In nitrosobenzene, there are two ways that the $\ce{-N=O}$ group can show mesomeric effect.

  1. It can show positive mesomeric effect by becoming $\ce{=N+=O}$
  2. It can show negative mesomeric effect by becoming $\ce{=N-O-}$

So will the electron density on the benzene ring increase or decrease?

I think it should decrease because in the first case we have a $\delta^+$ charge on nitrogen and a $\delta^-$ charge on carbon, and in the other case we have a $\delta^+$ charge on carbon and a $\delta ^-$ charge on oxygen.Is this reasoning correct? Or will there even be such an decrease?

  • $\begingroup$ hint: try drawing the resonance structures for the full benzene ring in each case. $\endgroup$ Commented May 23, 2020 at 7:17
  • $\begingroup$ $NO$ can show both ±M effect, however -M effect is stronger. It is a deactivating group, yet ortho para directing towards EAS. Have a look at chemistry.stackexchange.com/questions/57044/… $\endgroup$
    – user600016
    Commented May 23, 2020 at 17:01

1 Answer 1


Your reasoning is not quite correct. Since electron density on $\ce{N=O}$ bond is more around $\ce{O}$ than $\ce{N}$ (electronegativity of $\ce{O}$ is greater than that of $\ce{N}$), $\ce{N}$ should have a slight $\delta+$ charge, which demands electrons from adjacent $\pi$-system. As a result, the electron density on the phenyl nucleus of nitrozobenzene is less compared to that of benzene. This phenomena is shown as a ring deactivating factor. However, this fact may be hard to prove practically because of the instability of nitrozobenzene.

Yet, in computational studies, one set of descriptors of electron structure of aromatic compounds may come from the pEDA/sEDA approach (Ref.1). The pEDA and sEDA descriptors are defined as populations of the $\pi$- and $\sigma$-orbital electrons, respectively, in a given planar molecule or its planar part (Ref.1 & Ref.2):

Dependence of pEDA(Ring) on sEDA(Ring)

The abstract of Ref.2 states that:

An application of quantum chemical modeling allowed us to investigate a substituent effect on a $\sigma$ and $\pi$ electron structure of a ring and the nitro group in a series of meta- and para-$\ce{X}$-substituted nitrobenzene derivatives ($\ce{X =}$ $\ce{NMe2}$, $\ce{NHMe}$, $\ce{NH2}$, $\ce{OH}$, $\ce{OMe}$, $\ce{Me}$, $\ce{H}$, $\ce{F}$, $\ce{Cl}$, $\ce{CF3}$, $\ce{CN}$, $\ce{CHO}$, $\ce{COMe}$, $\ce{CONH2}$, $\ce{COOH}$, $\ce{NO2}$, and $\ce{NO}$). The obtained pEDA and sEDA parameters (the $\pi$- and $\sigma$-electron structure characteristics of a given planar fragment of the system obtained by the summation of $\pi$- and $\sigma$-orbital occupancies, respectively) of the $\ce{NO2}$ group and the benzene ring allowed us to reveal the impact of the substituents on their mutual relations as well as to analyze them from the viewpoint of substituent characteristics. The decisive factor for dependence of pEDA on sEDA of the ring is electronegativity of the atom linking the substituent with the ring; in subgroups an increase of sEDA is associated with a decrease of pEDA. The obtained mutual relation between pEDA($\ce{NO2}$) and pEDA(ring) characteristics documents strong resonance interactions for electron-donating substituents in the para position. The observed substituent effect on the $\sigma$-electron structure of the nitro group, sEDA($\ce{NO2}$), is significantly greater (∼1.6 times) for meta derivatives than for the para ones.

Although, there is no general correlation between these two contributions, pEDA(ring) and sEDA(ring), to the description of the electronic structure of the transmitting ring, it's worth comparing effect of $\ce{NO}$ substituent with the known effect of $\ce{NO2}$. It is clearly the population of the $\pi$-electrons are lower in nitrobenzene when $\ce{NO}$ group substituted in para- or meta-position of it compared to that of second $\ce{NO2}$ group substituted in either position (see $\color{green}{\text{green circle}}$ of the plot). Both $\ce{NO}$ and $\ce{NO2}$ groupd have shown $\pi$-electon withdrawing effects on the ring compared to nitrobenzene itself ($\ce{X = H}$; $\color{blue}{\text{blue circle}}$). Therefore, it is safe to say that the electron density on the phenyl ring decreases in nitrozobenzene compared to that of benzene. This conclusion is supported by the positive Hammett substituent constant ($\sigma$-value) listed for $\ce{NO2}$ substituent in benzoic acid: $\sigma_{p-\ce{NO}} = 0.91$ and $\sigma_{m-\ce{NO}} = 0.91$. By comparison, $\sigma_{p-\ce{NO2}} = 0.78$ and $\sigma_{m-\ce{NO2}} = 0.71$ (The authors referred Ref.3 for these $\sigma$-values).


  1. Halina Szatylowicz, Anna Jezuita, Tadeusz M. Krygowski, “On the relations between aromaticity and substituent effect,” Structural Chemistry 2019, 30, 1529–1548 (https://doi.org/10.1007/s11224-019-01360-7).
  2. Halina Szatylowicz , Anna Jezuita, Krzysztof Ejsmont, Tadeusz M Krygowski, “Substituent Effect on the σ- And π-Electron Structure of the Nitro Group and the Ring in Meta- And Para-Substituted Nitrobenzenes,” J. Phys. Chem. A 2017, 121(27), 5196-5203 (https://doi.org/10.1021/acs.jpca.7b03418).
  3. Corwin Hansch, A. Leo, R. W. Taft, “A survey of Hammett substituent constants and resonance and field parameters,” Chem. Rev. 1991, 91(2), 165–195 (https://doi.org/10.1021/cr00002a004).
  • $\begingroup$ My teacher just told me that whenever a substituent shows both +M and -M effect, we should just take the -M effect. Is that true? $\endgroup$ Commented May 25, 2020 at 4:25
  • $\begingroup$ Not necessarily. $\endgroup$ Commented May 25, 2020 at 4:44

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