Final answer:
The inaccurate option according to the valence bond model is 'wavefunctions must have the same azimuthal quantum number to overlap'. The valence bond theory allows for the overlap of wavefunctions with different azimuthal quantum numbers, as seen with the hybridization in water molecules.
Step-by-step explanation:
According to the valence bond model, option c, 'wavefunctions must have the same azimuthal quantum number to overlap' is not a requirement of bonding. This statement is not accurate because atomic orbitals with different azimuthal quantum numbers can overlap and form bonds.
For instance, in the water molecule, the hybrid orbitals of oxygen, which are a mixture of s and p orbitals, overlap with the s orbitals of hydrogen atoms to form covalent bonds.
The valence bond theory explains that a covalent bond forms when there is an overlap of atomic orbitals that each contain an unpaired electron.
This model also incorporates the Pauli exclusion principle, which states that no two electrons in a molecule can have identical quantum numbers, and the concept of hybridization, which describes the mixing of atomic orbitals to form new orbitals that can lead to the correct molecular geometry.
However, certain aspects such as electron delocalization in molecules like benzene are not easily explained by valence bond theory and are better described by molecular orbital theory.
Additionally, the existence of stable polyatomic molecules and peculiar bond angles in molecules like water demonstrate that atomic orbitals alone are not sufficient to explain bonding in molecules, and the concept of hybrid orbitals is necessary.