Diatomic oxygen has a single bond and two unpaired, unshared electrons. It isn't obvious to me why this should be, the two unpaired, unshared electrons should "pair and share", but they don't. I am told this is confirmed via their spectra.
I this is true, then
1) does that mean the two unpaired, unshared electrons are locked into the same spin as each other.
2) does that mean the oxygen molecule is magnetic
3) does that mean that oxygen molecule can be oriented in a strong magnetic field so that it won't effuse through holes too small for them to go through sideways. Nitrogen molecules do not have this unpaired, unshared electron phenomenon, so they would not orient in a magnetic field and they would effuse through the hole too small for them to go through sideways, because some of the molecules would randomly be oriented to go through longways.
Indeed, I have read that oxygen IS paramagnetic. Maybe this would work.
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