The three stable isotopes of neon: $_{10}^{20} Ne$ , $_{10}^{21} Ne$ and $_{10}^{22} Ne$ have respective abundances of $90.51 %, 0.27 %$ and $9.22 %$ . The atomic masses of the three isotopes are $19.99 u, 20.99 u$ and $21.99 u$ , respectively. Obtain the average atomic mass of neon.

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Solution

The average atomic mass is given by,

Average atomic mass $= \frac{\sum_{i = 1}^{n} (m a s s_{(i)}) (A b u n d a n c e_{(i)})}{100}$

$m = \frac{90.51 \times 19.99 + 0.27 \times 20.99 + 9.22 \times 21.99}{100}$

$= 20.18 u$

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The three stable isotopes of neon: 2010Ne, 2110Ne and 2210Ne have respective abundances of 90.51%,0.27% and 9.22%. The atomic masses of the three isotopes are 19.99u,20.99u and 21.99u, respectively. Obtain the average atomic mass of neon.

The average atomic mass is given by,Average atomic mass =∑ni=1(mass(i))(Abundance(i))100m=90.51×19.99+0.27×20.99+9.22×21.99100 =20.18u

The three stable isotopes of neon: $_{10}^{20} Ne$ , $_{10}^{21} Ne$ and $_{10}^{22} Ne$ have respective abundances of $90.51 %, 0.27 %$ and $9.22 %$ . The atomic masses of the three isotopes are $19.99 u, 20.99 u$ and $21.99 u$ , respectively. Obtain the average atomic mass of neon.

The average atomic mass is given by,

Average atomic mass $= \frac{\sum_{i = 1}^{n} (m a s s_{(i)}) (A b u n d a n c e_{(i)})}{100}$

$m = \frac{90.51 \times 19.99 + 0.27 \times 20.99 + 9.22 \times 21.99}{100}$

$= 20.18 u$