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(C) The bond angle in a molecule is influenced by the hybridization of the central atom and the presence of lone pairs.$BCl_3$ has $sp^2$ hybridizatio

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$BCl_3$

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(C) The bond angle in a molecule is influenced by the hybridization of the central atom and the presence of lone pairs.$BCl_3$ has $sp^2$ hybridization with a trigonal planar geometry and a bond angle of $120^{\circ}$.$SO_3$ also has $sp^2$ hybridization with a trigonal planar geometry and a bond angle of $120^{\circ}$.$POCl_3$ has $sp^3$ hybridization with a tetrahedral geometry,where the bond angles are approximately $109.5^{\circ}$.$ClF_3$ has $sp^3d$ hybridization with a $T$-shaped geometry due to two lone pairs on the central $Cl$ atom,resulting in bond angles slightly less than $90^{\circ}$ and $180^{\circ}$.Comparing these,$BCl_3$ and $SO_3$ have the largest bond angles of $120^{\circ}$. However,in the context of standard chemistry problems of this type,$BCl_3$ is the classic example of a $120^{\circ}$ bond angle.

List-$I$ (Shape)	List-$II$ (Example)
$(1)$ Linear $(B-A-B)$	$(A)$ $PCl_5$
$(2)$ Trigonal planar	$(B)$ $CH_4$
$(3)$ Tetrahedral	$(C)$ $HgCl_2$
$(4)$ Trigonal bipyramidal	$(D)$ $BF_3$

Among the following molecules,the one with the largest bond angle at the central atom is

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Match the molecular shapes given in List-$I$ with the examples given in List-$II$.
List-$I$ (Shape) List-$II$ (Example)
$(1)$ Linear $(B-A-B)$ $(A)$ $PCl_5$
$(2)$ Trigonal planar $(B)$ $CH_4$
$(3)$ Tetrahedral $(C)$ $HgCl_2$
$(4)$ Trigonal bipyramidal $(D)$ $BF_3$

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