The three stable isotopes of neon : $^{20}_{10}$Ne, $^{21}_{10}$Ne and $^{22}_{10}$Ne have respective abundances of 90.51%, 0.27%. and 9.22%. The atomic masses of the three isotopes are 19.99u, 20.99 u and 21.99u, respectively. Obtain the average atomic mass of Neon.
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Calculate the contribution of each isotope to the average atomic mass: - Isotope 20Ne contributes (90.51/100) * 19.99 u = 18.07 u - Isotope 21Ne contributes (0.27/100) * 20.99 u = 0.06 u - Isotope 22Ne contributes (9.22/100) * 21.99 u = 2.03 u Show more…
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The three stable isotopes of neon: ${ }_{10}^{20} \mathrm{Ne}_{10}{ }^{21} \mathrm{Ne}$ and ${ }_{10}^{22} \mathrm{Ne}$ have respective abundances of $90.51 \%, 0.27 \%$ and $9.22 \%$. The atomic masses of the three isotopes are $19.99 \mathrm{u}, 20.99 \mathrm{u}$ and $21.99 \mathrm{u}$, respectively. Obtain the average atomic mass of neon.
The naturally occurring isotopes of neon are 20Ne (19.99 amu), 21Ne(20.99 amu), and 22Ne(21.99 amu). The natural abundances of these isotopes are 90.48%, 0.27% and 9.25%, respectively. What is the average atomic mass of neon?
Kartik I.
Neon has three naturally occurring isotopes. They include Ne-20, atomic mass of 19.992 amu and percent abundance of 90.48%; Ne-21, atomic mass of 20.994 amu and percent abundance of 0.27%; Ne-22 has a mass of 21.991 amu and percent abundance of 9.25%. Calculate the average atomic mass of neon?
Susan H.
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