wat is meant by nitrogen is sp3 hybridised ?explain plz!
Here is the proper explanation of hybridization.....
Hybridisation
It states that atomic orbitals of slightly different energies combine to form a new set of equivalent orbitals (having the same energy and shape) known as hybrid orbitals.
These hybrid orbitals are more stable than atomic orbitals, and participate in bond formation.
Salient features:
1. Number of hybrid orbitals obtained = Number of atomic orbitals undergoing hybridisation
2. Hybrid orbitals are always identical in all respects.
3. To minimise electronic repulsion, they orient themselves in a preferred manner. Thus, the type of hybridisation indicates the geometry of a molecule.
Conditions required for hybridisation:
1. Orbitals in the valence shell should be hybridised.
2. Orbitals undergoing hybridisation should have almost equal energy.
3. Promotion of electrons is not essential prior to hybridisation.
4. Half as well as fully filled orbitals of the valence shell can take part in hybridisation.
Types of hybridisation:
sp
- Involves mixing of one s and one p (preferably pz) orbital to give two sp orbitals
- Hybrid orbitals have 50% s and 50% p character.
- Also known as diagonal hybridisation because if the central atom undergoes hybridisation, the orbitals are oriented in opposite directions at an angle of 180°, giving rise to linear geometry
- Example: Be atom in BeCl2 undergoes sp hybridisation.
sp2
- Involves mixing of one s orbital and two p orbitals to give three sp2 orbitals
- Hybrid orbitals have 33.33% s and 66.64% p character.
- Three hybrid orbitals orient themselves in a trigonal planar fashion at an angle of 120°.
- Example: B in BCl3 undergoes sp2 hybridisation.
sp3
- Involves mixing of one s orbital and three p orbitals to give four sp3 orbitals
- Hybrid orbitals have 25% s and 75% p character.
- Four hybrid orbitals orient themselves in such a manner that each orbital is directed toward the four corners of a tetrahedron.
- Example: C in CH4 undergoes sp3 hybridisation.
The geometry of H2O and NH3 can also be explained using sp3 hybridisation. In a water molecule, the oxygen atom undergoes sp3 hybridisation. Among the four hybrid orbitals, two contain the two lone pairs present on the O-atom, and the remaining two are involved in bonding. Similarly, in the case of NH3, one sp3 hybrid orbital contains a lone pair, and the remaining three are involved in bonding.
