![]() It is the weighted average of all the atoms as per the natural abundance. Since the practicality of measuring the mass of each and every atom is out of the question, we have to resort to the RAM. This is a huge number and there will be billions of atoms for each of the isotopes, according to the natural abundance. As we know, one mole of any element will have 6.02214179 x 10 23 number of atoms. Whenever we take a sample of an element, the ratio of the natural abundance is reflected in the sample. ![]() The isotopes of an element have different masses, due to the presence of the different number of neutrons. The answer lies in the natural abundance of isotopes. So, the obvious question is why do we need it at all? We can clearly see that is is numerically equal to the atomic mass. Since it is a ratio, it is unitless.įor example, let’s consider Magnesium-24. In other words, it is a mass of an atom, relative to the mass of C-12. Out of this need, the concept of Relative Atomic Mass has been born. Through various experiment, the isotope of carbon - C-12 has been found to be the most suitable standard to express the masses of all other elements (including all the isotopes). ![]() The masses of proton, neutron and electron have been determined experimentally. As a result, we need to understand the mass of an atom with respect to a standard. Is relative atomic mass the same as the mass number?Īn atom is too small and measurement of its mass by an instrument is not a practical solution for day-to-day science.Is relative atomic mass same as mass number?. ![]() Relevance of RAM and RMN in Mass spectrometry. ![]()
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