Sp² Hybridization in Ethene: The Secret of Double Bonds

The video tutorial explains the structure and bonding of ethane, focusing on its carbon-carbon double bond, which consists of a sigma and a pi bond. Ethane's SP2 hybridization results in a trigonal planar structure with a bond angle close to 120°. The double bond is strong, with a bond energy of 146 kcal/mol, and the pi bond has a shorter bond length of 1.34 angstroms. The tutorial visualizes the orbital structure, showing how SP2 hybrid orbitals form sigma bonds and how unhybridized p orbitals form pi bonds through lateral overlap, resulting in a delocalized orbital. The structure of ethane is also represented in different ways.

What is the bond energy of the double bond in ethane?

How do the valence electrons of carbon contribute to the bonding in ethane?