Which one of the following molecules will hav | vedclass

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(A) To determine which molecule has all equal $X-F$ bond lengths,we analyze the geometry and hybridization of each:$1$. $SOCl_2F_2$: The molecule has

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$SOCl_2F_2$

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(A) To determine which molecule has all equal $X-F$ bond lengths,we analyze the geometry and hybridization of each:$1$. $SOCl_2F_2$: The molecule has a trigonal bipyramidal geometry with $S$ as the central atom. The $S=O$ bond and the two $Cl$ atoms occupy positions such that the two $S-F$ bonds are equivalent due to symmetry,resulting in equal $S-F$ bond lengths.$2$. $SeF_4$: This molecule has a see-saw geometry ($sp^3d$ hybridization) with one lone pair. The axial and equatorial $Se-F$ bonds have different lengths.$3$. $PBr_2F_3$: This molecule has a trigonal bipyramidal geometry. The $F$ atoms occupy both axial and equatorial positions,which have different bond lengths.$4$. $IF_7$: This molecule has a pentagonal bipyramidal geometry. The axial and equatorial $I-F$ bonds have different lengths.Therefore,$SOCl_2F_2$ is the correct molecule where all $S-F$ bonds are equal.

Which one of the following molecules will have all equal $X-F$ bond lengths? (where $X =$ central atom)

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