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 known weighted-average
mass 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.
Atomic Mass The technical answer would be average atomic mass Is the "atomic mass found on the Periodic Table.
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 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.
What. (your question isn't even a complete sentence.)
This is the atomic weight.
Each isotope of an element has a different Atomic Mass, so an average is taken of all the isotopes, but the average is weighted because the natural abundance (%) of each isotope is factored in. If hydrogen-1 is much more abundant than deuterium and tritium, then the weighted average will be closer to 1 than 2 or 3 but not a whole number. The following equation shows how percent abundance factors into the weighted average. (atomic mass A)(X% abundance) + (atomic mass B)(Y% abundance)...=(weighted average of all isotopes of the element)(100% abundance)
The weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)
There is not an isotope number on the Periodic Table of Elements. There is an atomic number (# of protons) and the average atomic mass. The average atomic mass is the weighted average of all the naturally occurring isotopes for each element. This number is not a whole number, because it is an average of all the isotopes for a particular element.
The atomic weight of the element (syn.: mass number).
If the masses of the individual isotopes are on the scale where one atom of the isotope carbon-12 has a mass of 12 units, then the weighted average of the masses of all isotopes present in a natural sample of an element is called its relative atomic mass, r.a.m.
The weighted average for all isotopes that occur in nature for an element is its atomic weight listed on the Periodic Table of the elements.
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 weighted average for all isotopes that occur in nature for an element is its atomic weight listed on the Periodic Table of the elements.
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 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 mean Atomic Mass.
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 atomic mass of an element is the weighted average of the masses of all the stable isotopes of the element (if it has any), weighted by the natural occurrence levels of the isotopes in the elements as found on earth or in the atmosphere.
The atomic weight of the element (syn.: mass number).
It is its Atomic Mass and why atomic mass is frequently not a whole number.
Each isotope of an element has a different Atomic Mass, so an average is taken of all the isotopes, but the average is weighted because the natural abundance (%) of each isotope is factored in. If hydrogen-1 is much more abundant than deuterium and tritium, then the weighted average will be closer to 1 than 2 or 3 but not a whole number. The following equation shows how percent abundance factors into the weighted average. (atomic mass A)(X% abundance) + (atomic mass B)(Y% abundance)...=(weighted average of all isotopes of the element)(100% abundance)
The weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)