; Namihira, K.; Nishimura, D.; Ohtsubo, T.; Ooishi, H.; Suda, T.; Suzuki, H.; Suzuki, T.; Takechi, M.; Tanaka, K.; Yamaguchi, T. (16 August 2013). "Density distributions of 11 Li deduced from reaction cross-section measurements". Physical Review C. 88 (2): 024610. Bibcode:2013PhRvC..88b4610M. doi:10.1103/PhysRevC.88.024610.
  23. ↑ Brown, B. Alex (13 December 2010). "Islands of insight in the nuclear chart". Physics. 3 (25): 104. arXiv: 1010.3999 . doi:10.1103/PhysRevLett.105.252501. PMID   21231582. S2CID   43334780.

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