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. Using MO theory, predict which of the following species has the shortest bond length? It contains 2 unpaired electrons and is paramagentic. Bond order for O2- = (8-5) / 2 = 1.5. Assuming Covalent bonding between N a and C l, What is the expected bond order ? BOND ORDER of O2 is 2.0 bond order of O2+ is 2.5 bond order of O2- is 1.5 Its bond order is 2 8 − 4 = 2. To find the bond order, just draw the molecular orbital energy diagrams and you can find it easily. For a straightforward answer: use this formula: Bond order = [(Number of electrons in bonding molecules) - (Number of electrons in antibonding molecules)]/2. (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. Molecular orbital energy level diagram of CO molecule can be given as. The antibonding orbital is empty. Bond order. 5. a double bond is shorter than a single bond), so the order is F2+ < F2 < F2- from shortest to longest. Bond Order in Molecular Orbital Theory. Again, in the MO, there is no unpaired electron, so H 2 is diamagnetic. 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. In molecular orbital theory, bond order is also defined as half of the difference between the number of bonding and antibonding electrons. It contains 1 unpaired electron and is paramagnetic. 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. Question: The Bond Order For O22+ Using Molecularorbital Theory, Please Explain How You Arrived At Your Answer. 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. Bond order = There are 10 bonding and 5 non-bonding electrons in the orbitals according to the molecular orbital configuration. B) The highest bond energy would be O2, because bond order is directly related to bond energy. Thus, H 2 is a stable molecule. The formula for bond order is as follows. Step 2: Draw the molecular orbital diagram. ... For diatomic species are listed below, identify the correct order in which the bond order is increasing in them. View Answer. molecular orbital theory. The bond lengths are inverse to the bond order (e.g. Bond order for O2 2- = (8-6) / 2 = 1. Molecular Orbital Theory -- Homodiatomics use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-. 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