Question

Which molecule has V-shape? This question has multiple correct options
(A) \[{{\text{H}}_{\text{2}}}{\text{O}}\]
(B) \[{\text{SnC}}{{\text{l}}_{\text{2}}}\]
(C) \[{\text{PbC}}{{\text{1}}_{\text{2}}}\]
(D) None of these

Answer 1

Hint: In each molecule, determine the hybridization of the central atom. From the hybridization, determine the electron pair geometry and the molecular geometry.

Complete step-by-step answer:
\[{\text{PbC}}{{\text{1}}_{\text{2}}}\] molecule has linear geometry. In water molecules, the central oxygen atom has 2 bond pairs and 2 lone pairs of electrons. Oxygen atom is \[{\text{s}}{{\text{p}}^3}\] hybridized with tetrahedral electron pair geometry and V shaped molecular geometry. The ideal tetrahedral bond angle is \[{\text{10}}{{\text{9}}^o}{\text{28'}}\] , but in water molecule, the \[{\text{H}} - {\text{O}} - {\text{H}}\] bond angle is \[{\text{104}}{\text{.}}{{\text{5}}^o}\] . This is due to greater lone pair lone pair repulsion and lone pair bond pair repulsion as compared to bond pair bond pair repulsion.

 In \[{\text{SnC}}{{\text{l}}_{\text{2}}}\] molecule, the central tin atom has 2 bond pairs and 1 lone pair of electrons. Tin atom is \[{\text{s}}{{\text{p}}^2}\] hybridized with Trigonal planar electron pair geometry and V shaped molecular geometry. The ideal bond angle is \[{\text{12}}{{\text{0}}^o}\] , but in \[{\text{SnC}}{{\text{l}}_{\text{2}}}\] molecule, the \[{\text{Cl}} - {\text{Sn}} - {\text{Cl}}\] bond angle is less \[{\text{12}}{{\text{0}}^o}\] . This is due to greater lone pair bond pair repulsion as compared to bond pair bond pair repulsion. The molecules \[{{\text{H}}_{\text{2}}}{\text{O}}\]and \[{\text{SnC}}{{\text{l}}_{\text{2}}}\] have V-shaped geometries.

Hence, the options (A) and (B) are the correct answers.

Note: For several molecules, the electron pair geometry is different from the molecular geometry. This is due to the presence of lone pairs of electrons on the central atom.