Use MO theory to predict the bond orders of the following ions.Which one do you predict does NOT exist?

Question

Quizplus · Accepted Answer

The bond order can be calculated using Molecular Orbital (MO) Theory by subtracting the number of electrons in antibonding orbitals from the number of electrons in bonding orbitals and then dividing by two. The given symbols seem to represent the molecular orbital diagrams for various diatomic species, but without a clear interpretation of the symbols, we can apply general principles. Typically, a bond order of zero indicates that the molecule does not have enough bonding interactions to exist as a stable molecule. The choice D, which seems to represent a diatomic molecule with a negative charge, is indicated as not existing likely due to a misinterpretation of the symbols or an error in the representation. However, without clear and standard molecular orbital diagrams or a more straightforward representation of the electron configurations, this explanation assumes a general understanding of MO theory principles where bond order correlates with stability.

Use MO Theory to Predict the Bond Orders of the Following