Odd looking carbocation stability order [duplicate]








**This question already has an answer here**:
 
 




[Confused about carbocation stability](/questions/37427/confused-about-carbocation-stability)

 (1 answer)
 

Closed 3 years ago.



I am studying introductory organic chemistry, suddenly this one started looking odd, 


The carbocation stability for three compounds as given by my book is shown below, 


[![enter image description here](https://i.stack.imgur.com/Wy4Za.png)](https://i.stack.imgur.com/Wy4Za.png)


Let me call those as compounds **A>B>C** as given in image. It is very well known that 'N' and 'O' are electron withdrawing group(shows **-I effect**) and they can also show **+M effect**( some texts call it as Resonance effect ) by delocalising their lone pair over the vacant p-orbital of the carbocation. 


Now all i want to know is, How to decide whether **+M effect** or **-I effect** will operate in this case? If I consider only inductive effects, the order would be **C>A>B** which is wrong in this case. 


One part of my text book says that **+M effect > -I effect** (in more than 99% of cases). But then too the next question arises, why **+M effect** of 'N' is more than that of 'O'?


I got stuck in this one and i am now asking whether such questions are feasible without conducting experiments.


Explanation with the principles which are familiar to my level would be nice.





> 
> How to decide whether +M effect or -I effect will operate in this case?
> 
> 
> 


The extent of stabilizing effect follows the order: $\ce{\text{Mesomeric} > \text{Hyperconjugation} > \text{Inductive}}$. 


In general, this order is based on extent of $\ce{e-}$ transfer. In mesomeric effect, $\pi$-bonds are in conjugation which completely transfers $\ce{e-}$ density to carbocation. On the other hand, in inductive effect, induction of charge takes place, which partially transfers $\ce{e-}$ density through $\sigma$-bond. Hence, it is weaker.



> 
> why +M effect of 'N' is more than that of 'O'?
> 
> 
> 


As $\ce{N}$ has lower electronegativity than $\ce{O}$, hence it has greater $\ce{e-}$-donating tendency, therefore greater $\ce{+M-\text{effect}}$


 2

If hetro atom with lone pair is neighboring to carbocation, then that lone pair can be donated to empty orbital on carbocation (see figure below). These orbitals are said to be in **conjugation**. Conjugation leads to delocalization of electrons resulting in resonance structures.


[![enter image description here](https://i.stack.imgur.com/Di6uG.png)](https://i.stack.imgur.com/Di6uG.png)


Quoting from "Organic Chemistry" by T.W. GRAHAM SOLOMONS , CRAIG B. FRYHLE .SCOTT A.SNYDER
12edition:



> 
> Structures in which all the atoms have a complete valence shell of electrons
>  (i.e., the noble gas structure) are more stable.
> 
> 
> 


The third structure (your structure C) does not have conjugation. Hence it is comparatively less stable then 1st and 2nd structures.


Among 1st and 2nd structures , due to lower electronegativity of Nitrogen compared to Oxygen , Nitrogen has greater electron pair donating tendency. Therefor the order of stability is as follows.
[![enter image description here](https://i.stack.imgur.com/acox8.png)](https://i.stack.imgur.com/acox8.png)


 1

I'd try to give my explanation with the principles simple enough so that it would familiar to your level of education:


Rahul Verma has given simple enough explanation to answer most part of your question. I said here '*simple enough*' because of your subsequent comments. However, I have to point out that mesomeric effect ($M$) almost always predominate inductive effect ($I$), even when the distance between two concerning centers are neighbors like in the case in hands where inductive effect is in its highest level. 


When consider structures (**A**) and (**B**), the electron-withdrawing inductive effect ($-I$) of (**B**) is lager than that of (**A**) simply because electronegativity of $\ce{O}$ is higher than that of $\ce{N}$. However, the electron-donating mesomeric effect ($+M$) of (**A**) is lager than that of (**B**), which can be simply explained by following reason you have learned in general chemistry classes:


Consider $\ce{H2O}$ and $\ce{NH3}$ for their affinity for electron donating:


$$\ce{NH3 + H2O <=> NH4+ + OH-}$$ 


The solution is always basic ($\mathrm{p}K\_\mathrm{b}$ of ammonia is about 4.75) because ammonia donate its lone pair to grab a proton from water. It'd **never be** other way around like: $\ce{NH3 + H2O <=> NH2- + H3O+}$. By this phenomenon along, we can assume electron donating ability of $\ce{NH3}$ is comparatively larger than that of $\ce{H2O}$. Hence, one can consider that $(+M)\_\ce{N} \gt (+M)\_\ce{O}$. 


Based on these two comparisons, it is evident that $(-I+M)\_\ce{N} \gt\gt (-I+M)\_\ce{O}$ when compared to net positive value. Therefore, one can conclude that (**A**) is stable than (**A**).


 0