To determine which isotopes of boron are more abundant based on their atomic masses, we can compare the masses of the isotopes:
- Boron-10 (B-10) has an atomic mass of approximately 10 amu.
- Boron-11 (B-11) has an atomic mass of approximately 11 amu.
When considering the average atomic mass of natural boron, which is about 10.81 amu, the fact that this average is closer to 11 amu suggests that boron-11 is the more abundant isotope.
In natural abundance, boron-10 comprises about 20% of natural boron, while boron-11 makes up around 80%. Therefore, based on the calculation of atomic mass and the average atomic mass, boron-11 is the more abundant isotope.
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