To find the average atomic mass of the element given the data table with masses and abundances, follow these steps:
1. List the masses and their respective abundances:
- Mass: [tex]\( 12.00 \)[/tex] amu, Abundance: [tex]\( 98.93\% \)[/tex]
- Mass: [tex]\( 13.00 \)[/tex] amu, Abundance: [tex]\( 1.07\% \)[/tex]
2. Convert the abundances from percentages to fractions:
- For the first isotope: [tex]\( 98.93\% \)[/tex] becomes [tex]\( 0.9893 \)[/tex] (which is [tex]\( 98.93 \div 100 \)[/tex]).
- For the second isotope: [tex]\( 1.07\% \)[/tex] becomes [tex]\( 0.0107 \)[/tex] (which is [tex]\( 1.07 \div 100 \)[/tex]).
3. Multiply each mass by its respective fractional abundance to find the contribution of each isotope to the average atomic mass:
- Contribution of the first isotope: [tex]\( 12.00 \times 0.9893 = 11.8716 \)[/tex]
- Contribution of the second isotope: [tex]\( 13.00 \times 0.0107 = 0.1391 \)[/tex]
4. Sum these contributions to get the average atomic mass:
[tex]\[
11.8716 + 0.1391 = 12.0107
\][/tex]
Therefore, the average atomic mass of the element is [tex]\( 12.0107 \)[/tex] amu, which, when rounded to the nearest hundredth, is [tex]\( 12.01 \)[/tex] amu.
So, the correct answer is:
[tex]\[
\boxed{12.01 \text{ amu}}
\][/tex]
