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Mass Concepts, Atomic Mass, Gram Atomic Mass, Molecular Mass, Unit
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(i) Atomic Mass: The atomic mass of an element is a number which indicates how many times an atom of natural isotopic composition of an element is heavier as compared with 1/12 of mass of a atom of carbon-12.
(ii) Gram atomic mass: The atomic mass of an element expressed in grams is called Gram atomic mass e.g., Atomic mass of oxygen = 16 a.m.u.
Gram atomic mass of oxygen = 16 g
Note: (1 a.m.u. = 1.6 x 10
(iii) Molecular mass: The molecular mass of a substance (element or compound) is the number of times, the molecule of substance is heavier than 1/12th of the mass of an atom of corbon-12 isotope.
(iv) Gram molecular mass: The molecular mass of a substance expressed in grams is called its Gram molecular mass.
1 gram molecule of H
= 98.0 g
(v) Atomic Mass Unit: The quantity 1/12th mass of and atom of carbon.12 is known as atomic mass unit.
A mole is defined as number of atoms in 12g of carbo-12, which is experimentally found to be 6.023 x 10
Illustration 1: In naturally occurring neon, isotopes and their relative abundance are as follows:
Isotope Fractional Abundance
Average atomic mass of Ne is
(A) 20. 179
(C) 22. 179
Solution: (A) Average atomic mass of Ne = 20 x 0.9051 + 21 x 0.0027 + 22 x 0.0922 = 20.179
Aliter: From the fraction abundance of various isotopes, clearly shows that the average atomic mass should be near to 20 (
Ne). Hence, (A) is correct
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