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Isotopes
Different forms of the same element, which have the same number of protons but a different number of neutrons
so isotopes have the same atomic number, but different mass numbers
Relative Atomic Mass (Ar)
the average mass of one atom of the element, compared to 1/12 of the mass of one atom of carbon-12
Formula to calculate the Ar of an element from its isotopic abundance
Ar = sum of (isotopic abundance x isotope mass number)/ sum of abundances of all the isotopes x 100
are isotopes stupid?
yes
Note 
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