Why is atomic mass of an element not considered as the actual mass of its atom?
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Atomic masses expressed in daltons (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: protons and neutrons have different masses, and different nuclides have different ratios of protons and neutrons.
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mainly atomic mass is equal to atomic number but some element has different atomic mass due to isotopes and isobars
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