The compound in which the number of dpi - ppi | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) In the perchlorate ion $(ClO_4^{-})$,the central chlorine atom is $sp^3$ hybridized. It forms four $Cl-O$ bonds,out of which three are double bond

Vedclass · Accepted Answer

$XeO_3$

Vedclass · Answer

(B) In the perchlorate ion $(ClO_4^{-})$,the central chlorine atom is $sp^3$ hybridized. It forms four $Cl-O$ bonds,out of which three are double bonds involving $d\pi - p\pi$ back bonding between the filled $2p$ orbitals of oxygen and empty $3d$ orbitals of chlorine. Thus,$ClO_4^{-}$ contains $3$ $d\pi - p\pi$ bonds.Now,let us analyze the given options:$1$. $XeF_4$: It has no $d\pi - p\pi$ bonds.$2$. $XeO_3$: The xenon atom is $sp^3$ hybridized with one lone pair. It forms three $Xe=O$ double bonds,each involving $d\pi - p\pi$ bonding. Thus,it contains $3$ $d\pi - p\pi$ bonds.$3$. $XeO_4$: The xenon atom is $sp^3$ hybridized. It forms four $Xe=O$ double bonds,each involving $d\pi - p\pi$ bonding. Thus,it contains $4$ $d\pi - p\pi$ bonds.$4$. $XeF_6$: It has no $d\pi - p\pi$ bonds.Therefore,the compound with the same number of $d\pi - p\pi$ bonds as $ClO_4^{-}$ is $XeO_3$.

The compound in which the number of $d\pi - p\pi$ bonds are equal to those present in $ClO_4^{-}$ is:

Similar Questions

Explain the formation of a chemical bond.

What are the successes and failures of the Lewis theory in explaining chemical bonding?

The total number of lone pairs of electrons in the given molecule is

$S-O$ bond length is maximum in

What is the formal charge on the $N$ atom in the $[S-C \equiv N:]^-$ ion?

Vedclass Test Series

Exam Paper Generator

Online Exam Module