Molecular Orbital Theory -- Homodiatomics Use the molecularorbital model to fully describe the bonding in O2+, O2, O2-, andO22-. Determine which of the following statements are true andwhich are false.
The electron configuration of O2- is(σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)
The electron configuration of O2+ is(σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)
The number of unpaired electrons in O2+ and O22- is,respectively, 1 and 2.
The bond lengths increase in the order: O2+ < O2 < O2-< O22-.
The bond order in O2+ and O2 is, respectively, 2.5 and 2.
Bond length and bond energy both increase with increasing bondorder.
