Boron has two isotopes $B^{10}$ and $B^{11}$ whose relative abundances are $20 %$ & $80 %$ respectively. The average atomic weight of Boron is

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Solution

Step1. Formula for average atomic weight
$Averageatomicweight = f_{1} M_{1} + f_{2} M_{2} + \dots + f_{n} M_{n}$
Here $f$ is the fraction representing the natural abundance of the isotope and $M$ is the atomic mass of the isotope.
Step2. Calculation of average atomic weight
$Averageatomicweight = 0.20 \times 10 g + 0.8 \times 11 g = (2 + 8.8) g = 10.8 g$
Hence, the average atomic weight of Boron is $10.8 g$ .

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Boron has two isotopes B10 and B11 whose relative abundances are 20% & 80%respectively. The average atomic weight of Boron is

Boron has two isotopes $B^{10}$ and $B^{11}$ whose relative abundances are $20 %$ & $80 %$ respectively. The average atomic weight of Boron is