Which of the following molecules does not for | vedclass

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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

Vedclass · Accepted Answer

$SF_6$

Vedclass · Answer

(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.

Order	Property
$(A)$ $NO_2 > O_3 > H_2O$	Bond angle
$(B)$ $H_2O > HF > NH_3$	Dipole moment
$(C)$ $I_2 > F_2 > N_2$	Bond length

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

Similar Questions

Which of the following species is not a pseudo-halide?

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Which of the following formulas does not correctly represent the bonding capacity of the atom involved?

Choose the incorrect statement.

Consider the following pairs:
Order Property
$(A)$ $NO_2 > O_3 > H_2O$ Bond angle
$(B)$ $H_2O > HF > NH_3$ Dipole moment
$(C)$ $I_2 > F_2 > N_2$ Bond length

Which of the above pairs are correctly matched?

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