average atomic massof an element=(Atomic mass of first isotope X % of that isotope) + (Atomic mass of second isotope X % of the second isotope)
The atomic particles of an isotope are the proton, electron and neutron
You need to know the atomic # or the masses of each isotope of the element.
Curium has 96 protons. Number of neutrons = Atomic mass of an isotope - atomic number of the isotope The atomic number of curium is 96; for the isotopic masses of curium read at the link below.
Number of neutrons = atomic mass of an isotope - atomic number of the isotope The atomic number of curium is 96; for the isotopic masses read at: http://en.wikipedia.org/wiki/Isotopes_of_curium.
an isotope
Chemists use relative masses of atoms compared to a reference isotope because it allows for easier comparison and calculation of chemical reactions. Absolute masses can vary, but relative masses provide a consistent point of reference for analysis.
average atomic massof an element=(Atomic mass of first isotope X % of that isotope) + (Atomic mass of second isotope X % of the second isotope)
The isotope used as the reference for atomic masses is carbon-12, with a mass of 12 atomic mass units (amu).
its called an isotope c:
The atomic particles of an isotope are the proton, electron and neutron
The unit is such that the isotope Carbon 12 is exactly 12 by definition.
You need to know the atomic # or the masses of each isotope of the element.
If you mean an isotope of 23 Na; They all "look" the same; they simply have different masses.
Curium has 96 protons. Number of neutrons = Atomic mass of an isotope - atomic number of the isotope The atomic number of curium is 96; for the isotopic masses of curium read at the link below.
You must specify the element whose isotopes you want the weighted average mass for. Otherwise there is no answer as just averaging the masses of isotopes without accounting for how much of each isotope is present in a sample of an element is meaningless. Also averaging masses of isotopes of different elements is also meaningless.
The abundance percentage of each isotope