Question

Which atomic orbitals overlap to form the carbon-carbon σ and π bonding molecular orbitals of ethene, H2C=CH2?

Answer 1

Answer:

σ -> 2sp²

π -> 2p

Explanation:

The carbon has valence shell 2s 2p, and, both of them make 3 σ bonds and 1 π bond. The π bond only occurs in multiple bonds.

The σ bonds happen at the hybrids orbitals, which are orbitals formed by the association of the pure orbitals (s, p, d, f). The hybridization occurs to make possible to the atom to do the bonds because the electrons need to be isolated in it.

On the other hand, the π bonds only occur at pure orbitals. The subshell s only has 1 orbital, and the subshell p has 3 orbitals. So, because there are 3 σ bonds, it's necessary 3 hybrids orbitals (1 of s + 2 of p).

The σ bonds happen at the orbital 2sp² and the π bond at the 2p pure orbital.