The correct statement regarding perxenate ion | vedclass

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(D) The perxenate ion $(XeO_6^{4-})$ has a central $Xe$ atom surrounded by $6$ oxygen atoms.Its hybridization is $sp^3d^2$,resulting in an octahedral

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Molecular ion has only one type of bond angle

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(D) The perxenate ion $(XeO_6^{4-})$ has a central $Xe$ atom surrounded by $6$ oxygen atoms.Its hybridization is $sp^3d^2$,resulting in an octahedral geometry.In an octahedral geometry,all $Xe-O$ bond lengths are equal,and the bond angles are $90^{\circ}$ and $180^{\circ}$.Since the geometry is perfectly symmetrical (octahedral),the dipole moment is zero,making it a non-polar species.For the $Xe-O$ bond order: The total number of bonds is $12$ (each $Xe-O$ is a single bond,plus $6$ additional pi-bonds distributed via resonance) across $6$ positions,giving a bond order of $12/6 = 2$ is incorrect; rather,considering the resonance of $6$ double bonds across $6$ positions,the bond order is $1.5$ or $2$ depending on the model,but the statement regarding bond angles is the most accurate description of its symmetry.However,in the context of standard chemistry problems,the octahedral structure implies bond angles of $90^{\circ}$ and $180^{\circ}$,and the symmetry makes it non-polar. Option $D$ is the most chemically accurate statement regarding its high symmetry.

The correct statement regarding perxenate ion $(XeO_6^{4-})$ is

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