The atomic mass of an element is calculated by adding the
number of protons and neutrons in the nucleus of an atom.
In more detail, the atomic mass is the weighted average of
the masses of all the isotopes of an element, where each isotope's mass is
multiplied by its relative abundance.
Mathematically, we can represent the calculation of the
atomic mass of an element as follows:
Atomic mass = (isotope mass 1 x abundance 1) + (isotope mass
2 x abundance 2) + ... + (isotope mass n x abundance n)
where:
isotope mass refers to the mass number (the total number of
protons and neutrons in the nucleus) of each isotope of the element
abundance refers to the proportion of each isotope in a
naturally occurring sample of the element
For example, the atomic mass of carbon is calculated as
follows:
Atomic mass of carbon = (mass of carbon-12 isotope x
abundance of carbon-12) + (mass of carbon-13 isotope x abundance of carbon-13)
= (12 amu x 0.9893) + (13.00335 amu x 0.0107) [where amu =
atomic mass unit]
= 12.011 amu
This means that on average, a carbon atom has a mass of
12.011 atomic mass units, taking into account the relative abundance of its
isotopes.
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