What is the Hybridisation of Ethane?

The carbons in ethane comprise four bonds arranged with the tetrahedral geometry. Moreover, the carbon bond has a bond length of 1.54 Å and is made through the overlap of 1 sp3 orbital from each of the carbons, whereas the six carbon-hydrogen bonds are made with overlaps amid the leftover orbitals of sp3 on the two carbons as well as the 1s orbitals of hydrogen atoms. They rotate freely as they are made with the end-on-end overlap of two orbitals and are sigma bonds in nature. 

In the case of the ethane molecule, this states that the two methyls, i.e. CH3 groups can be pictured as two wheels on a hub, and each one of them rotates freely with respect to others.

Same as the carbon atom in methane, the central nitrogen is sp3 hybridised in ammonia. In the case of nitrogen, however, there are five valence electrons to account for, which means three of the four hybrid orbitals are partially filled and are capable of bonding. Whereas the fourth one is totally occupied by a non-bonding pair of electrons. 

Moreover, ethene, i.e. C2H4 or ethylene, is a type of gas made synthetically with the process of steam cracking. It is released in nature in trace amounts by the plants for providing signals for their fruits to ripen. Moreover, ethene comprises two sp2 hybridised carbon atoms; these are bonded to each other with sigma bonds and to two atoms of hydrogen each. The leftover unhybridized p orbitals on the carbon make a pi bond which provides reactivity to ethene.

What is Ethane?

It is a chemical compound that is organic in nature and has a chemical formula; C2H6. Ethane is colourless as well as odourless at the standard temperature. Just like many other hydrocarbons, ethane is isolated on an industrial scale from natural gas and in the form of a petrochemical by-product of petroleum refining. 

It is primarily used as feedstock for the production of ethylene. Moreover, the related compounds may be determined by the replacement of a hydrogen atom with some other functional group. The ethane moiety is known as the ethyl group. Such as, an ethyl group connected with a hydroxyl group yields ethanol which is the alcohol present in the beverages.

Hybridisation of Ethane

Ethane generally comprises two atoms of carbon and six atoms of hydrogen. However, carbon remains the central atom, and its orbitals get involved in the process of hybridisation. During the process of preparation of C2H6, 1s orbital and px, py, as well as pz orbitals, undergo sp3 hybridisation. This leads to the formation of four hybridised orbitals for each atom of carbon. 

However, the molecular hybrid orbitals now create different bonds between the electrons. From the four sp3 hybrid orbitals, one hybrid orbital of a carbon atom overlaps with one s-orbital of the atom of hydrogen for forming three sigma bonds. Furthermore, the last orbital overlaps with one sp3 orbital of another carbon atom, making a sigma bond between two atoms of carbon.

Representations of Ethane

Ethane is the simplest molecule having a carbon-carbon bond. In ethane, i.e. CH3CH3, both the carbons are sp3 hybridised, which means both comprise four bonds with the tetrahedral geometry. An sp3 orbital of a single atom of carbon overlaps end-to-end with an sp3 orbital of the second atom of carbon to make a carbon-carbon σ bond. 

This orbital overlap is defined with the use of the notation; sp3(C)-sp3(C). Every single leftover sp3 hybrid orbital overlaps with the s orbital of an atom of hydrogen for making carbon-hydrogen σ bonds.

The σ carbon-carbon bond has a bond with a length of 154 pm, as well as a bond with a strength of 377 kJ/mol. The carbon-hydrogen σ bonds are a bit weaker with a strength of 421 kJ/mol than that of methane. Moreover, the C-C-H bond angles in ethane are 111.2 degrees, and this is near about what is expected for the tetrahedral molecules.

Essential Points to Keep in Mind

• In C2H6 or CH3CH3, 1s orbital, as well as 3p orbitals: px, py, and pz, are involved in the process of hybridisation.
• There is a formation of four orbitals that are sp3 hybridised.
• At the time of the hybridisation of ethane, four similar bonds are created in perfect tetrahedral geometry.

Conclusion

In ethane, four hybridised orbitals are produced for every single atom of carbon. Moreover, at the time of the process of preparation of the C2H6, 1s orbital, including the px, py, as well as pz orbitals, undergoes sp3 hybridisation. This leads to the creation of four hybridised orbitals for each carbon atom. There is some hybridisation of ethane questions at the end of the article that will assist you in understanding the topic in a better way.