Among the oxides of nitrogen,N_2O,NO,and NO_2 | vedclass

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(B) To determine which molecules have unpaired electrons,we count the total number of valence electrons:$1. N_2O$: Total electrons = $(2 	imes 7) + 8

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$NO$ and $NO_2$

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(B) To determine which molecules have unpaired electrons,we count the total number of valence electrons:$1. N_2O$: Total electrons = $(2 	imes 7) + 8 = 22$ (even number,all electrons are paired).$2. NO$: Total electrons = $7 + 8 = 15$ (odd number,contains one unpaired electron).$3. NO_2$: Total electrons = $7 + (2 	imes 8) = 23$ (odd number,contains one unpaired electron).Therefore,$NO$ and $NO_2$ are paramagnetic due to the presence of unpaired electrons.

Among the oxides of nitrogen,$N_2O$,$NO$,and $NO_2$,molecules with unpaired electrons are:

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