What is the number of unpaired electrons pres | vedclass

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(B) $1$. The atomic number of Silicon $(Si)$ is $14$. Its electronic configuration is $1s^2 2s^2 2p^6 3s^2 3p^2$. In the $3p$ subshell, there are $2$

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$2$ and $6$

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(B) $1$. The atomic number of Silicon $(Si)$ is $14$. Its electronic configuration is $1s^2 2s^2 2p^6 3s^2 3p^2$. In the $3p$ subshell, there are $2$ unpaired electrons.$2$. The atomic number of Chromium $(Cr)$ is $24$. Its electronic configuration is $1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5$. In the $4s$ subshell, there is $1$ unpaired electron, and in the $3d$ subshell, there are $5$ unpaired electrons. Total unpaired electrons = $1 + 5 = 6$.$3$. Thus, the number of unpaired electrons in $Si$ and $Cr$ are $2$ and $6$ respectively.

What is the number of unpaired electrons present in the ground state of Silicon $(Si)$ and Chromium $(Cr)$, respectively?

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