A hybrid, you may think that it is a combination of different types of genes to make an extraordinary organism but in chemistry, there is a huge difference because we are talking about the different orbital hybrids. To be familiarized in this topic, I will show you easy to understand concepts and processes about HYBRIDIZATION

 

         It was developed by Sir Linus Pauling. The concept and theory of hybrid orbitals was created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals like sp, sp2 and sp3.

 

         I will now introduce to you some of the terms that will be mostly used in this article in order for you to have prerequisite knowledge about this topic.

 

1. Atomic orbital- an expected region of electron density around an atom based on a solution to the Schrödinger wave function.

2. Hybridization- the combining of solutions to the Schrodinger wave function for atomic orbitals to produce hybrid orbitals. Note: the total number of orbitals available for forming bonds does not change—a new set is simply formed.

3. Hybrid orbital- an orbital created by the combination of atomic orbitals in the same atom.

4.Linear sp hybrids- the two hybrid orbitals formed by the mixture of ons and one p orbital.

5.Trigonal sp2 hybrids- the three hybrid orbitals formed by the mixture of ones and two p orbitals.

6.Tetrahedral sp3 hybrids- the four hybrid orbitals formed by the mixture of one s and three p orbitals.

7.Triangular Bipyramidal sp3d hybrids- the five hybrid orbitals formed by the mixture of one s ,three p orbitals and one d orbital.

8.Triangular Bipyramidal sp3d2 hybrids- the six hybrid orbitals formed by the mixture of one s ,three p orbitals and two d orbitals.

 

          Now, we must be familiar about the different structures of the orbitals or their shapes. It is exhibited in the figure below.

 

 

 

 

 

 

 

 

 

 

 

 

 

              In order for a covalent bond to exist between two specific atoms, an overlap must occur between the orbitals containing the outermost electrons or valence electrons.

              If you want the best overlaps to occur, two orbitals are allowed to meet “head on” in a straight line.  When this occurs, the atomic orbitals combine to form a single bonding orbital and a “single bond” is formed, called a  sigma (s) bond.

 

              Also, valence electrons need to be re-oriented and electron clouds must be reshaped to allow the best possible contact. To form as many bonds as possible from the available valence electrons, sometimes separation of different electron pairs must also occur.

 

sp HYBRID ATOMIC ORBITALS

 

              The sp hybrid atomic orbitals are possible states of electron in an atom, especially when it is bonded to others. These electron states have half 2s and half 2p characters. These hybrid orbitals form a straight line. There is a 180 degree angle between one orbital and the other orbital. They are exactly opposite one another from the center of the atom.

             

              For example, we have beryllium cloride or BeCl2. Below is its orbital hybridization.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

sp2 HYBRID ATOMIC ORBITALS

 

              In sp2 hybridization, the 2s orbital is mixed with only two of the three available 2p orbitals. A sigma bond is formed between two sp2 hybrid orbitals of two carbon atoms, and a pi bond is formed between two p orbitals.

                     The figure below shows how orbitals undergo sp2 hybridization

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

                For example, we have Boron trifluoride or BF3

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

                 Each fluorine atom, 1s22s22p5, has one unshared electron in a p orbital.  The half filled p orbitaloverlaps head-on with a half full hybrid sp2 orbital of the boron to form a sigma bond.

 

sp3 HYBRID ATOMIC ORBITALS

 

            Sp3 hybridization are made from one’s orbital and three p orbitals. You should read "sp3" as "s p three" - not as "s p cubed".

 

             sp3 hybrid orbitals look a bit like half a p orbital, and they arrange themselves in space so that they are as far apart as possible.

 

               Now, let us make methane or CH4 as an example.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

sp3d HYBRID ATOMIC ORBITALS

 

             Sp3d Hybridization is the combination of one s, three p and a d-orbital to form a hybrid. sp3d hybridization forms five equivalent orbitals. sp3d hybridization forms a triangular bipyramidal molecular geometry.

 

               Now, let us make phosphorus pentafluoride or PF5 as an example.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

sp3d2 HYBRID ATOMIC ORBITALS

 

             In this case, one s, three p and two d-orbitals get hybridized to form six sp3d2 hybrid orbitals which adopt octahedral arrangement as given in the figure below.

 

 

 

 

 

 

 

            

 

 

            Now, let us make sulfur hexafluoride or SF5 as an example.