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 of an atom is determined by the number of sigma (\(\sigma\)) bonds it forms and the number of lone pairs on it.
Step 2: Key Formula or Approach:
Steric Number = (Number of sigma bonds) + (Number of lone pairs).
Steric Number 2 \(\rightarrow sp\); 3 \(\rightarrow sp^2\); 4 \(\rightarrow sp^3\).
Step 3: Detailed Explanation:
In Ethyne (\(H - C \equiv C - H\)):
1. Consider one carbon atom.
2. It forms one \(\sigma\) bond with a Hydrogen atom.
3. It forms a triple bond with the other Carbon atom. A triple bond consists of one \(\sigma\) bond and two \(\pi\) bonds.
4. Total sigma bonds for the carbon atom = 2.
5. Carbon has no lone pairs in this molecule.
6. Steric Number = \(2 + 0 = 2\).
7. Therefore, the hybridization is \(sp\).
Step 4: Final Answer:
The hybridization of carbon in ethyne is \(sp\).