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.

N2o4 Lewis Structure