Final answer:
Magnesium has three naturally occurring isotopes: magnesium-24, magnesium-25, and magnesium-26, all of which are stable and have distinct atomic masses. These isotopes have the same chemical behavior, as isotopes of the same element have the same number of protons. The average atomic mass of magnesium is calculated based on the abundance and mass of each isotope.
Step-by-step explanation:
The question is about the three naturally occurring isotopes of magnesium. These isotopes are all stable and have the same number of protons but different numbers of neutrons, resulting in different masses. The isotopes of magnesium consist of magnesium-24 with 12 protons and 12 neutrons, magnesium-25 with 12 protons and 13 neutrons, and magnesium-26 with 12 protons and 14 neutrons. They are all stable because they do not undergo radioactive decay. In terms of mass, they have similar masses but are distinguishable enough to be considered separate isotopes. These isotopes, like all isotopes, have identical chemical properties because they have the same number of protons and thus behave the same way in chemical reactions. To calculate the average atomic mass of magnesium, one must take into account the relative abundance and the atomic mass of each isotope. This is a reflection of both the physical and chemical characteristics of isotopes.