The discussion revolves around the bonding characteristics of nitrogen, particularly focusing on how nitrogen forms bonds with its electrons in the 2p orbital and the implications for nitric oxide. Participants explore the mechanisms of bond formation, including the roles of different electron orbitals and the concept of bond order.
Participants express differing views on the number of bonds nitrogen forms and the role of the extra electron in nitric oxide. The discussion remains unresolved regarding the exact mechanisms and implications of these bonding characteristics.
Participants reference concepts such as bond order and molecular orbital theory, indicating that a deeper understanding of these topics may be necessary to fully grasp the discussion.
This discussion may be useful for students or individuals interested in molecular chemistry, particularly those studying the bonding behavior of nitrogen and its compounds.
Karan Punjabi said:Guys, I'm just thinking about how Nitrogen makes two bonds if it has 3 electrons in 2p orbital. I made a judgement that one electron from 2s orbital will transfer to one of 2p orbitals then there are two 2p orbitals which can make a bond? Is this correct or there is other mechanism?
DrStupid said:Nitrogen actually makes 3 bonds. 2 p-electrons form a sigma-bond and 2 x 2 p-electrons form 2 pi-bonds. The s-electrons are not binding.[/QUOTE
Yeah but what's happening in the case of Nitric oxide?
Can you just elaborate. Extra electron means tha nitrogen gains a electron then it makes a bond?DrDu said:In nitric oxide, you have one additional electron, so you will get a 3-electron pi bond which is about half as strong as a 2 electron pi bond. So you will get an overall bond order of 2.5.
Karan Punjabi said:Can you just elaborate. Extra electron means tha nitrogen gains a electron then it makes a bond?
Ohk to understand this concept should I first understand MOTDrStupid said:The extra electron populates an anti-binding pi orbital. It belongs to the molecule and not to nitrogen or oxygen only.