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(D) In $CH_4$,the central atom is $C$ (Carbon). The ground state electronic configuration of $C$ is $[He] 2s^2 2p^2$. To form $4$ bonds,$C$ undergoes

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$SF_6$

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(D) In $CH_4$,the central atom is $C$ (Carbon). The ground state electronic configuration of $C$ is $[He] 2s^2 2p^2$. To form $4$ bonds,$C$ undergoes excitation to the $2s^1 2p^3$ state,which is the $I^{st}$ excited state. However,$CH_4$ is formed by $sp^3$ hybridization involving this state. In $BF_3$,$B$ (Boron) is in the $I^{st}$ excited state $(2s^1 2p^2)$ to form $3$ bonds. In $ICl_3$,$I$ (Iodine) is in the $I^{st}$ excited state to form $3$ bonds. In $SF_6$,$S$ (Sulfur) is in the $II^{nd}$ excited state to form $6$ bonds. Therefore,$SF_6$ is the molecule that does not form in the $I^{st}$ excited state,as it requires the $II^{nd}$ excited state.

Which of the following molecules does not form in the $I^{st}$ excited state of the central atom?

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