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.

List-$I$	List-$II$
$A. ICl$	$i. \text{Linear}$

$B. ICl_3$	$ii. \text{T-Shape}$
$C. ClF_5$	$iii. \text{Square pyramidal}$
$D. IF_7$	$iv. \text{Pentagonal bipyramidal}$

Similar Questions

The numbers of lone pair$(s)$ on $Xe$ in $XeF_2$ and $XeF_4$ are,respectively:

Match List-$I$ with List-$II$.
List-$I$ List-$II$
$A. ICl$ $i. \text{Linear}$
$B. ICl_3$ $ii. \text{T-Shape}$
$C. ClF_5$ $iii. \text{Square pyramidal}$
$D. IF_7$ $iv. \text{Pentagonal bipyramidal}$

Choose the correct answer from the options given below:

The geometry of $H_2S$ and its dipole moment are

In which of the following is the bond angle maximum?

The number of lone pairs of electrons present on $Xe$ in $XeF_4$ is

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