Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle. (a)



(b)



(c)

Verified step by step guidance

1. Identify the characteristic angles for each pair of hybrid orbitals: 45°, 80°, 120°, and 180°.
2. Recall the common hybridization angles: sp (180°), sp2 (120°), sp3 (109.5°), and other less common hybridizations.
3. Determine the hybridization for the 45° angle. Note that this angle is not typical for standard hybrid orbitals, suggesting no common hybridization.
4. Determine the hybridization for the 80° angle. This angle is also not typical for standard hybrid orbitals, suggesting no common hybridization.
5. Determine the hybridization for the 120° and 180° angles. The 120° angle corresponds to sp2 hybridization, and the 180° angle corresponds to sp hybridization.

Key Concepts

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that can accommodate bonding in molecules. The type of hybridization depends on the number of atomic orbitals mixed and the geometry of the resulting hybrid orbitals, which influences bond angles and molecular shape.

Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are determined by the arrangement of hybrid orbitals. Different types of hybridization lead to characteristic bond angles, such as 180° for sp hybridization, 120° for sp², and 109.5° for sp³, reflecting the geometry of the molecule.

Types of Hybridization

There are several types of hybridization, including sp, sp², and sp³, each corresponding to different geometrical arrangements. For example, sp hybridization results in linear geometry with a 180° bond angle, while sp² leads to trigonal planar geometry with 120° angles, and sp³ results in tetrahedral geometry with 109.5° angles.