Question

In formation of ethene, the bond formation between $s$ and $p$ -orbitals takes place in the following manner.

• A. $s{p}^2$ hybridised orbitals form sigma bond while the unhybridised ($p_x$ or $p_y$) overlaps sidewise to form $\pi$ -bond
• B. $s{p}^2$ hybridised orbitals form $\pi$ -bond while the unhybridised $(p_z)$ 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 $C$ atoms

Answer 1

Answer: (A)

Correct answer is (a) $s{p}^2$ hybridised orbitals form sigma bond while the unhybridised ($p_x$ or $p_y$) overlaps sidewise to form $\pi$ -bond