The three stable isotopes of neon `._10Ne^(20), ._10Ne^(21)` and `._10Ne^(22)` 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.

Explanation

To find the average atomic mass of neon based on its isotopes and their respective abundances, we can follow these steps:

### Step 1: Identify the isotopes and their properties
We have three stable isotopes of neon:
- Isotope: \(_{10}^{20}\text{Ne}\) with an abundance of 90.51% and an atomic mass of 19.99 u.
- Isotope: \(_{10}^{21}\text{Ne}\) with an abundance of 0.27% and an atomic mass of 20.99 u.
- Isotope: \(_{10}^{22}\text{Ne}\) with an abundance of 9.22% and an atomic mass of 21.99 u.

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