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    IsotopeAtomic mass (Da)Isotopic abundance (amount fraction)
    24Mg23.985 041 70(9)[0.7888, 0.7905]
    25Mg24.985 8370(3)[0.099 88, 0.100 34]
    26Mg25.982 5930(2)[0.1096, 0.1109]

    In 2011, the Commission has changed the standard atomic weight of magnesium to Ar(Mg) = [24.304, 24.307] based on an evaluation of the effect of variation in isotopic abundances in normal materials upon the atomic weight of magnesium. This change is intended to emphasize the fact that the atomic weight of magnesium is not a constant of nature, but depends upon the source of the material. The standard atomic weight was determined by combining (1) the best calibrated isotope-ratio measurement of magnesium in DSM3 isotopic reference material (a mono-elemental nitric solution of magnesium), and (2) the relative isotope-ratio differences between other magnesium-bearing materials and DSM3. Many of the δ(26/24Mg) measurements reported herein were made using DSM3 as the standard. However, the Commission does not recommend DSM3 as an international measurement standard for δ(26/24Mg) measurements because it is not readily available to laboratories worldwide.

    SOURCES  Atomic weights of the elements: Review 2000 by John R de Laeter et al. Pure Appl. Chem. 2003 (75) 683-800
    Atomic weights of the elements 2011 by M.E. Wieser et al. Pure Appl. Chem. 2013 (85) 1047-1078


    Ar(Mg) = [24.304, 24.307] since 2011

    The name derives from Magnesia, a district in the north-eastern region of Greece called Thessalia. The Scottish chemist Joseph Black recognized it as a separate element in 1755. In 1808, the English chemist Humphry Davy obtained the impure metal, and in 1831 the French pharmacist and chemist Antoine- Alexandre Brutus Bussy isolated the metal in the pure state.

    Natural variations of magnesium isotopic composition

    Isotopic reference materials of magnesium.