in case of some elements which has isotopes the atomic masses are different so the average is taken out which may come in decimals.
No.
Few elements have isotopes. their atomic mass is not a whole number.
Sulfur- Element Number 16 on the Periodic Table of Elements
The atomic number refers to the number of protons in the atom. Since the proton cannot be an in-between number, the atomic number will have to be a whole number. On the other hand, the atomic mass does not have to be a whole number because it is the mass of an atom and is roughly equivalent to the number of protons plus the average number of neutrons in that particular element.
The average atomic mass of an element would be closer to a whole number if there were few to no electrons. This means having little to no electrons in the element's isotopes.
It is its Atomic Mass and why atomic mass is frequently not a whole number.
The mass number of an element is the atomic mass rounded to the nearest whole number. For Example, if the atomic mass is 54.94 (Manganese [Mn]), then the mass number will be 55. You can use the mass number to calculate the amount of neutrons in an isotope.
Atomic mass is the mass of 1 mole of the element. Atomic number is the number of protons the element has
Mass number is the average of all the naturally occurring isotopes of that element. When calculated, this average is not a whole number.
Sodium is a metal element. Atomic mass number of it is 23.
Take the Atomic Mass and round it to the nearest whole number. Then subtract this number and the atomic number of that element.
Number of protons = atomic number Number of neutrons = Atomic Mass (rounded to the nearest whole number) minus the atomic number Number of electrons in a stable element = number of protons Number of electrons in an unstable element = atomic number minus the charge