Which of the following molecules has the weak | vedclass

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(A) Back bonding $(p \pi - d \pi)$ occurs when a lone pair from a $2p$ orbital of a central atom is donated into an empty $d$ orbital of the surroundi

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$OCl_2$

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(A) Back bonding $(p \pi - d \pi)$ occurs when a lone pair from a $2p$ orbital of a central atom is donated into an empty $d$ orbital of the surrounding atom.In $OCl_2$,the oxygen atom has lone pairs,but the chlorine atom has $3d$ orbitals. However,the energy gap between $O(2p)$ and $Cl(3d)$ is significant,and the electronegativity difference is small,making the back bonding very weak compared to $Si$ compounds.In $N(SiH_3)_3$,$O(SiH_3)_2$,and $SiF_4$,the back bonding is more effective due to the better energy match between the donor $p$-orbital and the acceptor $d$-orbital of silicon.Therefore,$OCl_2$ exhibits the weakest $(p \pi - d \pi)$ back bonding among the given options.

List-$I$	List-$II$
$A. PCl_5$	$I. \text{Tetrahedral}$
$B. BrF_5$	$II. \text{Square Planar}$
$C. BF_4^-$	$III. \text{Trigonal bipyramidal}$
$D. [Ni(CN)_4]^{2-}$	$IV. \text{Square pyramidal}$

Which of the following molecules has the weakest $(p \pi - d \pi)$ back bonding?

Similar Questions

In which of the following pairs of species is the bond length as well as the bond energy of the $I^{st}$ species less than the $II^{nd}$ species?

The formal charges of $N_{(1)}$,$N_{(2)}$ and $O$ atoms in the structure shown below are respectively:
$:N_{(1)}=N_{(2)}=\ddot{O}:$

In solid state,$PCl_5$ is a/an

Which of the following are isoelectronic species?
$I. CH_{3}^{+}$,$II. H_{3}O^{+}$,$III. NH_{3}$,$IV. CH_{3}^{-}$

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