Two isotopes of gallium are naturally occurring, with 31^69 Ga at 60.11 %(68.93 amu) and 31^71

step 1 Hello everyone. In this question we have been given the two isotopes of gallium, right? So galli

Two isotopes of gallium are naturally occurring, with 31^69...

Two isotopes of gallium are naturally occurring, with ${ }_{31}^{69} \mathrm{Ga}$ at $60.11 \%(68.93 \mathrm{amu})$ and ${ }_{31}^{71} \mathrm{Ga}$ at $39.89 \%$ (70.92 amu). Calculate the atomic mass for gallium using the weighted average mass method.

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Key Concepts

Weighted Average Calculation

This concept refers to the method of combining individual values, such as different isotopic masses, by multiplying each value by its corresponding weight (or fraction) and then summing these products to obtain an overall average. It is crucial for accurately representing the average mass of an element based on the varying contributions of its isotopes.

Isotopic Abundance

Isotopic abundance indicates the relative proportion of each isotope present in a natural sample of an element. It is commonly expressed as a percentage or decimal, and it is essential in calculating the weighted average atomic mass by determining how much each isotope contributes to the average.

Atomic Mass

Atomic mass is the weighted average mass of the atoms of an element, calculated using the masses of all naturally occurring isotopes and their respective abundances. This value, which reflects the natural isotopic composition, is used in chemical calculations and is typically recorded in the periodic table.

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