(a) What is the mass in amu of a carbon-12 atom? (b) Why is the atomic weight of carbon reported as 12.011 in the table of elements and the periodic table in the front inside cover of this text?

A carbon-12 atom is a specific isotope of carbon, made up of 6 protons, 6 neutrons, and 6 electrons. By definition, 1 atomic mass unit (amu) is equal to 1/12th the mass of a carbon-12 atom. Therefore, since the carbon-12 atom has 12 nucleons (protons and neutrons) and amu is defined based on the carbon-12 atom, the mass of a carbon-12 atom is exactly 12 amu.

The atomic weight of an element is the weighted average of the masses of its naturally occurring isotopes, taking into account their relative abundances. Carbon has several natural isotopes, including the aforementioned carbon-12, as well as carbon-13 and traces of carbon-14. The majority is carbon-12 (approximately 98.89%), with carbon-13 making up most of the remaining percentage (around 1.11%), and carbon-14 being extremely rare. The atomic weight of carbon, which is \(\text{12.011}\), is calculated as follows: Atomic weight of Carbon = (relative abundance of carbon-12 × mass of carbon-12) + (relative abundance of carbon-13 × mass of carbon-13) + (relative abundance of carbon-14 × mass of carbon-14) Atomic weight of Carbon ≈ (0.9889 × 12 amu) + (0.0111 × 13 amu) + (trace amount × 14 amu) Atomic weight of Carbon ≈ 12.011 amu Due to the presence of carbon isotopes, carbon's atomic weight is not exactly 12, but 12.011. This weighted average takes into account the different isotopes and their relative abundances and is used to report the atomic weight in the periodic table.