N2o4 Lewis Structure - How To Discuss
Sarah Scott
Published May 17, 2026
N2o4 Lewis Structure
Provide the Lewis structure, including the formal and resonant charges of N2O4, estimate the HÃ ° f in the gas phase at 25 ° C.
Use the table of binding enthalpies on page 311 of your text.
The details I used:
o = o 498.7
N ::: N 941.4
o = N 607
NN 193
No. 176
I have the answer +179.8
I think this is wrong because I got a negative answer to such a question.
I received an official rate of 0.
I have two different answers.
Many nitrogen compounds exhibit positive enthalpy changes due to strong bonds in elemental nitrogen.
Each nitrogen forms a bond with another, a double bond with oxygen, and a detachment bond with another. (The other S has a maximum of 8 electrons, so nitrogen, unlike pspre, cannot form 5 bonds)
I got the same result as BE, so we have to agree on the structure.
My database Delta says H f = + 9.2 kJ mol1.
This difference is due to the localization of electrons which stabilizes the molecule itself.
Lewis structure of N2o4
The problem is that NH2 has a charge of 1. The total number of valence electrons must be 8 (three of N, 1 of each H, and 1 of charge). Subtract 4 for each NH bond and you have 4 electrons left as two undivided pairs around N. The formal position in N is 1.
