Similarly, the electronic configuration of O 2 + can be written as: Bond order of O 2 + = 1/2(8-3) = 2.5 = paramagnetic . So the bond order of B2 is equal to 1, which you can get by drawing the molecular orbital diagram and performing the equation Bond Order = .5 * (# of bonding electrons - # of antibonding electrons). The bond order of NO- is 2.0. (σ2s)²(σ2s*)²(π2p)^4(σ2p)²(π2p*)³. Bond order is the number of bonds. How do you balance equation N2 plus O2 Yields N2O4? 2) O2 is stable molecule. Solution for For the O2, O2+, O2-, In each case (O2, O2+, O2-), calculate the bond order. The bond length in the oxygen species, O2+, O2, O2-, O2^(2-), can be explained by the positions of the electrons in molecular orbital theory. asked Jan 27 in Chemistry by SurajKumar ( 66.2k points) chemical bonding NO, or nitric oxide, is a diatomic gas vital for cell signalling in mammals, including us humans. Bond order =1/2(N b-N a) = 1/2(8-4) = 2 = Paramagnetic . Click here👆to get an answer to your question ️ Calculate the bond order of O2^+ To determine the bond order of a diatomic molecule such as H 2, CO or HCl, you simply look at the kind of bond involved and that is your answer. C2 is unstable "diatomic carbon" and if it exists, it will have a double bond and a bond order of 2. For a diatomic molecule e.g O2 has bond order two because O=O is a double bond. hope it helps:) So we have a total of 8 electrons in bonding orbitals and a total of 5 electrons in antibonding orbitals so we get. NO is produced when ammonia is oxidised. Na=number of electrons in antibonding orbitals Which one are paramagnetic? To get a negative charge on O2, you would have to have a single bond, so bond order is 1. Bond order is 3 in N2 since it has a triple bond. because not available for bonding. Nb=number of electrons in bonding orbitals. The stability of following species can be decided on the basis of bond order as follows: O2 : KK. I always thought bond order corresponded to the number of bonds. If you mean O2^-(O2 with a -1 charge) the bond order is 3/2. Assuming O2+ still has a double bond, then bond order is 2. A molecule of oxygen gas (O 2) has a double bond and a bond order of 2. However, when you draw the Lewis structure of B2, you get a triple bond. The electron configuration of the oxygen molecule must accommodate 16 electrons. Lewis structures are a bit sketchy for these. The electron configuration for the ion is. OF, or oxygen fluoride, is a compound used in toothpastes to get rid of plaque. Nb=number of electrons in bonding orbitals. The triple bond of CN gives it a bond order of 3. Bond order=(8-5)/2=3/2. A molecule of hydrogen gas (H 2) has single bond and a bond order of 1. Explain why the bond order of N2 is greater than N2^+, but the bond order of O2 is less than that of O2^+. Bond order=(Nb-Na)/2 where. Na=number of electrons in antibonding orbitals. 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