Question

explain sp3 d hybridization​

Answer 1

Answer:

heyyy mate here is your answer

Combination of 1s, 3p and 1d orbital result in the formation of sp3d orbital in which three lobes are oriented towards the corners of a triangle and the other lie perpendicular to them to minimize the repulsions.

In sp3d hybridization, one ‘s’, three ‘p’ and one ‘d’ orbitals of almost equal energy intermix to give five identical and degenerate hybrid orbitals, which are arranged in trigonal bipyramidal symmetry.

Among them, three are arranged in trigonal plane and the remaining two orbitals are present above and below the trigonal plane at right angles. The sp3d hybrid orbitals have 20% ‘s’, 60% ‘p’ and 20% ‘d’ characters.

Example: PF5

I hope it will help you pl select me as brainlist and follow me

Answer 2

Answer:

in sp3 d hybridization

5 bonds are there

for example SF4

when we find no.of bonds it comes out to be 5

like S=4

F=7*4 as 4F are there

so now add we get

4+28=32

now divide 32 with 8 we get 4 bonds + 1 lone pair which makes total 5 bonds

the condition for this hybridization is

(a)4 bond pair +1 lone pair

(b)3 bond pair+ 2 lone pair

(c)2 bond pair + 3 lone pair

and the shape formed is

trigonal bipyramidal(5 bond pair+0lone pair)

irregular tetrahedron(in a)

T shape (in b)

linear(in c)