Question

What is the hybridization of carbon in an Ethyne (\(\mathrm{C_2H_2}\)) molecule?

• A. \(sp^3\)
• B. \(sp^2\)
• C. \(sp\)
• D. \(sp^3d\)

Hint:

Number of sigma bonds around carbon determines hybridization: 2 sigma bonds \(\rightarrow sp\), 3 sigma bonds \(\rightarrow sp^2\), 4 sigma bonds \(\rightarrow sp^3\).

Answer 1

The Correct Option is C

Concept: Hybridization describes the mixing of atomic orbitals to form equivalent hybrid orbitals. In the ethyne molecule (\(\mathrm{C_2H_2}\)), each carbon atom forms a triple bond with another carbon atom and a single bond with hydrogen.

Step 1: Determine the bonding around carbon. Each carbon forms:
• One \(\sigma\)-bond with hydrogen
• One \(\sigma\)-bond with the other carbon
• Two \(\pi\)-bonds between the carbon atoms

Step 2: Count the regions of electron density. Each carbon has two regions of electron density (two \(\sigma\)-bonds).

Step 3: Identify the hybridization. Two regions of electron density correspond to \(sp\) hybridization, giving a linear geometry with a bond angle of \(180^\circ\).