Standard atomic weight

The standard atomic weight of a <a href="/facts/Chemical_element/0jducgWD">chemical element</a> (symbol Ar°(E) for element "E") is the <a href="/facts/Weighted_arithmetic_mean/VHyJfPxb">weighted arithmetic mean</a> of the <a href="/facts/Relative_isotopic_mass/J1FJY9MV">relative isotopic masses</a> of all <a href="/facts/Isotope/KD9B1y6o">isotopes</a> of that element <a href="/facts/Weighted_arithmetic_mean/VHyJfPxb">weighted</a> by each isotope's abundance on <a href="/facts/Earth/HLLmDfj0">Earth</a>. For example, isotope 63Cu (Ar = 62.929) constitutes 69% of the <a href="/facts/Copper/I8PEE8oX">copper</a> on Earth, the rest being 65Cu (Ar = 64.927), so

A
          
            r
          
        
        
          °
        
        
          (
          
            29
          
        
        
          Cu
        
        )
        =
        0.69
        ×
        62.929
        +
        0.31
        ×
        64.927
        =
        63.55.
      
    
    {\displaystyle A_{\text{r}}{\text{°}}(_{\text{29}}{\text{Cu}})=0.69\times 62.929+0.31\times 64.927=63.55.}

Relative isotopic masses <a href="/facts/Dimensionless_quantities/TINrpQIq">dimensionless</a>, and so is the weighted average. It can be converted into a measure of mass (with <a href="/facts/Dimensional_analysis/t6UskoCD">dimension</a> M) by multiplying it with the atomic mass constant <a href="/facts/Dalton_(unit)/IMATU3vf">dalton</a>.
Among various variants of the notion of <a href="/facts/Relative_atomic_mass/A3vbuz2n">atomic weight</a> (Ar, also known as <a href="/facts/Relative_atomic_mass/A3vbuz2n">relative atomic mass</a>) used by scientists, the standard atomic weight (Ar°) is the most common and practical. The standard atomic weight of each chemical element is determined and published by the <a href="/facts/Commission_on_Isotopic_Abundances_and_Atomic_Weights/WJGuHBB3">Commission on Isotopic Abundances and Atomic Weights</a> (CIAAW) of the <a href="/facts/International_Union_of_Pure_and_Applied_Chemistry/2AV6myCK">International Union of Pure and Applied Chemistry</a> (IUPAC) based on natural, stable, terrestrial sources of the element. The definition specifies the use of samples from many representative sources from the Earth, so that the value can widely be used as the atomic weight for substances as they are encountered in reality—for example, in pharmaceuticals and scientific research. Non-standardized atomic weights of an element are specific to sources and samples, such as the atomic weight of carbon in a particular bone from a particular archaeological site. Standard atomic weight averages such values to the range of atomic weights that a chemist might expect to derive from many random samples from Earth. This range is the rationale for the interval notation given for some standard atomic weight values.
Of the 118 known chemical elements, 80 have stable isotopes and 84 have this Earth-environment based value. Typically, such a value is, for example helium: Ar°(He) = 4.002602(2). The "(2)" indicates the uncertainty in the last digit shown, to read 4.002602±0.000002. IUPAC also publishes abridged values, rounded to five significant figures. For helium, Ar, abridged°(He) = 4.0026.
For fourteen elements the samples diverge on this value, because their sample sources have had a different decay history. For example, thallium (Tl) in sedimentary rocks has a different isotopic composition than in igneous rocks and volcanic gases. For these elements, the standard atomic weight is noted as an interval: Ar°(Tl) = [204.38, 204.39]. With such an interval, for less demanding situations, IUPAC also publishes a conventional value. For thallium, Ar, conventional°(Tl) = 204.38.

Standard atomic weight open-in-new

Standard atomic weight