Which of the following is not correctly match | vedclass

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(D) In $CH_4$ ($sp^3$ hybridization),there are $6$ bond angles of $109^{\circ} 28^{\prime}$. This is correct.In $SF_6$ ($sp^3d^2$ hybridization),there

Vedclass · Accepted Answer

Bond angle $IF_5 \longrightarrow 90^{\circ},$ Number of bond angles $\longrightarrow 8$

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(D) In $CH_4$ ($sp^3$ hybridization),there are $6$ bond angles of $109^{\circ} 28^{\prime}$. This is correct.In $SF_6$ ($sp^3d^2$ hybridization),there are $12$ bond angles of $90^{\circ}$ (in the equatorial and axial planes). This is correct.In $IF_7$ ($sp^3d^3$ hybridization,pentagonal bipyramidal),there are $10$ bond angles of $90^{\circ}$ (between axial and equatorial bonds). This is correct.In $IF_5$ ($sp^3d^2$ hybridization,square pyramidal),there are $8$ bond angles of $90^{\circ}$ (between the four basal fluorine atoms and the axial fluorine atom). However,the number of $90^{\circ}$ angles is actually $8$ in the square pyramidal structure. Wait,let us re-evaluate: $IF_5$ has $4$ equatorial-axial angles and $4$ other angles,totaling $8$. Actually,option $C$ is often cited as the mismatch in some contexts,but $IF_7$ has $10$ angles of $90^{\circ}$. Let us check $IF_5$ again: it has $4$ angles of $90^{\circ}$ between the basal plane and the apex. The statement in option $D$ is incorrect as the geometry is square pyramidal.

$A$. Trigonal planar	$I$. $PCl_5$
$B$. Tetrahedral	$II$. $SF_6$
$C$. Trigonal bipyramidal	$III$. $BF_3$
$D$. Octahedral	$IV$. $CCl_4$

Which of the following is not correctly matched$:-$

Similar Questions

Observe the following molecules: $PCl_5, BrF_5, ClF_5, PF_5, ClF_3, XeF_4, XeF_2, IF_5$. The number of molecules having square pyramidal geometry from the above is:

Match the molecular geometries in List-$I$ with their corresponding molecules in List-$II$:
$A$. Trigonal planar $I$. $PCl_5$
$B$. Tetrahedral $II$. $SF_6$
$C$. Trigonal bipyramidal $III$. $BF_3$
$D$. Octahedral $IV$. $CCl_4$

The correct match for $A, B, C, D$ is:

In which of the following pairs are the two species not isostructural?

The compound$(s)$ with $2$ lone pairs of electrons on the central atom is(are):
$(A)$ $BrF_5$
$(B)$ $ClF_3$
$(C)$ $XeF_4$
$(D)$ $SF_4$

Which of the following set of species have planar structures?

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