Relative Atomic Mass Notes

Relative Atomic Mass Notes page 33

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Calculate the atomic mass of an element that has two common isotopes of 12.000 amu (98.89 % abundance) and 13.003 amu (1.11 % abundance).

What is the element?

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Calculate the atomic mass of an element with two common isotopes of 14.003 amu (99.63% abundance) and 15.000 amu (0.37% abundance).

What is the element?

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Calculate the atomic mass of an element with three common isotopes; 15.995 amu (99.759% abundance), 16.995 amu (0.037 % abundance), and 17.999 amu (0.204 % abundance).

What is the element?

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An unknown element which occurs as two isotopes and has the following atomic masses abundances:

 

 6.017amu, 7.30%

7.018amu, 92.70%

What is the element?