Easy
Which of the following sets of quantum numbers is correct for an electron in a $3d$-orbital?
- A$n=3, l=2, m=-3, s=+\frac{1}{2}$
- B$n=3, l=3, m=+3, s=-\frac{1}{2}$
- C$n=3, l=2, m=-2, s=+\frac{1}{2}$
- D$n=3, l=2, m=-3, s=-\frac{1}{2}$
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Similar Questions
Identify the correct statements among the following:
$i. E_{2s}(H) > E_{2s}(Li) < E_{2s}(Na) > E_{2s}(K)$
$ii.$ The maximum number of electrons in the shell with principal quantum number $n$ is equal to $2n^2$.
$iii.$ Extra stability of half-filled subshell is due to smaller exchange energy.
$iv.$ Only two electrons,irrespective of their spin,may exist in the same orbital.
$i. E_{2s}(H) > E_{2s}(Li) < E_{2s}(Na) > E_{2s}(K)$
$ii.$ The maximum number of electrons in the shell with principal quantum number $n$ is equal to $2n^2$.
$iii.$ Extra stability of half-filled subshell is due to smaller exchange energy.
$iv.$ Only two electrons,irrespective of their spin,may exist in the same orbital.
DifficultKVPY 2019
View SolutionWhich of the following sets of quantum numbers is not correct?
Medium
View SolutionIdentify the impossible quantum number set for an electron from the following:
In an atom,the total number of electrons having quantum numbers $n=4, |m_{l}|=1$ and $m_{s}=-\frac{1}{2}$ is:
The number of $d-$ electrons in $Fe^{2+} \ (Z = 26)$ is not equal to the number of electrons in which one of the following?
MediumNEET 2015
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