Question

Most elements occur naturally as a mix of different isotopes. An element's atomic mass is the weighted average of the isotope masses. In other words, it is an average that takes into account the percentage of each isotope. For example, the two naturally occurring isotopes of boron are given here The atomic mass of boron is calculated as follows: (10.0 times 0.199) + (11.0 times 0.801) = 10.8 amu Because the heavier isotope is more abundant the atomic mass a closer to 11 amu than it a to 10 amu. What is the atomic mass of a hypothetical element that consist of the following isotopes in the indicated natural abundances? Express your answer to three significant figures and include the appropriate units. You did not open hints for this part. What a the atomic mass of the element that consists of the following isotopes in the indicated natural abundances? Express your answer to three significant figures and include the appropriate units.

Answer 1