In which hybridisation is an angular shape no | vedclass

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(A) For a molecule to have an angular (bent) shape,it must have at least one lone pair on the central atom and be bonded to two other atoms.In $sp$ hy

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$sp$

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(A) For a molecule to have an angular (bent) shape,it must have at least one lone pair on the central atom and be bonded to two other atoms.In $sp$ hybridisation,the geometry is linear with a bond angle of $180^{\circ}$. Even with lone pairs,the arrangement remains linear (e.g.,$XeF_2$ is linear,though it has $sp^3d$ hybridisation,but for simple $sp$ systems like $BeCl_2$,it is linear).In $sp^2$ hybridisation,the geometry is trigonal planar. If one lone pair is present,the shape becomes angular (e.g.,$SO_2$,$SnCl_2$).In $sp^3$ hybridisation,the geometry is tetrahedral. If two lone pairs are present,the shape becomes angular (e.g.,$H_2O$).Therefore,an angular shape is not possible in $sp$ hybridisation because the bond angle is fixed at $180^{\circ}$.

In which hybridisation is an angular shape not possible?

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Match the following:
| List-$I$ (Molecule/ion) | List-$II$ (Hybridisation) |
| :--- | :--- |
| $(A)$ $ICl_4^-$ | $(P)$ $sp^3$ |
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