Place the following molecular ions in order from smallest to largest bond order: [tex]C_2^{2+}, N^{2-}, O^{2-} and F^{2-}.[/tex][tex]1. F^{2-} \ \textless \ C_2^{2+} \ \textless \ O^{2-} \ \textless \ N^{2-}\\2. C_2^{2+} \ \textless \ N^{2-} \ \textless \ O^{2-} \ \textless \ F^{2-}\\3. C_2^{2+} \ \textless \ F^{2-} \ \textless \ O^{2-} \ \textless \ N^{2-}\\4. O^{2-} \ \textless \ C_2^{2+} \ \textless \ F^{2-} \ \textless \ N^{2-}\\5. F^{2-} \ \textless \ O^{2-} \ \textless \ N^{2-} \ \textless \ C_2^{2+}[/tex]

Bond order is a term used in chemistry to identify the number of electrons involved in making the bonding between two or more atoms in a molecule. Bond order is equal to half the difference between the number of bonds in the atoms minus the number of antibonds. Therefore, the correct order of bond order from smallest to largest is as follows:

1. F(2-): equals to 0.5 (it has 8 bonds and 7 antibonds)

2. C2(2+): equals to 1 (it has 4 bonds and 2 antibonds)

3. O(2-): equals to 2 (it has 8 bonds and 4 antibonds)

4. N(2-): equals to 2.5 (it has 8 bonds and 3 antibonds)