Ethylene molecules is formed as a result of `sp^(2)` hybridisation of carbon. Each carbon atom is excited state undergo `sp^(2)` hybridisation giving rise to three hybrid orbitals each. These hybrid orbtals lie in the xy plane while the fourth unhybridised orbital lies at right angles to the hybridised orbitals. in the overlap ethylene two hybrid orbitals, i.e., one from each carbon atom from a sigma bond by head on overlap while the remaining overlap with hydrogen atoms. the unhybridised p-orbitals undergo sidewise overlap to from a `pi` -bonds
Ground state of carbon atom
Excited state of carbon atom
The molecules of ethylene is planar
If molecular axis is z axis then
A. `p_(x) - p_(x)to pi` bond
B. `p_(z)-p_(z) to sigma` bonds
C. `p_(y) -p_(y) to pi` bond
D. All the above are correct
