Question

An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abudance with 21.99 amu. Calculate the average atomic mass of this elements.

Answer 1

Answer: The average atomic mass of element Z is 20.169 amu.

Step-by-step explanation:

Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.

Formula used to calculate average atomic mass follows:

`\text{Average atomic mass }=\sum_(i=1)^n\text{(Atomic mass of an isotopes)}_i* \text{(Fractional abundance})_i` .....(1)

• For isotope 1:

Mass of isotope 1 = 19.99 amu

Percentage abundance of isotope 1 = 90.92 %

Fractional abundance of isotope 1 = 0.9092

• For isotope 2:

Mass of isotope 2 = 20.99 amu

Percentage abundance of isotope 2 = 0.26 %

Fractional abundance of isotope 2 = 0.0026

• For isotope 3:

Mass of isotope 3 = 21.99 amu

Percentage abundance of isotope 3 = 8.82 %

Fractional abundance of isotope 3 = 0.0882

Putting values in equation 1, we get:

`\text{Average atomic mass of Z}=[(19.99* 0.9092)+(20.99* 0.0026)+(21.99* 0.0882)]`

`\text{Average atomic mass of Z}=20.169amu`

Hence, the average atomic mass of element Z is 20.169 amu.