If AB_{4} molecule is a polar molecule,a poss | vedclass

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(A) molecule is polar if its net dipole moment is non-zero.$(1)$ Square pyramidal geometry: This geometry typically involves $5$ electron pairs ($4$ b

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Square pyramidal

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(A) molecule is polar if its net dipole moment is non-zero.$(1)$ Square pyramidal geometry: This geometry typically involves $5$ electron pairs ($4$ bond pairs and $1$ lone pair). The presence of a lone pair on the central atom $A$ creates an asymmetric charge distribution,resulting in a non-zero net dipole moment. Thus,it is polar.$(2)$ Tetrahedral geometry: This is a highly symmetric structure with no lone pairs on the central atom. The bond dipoles cancel each other out,making the molecule non-polar.$(3)$ Square planar geometry: This is a symmetric structure where the bond dipoles cancel each other out,making the molecule non-polar.$(4)$ Rectangular planar geometry: Similar to square planar,the symmetry in this arrangement leads to the cancellation of bond dipoles,making the molecule non-polar.Therefore,the only polar geometry among the given options is square pyramidal.

If $AB_{4}$ molecule is a polar molecule,a possible geometry of $AB_{4}$ is :

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