In which molecule are all bonds not equal?

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(D) To determine if all bonds are equal,we look at the molecular geometry and hybridization:$1$. $SiF_4$: It has $sp^3$ hybridization and a tetrahedra

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$SF_4$

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(D) To determine if all bonds are equal,we look at the molecular geometry and hybridization:$1$. $SiF_4$: It has $sp^3$ hybridization and a tetrahedral geometry. All four $Si-F$ bonds are equivalent.$2$. $BF_4^-$: It has $sp^3$ hybridization and a tetrahedral geometry. All four $B-F$ bonds are equivalent.$3$. $XeF_4$: It has $sp^3d^2$ hybridization and a square planar geometry. All four $Xe-F$ bonds are equivalent due to symmetry.$4$. $SF_4$: It has $sp^3d$ hybridization and a see-saw geometry (derived from trigonal bipyramidal). It contains one lone pair on the sulfur atom. Due to the presence of the lone pair,the axial and equatorial $S-F$ bonds have different lengths (axial bonds are longer than equatorial bonds).Therefore,in $SF_4$,all bonds are not equal.

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