The discussion centers on the energy diagram for hybridized oxygen in carbon monoxide (CO). Participants clarify that oxygen has six electrons, yet the diagram displays only five, leading to confusion. The correct interpretation involves understanding bonding and anti-bonding orbitals, particularly in relation to the molecular orbital (MO) diagram for CO, which is isoelectronic to N2. The exercise aims to illustrate the energy splitting due to hybridization of s and p orbitals, although the necessity of hybridization for diatomic molecules like CO is questioned.
PREREQUISITESChemistry students, educators, and anyone interested in molecular orbital theory and hybridization concepts in diatomic molecules.
..., unless, it's for bonding electrons from both carbon and oxygen? Seem to recall some sort of quasi-quantum mechanical argument for "bonding/anti-bonding orbitals."TeethWhitener said:
