Recall Each Oxygen has 4 Electrons in its 2p bonding orbital. But Since it is 02- Total e- = 4(2)+1=9 Put 2 electrons in 2p, 4 in 2p with a remaining 3 electrons to be placed. By Aufbau principal, the next 3 electrons must go in the lowest energy state which would be 2p*. 3/4 electrons fill the 2p* leaving 1 unpaired. Bond order=(Bonding Electrons - Antibonding)/2 =(6-3)/2 B.O.=1.5 Therefore, we can conclude that O2- is relativly stable as it has 1 complete bond. It also has one unpaired electron in 2p* antibonding orbital which gives it paramagnetic properties. 2s and 1 s orbitals both have 2 electrons in bonding and antibonding orbitals if you draw them out, canceling out any bonds they might create. Only 9 electrons play a significant role in the bonding of O2- Solution Recall Each Oxygen has 4 Electrons in its 2p bonding orbital. But Since it is 02- Total e- = 4(2)+1=9 Put 2 electrons in 2p, 4 in 2p with a remaining 3 electrons to be placed. By Aufbau principal, the next 3 electrons must go in the lowest energy state which would be 2p*. 3/4 electrons fill the 2p* leaving 1 unpaired. Bond order=(Bonding Electrons - Antibonding)/2 =(6-3)/2 B.O.=1.5 Therefore, we can conclude that O2- is relativly stable as it has 1 complete bond. It also has one unpaired electron in 2p* antibonding orbital which gives it paramagnetic properties. 2s and 1 s orbitals both have 2 electrons in bonding and antibonding orbitals if you draw them out, canceling out any bonds they might create. Only 9 electrons play a significant role in the bonding of O2-.