Hybridization of atomic orbitals

Hybridization

This is the one inter mixing of phenomenon of atomic orbital explain the formation of covalent bond as well as geometry of
molecules.

Definition:-

When two or more atomic orbitals having nearly same energy intermixed with each other give rise  new orbital equivalent shape and energy and are called hybrid orbitals but the shape and energy of the hybrid orbitals are different and from the parent atomic orbitals and this phenomenon is equal hybridization.

Hybridization takes place in two step

                 (1)Excitation

                 (2)Intermixing.                                Conditions for hybridization:-

1. Atomic orbitals of only one and same atom can be inter mixed.
2. The atomic orbitals should have nearly same energy.

 3.Only the atomic orbitals but not the electrons get hybridised.

Characteristics of hybridization:

1. The number of hybrid orbitals produced are equal with the number of atomic orbital inter mixed.

2. The hybrid orbital Sahab equal and shape and energy.

3. The shape of the hybrid orbitals depends upon the shape of the atomic orbitals from which they are produced.

4. The hybrid orbitals having single electron can take part in Bond formation.

5. There is Electronic repulsion between the hybrid orbitals.

6. Eenadu to minimise the Electronic repulsion the hybrid orbitals stand to far away from each other.

Types of Hybridization:-

On the basis of the nature and the number of atomic orbitals intermediate there are following types of hybridization.

SP, SP2 ,SP3 SP³d,SP³d²,SP³d³ hybridization.

SP Hybridization:-

When one S atomic orbital intermixed with one P atomic orbital give rise to SP hybrid orbital and this process is called SP hybridization.

               One S atomic orbital  + one P atomic orbital =                      Two SP hybrid orbital

In order to minimise the Electronic repulsive the to SP hybrid orbitals Are linear to each other with bond angle 180 degree having linear shaped.

Each of the SP hybrid orbital has 50% S character and 50% P character.

Example:-

BeCl2

SP² Hybridization:-

When one S atomic orbital inter mixed with 2P atomic orbitals give rise 3 SP2 hybrid orbitals and this process is called SP2 hybridization.

One S atomic orbital + two P atomic orbital =3 SP2 hybrid orbital

In order to minimise the Electronic repulsion the three SP² hybrid orbitals are directed towards three corners of a triangle and regular trigonal geometry with bond angle 120 degree.

Each SP2 hybrid orbital has 33.3% S character and 66.6% P character.

Example

BF3

SP³ Hybridization:-

When one is atomic orbital intermixed 3 P atomic orbital give rise to four SP3 hybrid orbital and this process is called SP3 hybridization.

One S atomic orbital +3 P atomic orbital =4 SP3 atomic orbital

In order to minimise the Electronic repulsion the four SP3 hybrid orbitals are directed towards 4 corners of a tetrahedral  and has regular tetrahedral geometry with bond angle 109 . 28'.