Question

Equilateral shape has
(A) sp hybridisation
(B) $s{{p}^{2}}$ hybridisation
(C) $s{{p}^{3}}$ hybridisation
(D) $ds{{p}^{2}}$ hybridisation

Answer 1

Hint : To solve this question, we need to look for the angles associated with each type of hybridisation. We need to check each option separately and evaluate the angles of the hybridisations.

Complete Step By Step Answer:
In the question, we need to find the angle associated with each of the above hybridisations and then eliminate the one that does not match our requirements. According to the question, we have an equilateral shape, that is the angle must be of $120{}^\circ$ . Options not following this requirement will be eliminated.
Let us start with the first option, $sp$ hybridisation has a shape of linear. And in the case of linear, the bond angle is $180{}^\circ$ and that is not equal to the condition in the question which is required. This is why we have to move on to the next option eliminating the first option.
In the second option, we have $s{{p}^{2}}$ hybridisation. And such $s{{p}^{2}}$ hybridisation have the shape of trigonal planar and the bond angle between such is $120{}^\circ$ so this is the correct option. Moving on to the next option, the bond angle between molecules of $s{{p}^{3}}$ hybridisation is $109{}^\circ$ . And the molecules following the hybridisation of the last option have a bond angle of $90{}^\circ$ and $120{}^\circ$ .
So the correct option is option number (B).

Note :
The $s{{p}^{3}}$ hybridisation has a tetrahedral shape and so it has a unique angle. And the molecules having hybridisation of $ds{{p}^{2}}$ has trigonal bi-pyramidal shape and so it has two angles, in for the planar bonds and other for the perpendicular bonds.