Question

$C - C$ bond in ${{\text{C}}_{\text{2}}}{{\text{H}}_{\text{6}}}$ undergoes heterolytic fission, the hybridization of two resulting carbon atoms is/are
A.${\text{s}}{{\text{p}}^{\text{2}}}{\text{ both}}$
B.${\text{s}}{{\text{p}}^3}{\text{ both}}$
C.${\text{s}}{{\text{p}}^{\text{2}}},{\text{s}}{{\text{p}}^3}$
D.${\text{sp}},{\text{s}}{{\text{p}}^2}$

Answer 1

The splitting of molecules in such a way that one of the bonded atoms get both of the shared electrons is known as heterolytic fission. The hybridization of the molecule depends on the structure, it changes with the change in structure.

Complete step by step answer:
The term fission simply indicates the breaking of something. The fission are of two types, homolytic and heterolytic. The fission in which the electrons are equally shared to constituent bonded atoms is known as hemolytic fission while the fission in which one of the bonded atoms get both of the shared electrons is known as heterolytic fission.
Here in our case ethane undergoes heterolytic fission.
The heterolytic fission of the ethane will be as follows:
${{\text{H}}_{\text{3}}}{\text{C - C}}{{\text{H}}_{\text{3}}}\xrightarrow{{heterolytic}}{\text{C}}{{\text{H}}_{\text{3}}}^{\text{ + }}{\text{ + C}}{{\text{H}}_{\text{3}}}^{\text{ - }}$
Here in this fission we got two ions ${\text{C}}{{\text{H}}_{\text{3}}}^{\text{ + }}$ and ${\text{C}}{{\text{H}}_{\text{3}}}^{\text{ - }}$
So now we have to find out the hybridization of these two ions.
For ${\text{C}}{{\text{H}}_{\text{3}}}^{\text{ - }}$
The structure of ${\text{C}}{{\text{H}}_{\text{3}}}^{\text{ - }}$will be tetrahedral because it has three hydrogen atoms and an electron which will automatically gain their positions at an angle of $109^\circ 28'$ with each other. So from the structure of the molecule we can say that its hybridisation will be ${\text{s}}{{\text{p}}^{\text{3}}}$ .
For ${\text{C}}{{\text{H}}_{\text{3}}}^{\text{ + }}$
The structure of ${\text{C}}{{\text{H}}_{\text{3}}}^{\text{ + }}$will be trigonal because this molecule has three hydrogen atoms bonded with the carbon atom which is central atom, so the hydrogen atoms position themselves at an angle of $120^\circ$ and the positive is charge is present on the carbon atom so from the structure of molecule we can say that the hybridization of the molecule is ${\text{s}}{{\text{p}}^{\text{2}}}$ .

Hence option (C) is correct, ${\text{s}}{{\text{p}}^{\text{2}}},{\text{s}}{{\text{p}}^3}$ .

Note:
As we have seen above that the hybridization of the molecule changes when the charges are different. The negative charge occupies the position as the other bonded atoms do but the positive charge remains on the central atom.