The three stable isotopes of neon: 10^20 Ne10 ^21 Ne and 10^22 Ne have respective abundances o

step 1 In this problem we have three isotopes of neon and their abundances and the atomic mass of the t

The three stable isotopes of neon: 10^20 Ne10 ^21 Ne and ...

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.

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Key Concepts

Weighted Average Calculation

The weighted average calculation is a method used to determine the average atomic mass of an element from its isotopes. This involves multiplying the atomic mass of each individual isotope by its fractional abundance and summing the products. The resulting value is the average atomic mass, which is typically reported on the periodic table.

Isotopic Abundance

Isotopic abundance refers to the proportion of each isotope present in a naturally occurring sample of an element. It is usually expressed as a percentage or fraction of the total number of atoms in the element. These relative abundances are essential for calculating a weighted average atomic mass, reflecting the natural distribution of an element's isotopes.

Isotopes

Isotopes are variants of the same element that have the same number of protons but differ in the number of neutrons. This leads to differing atomic masses while maintaining the same chemical properties. Understanding isotopes is fundamental when discussing elements that appear on the periodic table, as their individual contributions must be taken into account for accurate mass measurements.

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