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Neon has three stable nautrally occurring isotopes. The isotopic mass and percent abundance of these isotopes are given inthe table.Isotope20 Ne21 Ne22 NeIsotopic mass (u)19.9920.9921.99Abundance (%)90.480.2279.25Calculate the average atomic mass of neon.

Neon has three stable nautrally occurring isotopes The isotopic mass and percent abundance of these isotopes are given inthe tableIsotope20 Ne21 Ne22 NeIsotopic class=
Neon has three stable nautrally occurring isotopes The isotopic mass and percent abundance of these isotopes are given inthe tableIsotope20 Ne21 Ne22 NeIsotopic class=
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To calculate the average mass of Ne (neon), we have to use this formula:

[tex]\text{Average atomic mass = }\frac{\sum ^{}_{}(\text{mass of isotopes)x(abundance \%)}}{100}[/tex][tex]\begin{gathered} \text{Average atomic mass = }\frac{(19.99ux90.48+20.99ux0.27\text{ +}21.99ux9.25)}{100} \\ \text{Average atomic mass = }20.18\text{ u} \end{gathered}[/tex]

The average atomic mass of Ne = 20.18 u

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