Final answer:
The question is asking about the average mass of atoms of an element relative to isotopic abundance, compared to 1/12th of the mass of a carbon-12 atom. In chemistry, the atomic mass of an element is the weighted average of the masses of all the naturally occurring isotopes of that element.
Step-by-step explanation:
The question is asking about the average mass of atoms of an element relative to isotopic abundance, compared to 1/12th of the mass of a carbon-12 atom. The question is asking about the average mass of atoms of an element relative to isotopic abundance, compared to 1/12th of the mass of a carbon-12 atom. In chemistry, the atomic mass of an element is the weighted average of the masses of all the naturally occurring isotopes of that element.
In chemistry, the atomic mass of an element is the weighted average of the masses of all the naturally occurring isotopes of that element. This average mass is compared to 1/12th of the mass of a carbon-12 atom, which is defined as 12 atomic mass units (amu). So, the question is essentially asking how the average mass of atoms of an element compares to the mass of a carbon-12 atom.