The hybridization on the carbons in the ethylene molecule below is referred to as

hybridization. The

angle of each $H-C-H$ angle, or

$C-C-H$ angle with carbon as the vertex and the two rays represented by the $C-H$ bonds or

one $C-H$ bond and one $C-C$ bond, is $120.$ The overall geometrical shape of the molecule is

referred to as a

planar. There is a double bond between the two

carbons. The sigma $()$ bond between the two carbon atoms is formed by the overlap of

two $\text{'}$

$"$ orbitals $($end$-$to$-$end$).$ The sigma $()$ bond between the hydrogen

and carbon atoms is formed by the overlap of a$/$an $\text{'}$

$"$ orbital $($end on$),$ respectively. The pi $()$ bond between the two

carbons is formed by the overlap of two unhybridized $\text{'}$

$"$ orbitals $($side$-$

to$-$side$).$