Which of the statements below is strictly INCORRECT regarding Molecular Orbital Theory?

• A. Molecular orbitals are formed by the linear combination of atomic orbitals.
• B. Bonding molecular orbitals are lower in energy than the corresponding antibonding molecular orbitals.
• C. The number of molecular orbitals always equals the number of atomic orbitals from which they are formed.
• D. Hybridizing two p orbitals with one s orbital yields three sp2 orbitals that form an equilateral triangle.

Answer: (D)

Verified step by step guidance

1. Understand the basics of Molecular Orbital Theory: Molecular orbitals are formed by the linear combination of atomic orbitals, and they can be classified as bonding or antibonding orbitals. Bonding orbitals are lower in energy compared to antibonding orbitals.
2. Recognize that the number of molecular orbitals formed is equal to the number of atomic orbitals combined. This is a fundamental principle of Molecular Orbital Theory.
3. Identify the incorrect statement: The statement about hybridizing two p orbitals with one s orbital to form three sp2 orbitals is related to Valence Bond Theory and hybridization, not Molecular Orbital Theory.
4. Clarify the concept of hybridization: In Valence Bond Theory, hybridization involves the mixing of atomic orbitals to form new hybrid orbitals. For example, mixing one s orbital with two p orbitals forms three sp2 hybrid orbitals, which are arranged in a trigonal planar geometry, not an equilateral triangle.
5. Conclude that the statement about hybridization is incorrect in the context of Molecular Orbital Theory, as it pertains to a different theoretical framework.