Why doesn't ethanol conduct electricity? [duplicate]








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




[Electrical conductivity of organic solvents](/questions/31507/electrical-conductivity-of-organic-solvents)

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Closed 3 years ago.



As far I know ethanol is soluble in water in all proportions, and since water is polar it would imply that ethanol is also polar and the only possible polar group in ethanol is the -OH group.


Oxygen is much more electronegative than hydrogen, so oxygen has to attract the electron pair towards itself forming a polar compound. 
This means it should have to disassociate into ions in aqueous solution and conduct electricity but it doesn't.


In some other posts of the same site mentions, why ethanol doesn't disassociate much in water, but it doesn't explain why the ethanol is still soluble in water in all proportion even it is not get disassociating much.


Why?




Why should pure water and pure ethanol dissociate ? Substances get dissociated into ions if they win some stability in this process. NaCl is more stable in the dissociated state than in the covalent. In ionic NaCl, all atoms look like rare gases, and respect the octet rule. In a theoretically covalent structure, Na does not respect the octet rule. So it is less stable. 
But ethanol is made of atoms which all respect the octet rule. So why should they dissociate ? 


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