Easy
Which of the following sets of quantum numbers is not possible?
- A$n = 3, l = 2, m = 1, s = +1/2$
- B$n = 3, l = 2, m = 1, s = -1/2$
- C$n = 3, l = 2, m = 1, s = 0$
- D$n = 3, l = 2, m = -1, s = +1/2$
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Easy
View SolutionWhen the value of the principal quantum number $n$ is $3$,what are the permitted values of the azimuthal quantum numbers $l$ and the corresponding magnetic quantum numbers $m$?
Medium
View SolutionGiven,
$(A)$ $n=5, m_l=-1$
$(B)$ $n=3, l=2, m_l=-1, m_s=+\frac{1}{2}$
The maximum number of electron$(s)$ in an atom that can have the quantum numbers as given in $(A)$ and $(B)$ respectively are:
$(A)$ $n=5, m_l=-1$
$(B)$ $n=3, l=2, m_l=-1, m_s=+\frac{1}{2}$
The maximum number of electron$(s)$ in an atom that can have the quantum numbers as given in $(A)$ and $(B)$ respectively are:
DifficultJEE MAIN 2026
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