Question

A hypothetical element, Marshallium (Mu), has an average atomic mass of 73.91 amu. Assuming it has 4 stable isotopes, Mu-73, Mu-74, Mu-77, and Mu-78, which of these would you expect to have the highest percent abundance and lowest percent abundance?

Option 1: Mu-73 with the highest percent abundance.
Option 2: Mu-78 with the highest percent abundance.
Option 3: Mu-74 with the highest percent abundance.
Option 4: Mu-77 with the highest percent abundance.

Answer 1

The isotope Mu-74 would have the highest percent abundance, while Mu-73 would have the lowest percent abundance.

Step-by-step explanation:

When determining the highest and lowest percent abundances of isotopes in an element, we look at their relative masses and the average atomic mass of the element. In this case, Marshallium (Mu) has an average atomic mass of 73.91 amu. To find the isotopes with the highest and lowest percent abundances, we compare their masses to the average atomic mass. The isotope with the highest percent abundance will have a mass closest to the average atomic mass, while the isotope with the lowest percent abundance will have a mass further away from the average atomic mass.

In this scenario, we compare the masses of the four stable isotopes of Marshallium (Mu-73, Mu-74, Mu-77, and Mu-78) to the average atomic mass of 73.91 amu. The isotope closest in mass to the average atomic mass will have the highest percent abundance, and the isotope further away will have the lowest percent abundance.

So, the answer to the question is Option 3: Mu-74 with the highest percent abundance and Option 1: Mu-73 with the lowest percent abundance.