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(B) The given electronic configuration is $1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1$. This configuration corresponds to the element Chromium $(Cr)$,which ha

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Ground state

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(B) The given electronic configuration is $1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1$. This configuration corresponds to the element Chromium $(Cr)$,which has an atomic number of $24$. According to the Aufbau principle,the expected configuration is $3d^4 4s^2$,but due to the extra stability of half-filled $d$-orbitals,one electron from the $4s$ orbital shifts to the $3d$ orbital. Therefore,$3d^5 4s^1$ is the stable ground state configuration of $Cr$.

The electronic configuration of an element is $1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1$. This represents its

Similar Questions

Which of the following sets of quantum numbers represents the orbital with the highest energy?

The $20^{th}$ electron of $Fe$ $(Z = 26)$ has which of the following sets of quantum numbers?

The number of unpaired electrons in $1s^2 2s^2 2p^3$ is:

For principal quantum number $n = 4$,the total number of orbitals having $l = 3$ is:

The correct order of decreasing energy for the electrons whose quantum numbers $n$ and $l$ are given below, is
$A$. $n=5, l=2$
$B$. $n=5, l=0$
$C$. $n=4, l=3$
$D$. $n=4, l=1$

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