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Mass of one atom compared to 1/12th the mass of a carbon-12 atom
Abundance of each isotope
Weighted average of all isotopes
Ar is average; mass number is for one isotope
∑(mass×abundance)total abundance\frac{\sum(\text{mass} \times \text{abundance})}{\text{total abundance}}total abundance∑(mass×abundance)
Chlorine-35 and Chlorine-37
75%
35.5
It's a weighted average of different isotopes
Periodic table
Moles=MassAr or Mr\text{Moles} = \frac{\text{Mass}}{\text{Ar or Mr}}Moles=Ar or MrMass
Relative formula mass (Mr)
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