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Commission on Isotopic Abundances and Atomic Weights


Commission on Isotopic Abundances and Atomic Weights

Commission on Isotopic Abundances and Atomic Weights
CIAAW logo
Abbreviation CIAAW
Formation 1899
Type International scientific organization
Purpose To provide internationally recommended values of isotopic composition and atomic weights of elements
Region served
Official language
Juris Meija (since 2014)
Parent organization
IUPAC (since 1920)

The Commission on Isotopic Abundances and Atomic Weights (CIAAW) is an international scientific committee of the atomic weights of chemical elements and other cognate data, such as the isotopic composition of elements.[1] The biennial CIAAW Standard Atomic Weights are accepted as the authoritative source in science and appear worldwide on the periodic table wall charts.[2]

The use of CIAAW Standard Atomic Weights is also required legally, for example, in calculation of calorific value of natural gas (ISO 6976:1995), or in gravimetric preparation of primary reference standards in gas analysis (ISO 6142:2006). In addition, the current definition of kelvin, the SI unit for thermodynamic temperature, makes direct reference to the isotopic composition of oxygen and hydrogen as recommended by CIAAW.[3] The latest CIAAW report was published in April 2013.[4][5]


  • Establishment 1
  • Function 2
  • Notable decisions 3
    • International atomic weight unit: H=1 or O=16 3.1
    • Modern unit: 12C=12 3.2
    • Uncertainty of the atomic weights 3.3
    • Interval notation 3.4
  • Affiliations and name 4
  • Notable members 5
    • Chairmen of the Commission 5.1
  • See also 6
  • References 7
  • External links 8


Although the atomic weight had taken on the concept of a constant of nature like the speed of light, the lack of agreement on accepted values created difficulties in trade. Quantities measured by chemical analysis were not being translated into weights in the same way by all parties and standardization became an urgent matter.[6] With so many different values being reported, the American Chemical Society (ACS), in 1892, appointed a permanent committee to report on a standard table of atomic weights for acceptance by the Society. Clarke, who was then the chief chemist for the U.S. Geological Survey, was appointed a committee of one to provide the report. He presented the first report at the 1893 annual meeting and published it in January 1894.[7]

In 1897, the German Society of Chemistry, following a proposal by Frank W. Clarke.[8] The large committee conducted its business by correspondence to Landolt which created difficulties and delays associated with correspondence among fifty-eight members. As a result, on 15 December 1899, the German committee asked the International members to select a small committee of three to four members.[9] In 1902, Prof. Frank W. Clarke (USA), Prof. Karl Seubert (Germany), and Prof. Thomas Edward Thorpe (UK) were elected, and the International Committee on Atomic Weights published its inaugural report in 1903 under the chairmanship of Prof. Clarke.[10]


Since 1899, the Commission periodically and critically evaluates the published scientific literature and produces the Table of Standard Atomic Weights. In recent times, the Table of Standard Atomic Weights has been published biennially. Each recommended standard atomic-weight value reflects the best knowledge of evaluated, published data. In the recommendation of standard atomic weights, CIAAW generally does not attempt to estimate the average or composite isotopic composition of the Earth or of any subset of terrestrial materials. Instead, the Commission seeks to find a single value and symmetrical uncertainty that would include almost all substances likely to be encountered.[11]

Notable decisions

Many notable decisions have been made by the Commission over its history. Some of these are highlighted below.

Atomic Weights
The inaugural 1903 report of the International Atomic Weights Commission

International atomic weight unit: H=1 or O=16

Though Dalton proposed setting the atomic weight of hydrogen as unity in 1803, many other proposals were popular throughout the 19th century. By the end of the 19th century, two scales gained popular support: H=1 and O=16. This situation was undesired in science and in October 1899, the inaugural task of the International Commission on Atomic Weights was to decide on the international scale and the oxygen scale became the international standard.[12] The endorsement of the oxygen scale created significant backlash in the chemistry community, and the inaugural Atomic Weights Report was thus published using both scales. This practice soon ceded and the oxygen scale remained the international standard for decades to come. Nevertheless, when the Commission joined the IUPAC in 1920, it was asked to revert to the H=1 scale, which it rejected.

Modern unit: 12C=12

With the discovery of oxygen isotopes in 1929, a situation arose where chemists based their calculations on the average atomic mass (atomic weight) of oxygen whereas physicists used the mass of the predominant isotope of oxygen, oxygen-16. This discrepancy became undesired and a unification between the chemistry and physics was necessary.[13] In the 1957 Paris meeting the Commission put forward a proposal for a carbon-12 scale.[14] The carbon-12 scale for atomic weights and nuclide masses was approved by IUPAP (1960) and IUPAC (1961) and it is still in use worldwide.[15]

Uncertainty of the atomic weights

In the early 20th century, measurements of the atomic weight of lead showed significant variations depending on the origin of the sample. These differences were considered to be an exception attributed to lead isotopes being products of the natural radioactive decay chains of uranium. In 1930s, however, Malcolm Dole reported that the atomic weight of oxygen in air was slightly different from that in water.[16] Soon thereafter, Alfred Nier reported natural variation in the isotopic composition of carbon. It was becoming clear that atomic weights are not constants of nature. At the Commission’s meeting in 1951, it was recognized that the isotopic-abundance variation of sulfur had a significant effect on the internationally accepted value of an atomic weight. In order to indicate the span of atomic-weight values that may apply to sulfur from different natural sources, the value ± 0.003 was attached to the atomic weight of sulfur. By the 1969, the Commission had assigned uncertainties to all atomic-weight values.

Atomic Weights
Excerpt of the IUPAC Periodic Table of the Elements 2011 showing the interval notation of the standard atomic weights of boron, carbon, and nitrogen

Interval notation

At its meeting in 2009 in Vienna, the Commission decided to express the standard atomic weight of hydrogen, carbon, oxygen, and other elements in a manner that clearly indicates that the values are not constants of nature.[17][18] For example, writing the standard atomic weight of hydrogen as [1.007 84, 1.008 11] shows that the atomic weight in any normal material will be greater than or equal to 1.007 84 and will be less than or equal to 1.008 11.[19]

Affiliations and name

The Commission on Isotopic Abundances and Atomic Weights has undergone many name changes:

  • The Great International Committee on Atomic Weights (1899-1902)
  • International Committee on Atomic Weights (1902-1920)
  • IUPAC Commission on Atomic Weights (1920-1922)
  • IUPAC Commission on Chemical Elements (1922-1930)
  • IUPAC Commission on Atomic Weights (1930-1979)
  • IUPAC Commission of Atomic Weights and Isotopic Abundances (1979-2002)
  • IUPAC Commission of Isotopic Abundances and Atomic Weights (2002–present)

Notable members

The Harvard chemist Theodore W. Richards, a member of the International Atomic Weights Commission, was awarded the 1914 Nobel Prize in Chemistry for his work on atomic weight determination

Since its establishment, many notable chemists have been members of the Commission. Notably, eight Nobel laureates have served in the Commission: Henri Moissan (1903-1907), Wilhelm Ostwald (1906-1916), Francis William Aston, Frederick Soddy, Theodore William Richards, Niels Bohr, Otto Hahn and Marie Curie.

Richards was awarded the 1914 Nobel Prize in Chemistry "in recognition of his accurate determinations of the atomic weight of a large number of chemical elements"[20] while he was a member of the Commission.[21] Likewise, Francis Aston was a member of the Commission when he was awarded the 1922 Nobel Prize in Chemistry for his work on isotope measurements.[22] Incidentally, the 1925 Atomic Weights report was signed by three Nobel laureates.[23]

Among other notable scientists who have served on the Commission were flerovium bears his name).,[24] Robert Whytlaw-Gray (first isolated radon), and Arne Ölander (Secretary and Member of the Nobel Committee for Chemistry).

Chairmen of the Commission

Since its establishment, the chairmen of the Commission have been:

In 1950, the renowned Spanish chemist Enrique Moles became the first Secretary of the Commission when this position was created.

See also


  1. ^
  2. ^
  3. ^
  4. ^
  5. ^
  6. ^
  7. ^
  8. ^ L.M. Dennis, Frank Wigglesworth Clarke (National Academy of Sciences 1932) at p.143
  9. ^
  10. ^
  11. ^
  12. ^ Theodore W. Richards, International Atomic Weights (Proceedings of the American Academy of Arts and Sciences, 1900) [1]
  13. ^
  14. ^
  15. ^ Encyclopaedia Britannica
  16. ^
  17. ^
  18. ^
  19. ^
  20. ^
  21. ^
  22. ^
  23. ^
  24. ^

External links

  • Official website
  • Atomic weights of the elements 2011 (IUPAC Technical Report)
  • Isotopic compositions of the elements 2009 (IUPAC Technical Report)
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