To calculate the relative atomic mass of boron, we need to consider the information regarding its isotopes. Boron has two naturally occurring isotopes: boron-10 and boron-11.
Boron-10 has 5 protons and 5 neutrons, while boron-11 has 5 protons and 6 neutrons. The difference between these two atoms lies in the number of neutrons in their nuclei.
To calculate the relative atomic mass, we need to take into account the abundance of each isotope. The atomic masses of boron-10 and boron-11 are approximately 10.0129 atomic mass units (u) and 11.0093 u, respectively.
Let's assume that the abundance of boron-10 is x, and therefore the abundance of boron-11 is (1 - x).
The relative atomic mass (M) can be calculated as:
M = (abundance of isotope 1 * atomic mass of isotope 1) + (abundance of isotope 2 * atomic mass of isotope 2) + ...
M = (x * 10.0129 u) + ((1 - x) * 11.0093 u)
We don't have specific information about the abundances, so we can't calculate the exact value. However, the relative atomic mass of boron typically falls within the range of 10.8 to 10.9 u, depending on the isotopic composition of the sample.
Please note that the atomic masses and abundance values used here are approximate and may vary slightly based on the source and measurement techniques.