Question

The hybridization of carbon in ethene is: ____.

• A. sp
• B. sp²
• C. sp³
• D. dsp²

Hint:

A quick way to tell hybridization for Carbon: - Only single bonds $\rightarrow sp^3$ - One double bond $\rightarrow sp^2$ - One triple bond (or two double bonds) $\rightarrow sp$

Answer 1

The Correct Option is B

Step 1: Understanding the Concept:
Hybridization explains the mixing of atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds in valence bond theory.

Step 2: Detailed Explanation:
Ethene ($C_2H_4$) contains a carbon-carbon double bond ($C=C$).
• Each carbon atom in ethene is bonded to three other atoms (two hydrogens and one carbon).
• To form three sigma ($\sigma$) bonds, one $2s$ orbital mixes with two $2p$ orbitals, resulting in $sp^2$ hybridization.
• The three $sp^2$ hybrid orbitals are arranged in a trigonal planar geometry with bond angles of approximately 120°.
• The unhybridized $2p$ orbital on each carbon overlaps laterally to form the pi ($\pi$) bond.

Step 3: Final Answer:
The hybridization of carbon in ethene is $sp^2$.