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 the difference, divided by two, between the number of bonding and antibonding electrons; this often, but not always, yields the same result. (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. Step 3: Calculate the bond order of the molecule/ion. Bond order. The bond order tells us the stability of a bond: a higher bond order means the bond is more stable and stronger. Its bond order is 2 8 − 4 = 2. For a straightforward answer: use this formula: Bond order = [(Number of electrons in bonding molecules) - (Number of electrons in antibonding molecules)]/2. Bond order for O2 2- = (8-6) / 2 = 1. Step 1: Calculate the total number of valence electrons present. Bond order for O2- = (8-5) / 2 = 1.5. Using MO theory, predict which of the following species has the shortest bond length? View Answer. Thus, the bond order of is 2.5. To find the bond order, just draw the molecular orbital energy diagrams and you can find it easily. 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. In molecular orbital theory, bond order is also defined as half of the difference between the number of bonding and antibonding electrons. ... For diatomic species are listed below, identify the correct order in which the bond order is increasing in them. The antibonding orbital is empty. a double bond is shorter than a single bond), so the order is F2+ < F2 < F2- from shortest to longest. It contains 2 unpaired electrons and is paramagentic. HARD aipmt. 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. molecular orbital theory. 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. The formula for bond order is as follows. Step 2: Draw the molecular orbital diagram. 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+? 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. The bond lengths are inverse to the bond order (e.g. It contains 1 unpaired electron and is paramagnetic. Question: The Bond Order For O22+ Using Molecularorbital Theory, Please Explain How You Arrived At Your Answer. 5. BOND ORDER of O2 is 2.0 bond order of O2+ is 2.5 bond order of O2- is 1.5 Therefore, Bond order = = = = 2.5. Bond Order in Molecular Orbital Theory. Molecular orbital energy level diagram of CO molecule can be given as. Bond order is also an index of bond strength, and it is used extensively in valence bond theory. ... 1 for O22- and 3 for O22+ The paramagnetism of O2 is explained by.