*, *-antibonding molecular orbital o, -bonding molecular orbital Bond orderN-N N No. of electron in bonding MOs N No. of electron in antibonding MO's (g) Ifbond order 0, it means species does not exist. (h) Bond order of 1, 2 & 3 corresponds to a single bond, double & triple bond respectively. 0 Bond order stability of molecule 1 bond length 6) If the molecule has one or more unpaired electron, i will be paramagnetic, while if all the electrons are paired it will be diamagnetic. Ex H2-Configuration : (1s)2 * (1s)0 Bond order=Nb-Na 2-0 1, Hence H H (dimagnetic) 2 2
I S c Para , IS B
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