Isotopes of lithium
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Overview
Naturally occurring lithium (Li) (standard atomic mass: 6.941(2) u) is composed of two stable isotopes (Template:SimpleNuclide and Template:SimpleNuclide, the latter being the more abundant (92.5% natural abundance). Seven radioisotopes have been characterized, the most stable being Template:SimpleNuclide with a half-life of Template:Val/delimitnum Template:Val/units and Template:SimpleNuclide with a half-life of Template:Val/delimitnum Template:Val/units. All of the remaining radioactive isotopes have half-lives that are shorter than Template:Val/delimitnum Template:Val/units. The shortest-lived isotope of lithium is Template:SimpleNuclide which decays through proton emission and has a half-life of Template:Val/delimitnum×10Template:Su Template:Val/units.
Template:SimpleNuclide is one of the primordial elements or, more properly, primordial isotopes, produced in Big Bang nucleosynthesis (a small amount of Template:SimpleNuclide is also produced in stars). Lithium isotopes fractionate substantially during a wide variety of natural processes, including mineral formation (chemical precipitation), metabolism, and ion exchange. Lithium ion substitutes for magnesium and iron in octahedral sites in clay minerals, where Template:SimpleNuclide is preferred to Template:SimpleNuclide, resulting in enrichment of the light isotope in processes of hyperfiltration and rock alteration.
Isotopes
Lithium-4
Lithium-4 contains 3 protons and one neutron. It is the shortest lived isotope of lithium. It decays by proton emission and has a half-life of Template:Val/delimitnum×10Template:Su Template:Val/units. It can be formed as an intermediate in some nuclear fusion reactions.
Lithium-6
Lithium-6 is valued as a source material for tritium production and as a neutron absorber in nuclear fusion. Large amounts of lithium-6 have been isotopically fractionated for use in nuclear weapons.
Lithium-7
Some of the material remaining from the production of lithium-6, which is depleted in lithium-6 and enriched in lithium-7, is made commercially available, and some has been released into the environment. Relative lithium-7 abundances as high as 35.4% greater than the natural value have been measured in ground water from a carbonate aquifer underlying West Valley Creek, Pennsylvania (USA), down-gradient from a lithium processing plant. In depleted material, the relative Template:SimpleNuclide abundance may be reduced by as much as 80% of its normal value, giving the atomic mass a range from Template:Val/delimitnum Template:Val/units to more than Template:Val/delimitnum Template:Val/units. As a result, the isotopic composition of lithium is highly variable depending on its source. An accurate relative atomic mass cannot be given representatively for all samples.
Table
Notes
- The precision of the isotope abundances and atomic mass is limited through variations. The given ranges should be applicable to any normal terrestrial material.
- Geologically exceptional samples are known in which the isotopic composition lies outside the reported range. The uncertainty in the atomic mass may exceed the stated value for such specimens.
- Commercially available materials may have been subjected to an undisclosed or inadvertent isotopic fractionation. Substantial deviations from the given mass and composition can occur.
- In depleted material, the relative Template:SimpleNuclide abundance may be reduced by as much as 80% of its normal value, giving the atomic mass a range from Template:Val/delimitnum Template:Val/units to more than Template:Val/delimitnum Template:Val/units.
- Values marked # are not purely derived from experimental data, but at least partly from systematic trends. Spins with weak assignment arguments are enclosed in parentheses.
- Uncertainties are given in concise form in parentheses after the corresponding last digits. Uncertainty values denote one standard deviation, except isotopic composition and standard atomic mass from IUPAC which use expanded uncertainties.
- Template:SimpleNuclide has a Nuclear halo of two weakly linked neutrons, thus explaining an important difference in the radius.
References
- Isotope masses from Ame2003 Atomic Mass Evaluation by G. Audi, A.H. Wapstra, C. Thibault, J. Blachot and O. Bersillon in Nuclear Physics A729 (2003).
- Isotopic compositions and standard atomic masses from Atomic weights of the elements. Review 2000 (IUPAC Technical Report). Pure Appl. Chem. Vol. 75, No. 6, pp. 683-800, (2003) and Atomic Weights Revised (2005).
- Half-life, spin, and isomer data selected from these sources. Editing notes on this article's talk page.
- Audi, Bersillon, Blachot, Wapstra. The Nubase2003 evaluation of nuclear and decay properties, Nuc. Phys. A 729, pp. 3-128 (2003).
- National Nuclear Data Center, Brookhaven National Laboratory. Information extracted from the NuDat 2.1 database (retrieved Sept. 2005).
- David R. Lide (ed.), Norman E. Holden in CRC Handbook of Chemistry and Physics, 85th Edition, online version. CRC Press. Boca Raton, Florida (2005). Section 11, Table of the Isotopes.
| Isotopes of helium | Isotopes of lithium | Isotopes of beryllium |
| Index to isotope pages · Table of nuclides | ||
Acknowledgement and Attribution Regarding Sources of Content
Some of the initial content on this page may be incorporated in part from copyleft sources in the public domain including wikis such as Wikipedia and AskDrWiki. Drug information for patients came from the The National Library of Medicine. Infectious disease information may have come from the Centers for Disease Control (CDC). Differential Diagnoses are drawn from clinicians as well as an amalgamation of 3 sources: 1.The Disease Database; 2. Kahan, Scott, Smith, Ellen G. In A Page: Signs and Symptoms. Malden, Massachusetts: Blackwell Publishing, 2004:3; 3. Sailer, Christian, Wasner, Susanne. Differential Diagnosis Pocket. Hermosa Beach, CA: Borm Bruckmeir Publishing LLC, 2002:7 .
