A sample of lithium contains a mixture of and isotopes with atomic masses 6.01512 u and 7.01600 u respectively. The sample is by mass.
Calculate, to 3 significant figures, the average atomic mass of the sample.
A second sample of lithium also contains a mixture of and but displays a higher abundance of . How does the average atomic mass of this sample compare with that of the first?
Protons and neutrons have masses of approximately 1 atomic mass unit (u) and cannot easily be split into smaller particles. Magnesium consists of protons, neutrons, and electrons and has a relative atomic mass of 24.3 u. Why is the relative atomic mass of magnesium significantly greater than 24 u?