Answer
The correct answer is option b: $Be_{2}, B_{2}, Ne_{2}$.
The molecular orbital (MO) model predicts the stability of diatomic species based on the filling of the available molecular orbitals. The stability of a diatomic species is determined by the net bond order, which is the difference between the number of bonding and antibonding electrons.
Work Step by Step
a. $N_{2}^{2-}, O_{2}^{2-}, F_{2}^{2-}$:
These species are not predicted to be stable by the MO model. The addition of extra electrons to the neutral diatomic molecules (N$_2$, O$_2$, F$_2$) would result in a net antibonding configuration, leading to instability.
b. $Be_{2}, B_{2}, Ne_{2}$:
These species are predicted to be stable by the MO model:
- $Be_{2}$ has a net bond order of 1, making it a stable diatomic species.
- $B_{2}$ has a net bond order of 1, making it a stable diatomic species.
- $Ne_{2}$ has a net bond order of 0, which corresponds to a stable non-bonding configuration.
Therefore, the diatomic species predicted to be stable by the molecular orbital model are $Be_{2}, B_{2}, Ne_{2}$.
