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.
(TABLE CANNOT COPY)

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Key Concepts

Element Identification via Atomic Mass

Element identification based on atomic mass involves comparing the calculated weighted average atomic mass with standard atomic masses found on the periodic table. By matching these values, one can deduce the identity of an element, a key step in many analyses in chemistry.

Isotopes

Isotopes are variations of a chemical element that have the same number of protons but different numbers of neutrons. This difference in neutron count leads to variations in their atomic masses while retaining the same chemical properties, making the concept of isotopes crucial for understanding atomic mass calculations.

Isotopic Abundance

Isotopic abundance refers to the relative quantities of each isotope present in a naturally occurring element, usually expressed as percentages or fractions. These percentages determine the contribution of each isotope's mass to the overall atomic mass of the element.

Weighted Average Atomic Mass

The weighted average atomic mass is calculated by multiplying the atomic mass of each isotope by its relative abundance and then summing these values. This calculation reflects the average mass of the atoms of an element as found in nature and accounts for the distribution of its isotopes.

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