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There are only two naturally-occuring stable isotopes of lithium, the masses of which are listed in the table below. Use whatever data you need from the ALEKS Periodic Table to calculate the natural abundance of each isotope and complete the table.

Respuesta :

The natural abundance of each isotope of lithium:

For [tex]^{6} Li[/tex] = 7.5%

For  [tex]^{7} Li[/tex] = 92.5%

Due to the fact that lithium only has two stable isotopes, it follows that only two isotopes contribute to its average atomic mass.

Then, if we take x the proportional abundance of [tex]^{6} Li[/tex] it is possible to state that the decimal abundance of [tex]^{7} Li[/tex] need to be equivalent to 1−x.

Lithium's typical atomic mass will now be equal to =

avg. Atomic weight Li = Atomic weight of [tex]^{6} Li[/tex]× quantile abundance of [tex]^{6} Li[/tex]+ Atomic weight of [tex]^{7} Li[/tex]× quantile abundance of [tex]^{7} Li[/tex]

Since you are aware that the average atomic mass of lithium is

6.941 you can construct the equation as follows.

6.941 = 6.015 × x + 7.016 × (1-x)

x = 0.075

This is the decimal abundance of [tex]^{6} Li[/tex]. The decimal abundance of [tex]^{7} Li[/tex] is 1 - 0.075 = 0.925.

Percent abundances :

For [tex]^{6} Li[/tex] = 7.5%

For  [tex]^{7} Li[/tex] = 92.5%

Learn more about isotope of lithium here;

https://brainly.com/question/11919522

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