Na=number of electrons in antibonding orbitals Determining the bond order starting from a Lewis structure is a task that can range from very easy to rather difficult. Nb=number of electrons in bonding orbitals. Bond order=(8-5)/2=3/2. Bond Order. because not available for bonding. For example, the bonding molecular orbital of the oxygen molecule has eight valence electrons while the anti-bonding molecular orbital of the same molecule has four valence electrons. The electron configuration for the ion is. Calculate the bond order of: N 2, O 2,O 2 +,and O 2-. Bond order is 3 in N2 since it has a triple bond. Answer Bond order is defined as the number of covalent bonds in a covalent molecule.It is equal to one half of the difference between the number of electrons in the bonding & antibonding molecular orbitals. Draw the M.O diagram for oxygen molecule and calculate its bond order and show that O2 is paramagnetic. (σ2s)²(σ2s*)²(π2p)^4(σ2p)²(π2p*)³. Bond order in Oxygen molecule (O 2-2) =½ [(Number of bonding electrons) – (number of anti-bonding electrons)] = ½ [10 – 8] = 1 With the increase in number of electrons in anti-bonding orbital the stability and bond order of the molecule decreases. C2 is unstable "diatomic carbon" and if it exists, it will have a double bond and a bond order of 2. Bond order=(Nb-Na)/2 where. In a covalent bond between two atoms, a single bond has a bond order of one, a double bond has a bond order of two, a triple bond has a bond order of three, and so on. O2 2- bond order = 1 O2 - bond order = 1.5 O2 bond order = 2 O2+ bond order = 2.5 O2 2+ bond order =3 I hope it’ll work out :) So, the bond order of the oxygen molecule can be calculated as follows: Bond order = (Bonding electrons - Anti-bonding electrons) / 2. The first step should always be to draw out your molecules. The graphical representation presented in Fig. Thus Decreasing order of stability is: O 2 > O 2-> O 2-2. Graphical Presentation of Bond-Order. Nb=number of electrons in bonding orbitals. Bond order=(Nb-Na)/2 where. Bond order = (8 - 4) / 2 According to the chart, the covalent radius of carbon double bond is 67 picometers and that of oxygen double bond is 57 picometers. Na=number of electrons in antibonding orbitals. So we have a total of 8 electrons in bonding orbitals and a total of 5 electrons in antibonding orbitals so we get. Luckily, most cases you will encounter are the easy ones. 2) O2 is stable molecule. Therefore, the bond length of carbon dioxide is approximately 124 picometers (57 pm+ 67 pm). To determine the bond order between two covalently bonded atoms, follow these steps: Bond order is the number of bonding pairs of electrons between two atoms. To get a negative charge on O2, you would have to have a single bond, so bond order is 1. Lewis structures are a bit sketchy for these. hope it helps:) If you mean O2^-(O2 with a -1 charge) the bond order is 3/2. 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