which of the following are predicted by the molecular orbital model to be stable diatomic species N22-, O22-, F22-

Lying Larry says it's none of them because he doesn't believe in the elements.

N22-

The stability of diatomic species can be predicted using the molecular orbital model. In this model, we consider the combination of atomic orbitals to form molecular orbitals. If the molecular orbitals are lower in energy compared to the atomic orbitals from which they are formed, the diatomic species is predicted to be stable.

Now, let's analyze each of the species:

1. N22-:
The atomic number of nitrogen is 7, so the electronic configuration of a neutral nitrogen atom is 1s^2 2s^2 2p^3. When two nitrogen atoms combine to form N2, they share six electrons and form a triple bond. In the molecular orbital model, N22- would have two extra electrons. The additional electrons would occupy the antibonding π*2p orbital, resulting in an unpaired electron. Therefore, N22- is not predicted to be stable according to the molecular orbital model.

2. O22-:
The atomic number of oxygen is 8, so the electronic configuration of a neutral oxygen atom is 1s^2 2s^2 2p^4. When two oxygen atoms combine to form O2, they share six electrons and form a double bond. In the molecular orbital model, O22- would have two extra electrons. The additional electrons would occupy the antibonding π*2p orbitals, resulting in two unpaired electrons. Therefore, O22- is not predicted to be stable according to the molecular orbital model.

3. F22-:
The atomic number of fluorine is 9, so the electronic configuration of a neutral fluorine atom is 1s^2 2s^2 2p^5. When two fluorine atoms combine to form F2, they share six electrons and form a single bond. In the molecular orbital model, F22- would have two extra electrons. The additional electrons would occupy the antibonding 2p orbitals, resulting in two unpaired electrons. Therefore, F22- is not predicted to be stable according to the molecular orbital model.

In summary, none of the diatomic species N22-, O22-, or F22- are predicted to be stable according to the molecular orbital model.

To understand which of the diatomic species N22-, O22-, and F22- are predicted to be stable according to the molecular orbital (MO) model, we need to analyze their electronic configurations and the relative energies of their molecular orbitals.

The molecular orbital theory defines bonding and antibonding molecular orbitals that result from the combination of atomic orbitals. In a stable diatomic molecule, the electrons occupy the bonding molecular orbitals, which are lower in energy, resulting in a net stabilizing effect.

Let's evaluate each species individually:

1. N22-:
The molecular orbital diagram for N2 molecule (neutral form) shows that there are three electrons in the π2px* and π2py* antibonding molecular orbitals. Therefore, if we add two more electrons to form N22-, they will occupy the lower-energy π2px and π2py bonding molecular orbitals, resulting in a fully filled bonding and antibonding orbitals. This gives a bond order of 3/2 [(5-3)/2], suggesting that N22- is predicted to be stable according to the MO model.

2. O22-:
In the O2 molecule (neutral form), there are two electrons in the π2px* antibonding molecular orbital. Adding two more electrons to form O22- will fill up this antibonding orbital, resulting in a bond order of 0 [(6-4)/2]. This indicates that there are equal numbers of bonding and antibonding electrons, which suggests that O22- is not stable according to the MO model.

3. F22-:
The F2 molecule (neutral form) has an electron configuration with a lone pair on each fluorine atom in the σ2s orbital. Adding two more electrons to form F22- will fill up this σ2s bonding orbital and result in a bond order of 1/2 [(7-5)/2]. This means that F22- has a partially filled bonding molecular orbital and is predicted to be stable according to the MO model.

In summary, according to the molecular orbital model, N22- and F22- are predicted to be stable diatomic species, whereas O22- is not stable.