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To add confusion:
The AMU number on the periodic table gives the "average" mass of 1 mole of element.
Consider that ~75% or so of Carbon in nature is "C-12" [ie. 6 protons and 6 neutrons, hence mass of ~12g/mol] however, if you look on the periodic table, Carbon has a mass of 12.011.
Why?
Because the remaining ~25% of Carbon is in the form of isotopes such as "C-13" [ie. 6 protons, 7 neutrons, which gives a mass of ~13g/mol].
The AMU given on the periodic table accounts for these isotopes.
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