Question

3 bellringer: abundance of isotopes 2526 what is the average atomic mass of element \g\ if it has two isotopes of g - 210 with 77.42% abundance and mass 209.99 amu, and g - 211 with 22.58% abundance and mass 210.99 amu? enter your answer with two decimal places average atomic mass= amu

Explanation:

Step1: Convert percentages to decimals

The abundance of G - 210 is $77.42\%=0.7742$, and the abundance of G - 211 is $22.58\% = 0.2258$.

Step2: Calculate the weighted - average atomic mass

The formula for the average atomic mass $A$ of an element with two isotopes is $A=m_1x_1 + m_2x_2$, where $m_1$ and $m_2$ are the masses of the isotopes and $x_1$ and $x_2$ are their respective abundances. Here, $m_1 = 209.99$ amu, $x_1=0.7742$, $m_2 = 210.99$ amu, and $x_2 = 0.2258$.

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Rounding to two decimal places, we get $210.28$ amu.

Answer:

$210.28$ amu