What are the necessary conditions for hybridisation?
Hybridization may be defined as the phenomenon of mixing up (or merging) of orbitals of an atom of nearly equal energy, giving rise to entirely new orbitals equal in number to the mixing orbitals and having same energy contents and identical shapes.
For hybridization to occur, it is necessary for the atom to satisfy the following conditions-
1. Orbitals on a single atom only would undergo hybridization.
2. There should be very little difference of energy level between the orbitals mixing to form hybrid orbitals.
3. Number of hybrid orbitals generated is equal to the number of hybridizing orbitals.
4. The hybrid orbitals assume the direction of the dominating orbitals. For example, if s and p orbitals are to hybridize, the s orbital having no directional character, does not contribute towards the direction when p orbitals determine the directional character of the hybrid orbitals.
5. It is the orbitals that undergo hybridization and not the electrons. For example, four orbitals of an oxygen atom (2s2, 2px2, 2py1, 2pz1) belonging to second level (i.e., 2s, 2px, 2py, 2pz) can hybridize to give four hybrid orbitals, two of which have two electrons each (as before) and the other two have one electron each.
6. The electron waves in hybrid orbitals repel each other and thus tend to be farthest apart.
Which of the following conditions is important for hybridization?
A. Promotion of electron is not essential condition prior to hybridizationB. The orbitals present in the valence shell of the atom are hybridized
C. The orbitals undergoing hybridization should have almost equal energy
D. All of the above
