Use molecular orbital theory to explain the magnetic behaviour and bond order of o2 negative and o2+ molecules
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there is a trick I would say to learn u ,, every even electron containing molecules except B2 and O2 are diamagnetic ....even electron containing O2 and B2 are only paramagnetic with total of even electron 16 and 10 respectively..other even electron containing are diamagnetic...and other odd electron molecules are paramagnetic...here we have by this trick => O2^- which contain total 17 electron which is odd , so it is paramagnetic .similarly for o2+ which contain 15 electron which is also paramagetic...
anand782000:
now coming back qith proper hint,,
we use to calculate bond order by 1/2( BMOe's - ABMOe's)
for o2+ no of electron in bmo is 6 and in abmo it is 1 so apply above formula and ur answer is 2.5 that is bond order for o2+'....similarly electron in bmo of o2- is 6 and that of abmo is 3 so apply above formula and get ur bond order 1.5
be tricky sometimes ,, it helps in exams
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