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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

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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