CHEM 012 7

00 x 108 ms and is the wavelength in meters energy of

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Unformatted text preview: n, the lone pair (just one in this case) is influencing the angle between the bonded pairs, making it a liele smaller than the perfect tetrahedral angle. hep://www.elmhurst.edu/~chm/vchembook/205trigpyramid.html 16 9/29/11 Lewis Structure of Radicals •  Chemical species with an odd number of electrons are called radicals and will have an electron that is unpaired (i.e. not part of a lone pair or a bond) •  Examples: Cl, ClO, OH (don’t confuse with OH- !), NO •  These Lewis structures are created in the same manner that we discussed. The only complicaCon is that one must decide where the unpaired electron must be placed, and it is not always obvious. The OH radical •  Oxygen has 6 valence, hydrogen has one, so there are seven valence electrons •  Drawing the skeleton structure uses two electrons, so five remain for creaCng octets O H •  Here, hydrogen’s valence is already saCsfied (remember it can only hold two electrons) so the remaining five electrons must be placed on oxygen O H Owen this species will be shown as simply OH or OH•, omiyng the lone pairs. 17 9/29/11 NO2 •  Total valence electrons are 17 •  N is the central atom •  In this molecule, there is a quesCon about where the free electron should be placed –  Generally: the unpaired electron should go on C, O, hydrogen, or a halogen (Cl, F, Br) –  Unpaired electrons cannot be used in bonding •  Following the normal checklist will result in the free elect...
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