The number of peroxide bonds in the perxenate | vedclass

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(A) In the perxenate ion $[XeO_6]^{4-}$,the oxidation state of Xenon $(Xe)$ is calculated as follows: $x + 6(-2) = -4$,which gives $x = +8$. Since the

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(A) In the perxenate ion $[XeO_6]^{4-}$,the oxidation state of Xenon $(Xe)$ is calculated as follows: $x + 6(-2) = -4$,which gives $x = +8$. Since the maximum oxidation state of Xenon is $+8$,all oxygen atoms are bonded to Xenon via single bonds. The structure of $[XeO_6]^{4-}$ is an octahedral geometry where Xenon is at the center and six oxygen atoms are attached to it. There are no oxygen-oxygen $(O-O)$ bonds present in this structure. Therefore,the number of peroxide bonds is $0$.

The number of peroxide bonds in the perxenate ion $[XeO_6]^{4-}$ is ........

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