Question

The shape of \[{\text{SC}}{{\text{l}}_2}\] molecule is:
A.Linear
B.Triangular
C.Angular
D.Pyramidal

Answer 1

Hint: The hybridisation of the molecule is calculated using the help of a number of bond pairs and lone pairs. The lone pair of electrons is not included in the shape of the molecule. The lone pair on the central atom is 2.

Complete step by step answer:
The central atom in \[{\text{SC}}{{\text{l}}_2}\] is sulphur. Sulphur belongs to group number 16, that is, oxygen family. It has 6 electrons in its valence shell. Chlorine is a group number 17 element. It is a monovalent atom, that is, it attaches with a single bond. Hence there will be 2 bond pairs and 2 lone pairs of electrons. One lone pair of electrons consists of 2 electrons. The hybridisation of the element having 2 bond pairs and 2 lone pairs will be \[{\text{s}}{{\text{p}}^3}\] . The geometry and shape with \[{\text{s}}{{\text{p}}^3}\] hybridisation is tetrahedral only when all four bond pairs of electrons are there. In our case there are 2 lone pairs of electrons and hence the geometry will still be tetrahedral but the shape will become angular or we can say bent shape.

Hence, the correct option is C.

Note:
The shape and geometry are often confused. The geometry is the complete structure that includes a bond pair as well as lone pair but the shape of the molecule always contains a bond pair of electrons. A pyramidal shape also falls under the tetrahedral geometry when the bond pair is 3 and lone pair is 1 with the hybridisation \[{\text{s}}{{\text{p}}^3}\] . The linear shape arises from sp hybridisation. The triangular shape arises from \[{\text{s}}{{\text{p}}^2}\] hybridisation. This is the standard shape when no lone pairs are present.