Final answer:
sp hybridization of carbon involves the mixing of one S and one P orbital to form two equivalent sp orbitals oriented 180° apart in a straight line, resulting in a linear geometry. This configuration allows the formation of σ-bonds using the sp orbitals and π-bonds using the remaining unhybridized p orbitals. It is crucial in determining the physical and chemical properties of organic molecules such as ethyne.
Step-by-step explanation:
sp Hybridization in Carbon
sp hybridization of carbon involves the mixing of one S orbital and one P orbital from the valence shell to form two sp hybrid orbitals. These orbitals are equivalent and arranged in a linear geometry 180° apart. This structure allows a carbon atom to form two σ-bonds with its sp orbitals, which results in a linear molecular shape, an example of which is the ethyne (HC=CH) molecule.
The unhybridized p orbitals are perpendicular to each other and to the axis of the sp orbitals, enabling the formation of two π-bonds around the sigma bond axis. This results in a linear geometry around the sp hybridized carbon. Moreover, the electrostatic map of such a molecule displays a red region around the C=C bond axis due to the presence of 7-electrons, indicating electron density, and shows the C-H bond in ethyne with a partial positive (Δ+) charge on the hydrogen atom due to its lower electronegativity compared to carbon.
The concept of hybridization helps explain the bonding and geometry of molecules, with sp2 hybridization and sp3 hybridization constituting other common forms. For instance, an sp2 hybridized carbon with one s and two p orbitals forms three hybrid orbitals in a trigonal planar geometry at 120° from each other. Contrastingly, an sp hybridized carbon atom's linear arrangement leads to unique physical and chemical properties that are crucial in organic chemistry.