Use MO theory to predict the bond orders of the following molecular ions. Which one do you predict does not exist? A)N₂ + B)O₂⁺ C)C₂⁺ D)F₂^2- E)O₂^2-

Question

Quizplus · Accepted Answer

The molecular ion in option D has an odd number of electrons, which leads to an unpaired electron in the molecular orbital diagram. This would make the ion paramagnetic and less stable. Therefore, option D is predicted to not exist. The other molecular ions have an even number of electrons and would have stable bonding interactions, leading to predicted bond orders of 1 or 2.

Use MO Theory to Predict the Bond Orders of the Following