Question

The nature of hybridisation in \[{\rm{C}}{{\rm{H}}_{\rm{2}}}{\rm{Cl}} - {\rm{C}}{{\rm{H}}_{\rm{2}}}{\rm{Cl}}\] for carbon is
A) \[sp\]
B) \[s{p^2}\]
C) \[s{p^3}\]
D) \[s{p^2}d\]

Answer 1

Hint: The hybridisation of an atom can be found by counting the number of groups surrounding the atoms. The surrounding groups are atoms that form covalent bonds with the atom and the lone pairs of the atom.

Complete Step by Step Answer:
Here, we will count the number of surrounding groups around the two carbon atoms. The given molecule is,
\[\mathop {\rm{C}}\limits_1 {{\rm{H}}_{\rm{2}}}{\rm{Cl}} - \mathop {\rm{C}}\limits_2 {{\rm{H}}_{\rm{2}}}{\rm{Cl}}\]

From the above molecule, we see that four groups surround the C1 atom, they are, two H atoms, one Chlorine atom, and one carbon atom. So, the hybridisation of the C1 atom is \[s{p^3}\].

Similarly, C2 is also surrounded by four atoms, namely, two hydrogen atoms, one chlorine atom, and one carbon atom. So, C2 has hybridisation of \[s{p^3}\]. Therefore, the carbon atoms of the given compound are \[s{p^3}\] hybridised.
Therefore, option C is right.

Additional Information: Hybridisation also helps to give an idea of the shapes of the molecules. The \[s{p^3}\] hybridisation means the shape is tetrahedral if no lone pair is present. The \[s{p^2}\] hybridisation means the molecular shape is trigonal planar. And the sp hybridisation means the shape is linear.

Note: According to the VSEPR theory, if the count of surrounding groups is three and no lone pair is present, then the molecular shape is tetrahedral. If one lone pair and three bond pair are present, then the molecular shape is trigonal bipyramidal and if two bond pair and two lone pair is present, the molecular shape is bent.