Explain the term hybridization with the help of suitable example
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Hybridization
Hybridization is defined as the concept of mixing two atomic orbitals with the same energy levels to give a degenerated new type of orbitals. This intermixing is based on quantum mechanics. The atomic orbitals of the same energy level can only take part in hybridization and both full filled and half-filled orbitals can also take part in this process, provided they have equal energy.
During the process of hybridization, the atomic orbitals of similar energy are mixed together such as the mixing of two ‘s’ orbitals or two ‘p’ orbital’s or mixing of an ‘s’ orbital with a ‘p’ orbital or ‘s’ orbital with a ‘d’ orbital.
What is Hybridization?
Redistribution of the energy of orbitals of individual atoms to give orbitals of equivalent energy happens when two atomic orbitals combine together to form hybrid orbital in a molecule. This process is called hybridization. The new orbitals thus formed are known as hybrid orbitals.
⇒ Also Read
Chemical Bonding
Molecular Orbital Theory
Types of Hybridization
Based on the types of orbitals involved in mixing, the hybridization can be classified as sp3, sp2, sp, sp3d, sp3d2, sp3d3. Let us now discuss the various types of hybridization, along with their examples.
sp Hybridization
sp hybridization is observed when one s and one p orbital in the same main shell of an atom mix to form two new equivalent orbitals. The new orbitals formed are called sp hybridized orbitals. It forms linear molecules with an angle of 180°
This type of hybridization involves the mixing of one ‘s’ orbital and one ‘p’ orbital of equal energy to give a new hybrid orbital known as an sp hybridized orbital.
sp hybridization is also called diagonal hybridization.
Each sp hybridized orbital has an equal amount of s and p character, i.e., 50% s and p character.
sp2 Hybridization
sp2 hybridisation is observed when one s and two p orbitals of the same shell of an atom mix to form 3 equivalent orbital. The new orbitals formed are called sp2 hybrid orbitals.
sp2 hybridization is also called trigonal hybridization.
It involves mixing of one ‘s’ orbital and two ‘p’ orbital’s of equal energy to give a new hybrid orbital known as sp2.
A mixture of s and p orbital formed in trigonal symmetry and is maintained at 1200.
All the three hybrid orbitals remain in one plane and make an angle of 120° with one another. Each of the hybrid orbitals formed has 33.33% s character and 66.66% ‘p’ character.
The molecules in which the central atom is linked to 3 atoms and is sp2 hybridized have a triangular planar shape.
Examples of sp2 Hybridization
All the compounds of Boron i.e. BF3, BH3
All the compounds of carbon containing a carbon-carbon double bond, Ethylene (C2H4)
sp3 Hybridization
When one ‘s’ orbital and 3 ‘p’ orbitals belonging to the same shell of an atom mix together to form four new equivalent orbital, the type of hybridization is called a tetrahedral hybridization or sp3. The new orbitals formed are called sp3 hybrid orbitals.
These are directed towards the four corners of a regular tetrahedron and make an angle of 109°28’ with one another.
The angle between the sp3 hybrid orbitals is 109.280
Each sp3 hybrid orbital has 25% s character and 75% p character.
Example of sp3 hybridization: ethane (C2H6), methane.sp3d Hybridization
sp3d hybridization involves the mixing of 3p orbitals and 1d orbital to form 5 sp3d hybridized orbitals of equal energy. They have trigonal bipyramidal geometry.
The mixture of s, p and d orbital forms trigonal bipyramidal symmetry.
Three hybrid orbitals lie in the horizontal plane inclined at an angle of 120° to each other known as the equatorial orbitals.
The remaining two orbitals lie in the vertical plane at 90 degrees plane of the equatorial orbitals known as axial orbitals.
Example: Hybridization in Phosphorus pentachloride (PCl5)
it may help you
hybridisation (or hybridization) is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory.
Example. In their ground state, carbon atoms naturally have electron configuration