N2 vs. O2

N2 vs. O2 - not represented well by a Lewis structure....

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Chem 101 Discussion Board for Science Salon O 2 vs. N 2 So, liquid N 2 and liquid O 2 were both poured over a magnet. The liquid N 2 poured right through. The liquid O 2 was attracted to the magnet and was held between the poles of the magnet until it evaporated. Now what you may not know is that paramagnetism is a property of materials that have unpaired electrons. 1. Fe is magnetic. Draw the electron configuration of Fe in an orbital diagram. How many unpaired electrons does Fe have? 2. Draw the Lewis structures of N 2 and O 2 . How many unpaired electrons do they have? 3. We have seen that Lewis structures don’t always give us the best representations of molecules. This is another example where the actual property of a molecule is
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Unformatted text preview: not represented well by a Lewis structure. Molecular orbital theory is a different theory of orbitals and bonding than the bonding theory we have been discussing in class. Below are the molecular orbitals for N 2 and O 2 in this other theory. (I know weird huh.) Put valence electrons in the orbitals for N 2 and O 2 . How many unpaired electrons do they have? N 2 __ __ __ __ __ __ __ __ 2s * 2s 2p 2p * 2p * 2p O 2 __ __ __ __ __ __ __ __ 2s * 2s 2p 2p * 2p * 2p 4. Any comments on the ping-pong ball of flame? How would the fire have compared if we had immersed the ball in N 2 , instead of O 2 ? Thank you Ashley!...
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This note was uploaded on 03/08/2012 for the course CHEM 101 taught by Professor Anderson,w during the Fall '08 term at BYU.

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