The correct option is
A O+2<O2<O−2Bond length is inversely proportional to bond order
Bond length∝1Bondorder
Bond order can be foundd on apply molecular orbital theory in the given examples B.O=BMOelectron−ABMOelectron2
O+2 (Total electron=15)
⇒σ1s2,σ∗1s2σ2s2,σ∗2s2,σ2p2z,(π2p2xπ2p2y),(π∗2p1xπ∗2px)
B.O=6−12=2.5
O2 (Total electron=16)
⇒σ1s2,σ∗1s2σ2s2,σ∗2s2,σ2p2z,(π2p2xπ2p2y),(π∗2p1xπ∗2p1y)
B.O=6−22=2
O−2 (Total electron=17)
⇒σ1s2,σ∗1s2σ2s2,σ∗2s2,σ2p2z,(π2p2xπ2p2y),(π∗2p1xπ∗2p1y)
B.O=6−32=1.5
∴ Order of bond order=O−2<O2<O+2
Order of Bond length=O+2<O2<O−2