the isotope 32 is the most abundant because its the closest to 32.06 numerically
The isotope with a mass of 32 amu is the most abundant. This can be determined by comparing the Atomic Mass of sulfur (32.06 amu) to the masses of the isotopes. Since the atomic mass is closest to 32 amu, this isotope is the most abundant.
Because the naturally occurring isotopes of tellurium have fewer neutrons than the naturally occurring isotopes of iodine.
Atomic weight or gram-atomic mass.
Atomic masses are a weighted average of the naturally occurring isotopes.
Atomic mass is the number of protons and neutrons in an atom.
For the chemical elements the correct expression is atomic weight.This value is the weighted average mass of the natural isotopes of this 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 of all the naturally occurring isotopes of a particular element are an element's 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 weight that is listed on the periodic table for each element is the weighted average of the atomic masses of an element's naturally occurring isotopes. So you are describing atomic weight as it is used on the periodic table.
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.
Isotopes and their prevalence are not shown on the periodic table. Instead, the atomic weight shown for each element is an average of the atomic weights of all naturally-occurring isotopes (calculated from percentages occurring on Earth).
Because the naturally occurring isotopes of tellurium have fewer neutrons than the naturally occurring isotopes of iodine.
The mean Atomic Mass.
The result is the atomic weight.
By taking the wieghted averages of naturally occurring isotopes of that element. :)
... atomic mass or atomic weight.
Atomic weight or gram-atomic mass.