Question

One isotope of tungsten (W) has 110 neutrons (isotope A), and another isotope has 108 neutrons (isotope B). What are their isotopic masses? Based on tungsten's average atomic mass, which isotope would you expect to have a greater natural abundance?

a) Isotope A: 184 amu;Isotope B: 182 amu
b) Isotope A: 110 amu; Isotope B: 108 amu
c) Isotope A: 183.84 amu; Isotope B: 183.86 amu
d) Isotope A: 183.86 amu; Isotope B: 183.84 amu

Answer 1

The isotopic masses of two isotopes of tungsten can be calculated by adding the number of protons and neutrons. Based on tungsten's average atomic mass, the isotope with the mass closest to the average mass would have the greater natural abundance.

Step-by-step explanation:

The isotopic masses of two isotopes of tungsten (W) can be calculated by adding the number of protons and neutrons. Isotope A has 110 neutrons, so the mass would be 110 + atomic number. Isotope B has 108 neutrons, so the mass would be 108 + atomic number. Based on tungsten's average atomic mass, we can determine the isotope with the greater natural abundance. The isotope with the mass closest to the average atomic mass of tungsten would have the greater natural abundance.