Question

Which of the following sets of quantum numbers represents the highest energy for an atom?

• A. $n=4,l=0,m=0,s=+\frac{1}{2}$
• B. $n=3,l=0,m=0,s=+\frac{1}{2}$
• C. $n=3,l=1,m=1,s=+\frac{1}{2}$
• D. $n=3,l=2,m=1,s=+\frac{1}{2}$

Answer 1

The correct option is D $n=3,l=2,m=1,s=+\frac{1}{2}$

Energy is given by $(n+l)$ value where $n$ is principal quantum number and $l$ is azimuthal quantum number.

For(a) $n=4,l=0(n+l)=(4+0)=4$

(b) $n=3,l=0(n+l)=(3+0)=3$

(c) $n=3,l=1(n+l)=3+1=4$

(d) $n=3,l=2(n+l)=3+2=5$

Hence, (d) set of quantum number represents the highest energy of an atom.