Hybridization of orbitals depends on what aspect of a molecule?

The hybridization of orbitals in a molecule is determined by the electronic arrangements and the way atoms share electrons to form bonds. When atoms come together to form molecules, their atomic orbitals can mix or "hybridize" to create new hybrid orbitals that can effectively explain the structure and bonding properties of the molecule.

This process is influenced by the number of electron pairs surrounding a central atom, including both bonding pairs (shared between atoms) and lone pairs (non-bonding pairs that affect the shape of the molecule). Understanding the electronic geometry—defined by the spatial arrangement of all electron pairs around the central atom—provides insights into how orbitals will hybridize. For example, if there are four regions of electron density around a central atom, the atom typically undergoes sp³ hybridization, resulting in a tetrahedral arrangement.

In contrast, aspects such as molecular mass, shape, type of chemical bonds, and thermal stability do not directly dictate how orbitals hybridize, although they can be influenced by the hybridization model. Thus, the dependency on electronic geometries and electron sharing makes this answer the most accurate in the context of understanding molecular structure and bonding.