Hybridisation

Hybridisation is defined as the mixing of the atomic orbitals belonging to the same atom but having slightly different energies so that a redistribution of energy takes place between them resulting in the formation of new orbitals of equal energies and identical shape.

The new orbitals thus formed are known as hybrid orbitals.

Important points about hybridisation

1)Only those orbitals which have approximately equal energies and belong to the same atom or ion can undergo hybridisation.

2)Number of hybrid orbitals produced is equal to the number of atomic orbitals mixed.

3)It is not necessary that all the half filled orbitals must participate in hybridisation. Even completely filled orbitals with slightly different energies can also participate.

4)Hybridisation never take place in isolated atoms but it occurs only at the time of bond formation.

5)One can tell the shape of a molecule by knowing the kind of hybridisation involved.

6)The bigger lobe of the hybrid orbital always have positive sign while the smaller lobe on the opposite side has negative sign.

 

Types of hybridisation

1) sp hybridisation

When one s and one p orbital belonging to the same main shell of an atom mix together to form two new equivalent orbitals ,the type of hybridisation is called sp hybridisation.

The new orbitals formed are called sp hybrid orbitals.

They are collinear with an angle of 180° .

Each of the hybrid orbitals formed has 50% s character and 50% p character.

The remaining two p orbitals which do not participate in hybridisation remains as such.

Example:

1)All compounds of beryllium like BeF₂ , BeH₂

2)All compounds of carbon containing triple Bond like C₂H₂.

2) sp² hybridisation

When one s and two p orbitals of the same shell of an atom mix to form 3 equivalent orbitals, the type of hybridisation is called sp² hybridisation.

The new orbitals formed are called sp² hybrid orbitals.

All the three hybrid orbitals remain in the same plane making an angle of 120° with one another.

Each of the hybrid orbitals formed has 1/3^rd s character and 2/3^rd  p character.

 

The non-participating p-orbital ,if half filled ,can form bond with other atoms having half filled orbitals.

For example:

1)All compounds of Boron i.e. BF₃ , BH₃

2)All compounds of carbon containing carbon carbon double bond.

3) sp³ hybridisation

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 hybridisation is called a tetrahedral hybridisation  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.

Each sp³ hybrid orbital has 25% s character and 75% p character.

Example

Methane, ethane