Question

Is \[s{p^3}{d^2}\] hybridization the same as ${d^2}s{p^3}$ hybridization?

Answer 1

Hint: Hybridization is the concept of mixing of the orbitals into the new hybrid orbitals so as to redistribute the energies between the different structures and shapes so as to stabilise the molecule. Since the lower energy of the molecule corresponds to the high stability of the molecule.

Complete step by step answer:
There are 4 orbitals in which the filling of the electrons takes place these orbitals are s, p, d and f orbitals namely. The distribution of the electrons within these orbitals takes place do stabilise the molecule so that it acquires the lowest energy state.
The \[s{p^3}{d^2}\] hybridization the overlap of the s, p and d orbital takes place so as to stabilise the molecule and reach the lowest energy state, the overlap takes place between the same atomic orbitals. One s, three p and two d orbitals overlap with each other to undergo \[s{p^3}{d^2}\]hybridisation. Thus the six hybrid orbitals are formed which are of same size and shape but the orientation of these orbitals is different.

The${d^2}s{p^3}$ hybridization again the overlap of the s, p and d orbital takes place so as to stabilise the molecule but the mixing here is between the same electron shell with the d orbitals of another electron shell takes place and here two d orbitals, one s orbital and three p overlap with each other to undergo ${d^2}s{p^3}$ hybridisation. Thus the six hybrid orbitals are also formed in such cases. Thus both the types of hybridisation are different since the different shell orbitals are involved in the hybridisation process.

Note:
In the concept of hybridization the redistribution of energy takes place between the different forms or structures of the compound, there is no overall increase or decrease in the energy of the molecule it remains the same and only the stability of the molecule is affected by the redistribution of the energy.