why the bond order N2 is greater than N2+
Answers
bond order depend on number of anti bonding electron if anti bonding electron or is more molecule become less stable like N2plus (or any molecules) so it is less stable
and bond order is less
bond order =(no of bonding electron - no of anti bonding electron )/2
above equation it is shown that if anti bonding electron is more bond order is less and bonding electron is more then bond order is more
in N2 molecule
anti bonding electron=6
bonding=8
in N2PLUS plus
anti bonding=6
bonding=6
in N2 and N2+ it is observed that anti bonding electron is same but bonding electron of N2is more than N2+ so It depend on factor of bonding electron and N2 is more stable
The bond of N2 is greater than N2+ because, N2 is neutral so, it does not attract other atoms but N2+ has a net positive charge so, it attracts the atom with net negative charge and that's why the bond of N2+ is not stable.
The bond order of O2 is less than that of O2+ because, O2 has a net negative charge so, it accepts electrons but, on the other hand O2+ does not accept but loses electrons and in this condition, O has 4 electrans on its outermost shell and with 4 electrons at its outermost shell an atom is partially stable.
[ Sorry! I did not follow the second part of the question so, I had to edit it.]