Question
In formation of ethene, the bond formation between $$s$$ and $$p$$ - orbitals takes place in which of the following manner?
A.
$$s{p^2}$$ hybridised orbitals form sigma bond while the unhybridised $$\left( {{p_x}\,\,{\text{or}}\,\,{p_y}} \right)$$ overlaps sidewise to form $$\pi $$ - bond.
B.
$$s{p^2}$$ hybridised orbitals form $$\pi $$ - bond while the unhybridised $$\left( {{p_z}} \right)$$ overlaps to form $$\sigma $$ - bond.
C.
$$s{p^2}$$ hybridised orbitals overlap with $$s$$ - orbitals of $$H$$ atoms while unhybridised orbitals form $$C-C$$ bond.
D.
$$s{p^2}$$ hybridised orbitals form sigma bonds with $$H$$ atoms while unhybridised orbitals form $$\pi $$ - bonds between $$C$$ and $$H$$ atoms.
Answer :
$$s{p^2}$$ hybridised orbitals form sigma bond while the unhybridised $$\left( {{p_x}\,\,{\text{or}}\,\,{p_y}} \right)$$ overlaps sidewise to form $$\pi $$ - bond.
Solution :
