Whole Number Rule
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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

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, http://web.lemoyne.edu/~giunta/PROUT.HTML. Retrieved on 8 September 2007. 
  3. ^ Aston, Francis W. (1920). "The constitution of atmospheric neon". Philosophical Magazine 39 (6): 449–455. 

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. 

External links

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