Question

6. Use molecular orbital theory to predict the following properties of the F2 + ion: (a) electron configuration; (b) bond order; (c) magnetic character (paramagnetic or diamagnetic); (d) whether the bond length is longer or shorter than in the F2 molecule; (e) whether the bond strength is greater or less than in the F2 molecule. Use the M.O. diagram for F2 in Figure 10.13 of Tro, Fridgen and Shaw, 8 th edition as a starting point for this question.

Answer 1

Answer 2

In molecular orbital theory, the electronic structure of a molecule is described by forming molecular orbitals (MOs) from the combination of atomic orbitals (AOs) of the constituent atoms. For the F2+ ion, we need to consider the removal of one electron from the F2 molecule.

(a) Electron Configuration: The F2 molecule has a total of 14 valence electrons (7 electrons from each fluorine atom). When one electron is removed to form the F2+ ion, we subtract one electron, resulting in 13 valence electrons. These electrons will occupy the molecular orbitals based on their increasing energy levels, following the Aufbau principle.

(b) Bond Order: The bond order is calculated as (Number of bonding electrons - Number of antibonding electrons) / 2. By filling the molecular orbitals with the 13 valence electrons, you can determine the number of bonding and antibonding electrons. The bond order will indicate the stability and strength of the bond in the F2+ ion.

(c) Magnetic Character: To determine the magnetic character, you need to assess whether the molecule or ion has any unpaired electrons. If there are unpaired electrons, it will be paramagnetic, indicating attraction to a magnetic field. If all electrons are paired, it will be diamagnetic, showing no attraction to a magnetic field.

(d) Bond Length: In general, the bond length is determined by the internuclear distance between the two atoms. The removal of an electron from the F2 molecule to form the F2+ ion can affect the bond length. Factors such as the change in electron-electron repulsion and the change in nuclear charge can influence the bond length.

(e) Bond Strength: The bond strength is related to the bond dissociation energy, which is the energy required to break the bond. The removal of an electron and the formation of the F2+ ion can affect the bond strength. The change in electronic structure and the resulting changes in bonding and antibonding interactions can influence the bond strength.

To make more accurate predictions and provide specific values, it would be helpful to refer to the molecular orbital diagram for F2+ or access the specific diagram mentioned in the textbook.