A number of authors have published criticisms of the revised definitions in particular that proposal had failed to address the impact of breaking the link between the dalton and the unified atomic mass unit, and the Avogadro constant and Avogadro's number.
12.
Atomic masses expressed in unified atomic mass units ( i . e . relative isotopic masses ) are always close to whole-number values, but never ( except in the case of carbon-12 ) exactly a whole number, for two reasons:
13.
This shift in nomenclature reaches back to the 1960s and has been the source of much debate in the scientific community, which was triggered by the adoption of the unified atomic mass unit and the realization that weight was in some ways an inappropriate term.
14.
The mass number should also not be confused with the relative atomic mass ( also called atomic weight ) of an element, which is the ratio of the average atomic mass of the different isotopes of that element ( weighted by abundance ) to the unified atomic mass unit.
15.
When compared to the average mass per nucleon in carbon-12, which is moderately strongly-bound compared with other atoms, the mass defect of binding for most atoms is an even smaller fraction of a dalton ( unified atomic mass unit, based on carbon-12 ).
16.
An atomic mass of 16 was assigned to oxygen prior to the definition of the unified atomic mass unit based upon 12 C . Since physicists referred to 16 O only, while chemists meant the naturally-abundant mixture of isotopes, this led to slightly different mass scales between the two disciplines.
17.
Since 1961 the unified atomic mass unit " u " has been defined as 1 / 12 the mass of 12 C . Before that the atomic mass unit " amu " was defined as 1 / 16 the mass of 16 O ( physics ) and as 1 / 16 the mass of O ( chemistry ).
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