Vincent combines sodium and chlorine in two different beakers (beaker X and beaker Y). In both beakers, the chemical reaction sh
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The given question is incomplete. The complete question is:What is the relative atomic mass of a hypothetical element that consists isotopes in the indicated natural abundances.
Isotope mass amu Relative abundance
1 77.9 14.4
2 81.9 14.3
3 85.9 71.3
Express your answer to three significant figures and include the appropriate units.
Answer: 84.2 amu
Explanation:
Mass of isotope 1 = 77.9
% abundance of isotope 1 = 14.4% =
Mass of isotope 2 = 81.9
% abundance of isotope 2 = 14.3% =
Mass of isotope 3 = 85.9
% abundance of isotope 2 = 71.3% =
Formula used for average atomic mass of an element :
Therefore, the average atomic mass of a hypothetical element that consists isotopes in the indicated natural abundances is 84.2 amu
They are two representatives of the sublevels/energy levels.
