Carbon's ability to form a vast array of molecules stems from its hybridization. With four valence electrons, carbon can achieve a stable octet through hybridization, where atomic orbitals combine to form new hybrid orbitals. The most common types are sp, sp2, and sp3. sp hybridization involves one s and one p orbital, creating two linear hybrid orbitals with 180° bond angles, as seen in alkynes. sp2 hybridization uses one s and two p orbitals, resulting in three trigonal planar hybrid orbitals with 120° bond angles, found in alkenes. Finally, sp3 hybridization combines one s and three p orbitals, producing four tetrahedral hybrid orbitals with 109.5° bond angles, typical of alkanes. The type of hybridization dictates the molecular geometry and influences the molecule's reactivity and properties. For instance, the stronger sigma bonds in sp hybridized carbons lead to higher bond energies and less reactivity compared to sp3 hybridized carbons.
What is the hybridization of carbon atoms in ethyne (acetylene, C2H2)?
Which hybridization results in a tetrahedral geometry around the carbon atom?
In which type of hybridization are the hybrid orbitals arranged in a trigonal planar geometry?
What is the bond angle between the hybrid orbitals in a molecule with sp3 hybridized carbon atoms?