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No, it is not.
The Atomic Mass for an isotope of an element is usually close to a whole number but never exactly so. This is because most elements exist in a number of isotopic forms: they are made up of the same number of protons and electrons but differ in the number of neutrons. So the mass of each isotope of the same element will differ from other isotopes by a whole number of mass units. The atomic mass of the element is the average mass of all its isotopes, weighted together in proportion of the abundance of the elements.
The worst offender is dysprosium. The element has 66 proton and electrons 162.5.
164-Dy has a mass of 163.929 and accounts for 28.3% of the Dy on earth,
162-Dy has a mass of 161.927 and accounts for 25.5% of the Dy on earth,
163-Dy has a mass of 162.929 and accounts for 24.9% of the Dy on earth,
and there are 4 more isotopes accounting for smaller proportions. When averaged, the atomic mass for Dy is 162.5 - as far from a whole number as you can get!
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Why at atomic number not whole number in most case?
The question is based on an ignorance of what an atomic number is. It represents the number of protons in an atom of the element and is always, ALWAYS a whole number.
How do you converting from atomic percent to weight percent?
How can I convert atomic percent to weight percent for example TiC -45%atomic C convert to weight percentage?
What does the number 2 and 4003 mean of helium?
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A fraction and a whole number with a whole number product?
The answer can be another fraction and a whole number or it can be a whole number.
A product of a given whole number and another whole number?
A product of a given whole number and another whole number = whole numbers
