Indium (In ) has two naturally occurring isotopes: In−113 and In−115 . In−113 has a 4.30 % abundance and a mass of 112.9 amu , and In−115 has a 95.70 % abundance and a mass of 114.9 amu .
Part A
Calculate the atomic mass for indium using the weighted average mass method.
The average atomic mass is the sum of masses of isotopes, each multiplied by their natural abundance.
So for indium ,
Atomic mass = ( 4.30 × 112.9) / 100 + (95.70 × 114.9) / 100
= 114.8 amu
So the atomic mass of indium is 114.8 amu
Indium (In ) has two naturally occurring isotopes: In−113 and In−115 . In−113 has a 4.30...
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