Concept:Ethyne has a linear geometry, which corresponds to
sp hybridization on each carbon atom.
Explanation:In ethyne, each carbon atom forms two sigma bonds: one to hydrogen and one to the other carbon atom.
To form these two sigma bonds, one
2s orbital mixes with one
2p orbital.
This mixing produces two equivalent
sp hybrid orbitals.
The two hybrid orbitals arrange themselves as far apart as possible, giving a bond angle of
180∘.
The two remaining unhybridized
2p orbitals on each carbon overlap side-by-side to form two pi bonds.
Therefore, the carbon-carbon bond in ethyne is a triple bond: one sigma bond and two pi bonds.
This linear arrangement confirms that the hybridization scheme is
sp.
Answer:The hybridization scheme in ethyne is
sp, so the correct option is A.