Copper has only two naturally occurring isotopes, Cu63 and Cu-65 . The mass of Cu-63 is 62.9396

step 1 To answer this question, we're going to need to look up the average atomic mass of copper. We al

Copper has only two naturally occurring isotopes, Cu63 and...

Copper has only two naturally occurring isotopes, Cu63 and $\mathrm{Cu}-65 .$ The mass of $\mathrm{Cu}-63$ is $62.9396 \mathrm{amu},$ and the mass of $\mathrm{Cu}-65$ is 64.9278 amu. Use the atomic mass of copper to determine the relative abundance of each isotope in a naturally occurring sample.

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Key Concepts

Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses while retaining nearly identical chemical properties. This concept is essential when analyzing the composition of an element as found in nature.

Atomic Mass

Atomic mass is a weighted average of the masses of all the isotopes of an element, taking into account their relative abundances. It represents the average mass of atoms of an element as they occur naturally, and it is typically expressed in atomic mass units (amu).

Relative Abundance

Relative abundance refers to the proportion or percentage of each isotope present in a naturally occurring sample of an element. It is used to determine the contribution of each isotope to the overall atomic mass of the element.

Weighted Average Calculation

Weighted average calculation involves multiplying the mass of each isotope by its relative abundance and then summing these products to determine the overall atomic mass of the element. This approach is fundamental for linking the individual properties of isotopes to the average properties of the element as a whole.

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