Hybridization: The Process of Mixing Atomic Orbitals

Hybridization: The Process of Mixing Atomic Orbitals

Hybridization is a fundamental concept in chemistry that explains the mixing of atomic orbitals to form new hybrid orbitals. This process is essential for understanding the structure and geometry of molecules.

In this presentation, we will explore:

- The different types of hybridization (sp3, sp2, sp, dsp3, d2sp3)
- The formation of hybrid orbitals and their shapes
- The role of hybridization in determining molecular geometry and shape
- Examples of molecules that exhibit hybridization

Join us as we delve into the world of hybridization and uncover the secrets of molecular structure!"
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1. According to valance bond theory (VBT), only half filled orbitals can take part in bond formation. But when we look at the electronic configuration of carbon . C = 1s² 2s² 2p² We see that there are only two half-filled orbitals. But still it can form four bonds instead of two ( e.g. in CH₄ ). Similarly , consider the electronic configuration of Beryllium ( Be ) Be = 1s² 2s² This atom has no half-filled orbital, but it can form two bonds ( e.g., in BeCl ₂ ).

2. The answer to this question was given by Pauling and Slater when they introduced a new phenomenon called Hybridization.

3. Definition Hybridization is a process in which two or more orbitals of the same atom, having different shapes and energies combine and mix together to give equivalent no. of orbitals of same shape and energy .

4. The combining orbitals must belong to the same atom. The combining orbitals have different shapes and energies. The hybrid orbitals formed have same shape and energies. No. of Hybrid orbitals formed = No. of combining orbitals (Law of conservation of Orbitals) The energy of the hybrid orbitals is equal to the average of the energies of the combining orbitals.

5. There are many types of hybridization, but we will study only three types . sp hybridization . sp² hybridization . sp³ hybridization

6. The type of hybridization in which one "s" orbital combines with one "p" orbital of the same atom to form two hybrid orbitals called "sp orbitals" is called sp hybridization . i.e . S + p 2sp Characteristics of sp hybridization : Each sp orbital has s-character = 50 % p-Character = 50 % Angle between two sp orbitals = 180°iii. Shape = Linear

7. Ethyne (C₂H₂) molecule is the best example of sp hybridization. Ethyne molecule has two carbon atoms each carbon atom is sp Hybridized . The electronic configuration of ground state carbon is given as.

8. When energy is provided, one of the electrons from 2s orbital is excited to the empty 2pₓ Orbital as shown:

9. Now you can see that carbon has four half-filled orbitals and this is the answer to the question how carbon can form four bonds . Now , as the name indicate, in sp hybridization, one "s" will combine with one "p" orbital. As a result, two "sp" hybrid orbitals are formed.

10. The remaining two p orbitals (say Py and Pz) remain unhybridized on each carbon. The remaining two P orbitals (say Py and Pz) remain unhybridized on each carbon . One of the "sp" hybrid orbitals of each carbon forms Sigma (σ) Bond with the "sp" of the other carbon. The 2nd"sp" orbital forms Sigma (σ) Bond with the "s" orbital of the H-atom. Thus a total of three σ bonds are formed .

11. The remaining unhybridized orbital of each carbon forms π bond by sidewise collision with the unhybridized Py and Pz orbital of the other carbon. All these collisions are shown in the following fig.

12. The type of hybridization in which one "s" orbital combines with two "p" orbitals of the same atom to form three hybrid orbitals called Sp² orbitals

13. Ethene (C₂H₄) is a typical example of Sp² hybridization. Each carbon of ethane is Sp² hybridized. The ground and excited state of electronic configuration of carbon is given as:

14. One "s" orbital combines with two "p" orbitals ( Px and Py) and the remaining Pz orbital remains unhybridized.

15. So, three Sp² orbitals are formed on each carbon.

16. 1.Three hybrid orbitals: sp² hybridization results in three hybrid orbitals, which are shaped like a trigonal planar. 2. 120° bond angle: The bond angle between the three hybrid orbitals is 120°, which is a result of the sp² hybridization. 3 . Planar shape: The molecule has a planar shape, with all the atoms in the same plane.

17. 4 . Sigma bonds: The sp² hybrid orbitals form sigma bonds with the s orbitals of the surrounding atoms. 5. One unhybridized p orbital: There is one unhybridized p orbital remaining on each carbon atom, which is perpendicular to the plane of the molecule. 6. Pi bonds: The unhybridized p orbitals can form pi bonds with the p orbitals of other atoms. These characteristics are typical of sp² hybridization and are seen in molecules like ethene (C₂H₄) and benzene (C₆H₆).

18. One "s" orbital combines with three "p" orbitals to form four equivalent "sp³" orbitals, which are arranged in a tetrahedral shape.

19. E xample of Sp³ Hybridization : Methane molecule (CH₄) is the best example of sp³ hybridization. CH₄ has one carbon. The ground and excited state electronic configuration of carbon is given as.

20. One s orbital combine with all three P-orbitals (Px,Py,Pz) to form four Sp3 hybrid orbitals on carbon. Each Sp3 orbital then form a sigma bond with unhybrid spherical orbital of hydrogen. This is shown in the following fig.

21. Four hybrid orbitals : sp3 hybridization forms four hybrid orbitals, which are shaped like a tetrahedron . Tetrahedral shape : The four hybrid orbitals are arranged in a tetrahedral shape, with 109.5° angles between them Equal energy: The four hybrid orbitals have equal energy. s-character : Each hybrid orbital has 25% s-character and 75% p-character .

22. Sigma bonds: sp3 hybridization forms sigma bonds, which are strong and rigid. No unhybridized p-orbital : All three p-orbitals are hybridized, leaving no unhybridized p-orbital . Tetrahedral molecule: The molecule is tetrahedral, with all atoms in a three-dimensional arrangement.