We will look at the hybridization of C2H6 (Ethane) here on this page and understand the process in detail. Students will also learn about the molecular geometry, bond formation and the bond angles between the different atoms.
|Name of the Molecule||Ethane|
What is the Hybridization of Ethane?
Before we dive into the hybridization of ethane we will first look at the molecule. Ethane basically consists of two carbon atoms and six hydrogen atoms. However, carbon will be the central atom and its orbitals will take part in hybridization.
During the formation of C2H6, 1 s orbital and px, py, and pz orbitals undergo sp3 hybridization. This results in the formation of four hybridized orbitals for each carbon atom. The molecular hybrid orbitals now form different bonds between the electrons.
Among the four sp3 hybrid orbitals, one hybrid orbital of one carbon atom will overlap with 1 s-orbital of the hydrogen atom to produce 3 sigma bonds. In addition, the last orbital will overlap with one sp3 orbital of another carbon atom forming a sigma bond between two C-atoms.
Important Points To Remember
- In C2H6, 1 s orbital and three p-orbitals (px, py, pz) take part in hybridization.
- There is a formation of four sp3 hybridized orbitals.
- During the hybridization of ethane four identical bonds are formed in a perfect tetrahedral geometry.
C2H6 Molecular Geometry And Bond Angles
If we look at the C2H6 molecular geometry, the molecule is arranged in a tetrahedral geometry. The central carbon atoms are surrounded by H-atoms with a bond angle of 109.5o.