Question

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

• A. $sp^{2}$hybridized orbtials form sigma bond while the unhybridised $(P_{x}orp_{y})$ overlaps sidewise to form $\pi -$bond.
• B. $sp^{2}$hybridized orbitals form $\pi -$bond while the unhybridised $(P_{Z})$ overlaps to form $\sigma -$bond.
• C. $Sp^{2}$hybridized orbitals overlap with $s -$orbitals of H atoms while unhybridised orbitals form C – C bond
• D. $Sp^{2}$hybridized orbitals form sigma bonds with H atoms while unhybridised orbitals form $\pi -$bonds between C atoms.

Answer 1

Answer: (A)

$sp^{2}$hybridized orbtials form sigma bond while the unhybridised $(P_{x}orp_{y})$ overlaps sidewise to form $\pi -$bond.

Answer 2

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