N2+ Hybridization: An Explanation

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N2+ is identified as having sp2 hybridization, which is scientifically valid. The electronic configuration of N2+ involves removing one electron from the nitrogen molecule, leading to discussions about its box configuration and hybrid orbitals. The hybridization of the nitrogen atom with a positive charge is debated, with some suggesting it results in sp hybridization. The choice of hybridization is subjective and not strictly governed by scientific laws. The bonding in N2+ is explained through the interaction of p_z orbitals forming a sigma bond, while p_x and p_y orbitals contribute to pi bonds. There is speculation that hybridization between s and p_z orbitals could enhance bond energy, but definitive conclusions require quantum chemical calculations.
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N2+ is sp2 hybridiztion (it is scientifically correct)
Can anyone explain this ?
 
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Write its electronic configuration, draw its box configuration and see if you can make a hybrid orbital by combining some valence orbitals.
 
i tried but the hybridization of atom N (with positive charge) comes out to be sp.
 
Do you mean N_2^+ or N^{2+}, to begin with?
 
N2+.nitrogen molecule with 1 electron removed.
 
The choice of the hybridization of an atom in a compound is a freedom you have and not something that is determined by some scientific law. Why do you want to use hybrids at all in the description of this molecule? s orbitals are full and don't contribute to bonding in a first approximation.
The two p_z orbitals along the molecule axis (z-axis) form a sigma bond and the rest of the electrons occupy the p_x and p_y orbitals forming a two and a one electron pi bond.
Maybe bond energy increases somehow if you allow for some hybridization between the s and the p_z orbitals. However without quantum chemical calculations, it is hard to say to what extent hybridization will increase bond energy.
 

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