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Whole Number Rule



The Whole Number Rule states that the masses of the elements are whole number multiples of the mass of the hydrogen atom.[1] The rule can be formulated from Prout's hypothesis put forth in 1815.[2] In 1920, Francis W. Aston demonstrated through the use of a mass spectrometer that apparent deviations from the rule were due to the existence of isotopes.[3]

Additional recommended knowledge

See also

References

  1. ^ Budzikiewicz H, Grigsby RD (2006). "Mass spectrometry and isotopes: a century of research and discussion". Mass spectrometry reviews 25 (1): 146-57. doi:10.1002/mas.20061. PMID 16134128.
  2. ^ Prout, William (1815). "On the relation between the specific gravities of bodies in their gaseous state and the weights of their atoms.". Annals of Philosophy 6: 321–330. Retrieved on 2007-09-08.
  3. ^ Aston, Francis W. (1920). "The constitution of atmospheric neon". Philosophical Magazine 39 (6): 449-455. Retrieved on 2007-09-08.

Harkins WD (1925). "The Separation of Chlorine into Isotopes (Isotopic Elements) and the Whole Number Rule for Atomic Weights". Proc. Natl. Acad. Sci. U.S.A. 11 (10): 624–8. PMID 16587053.

 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Whole_Number_Rule". A list of authors is available in Wikipedia.
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