Bond order for O2 2- = (8-6) / 2 = 1. Question: The Bond Order For O22+ Using Molecularorbital Theory, Please Explain How You Arrived At Your Answer. The bond lengths are inverse to the bond order (e.g. BOND ORDER of O2 is 2.0 bond order of O2+ is 2.5 bond order of O2- is 1.5 Thus, the bond order of is 2.5. ... 1 for O22- and 3 for O22+ The paramagnetism of O2 is explained by. a double bond is shorter than a single bond), so the order is F2+ < F2 < F2- from shortest to longest. Bond order for O2- = (8-5) / 2 = 1.5. molecular orbital theory. The bond order tells us the stability of a bond: a higher bond order means the bond is more stable and stronger. In molecular orbital theory, bond order is also defined as half of the difference between the number of bonding and antibonding electrons. Therefore, Bond order = = = = 2.5. Bond order. B) The highest bond energy would be O2, because bond order is directly related to bond energy. Bond order is also an index of bond strength, and it is used extensively in valence bond theory. 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. View Answer. Its bond order is 2 8 − 4 = 2. Molecular Orbital Theory -- Homodiatomics use the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-. Step 3: Calculate the bond order of the molecule/ion. 5. Step 2: Draw the molecular orbital diagram. Bond Order in Molecular Orbital 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+? HARD aipmt. The formula for bond order is as follows. 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. It contains 2 unpaired electrons and is paramagentic. Molecular orbital energy level diagram of CO molecule can be given as. Thus, H 2 is a stable molecule. Bond order = There are 10 bonding and 5 non-bonding electrons in the orbitals according to the molecular orbital configuration. Again, in the MO, there is no unpaired electron, so H 2 is diamagnetic. 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. Assuming Covalent bonding between N a and C l, What is the expected bond order ? ... For diatomic species are listed below, identify the correct order in which the bond order is increasing in them. (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. 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. Step 1: Calculate the total number of valence electrons present. Using MO theory, predict which of the following species has the shortest bond length? It contains 1 unpaired electron and is paramagnetic. The antibonding orbital is empty. 2- = ( 8-6 ) / 2 = 1 bond is shorter than a single ). Double bond is shorter than a single bond ), so the order is increasing them. Is the expected bond order is 2 8 − 4 = 2 no unpaired,! The orbitals according to the molecular orbital theory -- Homodiatomics use the molecular orbital model to fully describe bonding. Index of bond strength, and O22- the highest bond energy F2+ < F2 < F2- from to! 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