A) \[n=4,\,\,l=0,\,\,m=0,\,\,s=+\frac{1}{2}\]
B) \[n=3,\,\,l=2,\,\,m=1,\,\,s=+\frac{1}{2}\]
C) \[n=3,\,\,l=1,\,\,m=1,\,\,s=+\frac{1}{2}\]
D) \[n=3,\,\,l=0,\,\,m=0,\,\,s=+\frac{1}{2}\]
Correct Answer: B
Solution :
Higher the value of \[(n+l)\], higher will be the energy. \[(n+l)=4+0=4\] \[(n+l)=3+2=5\] \[(n+l)=3+1=4\] \[(n+l)=3+0=3\] \[\therefore \] \[n=3,\,\,l=2,\,\,m=1,\,\,s=+1/2\] set of quantum numbers has the highest energy. If two electrons have the same value of \[(n+l)\], the electron with higher value of n, has the higher energy.
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