Select the hybridisation which has non-planar | vedclass

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(D) For $sp^3$ hybridisation: When all are bond pairs,the geometry is tetrahedral (non-planar). When there are $2$ lone pairs,the shape is bent (plana

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All of the above

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(D) For $sp^3$ hybridisation: When all are bond pairs,the geometry is tetrahedral (non-planar). When there are $2$ lone pairs,the shape is bent (planar).For $sp^3d$ hybridisation: When all are bond pairs,the geometry is trigonal bipyramidal (non-planar). When there are $2$ lone pairs,the shape is $T$-shaped (planar).For $sp^3d^2$ hybridisation: When all are bond pairs,the geometry is octahedral (non-planar). When there are $2$ lone pairs,the shape is square planar (planar).Since all given hybridisations satisfy the condition,the correct answer is $D$.

Select the hybridisation which has non-planar geometry when all are bond pairs,but planar when there are $2$ lone pairs on the central atom:

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