Chlorine exists as two isotopes in nature, 1^5 Cl (atomic mass 34.969 amu, abundance 75.77 % )

step 1 To determine the percent of the other isotope, because there are two isotopes, both of their per

Chlorine exists as two isotopes in nature, 1^5 Cl (atomic...

Chlorine exists as two isotopes in nature, ${ }_{1}^{5} \mathrm{Cl}$ (atomic mass $34.969$ amu, abundance $75.77 \%$ ) and ${ }_{17}^{37} \mathrm{Cl}$ (atomic mass $36.966$ amu). (a) What is the percent abundance of the ${ }_{1}^{37} \mathrm{Cl}$ isotope? (b) Calculate the weighted average of the atomic mass of naturally occurring chlorine. (c) How many times more massive is ${ }_{1}^{37} \mathrm{Cl}$ than ${ }_{17}^{35} \mathrm{Cl} ?$

Chlorine exists as two isotopes in nature, ${ }_{1}^{5} \mathrm{Cl}$ (atomic mass $34.969$ amu, abundance $75.77 \%$ ) and ${ }_{17}^{37} \mathrm{Cl}$ (atomic mass $36.966$ amu).
(a) What is the percent abundance of the ${ }_{1}^{37} \mathrm{Cl}$ isotope?
(b) Calculate the weighted average of the atomic mass of naturally occurring chlorine.
(c) How many times more massive is ${ }_{1}^{37} \mathrm{Cl}$ than ${ }_{17}^{35} \mathrm{Cl} ?$

Key Concepts

Weighted Average Atomic Mass

The weighted average atomic mass of an element is calculated by summing the products of each isotope’s atomic mass and its percent abundance (expressed as a fraction). This calculation provides a single value that reflects the average mass of atoms in a naturally occurring sample of the element, taking into account the contribution of each isotope.

Mass Ratio Calculation

A mass ratio calculation compares the masses of two different isotopes or entities by dividing one mass by another. This concept is useful to determine how many times more massive one isotope is compared to another and helps in understanding relative differences in mass between isotopes.

Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, leading to different atomic masses. Their properties are usually quite similar chemically, but the differences in mass can affect physical properties and processes such as nuclear reactions and radioactive decay.

Percent Abundance

Percent abundance describes the relative proportion of each isotope present in a naturally occurring sample of an element. It is expressed as a percentage that indicates how much of the sample's overall atomic makeup is made up of a particular isotope, and it is crucial for determining the weighted average atomic mass.

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