Jor
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sodium azide
I can obtain 10g of sodium azide for 2 euros. I was wondering if there are any interesting uses, besides the synthesis of explosives (I'm not
interested in explosives) or use in organic synthesis.
Are there any STABLE (so not explosive) metal complexes? Or other uses in inorganic chemistry?
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DJF90
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Sodium azide has many uses in organic chemistry;
The Curtius rearrangement:
http://www.organic-chemistry.org/namedreactions/curtius-rear...
The Schmidt reaction (via rearrangement):
http://www.organic-chemistry.org/namedreactions/schmidt-reac...
Also the Straudinger reaction (forms primary amines using Ph3P):
http://www.organic-chemistry.org/namedreactions/staudinger-r...
Possibly many more I am unaware of or have not considered. Reduction of an alkyl azide with LiAlH4 produces primary amines.
You could also heat NaN3 carefully to yield pure sodium metal protected by the evolved nitrogen atmosphere.
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a_bab
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On the mild decomposition note, used to get extremly pure Na in laboratories, does anyone know if the azides could be used to render other pure
metals, particulary Ca, Ba, Sr? Maybe specific prolonged heating at a certain temperature ranges to ensure a slow decomposition?
So far in my research, it looks that besides violent primaries, there is no use for metallic azides. The most stable azide is LiNO3, but further down
the periodic system the things change. Explosively. 
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DJF90
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LiNO3 is a nitrate a_bab... You surely mean LiN3
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a_bab
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Yes, stupid me.
Too many nitrations will nitrate one's brain, the NO3 radical becoming an obsession
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DJF90
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NO3 is not a radical my friend... And Nitrations are usually done with NO2(-) or NO2(+)
[Edited on 8-5-2009 by DJF90]
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Jor
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Quote: Originally posted by DJF90  | NO3 is not a radical my friend... And Nitrations are usually done with NO2(-) or NO2(+)
[Edited on 8-5-2009 by DJF90] |
Nitrations done with nitrite? How?
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a_bab
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Too many brainfarts here. Back on topic please.
Does anyone know if Ba(N3)2 can be decomposed without explosion?
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DJF90
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Nucleophilic substitution with aliphatic chloride. Nitrites are generally formed but with the silver salt you increase the "hardness" of the carbon
and so the "harder" nuclophilic site on NO2(-) (the nitrogen of course...) is the one that attacks, yielding a nitroalkane.
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Jor
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Anyways, i'm NOT interested in organic synthesis with azides, and also not in explosives. Is azide interesting in aqeous inorganic chemistry?
Otherwise I will not buy it.
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DJF90
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Not a huge amount I can think of to be honest, there was an article on liquid azide salts but you wouldnt like it, its quite organic...
In my opinion though I would get it anyway, a decent chemical as cheap as that (and in small quantity too) is always worth getting even if there is no
immediate use for it, and perhaps one day you will decide organic chem. is far more enjoyable than inorganic and wish that you did buy that azide when
you had the chance.
Just found this paper on covalent inorganic azides. I haven't read through because it doesnt particularly interest me but find the article attached.
[Edit: It gives me a server error when I try to attach the document. Will try again later]
[Edited on 8-5-2009 by DJF90]
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woelen
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Sodium azide is a nice chemical to have around and EUR 2 for 10 grams is a good price. Not something to let go. You are lucky with that price. I
purchased 50 grams of NaN3 at the drugstore near the place where I live, and I had to pay EUR 35 for that!
It can be used to make metal complexes, but beware, most of them are explosive in the dry state, but in the wet state (in solution, or as suspension),
they are not explosive and can be handled safely. Getting rid of these azide complexes is easy, by adding some acid, and then adding some
hypochlorite.
With this you can also make the remarkable compound ClN3, an interesting gas, which is explosive, but also has other interesting properties.
[Edited on 9-5-09 by woelen]
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