How would you compare the abundance of the two naturally occurring isotopes of boron?

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How would you compare the abundance of the two naturally occurring isotopes of boron?

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Answer 1 · 2017-01-05T15:59:33

By the atomic mass quoted on the Periodic Table.......

Explanation:

The Periodic Table lists the atomic mass of boron as $10.81 \cdot g \cdot m o l^{- 1}$ $10.81*g*mol^-1$ . This site informs me that the percentage occurrence of $^{10} B$ $""^(10)B$ is $19.9 %$ $19.9%$ , and of $^{11} B$ $""^(11)B$ , $80.1 %$ $80.1%$ .

These are the only significant isotopes of boron, and their weighted average is:

$(10 \times 19.9 % + 11 \times 80.1 %) \cdot g \cdot m o l^{- 1}$ $(10xx19.9%+11xx80.1%)*g*mol^-1$ $=$ $=$ $10.81 \cdot g \cdot m o l^{- 1}$ $10.81*g*mol^-1$

And thus, when you look on your copy of the Periodic Table, you find this molar mass quoted.

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How would you compare the abundance of the two naturally occurring isotopes of boron?

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