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

hybridization. The

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

carbon as the vertex and the two rays represented by the $C-H$ bond and the $C-C$ bond, is

$180.$ The overall geometrical shape of the molecule is referred to as linear because all the

atoms lie in a

line. There is a triple bond between the two carbons. The

sigma $()$ bond between the two carbon atoms is formed by the overlap of two $"$

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

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

$"$ orbital and a$/$an $"$

$"$ orbital $($end on$),$ respectively. Each of the two pi $()$ bonds between

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