Question

1. calculate the average atomic mass

Explanation:

Step1: Recall average atomic mass formula

The formula for average atomic mass $A = \sum_{i} (m_i\times p_i)$, where $m_i$ is the mass - charge ratio and $p_i$ is the percentage abundance.

Step2: Convert percentages to decimals

$p_1=\frac{2}{100} = 0.02$, $p_2=\frac{24}{100}=0.24$, $p_3=\frac{22}{100}=0.22$, $p_4=\frac{52}{100}=0.52$. And $m_1 = 204$, $m_2=206$, $m_3 = 207$, $m_4=208$.

Step3: Calculate the product for each isotope

$m_1\times p_1=204\times0.02 = 4.08$, $m_2\times p_2=206\times0.24 = 49.44$, $m_3\times p_3=207\times0.22 = 45.54$, $m_4\times p_4=208\times0.52 = 108.16$.

Step4: Sum up the products

$A=4.08 + 49.44+45.54 + 108.16=207.22$.

Answer:

$207.22$