Chromium has four naturally occurring isotopes: 4.34 % of ^50 Cr, with an atomic weight of 49.9

step 1 We are asked to calculate the atomic mass of chromium. And we're told that chromium has four nat

Chromium has four naturally occurring isotopes: 4.34 % of ...

Chromium has four naturally occurring isotopes: $4.34 \%$ of ${ }^{50} \mathrm{Cr}$, with an atomic weight of $49.9460$ amu; $83.79 \%$ of ${ }^{52} \mathrm{Cr}$, with an atomic weight of $51.9405 \mathrm{amu} ; 9.50 \%$ of ${ }^{53} \mathrm{Cr}$, with an atomic weight of $52.9407 \mathrm{amu} ;$ and $2.37 \%$ of ${ }^{54} \mathrm{Cr}$, with an atomic weight of $53.9389$ amu. On the basis of these data, confirm that the average atomic weight of $\mathrm{Cr}$ is $51.9963 \mathrm{amu}$

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Key Concepts

Percentage Composition

This term describes the fraction or percentage of each isotope present in a sample. It is essential for performing weighted calculations, as it determines the contribution of each isotope to the overall atomic weight.

Atomic Weight

Atomic weight is the average mass of atoms of an element, accounting for all the isotopes and their relative abundances. It provides a representative value that reflects the mixture of isotopes present naturally.

Weighted Average Calculation

This refers to the process of computing an overall value using individual values that are weighted according to their relative importance. In the context of atomic weights, each isotope's mass is multiplied by its fractional abundance, and the sum of these products is the average atomic weight.

Isotopic Abundance

This concept involves the relative amounts of each naturally occurring isotope of an element. It is usually expressed as a percentage, and it plays a crucial role in determining the average atomic weight by indicating how much each isotope contributes.

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