Hybridization significantly influences bond angles in molecules by defining the spatial arrangement of electron pairs surrounding the central atom.

Hybridization is a key concept in molecular chemistry that refers to the combination of atomic orbitals to create new hybrid orbitals. These hybrid orbitals facilitate the formation of chemical bonds. The specific type of hybridization—such as $sp$, $sp^2$, $sp^3$, and so forth—dictates the molecular geometry and, consequently, the bond angles.

For example, in $sp$ hybridization, two hybrid orbitals are generated. These orbitals orient themselves linearly to minimize electron repulsion, resulting in a bond angle of $180^\circ$. This arrangement is exemplified by molecules such as BeCl$_2$.

In the case of $sp^2$ hybridization, three hybrid orbitals are formed. These orbitals arrange themselves in a trigonal planar configuration, leading to bond angles of $120^\circ$. This geometry is observed in molecules such as BF$_3$.

When considering $sp^3$ hybridization, four hybrid orbitals are produced. These orbitals adopt a tetrahedral arrangement, resulting in bond angles of $109.5^\circ$. An example of this type of hybridization can be seen in molecules like CH$_4$.

The concept of hybridization is closely associated with Valence Shell Electron Pair Repulsion (VSEPR) theory. According to VSEPR theory, electron pairs around a central atom position themselves to minimize repulsion, which ultimately determines the molecular shape and bond angles. The type of hybridization provides insight into the number of electron pairs surrounding the central atom, which in turn informs us about the molecule’s geometry.

In summary, hybridization is essential for understanding the bond angles in molecules. By identifying the type of hybridization, we can predict the molecular geometry and associated bond angles. This fundamental concept in chemistry enhances our comprehension of molecular structure and properties.