Identify the pair in which the geometry of th | vedclass

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(D) To determine the geometry,we calculate the number of electron pairs around the central atom using the formula: $Total \ electron \ pairs = \frac{1

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$XeOF_2$ and $XeOF_4$

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(D) To determine the geometry,we calculate the number of electron pairs around the central atom using the formula: $Total \ electron \ pairs = \frac{1}{2} (V + M - C + A)$,where $V$ is the number of valence electrons,$M$ is the number of monovalent atoms,$C$ is the cationic charge,and $A$ is the anionic charge.$1$. For $XeOF_2$: The central atom $Xe$ has $8$ valence electrons. $M = 2$ ($F$ atoms),$O$ is divalent (does not contribute to $M$). Total electron pairs = $\frac{1}{2}(8 + 2) = 5$. This corresponds to $sp^3d$ hybridization with $3$ bond pairs and $2$ lone pairs,resulting in a $T$-shape geometry.$2$. For $XeOF_4$: The central atom $Xe$ has $8$ valence electrons. $M = 4$ ($F$ atoms),$O$ is divalent. Total electron pairs = $\frac{1}{2}(8 + 4) = 6$. This corresponds to $sp^3d^2$ hybridization with $5$ bond pairs and $1$ lone pair,resulting in a square pyramidal geometry.Therefore,the correct pair is $XeOF_2$ and $XeOF_4$.

Identify the pair in which the geometry of the species is $T$-shape and square pyramidal,respectively.

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