In this worksheet, we will practice calculating the relative atomic masses of elements based on the relative abundance of their isotopes.
A sample of lithium contains a mixture of and isotopes, with atomic masses of 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 6.06 u
- B 6.04 u
- C 6.52 u
- D 6.97 u
- E 6.96 u
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?