The correct option is C O+2,O2 - Both paramagnetic
The molecular orbital configurations of O+2,O−2,O2−2 and O2 are
O+2=σ1s2,∗σ1s2,σ2s2,∗σ2s2,σ2p2z,π2p2x
≈π2p2y,∗π2p1x≈∗π2p0y
O−2=σ1s2,∗σ1s2,σ2s2,∗σ2s2,σ2p2z,π2p2x
≈π2p2y,∗π2p2x≈∗π2p1y
O2−2=σ1s2,∗σ1s2,σ2s2,∗σ2s2,σ2p2z,π2p2x
≈π2p2y,∗π2p2x≈∗π2p2y
O2=σ1s2,∗σ1s2,σ2s2,∗σ2s2,σ2p2z,π2p2x
≈π2p2y,∗π2p1x≈∗π2p1y
and the electronic configuration of O and O+ are
O=1s2,2s2,2p2x,2p1y,2p1z
O+=1s2,2s2,2p1x,2p1y,2p1z
As O+2,O2,O−2,O andO+ have unpair electrons, hence are paramagnetic.