Carbon-12 is commonly used as the reference isotope for determining the relative atomic mass of elements. Here are a few reasons why carbon-12 is chosen as the standard:
Abundance: Carbon-12 is the most abundant isotope of carbon, making up approximately 98.9% of naturally occurring carbon. Its high abundance means that it is readily available and provides a reliable basis for comparison with other elements.
Stability: Carbon-12 is a stable isotope that does not undergo radioactive decay. Its stability ensures that its atomic mass remains constant over time, making it a suitable reference for measuring the atomic masses of other elements.
Mass convenience: Carbon-12 has a mass that is close to the average mass of most other elements. This makes it a convenient reference point for comparison and calculation purposes, as it avoids the use of excessively large or small numbers when expressing atomic masses.
By choosing carbon-12 as the reference isotope, scientists have established a consistent and widely accepted scale for expressing the relative atomic masses of elements. The relative atomic mass of an element is determined by comparing the masses of its isotopes to the mass of carbon-12. This scale allows for easier comparison of atomic masses and provides a standardized system for scientific measurements and calculations.