Question

If an atom has sp3d2 hybridization in a molecule:

Answer 1

Answer : The maximum number of σ bonds that the atom can form is 6.

The maximum number of p-p bonds that the atom can form is 0.

Explanation :

As we are given that the hybridization is $sp^3d^2$.

Bond pair = 6

Lone pair = 0

The number of electron density around the central atom is 6.

That means these molecule have central atoms with 0 lone pair and 6 atoms bond pair. Thus, the electronic geometry or molecular geometry of the molecule will be octahedral.  For example : $SF_6$

The maximum number of σ bonds that the atom can form is 6.

The maximum number of p-p bonds that the atom can form is 0.

Answer 2

Answer:

a. the maximum number of σ bonds that the atom can form is 4

b. the maximum number of p-p bonds that the atom can form is 2

Explanation:

Hybridization is the mixing of at least two nonequivalent orbitals, in this case, we have the mixing of one s, 3 p and 2 d orbitals. In hybridization the number of hybrid orbitals generated  is equal to the number of pure atomic orbital, so we have 6 hybrid orbital.

The shape of this hybrid orbital is octahedral (look the attached image) , it has 4 orbital located in the plane and 2 orbital perpendicular to it.

This shape allows the formation of maximum 4 σ bond, because σ bonds are formed by orbitals overlapping end to end.

And maximum 2 p-p bonds, because p-p bonds are formed by sideways overlapping orbitals. The atom can form one with each one of the orbitals located perpendicular to the plane.