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 Mass
Example: 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
Atomic mass is the sum of neutrons and protons in an atom's nucleus. == == Atomic mass is the mass of an element in addition to all of its isotopes found in nature.
Average atomic mass = (fraction1 x atomic mass1) + (fraction2 x atomic mass2) + (fraction3 x atomic mass3) ...
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 listed on most periodic tables is actually the average atomic mass representing the average atomic masses of the various isotopes of an element depending on their percent natural abundance. Refer to the answers.com question: What is the formula for finding average atomic mass? for a detailed explanation on how to calculate this value. (What_is_the_formula_for_finding_average_atomic_mass)
To calculate the atomic mass of any element, add the no. of protons and neutrons. There sum will be the atomic mass. The mass of electrons is not counted towards the atomic mass.
"Atomic Mass" is not an average, it is tje total mass of all the electrons, protons and neutrons in an atom of an element. AVERAGE Atomic Mass is the AVERAGE of the Atomic Masses of all of the Isotopes of an element according to their natural proportions.
Average weight of an element expressed in Atomic Mass units.
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 number of each isotope-apex;)
The atomic mass listed on most periodic tables is actually the average atomic mass representing the average atomic masses of the various isotopes of an element depending on their percent natural abundance. Refer to the answers.com question: What is the formula for finding average atomic mass? for a detailed explanation on how to calculate this value. (What_is_the_formula_for_finding_average_atomic_mass)
the Atomic Mass
weighted average of the various iisotopes
To calculate the atomic mass of any element, add the no. of protons and neutrons. There sum will be the atomic mass. The mass of electrons is not counted towards the atomic mass.
"Atomic Mass" is not an average, it is tje total mass of all the electrons, protons and neutrons in an atom of an element. AVERAGE Atomic Mass is the AVERAGE of the Atomic Masses of all of the Isotopes of an element according to their natural proportions.
Average weight of an element expressed in Atomic Mass units.
The average atomic mass of an element is the average of the atomic masses of its isotopes (that is a weighted average). You have to take into account the abundance of each isotope when they do your averaging.
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 mass unit (amu) is a unit of mass used to express the average mass of an atom or molecule. To calculate the atomic mass unit of gold (Au), you would look at the atomic mass of gold on the periodic table, which is approximately 197 amu.