Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Chaste on September 20, 2008, 11:09:41 PM
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Can anyone explain that in terms of molecular energy level diagram preferably?
Thanks.
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Have you drawn the molecular orbital diagram for NO?
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yep yep I've drawn the MO diagram for NO. so I can drawn reference from your textual explanations.
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Do you notice anything strange about the MO diagram, such as unfilled levels or unpaired electrons?
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There is 1 unpaired electron at the pi* 2p hybridized orbital. Does that mean, that electron being in a higher enery antibonding orbital is unstable compared to the rest and requires less energy to get ionized?
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In general, compounds that contain an unpaired electrons (i.e. radical) are fairly unstable and have a preference for getting rid of the unpaired electron. Furthermore, the unpaired electron resides in an antibonding orbital which makes the electron destabilize the N-O bond.
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Thanks for replying.