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Hybridization



Definition:

When atomic orbitals mix to form new atomic orbitals is called hybridization.

Valence bond theory explains bond is formed by overlapping of two half-filled valence atomic orbitals



The electrons in overlapping get paired and confined b/w nuclei of two atoms and electron density can be increased

Types of Covalent Bonds

There are 2 types of covalent bonds based on pattern of overlapping 
1; SIGMA BONDS 
2; PI BONDS


1: SIGMA BONDS

  • A sigma bond is formed by the linear or end to end overlap of orbitals
  • STRONG in nature



(A) Overlapping Of 2s Orbitals 



(B) By Overlapping Of Px And S Orbitals
  


(C) By Overlapping Of 2 P Orbitals





2: PI BONDS

  • it is formed by parallel or side to side overlap of orbitals



Characteristics;
  • pi-electrons are loosely held then a pair of electrons in sigma bond
  • highly reactive
  • cis-trans isomers, rotation of atoms is not possible around pi-bonds

ILLUSTRATIONS AND EXAMPLES


1. H2 MOLECULES
Electronic configuration of hydrogen is 1S1 two half filled S-orbitals of hydrogen overlaps.





CHLORINE
The electronic configuration of chlorine is (1S2, 2S2, 2P6, 3S2, 3P5)    
The valence electrons are (3S2 3P5) that makes   ———> 7 ELECTRONS, so in case of Hydrochloric Acid we do hybridization as follows

 2. HCL MOLECULE

  • hydrogen = 1s1  1
  • chlorine = 1s2, 2s2, 2p6, 3s2, 3p5  17



Updates:
Last update 10 Feb 2015

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