For the imaginary element abdicinium (Ab),two isotopes exist.Isotope one has a mass of 40.005 amu with a relative abundance of 14.00%.Isotope two has a mass of 41.008 amu with a relative abundance of 86.00%.What is the atomic mass of the element?

Question

Quizplus · Accepted Answer

The atomic mass of the element can be calculated by multiplying the mass of each isotope by its relative abundance (expressed as a fraction), then summing these products. For abdicinium:- Isotope 1: $40.005 \, \text{amu} \times 0.14 = 5.6007 \, \text{amu}$- Isotope 2: $41.008 \, \text{amu} \times 0.86 = 35.26688 \, \text{amu}$Adding these together gives the atomic mass of abdicinium as $5.6007 + 35.26688 = 40.86758 \, \text{amu}$, which rounds to $40.87 \, \text{amu}$.

For the Imaginary Element Abdicinium (Ab),two Isotopes Exist