An element has two naturally occurring isotopes. Isotope A has a mass of 10.01 amu and an abundance of 20%. Isotope B has a mass of 11.01 amu and an abundance of 80%. What is the average atomic mass of the element?
- 10.21 amu
- 10.51 amu
- 10.81 amu
- 11.01 amu
📝 Detailed explanation
Average atomic mass = (Mass A × %A) + (Mass B × %B).Calculation: (10.01 × 0.20) + (11.01 × 0.80) = 2.002 + 8.808 = 10.81 amu.