The known weighted-average
mass of all the naturally occurring* isotopes for an element is the atomic mass of the element.
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*This is not the same as "all the known isotopes", becausemost elements have known isotopes that are not naturally occurring.
The known weighted-averagemass of all the naturally occurring* isotopes for an element is the atomic mass of the element.____________________*This is not the same as "all the known isotopes", becausemost elements have known isotopes that are not naturally occurring.
The weighted-average mass of all the known isotopes for an element is called the atomic weight or atomic mass. It is calculated by taking into account the abundance of each isotope and its mass to determine the average mass of all isotopes present in nature for that element.
The known weighted-averagemass of all the naturally occurring* isotopes for an element is the atomic mass of the element.____________________*This is not the same as "all the known isotopes", becausemost elements have known isotopes that are not naturally occurring.
the average mass numbers of the isotopes of an element
average atomis mass
The answer is the atomic weight of the original element: It's the number on the top left of each element square of the Periodic Table.
the atomic mass
All of the isotopes in an element's atomic masses divided by the amount of isotopes there are is the weighted-average mass of the mixture of an elements isotopes.
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
The characteristic of an element that represents the average mass of its isotopes is called the atomic mass. Atomic mass takes into account the abundance of each isotope of the element and is typically listed on the periodic table as a weighted average.
The weighted average mass of all the known isotopes of an element is calculated by taking the mass of each isotope, multiplying it by its natural abundance, and then summing up these values for all isotopes. This calculation takes into account the relative abundance of each isotope in nature to give a more accurate representation of the average mass of the element.