Question

The hybridization of carbon in ethyne ($C_2H_2$) is:

• A. $sp^3$
• B. $sp^2$
• C. $sp$
• D. $dsp^2$

Hint:

Single bond ($C-C$) $\rightarrow$ $sp^3$
Double bond ($C=C$) $\rightarrow$ $sp^2$
Triple bond ($C\equiv C$) $\rightarrow$ $sp$

Answer 1

The Correct Option is C

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. The type of hybridization depends on the number of sigma ($\sigma$) bonds and lone pairs around the atom.

Step 2: Detailed Explanation:
In ethyne ($H-C\equiv C-H$):
• Each carbon atom is bonded to one Hydrogen atom (one $\sigma$ bond) and one Carbon atom (one $\sigma$ bond and two $\pi$ bonds).
• Total number of $\sigma$ bonds per carbon = 2.
• There are no lone pairs on the carbon atoms.
• A total of 2 hybrid orbitals are needed, which corresponds to $sp$ hybridization.

Step 3: Final Answer:
The hybridization of carbon in ethyne is $sp$.