Sorry if this seems basic, but I can't find anything.
C6H5Na+H2O>NaOH+C6H6
Maybe peroxide?
[Edited on 15-5-2006 by =SkyNET=]Maja - 15-5-2006 at 08:09
C6H6 is benzene, not phenol. I think it should work with HCl.
[Edited on 15-5-2006 by Maja]12AX7 - 15-5-2006 at 08:14
I don't see it, HCl would just leave the Na with the Cl and H with the C6H5 part.
A load of OH radicals probably would do it, H2O2 for instance, but I get the feeling weird stuff like peroxides and other reactions like straight
hydration would be preferred (unless you have nasty high test peroxide).
Tim=SkyNET= - 15-5-2006 at 08:27
I figured peroxide might work.
I guess i should expect a vigorous reaction.
Quote:
C6H6 is benzene, not phenol. I think it should work with HCl.
I left off a sentence in my post explaining why i hydroxide wouldnt work. :p
[Edited on 15-5-2006 by =SkyNET=]unionised - 15-5-2006 at 09:35
Phenyl sodium wil deprotonate H2O2 to give sodium peroxide and benzene. The reaction will probably be fast enough to start thermally decomposing the
peroxide and I wouldn't like to be there when it happens.
I think that iodination then hydrolysis of the iodobenzene might work but I wouldn't like to bet on it and the hydrolysis isn't easy anyway.
C6H5Na +I2 --> C6H5I + NaI
I would assume phenyl sodium would be enough reactive to get oxidized by oxygen to sodium phenolate. However bubbling oxygen trough a solution of
phenyl sodium would be extremely stupid with regards of safety. Especially if the solvent would be combustible, it would be a bomb just waiting to
explode (all alkyl metals are highly pyrophoric and I never heard of their "controlled combustion"). I can't remember any noncombustible solvent that
would be able to solvate PhNa so you better forget such an experiment.
Why do you want to perform such a useless transformation anyway?
[Edited on 15-5-2006 by Nicodem]=SkyNET= - 15-5-2006 at 19:01
I agree with the safety mentions, but I have a certain plan for it.
How about chlorine?
C6H5Na+Cl2>C6H5Cl+NaCl
Then Cl>OH?chemoleo - 15-5-2006 at 19:30
Sorry you realise that phenylsodium isn't exactly an easy to come by compound? Most amateur chemists would sell their mother for it!
You do realise there are plenty ways for making phenol with over the counter compounds??leu - 15-5-2006 at 20:18
Clearly the originator of this thread has little knowledge of the properties of phenylsodium, or alkali metals as far as that goes There is no substitute for diligent study habits and the proper equipment when it comes
to compounds as dangerous as phenylsodium, please listen to Nicodem unless you have a death wish =SkyNET= - 16-5-2006 at 19:16
I planned on only using milligram quantities of course. Anyone who has worked with sodium knows how hazardous it is. :Oturd - 17-5-2006 at 09:34
Quote:
Originally posted by =SkyNET=
I planned on only using milligram quantities of course. Anyone who has worked with sodium knows how hazardous it is. :O
Sodium is completely harmless as long as you don't throw it in a bucket 'o water.
The problem with PhNa is the Ph-, not the Na+.
There is no substitute for diligent study habits and the proper equipment when it comes
to compounds as dangerous as phenylsodium, please listen to Nicodem unless you have a death wish 
