Mass number is the average of all the naturally occurring isotopes of that element. When calculated, this average is not a whole number.
The atomic mass is an average, allowing for the relative abundances of different isotopes.
It's an average number allowing for the relative abundances of different isotopes.
In the Handbook of Chemistry and Physics (and in many other references), there is a "Table of Isotopes" that lists all known isotopes, first by atomic number and then by increasing mass number.
It's an average number allowing for the relative abundances of different isotopes.
It's an average number allowing for the relative abundances of different isotopes.
It's an average number allowing for the relative abundances of different isotopes.
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.
Isotopes of the same element have the same number of protons (atomic number) but differ in number of neutrons (hence atomic masses).
Isotopes. They differ in the number of neutrons in the nucleus.
The Atomic Mass number of an element is the sum of the protons and neutrons in the nucleus of an atom of that element.The relative atomic mass is the average atomic mass number of all the known isotopes of an element.
The atomic mass is the mass of an atom of that element in AMUs. (Atomic Mass Units)The atomic number, however, is equivalent to the number of protons in an atom of that element.The mass number of an atom is the total number of protons and neutrons in the nucleus of an atom. This is therefore always a whole number. The relative atomic mass of an element is the weighted average of the masses of the isotopes relative to 1/12 of the mass of a carbon-12 atom.It is a weighted average as it takes into account the relative abundances of the different isotopes (atoms of the same element but with different numbers of neutrons) of an element. This number is found in the periodic table.For example chlorine has two isotopes, 35Cl and 37Cl, in the approximate ratio of 3 atoms of 35Cl to 1 atom of 37Cl.The number of protons and neutrons in a 35Cl atom must add up to 35, the mass number. The relative atomic mass of chlorine takes into account both isotopes and is therefore 35.5.
To calculate average atomic mass from different isotopes of an element, we take into account the relative atomic masses of isotopes and their relative abundance on Earth. The following formula is used to calculate the needful : atomic mass = mass of isotope x percent abundance + mass of isotope x percent abundance / 100 (whole expression divided by 100)