Which of the following is not consistent with the valence bond theory description of the formation of a chemical bond?

• A. Chemical bonds can form from the overlap of half-filled orbitals.
• B. Electrons forming chemical bonds are found only in quantum-mechanical atomic orbitals.
• C. Chemical bonds can form from the overlap of a completely filled orbital and an empty orbitals.
• D. The geometry of the overlapping orbitals determines the geometry of the molecule.

Answer: (B)

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1. Valence bond theory describes how chemical bonds form through the overlap of atomic orbitals. It emphasizes the importance of orbital overlap in bond formation.
2. According to valence bond theory, chemical bonds can form from the overlap of half-filled orbitals, where each orbital contributes one electron to the bond.
3. The theory also allows for the formation of bonds from the overlap of a completely filled orbital and an empty orbital, as long as the overlap is significant enough to allow for electron sharing.
4. The geometry of the overlapping orbitals is crucial in determining the geometry of the molecule, as the spatial arrangement of the orbitals influences the shape of the molecule.
5. The statement 'Electrons forming chemical bonds are found only in quantum-mechanical atomic orbitals' is inconsistent with valence bond theory, as it suggests a limitation that does not align with the theory's principles of orbital overlap and electron sharing.