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 hybridization of carbon atoms in ethane?

• SP

• SP2

• None of the above

• SP3

What is the bond angle in the trigonal planar structure of ethane?

• 180°

• 120°

• 109.5°

• 90°

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

• 100 kilocalories per mole

• 146 kilocalories per mole

• 250 kilocalories per mole

• 200 kilocalories per mole

Which orbitals overlap to form the sigma bond in ethane?

• SP2 and SP2

• P and P

• S and P

• SP3 and SP3

What is the nature of the pi orbital in ethane?

• Delocalized

• Non-existent

• Hybridized

• Localized