Chapter 4, Problem 14STP

Interpretation Introduction

Interpretation:

The most abundant isotope amongst ${}^{248}Q,{}^{252}Q,and{}^{259}Q$, if the atomic mass of Q is $258.63$ is to be determined.

Concept introduction:

Isotope is the same number of protons and electrons but has a different number of neutrons in an atom of the same element. The average atomic mass is the sum of the masses of all the isotopes multiplied by their respective percent of natural abundance.

Answer to Problem 14STP

The most abundant isotope is $Q$.

Explanation of Solution

The most abundant isotope is $Q$ as the average atomic mass that is 258.63 is closer to 259. The average atomic mass is calculated by taking average of masses of all the possible isotopes of an element with respect to their natural abundance thus, the average atomic mass will be more closer to the atomic mass of the isotope with more natural abundance.

Conclusion

Hence, $Q$ is the most abundant isotope.