What is the bond angle in a tetrahedral molecular shape?

A tetrahedral molecular shape is characterized by a central atom bonded to four other atoms that are positioned at the corners of a tetrahedron. In this arrangement, all bond pairs repel each other equally due to the principles of VSEPR (Valence Shell Electron Pair Repulsion) theory. This equal repulsion results in the bond angles between each pair of bonds being approximately 109.5 degrees.

This specific angle allows for the most stable arrangement of atoms around the central atom, minimizing repulsions among the electron pairs. Such examples include molecules like methane (CH₄), where the carbon atom is at the center with hydrogen atoms at the corners of the tetrahedron.

The other angles listed, such as 120° or 90°, represent different geometries, such as trigonal planar or octahedral arrangements, and thus do not apply to tetrahedral molecular shapes.