Why the average atomic mass makes sense when compared to the percent abundance?

The average Atomic Mass of an element reflects the weighted average of its isotopes based on their relative abundances. Since isotopes of an element have different masses, the average takes into account both the mass of each isotope and its percent abundance in nature. This means that isotopes that are more abundant have a greater influence on the average atomic mass, resulting in a value that accurately represents the composition of the element as found in nature. Thus, the average atomic mass provides a meaningful representation that aligns with the actual distribution of isotopes.