Answer:
the atomic mass of magnesium from the Periodic Table is the average sum of it's three most abundant isotopes.
Explanation:
We are told that the atomic mass of magnesium from the Periodic Table is
24.31 amu.
Now, this atomic mass is simply the weighted average of the individual isotopes.
This is because the common isotopes of magnesium are 24Mg, 25Mg, and
26Mg and they are respectively 79%, 10%, and 11% in abundance. The weighted average of these 3 listed isotopes of magnesium add up to 24.3 amu.
Thus, the atomic mass of magnesium from the Periodic Table is the average sum of it's three most abundant isotopes.
Taking into account the definition of isotopes and atomic mass of an element, the atomic mass of magnesium from the Periodic Table is 24.31 amu and represent the weighted average of the individual isotopes.
In first place you must know that isotopes are atoms whose atomic nuclei have the same number of protons but different numbers of neutrons.
So, the relative atomic mass is an average of the atomic masses of the different isotopes in a sample, considering the contribution of each isotope.
This is, the atomic mass of an element is the weighted average mass of its natural isotopes. Therefore, the atomic mass of an element is not a whole number.
In summary, the atomic mass of magnesium from the Periodic Table is 24.31 amu. This mass represent the weighted average of the individual isotopes.
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