Neon is naturally available as `""^(20)Ne and ""^(22)Ne` with average atomic mass 20.2. Calculate the relative abundance of heavier isotope.

Explanation

To solve the problem of calculating the relative abundance of the heavier isotope of neon, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Isotopes and Their Masses**:
- The isotopes of neon are \(^{20}\text{Ne}\) and \(^{22}\text{Ne}\).
- The mass of \(^{20}\text{Ne}\) (lighter isotope) is 20 amu.
- The mass of \(^{22}\text{Ne}\) (heavier isotope) is 22 amu.
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