Percentage abundances and atomic masses (amu) of the natural...

Percentage abundances and atomic masses (amu) of the natural isotopes of an element are given.
(a) Calculate the atomic mass of each element from these data.
(b) Using other information that is available to you, identify the element.
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Key Concepts

Isotopic Abundances

This concept refers to the relative amounts of different isotopes of an element present in a natural sample. It is usually expressed as a percentage or fraction and is key to calculating properties like the atomic mass by considering the contribution of each isotope proportionally.

Atomic Mass

Atomic mass is the mass of an atom, typically measured in atomic mass units (amu). It represents an average value that takes into account the different masses and natural abundances of the isotopes of an element, forming a fundamental property in the study of atomic and molecular structures.

Weighted Average Calculation

The weighted average calculation is a method used to determine the average atomic mass of an element from its isotopes. Each isotope's mass is multiplied by its fractional abundance, and the results are summed to yield the overall atomic mass, reflecting the relative contribution of each isotope.

Element Identification via Atomic Mass

Identifying an element by its atomic mass involves comparing the calculated weighted average atomic mass with known values listed on the periodic table. Since each element has a unique atomic mass range, this approach allows one to pinpoint the specific element based on its isotopic composition.

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