Apply molecular orbital theory to predict which species has the strongest bond. apply molecular orbital theory to predict which species has the strongest bond. o+2 o−2 o2 all bonds are equivalent according to molecular orbital theory.

Explanation:

We must fill in the MO diagrams and calculate the bond orders for each species.  

1. O₂⁺

An O atom has six valence electrons, so two O atoms have 12 valence electrons.

O₂⁺ has lost an electron. In Figure 1, we give one O atom six electrons and the other atom five.

Then we add 11 electrons to the molecular orbitals, using the same rules as for atomic orbitals.

Bond order = (Bonding electrons – antibonding electrons)/2

BO = ½(B – A)

B = ½ (8 – 3) = 2.5

2. O₂

O₂ has 12 valence electrons, so we put 12 electrons in Figure 2 and calculate the bonding order.

B = ½ (8 - 4) = 2

3. O₂⁻

O₂⁻ has 13 valence electrons, so we put 13 electrons in Figure 3 and calculate the bonding order.

B = ½ (8 – 5) = 1.5

The species with the highest bond order has the strongest bonds.

O₂⁺ has the highest bond order, so has the strongest bonds.

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell