Chapter 9 Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals - 9-3 Molecular Orbital Theory - Review & Check for Section 9-3 - Page 365: 4

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Oxygen has six valence electrons, so these species have 11 to 14 valence electrons respectively: $O_2^+$ $[core]\ (\sigma_{2s})^2\ (\sigma_{2s}^*)^2\ (\sigma_{2p})^2\ (\pi_{2p})^4\ (\pi_{2p}^*)^1\ (\sigma_{2p}^*)^0$ $B.O.=(N.\ Bonding -N.\ Antibonding)/2$ B.O.=5/2=2.5 $O_2^{2-}$ $[core]\ (\sigma_{2s})^2\ (\sigma_{2s}^*)^2\ (\sigma_{2p})^2\ (\pi_{2p})^4\ (\pi_{2p}^*)^4\ (\sigma_{2p}^*)^0$ $B.O.=(N.\ Bonding -N.\ Antibonding)/2$ B.O.=2/1=1 $O_2^+$ will have the shortest bond length because it has the highest bond order.