Molecular Orbital Theory -- Homodiatomics 1 Use the molecular orbital model to fully describe the bonding in O2+, 02, 02

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Molecular Orbital Theory Homodiatomics 1 Use The Molecular Orbital Model To Fully Describe The Bonding In O2 02 02 1 (99.73 KiB) Viewed 147 times

Molecular Orbital Theory -- Homodiatomics 1 Use the molecular orbital model to fully describe the bonding in O2+, 02, 02 ; and 022-. Determine which of the following statements are true and which are false. true v The number of unpaired electrons in O2 and O2 is, respectively, 1 and 0. false v The electron configuration of O2 is (02)2(025*)2(02p)2 (12p)4(120*)1. true v The bond order in O2 and 022-is, respectively, 1.5 and 1. false v Bond length and bond energy both increase with increasing bond order. The electron configuration of O2 is (02s)?(025*)-(2p)?(n2p)^(n2p*34. false v The bond energies increase in the order: Oz+ < 02 < Oz: < 022-. 2s <