Which bond angle is associated with sp hybridization?

The bond angle associated with sp hybridization is indeed 180 degrees. This type of hybridization occurs when one s orbital and one p orbital combine to form two equivalent sp hybrid orbitals. These sp hybrid orbitals are arranged in a linear geometry, which maximizes their distance from each other to minimize electron pair repulsion, leading to a straight line formation.

In a molecule with sp hybridization, such as acetylene (C2H2), the two sp hybrid orbitals are oriented 180 degrees apart. This configuration allows for the formation of strong sigma bonds with other atoms. The linear shape is a fundamental characteristic of molecules with sp hybridization, clearly defining the angle associated with this type of bonding.

Other bond angles like 120 degrees, 109.5 degrees, and 90 degrees correspond to different types of hybridization. For instance, 120 degrees is typical of sp² hybridization, where three hybrid orbitals are arranged in a trigonal planar shape, while 109.5 degrees corresponds to sp³ hybridization, which involves four orbitals arranged tetrahedrally. The 90 degrees angle usually pertains to d orbital involvement in sp³d hybridization, common in certain transition metal compounds. Thus, 180