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If an element \(X\) has two isotopes, \[tex]{}^{100}X\] (80%) and \[tex]{}^{102}X\] (20%), then the weighted average atomic mass of the naturally occurring element \(X\) will be:

A. 100.4 amu
B. 101.8 amu
C. 101.2 amu
D. 100.8 amu

Answer :

Final answer:

The weighted average atomic mass of an element is calculated using the masses and relative abundances of its naturally occurring isotopes. In the case of element X with isotopes ¹⁰⁰X (80%) and ¹⁰²X (20%), the average atomic mass would be 100.4 amu.

Explanation:

The weighted average atomic mass of an element is calculated by summing up the product of each isotope's mass and its fractional abundance. In the case of element X with isotopes ¹⁰⁰X (80%) and ¹⁰²X (20%), we'd calculate this as (100*0.8) + (102*0.2), which results in 100.4 amu. So, the correct answer is 100.4 amu (option a).

This calculation takes into account the relative abundance of each isotope in a naturally occurring sample of the element. Much like how the atomic mass of boron is calculated using the masses and relative abundances of its two isotopes, ¹⁰B and ¹¹B, and the atomic mass of copper is calculated using its stable isotopes, Cu and 65 Cu.

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