Atomic weight is fundamental to chemistry as the most chemical reaction takes place via numerical relationships between atoms.Atomic weights are expressed in terms of atomic mass units (AMU), which are also called daltons.The value of atomic weight might be slightly different than the atomic mass as a substance contains different isotopes that have different atomic or isotopic mass.Besides, atomic weight can also be related to the sum of the total number of protons and neutrons present in an atom.Read Also: Atom vs Molecule- Definition, 12 Major Differences, Examples Atomic Weight DefinitionĪtomic weight, also called relative atomic mass, is the weighted arithmetic mean of the relative isotopic mass of all the isotopes of a particular element depending on the abundance of each of those isotopes. Atomic mass can also be used for the determination of molecular mass, which differs slightly in numerical value from the molar mass.This allows precise measurement of different atoms in contrast to the abundance-weighted average, like in relative atomic weight. Atomic mass represents the mass of an atom which can only be one isotope.The atomic mass of a chemical species is often slightly less than the sum of the masses of protons, neutrons, and electrons due to the loss of some energy due to binding energy mass loss.1 Dalton is defined as the 1/12 th of the mass of a single carbon-12 atom. The SI unit of atomic mass is the kilogram (kg), but it is often expressed in terms of non-SI unit, Dalton.Most of the contribution is made by the nucleus as it contains the heavier subatomic particles, while lesser contributions are made by the electrons and nuclear binding energy.Atomic Weight (Video By MedSchoolCoach)Ītomic mass is the mass of an atom or an isotope which includes the total mass of the nucleus and the electrons present in the periphery. 7 Key Differences (Atomic Mass vs Atomic Weight).Read Also: Atom vs Molecule- Definition, 12 Major Differences, Examples.
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