Hybridization and their types for pro beginners (hybridization chemistry)

                              Hybridization

Definition

        Hybridization is the process in which atomic orbitals mix with each other and converted into a new set of hybrid orbitals are known as hybridization. The new hybrid orbitals have different properties from their atomic orbitals.

          On the basis of hybridization, we can easily explore the molecular geometry of different compounds. If there is no concept of hybridization, then we are unable to explain the geometry of many compounds because most of the elements of compounds do not obey the duplet or octet rule to complete their valence shell.

Hybridization orbitals

          Only those atomic orbital mixes with each other which are present in the same energy level. Every atomic orbital has its own proper shape but after mixing hybrid orbitals attain a new shape by combining the shapes of their atomic orbitals.

Types of hybridization

          The division of hybridization depends on:

·       Which atomic orbitals combine

·       How many combine with each other.

On this basis hybridization has the following types.

v sp

^v   sp²

^v   sp³

^v   dsp²

^v   dsp³

^v   d²sp³

sp hybridization

          When one “s’ and one ‘p’ atomic orbital combine with other, then two new sp hybrid orbitals are formed.

                           S +p                            sp + sp

sp hybrid orbitals 

Shape:

          linear shape

Examples:

          Beryllium chloride

 

sp hybridization

sp² hybridization

          When one ‘s’ and two ‘p’ atomic orbitals combine with each other, then 3 new sp² hybrid orbitals are formed.

     s+ p + p                             sp² + sp² + sp²

sp² hybrid orbital

Shape:

           triangular planner

Examples:

          Boron  trifluoride

sp² hybridization

sp² hybridization

          When one ‘s’ and three ‘p’ atomic orbitals combine with each other than 4 sp³ hybrid orbitals are formed.

     s+ p + p +p                               sp³+ sp³+ sp³+ sp³

Shape:

          Tetrahedral

Examples:

          Carbon tetrachloride, methane

sp³ hybridization

dsp² hybridization

          When one ‘s’ and two ‘p’  and one ‘d’ atomic orbitals combine with each other than 4 dsp² hybrid orbitals are formed.

s+ d + p +p                             dsp²+ dsp²+ dsp²+ dsp²

Shape:

          Square planner

Examples:

          ICl₄

 

dsp³ hybridization

          When one ‘s’ and three ‘p’ and one ‘d’ atomic orbitals combine with each other than 5 dsp³ hybrid orbitals are formed.

s+ d + p +p+ p                             dsp³+ dsp³+ dsp³+ dsp³ + dsp³

Shape:

          trigonal bypriyamidal

Examples:

 

dsp³ hybridization

d²sp³ hybridization

          When one ‘s’ and three ‘p’  and two ‘d’ atomic orbitals combine with each other then 6 d²sp³ hybrid orbitals are formed.

s+ d+ d + p +p+ p                             d²sp³+ d²sp³+ d²sp³+ d²sp³ + d²sp³+ d²sp³

Shape:

          Octahedral

Examples:

          Sulfur hexafluoride

d²sp³ hybridization