Please explain how to solve this problem? Why can't option 2 be the answer?
@anag bond forms(bonding molecular orbital) because of combining orbital of same sign.. in (3) this type of overlapping is not possible because of axis of both orbitals.
I hope you got it.
Harshal Patil last edited by
@dikshant-gautam what about 4th option?? Can u pls clarify?
@harshal-patil In (4), overlapping will take place(as there axis are also same) but molecular bonding orbitals will form....
when opposite sign of orbital overlap it forms anti-bonding molecular orbitals and when same sign of molecular orbital overlap they form bonding molecular orbitals as you have read in MOT..
I HOPE YOU GOT THE CONCEPT.
Harshal Patil last edited by
@dikshant-gautam thank you very helpful👍
anag last edited by anag
@dikshant-gautam So is this wrong?
Here, same sign of orbital overlap is forming bonding orbital. Please explain.
I HOPE THIS WOULD HELP YOU.
@dikshant-gautam So that means
same sign: destructive interference?
opposite sign: constructive interference?
This pic is wrong?
@anag no,this pic is right..
@dikshant-gautam So in option 2 there is destructive interference.
But at the place where nodal plane is formed, there is no electron density. Isn't it?
@anag yes,there is destructive interference...
nodal plane will also form..
whats your doubt now?
@dikshant-gautam in option 3, one is s orbital (no specific direction) & the other is p orbital (has specific direction along a specific axis)? So there is no overlap? Please explain.
@anag In (3),s orbital has no specific axis(let its axis is x i.e we are considering it horizontally) then for p-orbital its axis would be y..since we know that overlapping is possible only for same axis (whether it is constructive or destructive).so,here overlapping is not possible..
you can also think as along x axis there is a nodal point in p- orbital.If there is no electron density then overlapping is also not possible...
I THINK YOU ARE GETTING MY POINT .IF NOT THEN LET ME KNOW...
@dikshant-gautam Thanks a lot. So is this pic wrong? There can be no overlap of s & p orbital?
But in option 2, there is a nodal plane (zero electron density). In the question, they want zero overlap, which is also zero electron density. So why is opt 2 wrong?
@anag I didn't said that overlapping is not possible.Its internuclear axis should be same like in this figure you have uploaded.
Acc. to you which would be your answer?
@dikshant-gautam If zero overlapping means overlapping is not possible, why isn't zero electron density.
Is electron of individual atom present but overlap (common region of presence of electron of both atoms) is absent? Please explain.
I had thought destructive interference will cause zero electron density at nodal plane in opt 2.
The conclusion of whole thing is that-
same sign of wave function- contructive interference
opposite sign of wave function-destructive interference
(considering inter nuclear axis)
And there is no. role of nodal plane.The question is simply to find zero overlapping.So don't go in wrong way.Nodal plane will form but after overlapping.