How to compare them and which is more stable
Solution given by resonance:
Bond order of He_2^+ = 1/2
Some energy is released during the formation of He_2^+ from two isolated He atoms.
Abit related to this.
Just search helium
Bro a similar question was asked in one of our examinations in FIITJEE whereby they had compared a pair of gas molecule and gaseous molecular ions (I don't remember the exact question) and similar reasoning was given wrt bond order. My sir said that this is absolutely garbage but JEE keep liye kuch compromise karna padega so just learn the wrong thing for the test. JEE will not make such a mistake (and it is evident here since D is incorrect as per official answer key).
Why is it option C?
Shouldn't it be D ?
Coz C won't get filled !
Yeah the question actually doesn't seem clear
Wait is that ATP ? @Viraam_Rao
I actually dont know on what basis to compare?
In N2 the orbitals which r differently formed like in O2 are sigma * 2p , and pi* 2pz ,pi* 2py, that's likely what the question wants @Viraam_Rao bro
Ohh ok. That could be it.
I actually took this from a video and while discussing solution they were talking about orbitals being pure and hybrid but I couldn't understand.
As such for below 14 the energy levels r contrasting than greater than 14 only in these
But N2 and O2 mean difference of order comes with sigma and pi bonding right?
Yup , but when u write down the molecular configuration : energy levels bit differ in these only .
Haan. Then why answer is C ?
Shouldn't it be AB then? Cuz energy level order changes in AB?
Shouldn't it be D too ? @Viraam_Rao Coz D is not even getting filled in N2
Also how C ??
Option C remains unfilled in both N2 and O2 and I guess it has the same energy for both the molecules @Azimuddin_Sheikh @Viraam_Rao
I also think it should be AB then , language is bit unclear. Then C also @Mayank_Chowdhary bro.
Well how does unfilled tells u that both have same energy? @Mayank_Chowdhary bro I think it also differ , it should be ABCD
You can check their reasoning here:
Yeah you are correct @Azimuddin_Sheikh bro ... Energy will depend on the no. of filled electrons too
Wait what do they mean by pure pi orbitals ?
I mean why are they pure ?
Oh ... Now I get it !
Pi orbitals here are pure
This is because Pi orbitals are formed only from p/d orbitals only ( s can never form pi orbitals) and here only p orbital being present there is no question of hybridization
But still I am unable to understand how sigma will be hybrid and pure for N2 and O2 respectively