To calculate the relative Atomic Mass of an element (which is by its definition an average), you need the mass number and relative abundance of each isotope present.
Suppose we have the following data from the mass spectrometer:
first isotope mn X, abundance A%
second isotope mn Y, abundance B%
third isotope mn Z, abundance C%.
Then ram = (A/100 x X) + (B/100 x Y) + (C/100 x Z)
If there are more than 3 isotopes, just do the same for each one and add all the expressions together.
The masses and relative abundances of all naturally occurring isotopes of the element are required to calculate average atomic mass of the element.
The atomic mass is an average, allowing for the relative abundances of different isotopes.
The mass of the isotope multiplied by its relative abundance plus the the mass times abundance of other isotopes.(mass of isotope)(relative abundance) + (mass of isotope)(relative abundance) = average atomic massExample: Carbon can be naturally found as carbon- 12 or carbon- 13. The mass of carbon- 12 is 12 amu and it makes up 98.93% of naturally found carbon. The mass of carbon- 13 is 13.00335 amu, and it makes up 1.07% of naturally found carbon. So the equation to calculate the average atomic mass of carbon is:(0.9893)(12 amu) + (0.0107)(13.00335 amu) = 12.01 amu
To calculate the median atomic weight, the relative abundance of each isotope could be calculated or given.
63.6166 Relative abundance of Copper-63 is 69.17% and Copper-65 is 30.83%
None. The relative abundance of isotopes is used to calculate the Average Mass (by multiplying the Atomic Mass of the isotopes by their relative abundancies and adding the products together) while the Atomic Mass is simply the number of protons plus the number of neutrons.
The masses and relative abundances of all naturally occurring isotopes of the element are required to calculate average atomic mass of the element.
The atomic mass is an average, allowing for the relative abundances of different isotopes.
It allows for the relative abundances of different isotopes.
It allows for the relative abundances of different isotopes.
The mass of the isotope multiplied by its relative abundance plus the the mass times abundance of other isotopes.(mass of isotope)(relative abundance) + (mass of isotope)(relative abundance) = average atomic massExample: Carbon can be naturally found as carbon- 12 or carbon- 13. The mass of carbon- 12 is 12 amu and it makes up 98.93% of naturally found carbon. The mass of carbon- 13 is 13.00335 amu, and it makes up 1.07% of naturally found carbon. So the equation to calculate the average atomic mass of carbon is:(0.9893)(12 amu) + (0.0107)(13.00335 amu) = 12.01 amu
To calculate the median atomic weight, the relative abundance of each isotope could be calculated or given.
It is called the Relative Atomic Mass.
Atomic weight or atomic mass used in stoichiometric calculations.
63.6166 Relative abundance of Copper-63 is 69.17% and Copper-65 is 30.83%
relative Atomic Mass
relative atomic mass