Average Atomic Mass If there are 2 naturally occurring isotopes of Neon including Ne-20 and Ne-22. then the average mass of Neon atoms should be ___ amu. Why does the PT lists it as 20.18 amu? Calculated as a weighted average of atoms in a sample of naturally occurring isotopes.
63Cu is 69% abundant 65Cu is 31% abundant Average Atomic Mass A weighted average atomic mass is calculated from both the masses of each isotope and the relative abundance (%) of each isotope. 63Cu is 69% abundant 65Cu is 31% abundant To which will the average mass be closer, 63 or 65?
= 63.55 Calculating Average Atomic Mass copper-63 has a mass of 62.93 amu and natural abundance of 69.15% copper-65 has a mass of 64.93 amu and has a natural abundance of 30.85% Calculating Average Atomic Mass Avg. Mass = (Mass1)(%) + (Mass2)(%) … = (62.93)(0.6915) + (64.93)(0.3085) = 63.55
neon-20 neon-22 Which isotope is in greater relative abundance in natural samples of neon? because… the weighted average atomic mass of neon from the PT is 20.18 amu. 90% - 20, <1% - 21, 9% - 22
= 32.2 Avg. = (M1)(%) + (M2)(%) = (32)(0.900) + (34)(0.100) Quick Quiz! 1. If an unusually selected sample of sulfur contained 90.0% sulfur-32 and 10.0% sulfur-34, what would be its average atomic mass? 32.2 amu 32.9 amu 33.5 amu 34.2 amu Avg. = (M1)(%) + (M2)(%) = (32)(0.900) + (34)(0.100) = 32.2