Identify the number of molecules in which the | vedclass

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(B) $PbCl_2$: $sp^2$ Hybridisation,bent geometry,one lone pair.$PH_3$: $sp^3$ Hybridisation,pyramidal geometry,one lone pair.$ClF_3$: $sp^3d$ Hybridis

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$4$

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(B) $PbCl_2$: $sp^2$ Hybridisation,bent geometry,one lone pair.$PH_3$: $sp^3$ Hybridisation,pyramidal geometry,one lone pair.$ClF_3$: $sp^3d$ Hybridisation,$T$-shaped geometry,two lone pairs.$SF_4$: $sp^3d$ Hybridisation,see-saw geometry,one lone pair.$BF_3$: $sp^2$ Hybridisation,trigonal planar geometry,zero lone pairs.$SnCl_2$: $sp^2$ Hybridisation,bent geometry,one lone pair.Thus,the molecules with one lone pair on the central atom are $PbCl_2, PH_3, SF_4$,and $SnCl_2$.Total number of such molecules = $4$.

Identify the number of molecules in which the central atom has one lone pair of electrons from the following list:
$PbCl_2, PH_3, ClF_3, SF_4, BF_3, SnCl_2$

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Identify the number of molecules in which the central atom has one lone pair of electrons from the following list:$PbCl_2, PH_3, ClF_3, SF_4, BF_3, SnCl_2$