Bond order for O2- = (8-5) / 2 = 1.5. Question: The Bond Order For O22+ Using Molecularorbital Theory, Please Explain How You Arrived At Your Answer. It contains 2 unpaired electrons and is paramagentic. In molecular orbital theory, bond order is also defined as the difference, divided by two, between the number of bonding and antibonding electrons; this often, but not always, yields the same result. Step 2: Draw the molecular orbital diagram. To find the bond order, just draw the molecular orbital energy diagrams and you can find it easily. The antibonding orbital is empty. ... 1 for O22- and 3 for O22+ The paramagnetism of O2 is explained by. ... For diatomic species are listed below, identify the correct order in which the bond order is increasing in them. Molecular Orbital Theory -- Homodiatomics use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-. In molecular orbital theory, bond order is also defined as half of the difference between the number of bonding and antibonding electrons. Bond order. Bond order = There are 10 bonding and 5 non-bonding electrons in the orbitals according to the molecular orbital configuration. Using MO theory, predict which of the following species has the shortest bond length? BOND ORDER of O2 is 2.0 bond order of O2+ is 2.5 bond order of O2- is 1.5 HARD aipmt. Thus, the bond order of is 2.5. B) The highest bond energy would be O2, because bond order is directly related to bond energy. Therefore, Bond order = = = = 2.5. Bond order = 1/2 (#e- in bonding MO - #e- in antibonding MO) For H 2, bond order = 1/2 (2-0) = 1, which means H 2 has only one bond. (2) The electronic configuration of O 2 + ion is K K (σ 2 s) 2 (σ ∗ 2 s) 2 (σ 2 p z ) 2 (π 2 p x ) 2 (π 2 p y ) 2 (π ∗ 2 p x ) 1 Its bond order is 2 8 − 3 = 2. Bond order for O2 2- = (8-6) / 2 = 1. 5. Bond order is also an index of bond strength, and it is used extensively in valence bond theory. Given that O2 is paramagnetic and has a bond order of 2, and its highest occupied molecular orbital is antibonding, what would be the expected bond orders for O22- and O22+? Step 3: Calculate the bond order of the molecule/ion. It contains 1 unpaired electron and is paramagnetic. If you use the Aufbau process to populate the sigma, pi, pi*, and sigma* orbitals of these species, you will find that F2+ has bond order 1.5, F2 has bond order 1.0, and F2- has bond order 0.5. The bond order tells us the stability of a bond: a higher bond order means the bond is more stable and stronger. Bond Order in Molecular Orbital Theory. Its bond order is 2 8 − 4 = 2. Assuming Covalent bonding between N a and C l, What is the expected bond order ? Again, in the MO, there is no unpaired electron, so H 2 is diamagnetic. Thus, H 2 is a stable molecule. 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