What is the type of hybridization in Ethane (#C_2H_6#)?

1 Answer
Nov 19, 2017

Answer:

#sp^3# hybridization.

Explanation:

From the Lewis structure below, you can count 4 sigma bonds and 0 lone electron pairs (unshared electrons) around the central atom (carbon).

Sigma bonds are 'overlaps' of electron clouds between two atoms' nuclei (a single bond). Pi bonds, on the other hand, are bonds that do not get hybridized and are double and triple bonds; however, there is always 1 sigma bond in each double and triple bond.

The hybridization of sigma bonds and lone electron pairs goes as such:

1 cloud: #sp#
2 clouds: #sp^2#
3 clouds: #sp^3#
4 clouds: #sp^3d#
5 clouds (maximum): #sp^3d^2#

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