This is really a math question. Remember that the atomic masses of elements is a weighted average of each of the isotopes.
So you have one isotope with a mass of 14.00 and another with a mass of 15.00. If the average of the two is 14.01 it should be logical that there is much more of the 14.00 than the 15.00. Think about it. If they were 50% each then the mass of the element would be 14.50 so it's much much less than 50%.
The average atomic mass of nitrogen is 14.01 u.
Nitrogen exists naturally as nitrogen-14 (mass =
14.00 u) and nitrogen-15 (mass = 15.00 u). What can
you infer about the isotopic abundances for nitrogen?
PLEASE EXPLAIN THE ANSWER
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would be 14.50 so it's much much less than 50%.
Meaning that it is about 99% of the 14.00 and about 1% of the 15.00. On the web I found these numbers. 99.636% for the 14.00 and 0.00364% for the 15.00.
Meaning that it is about 99% of the 14.00 and about 1% of the 15.00. On the web I found these numbers. 99.636% for the 14.00 and 0.00364% for the 15.00.
i have the same question the teacher said she will put it on the teset but diffrent element can some expalin more
1 answer