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jlithen
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I just have to say one thing related to my previous post on this thread (long time ago now).
LNP (Lead nitrato phosphite) is actually very sensitive to friction...when I noticed it I got very frightened as I have handled it rather uncarefully.
It say on megas site that it is "stable" of course not necessarily meaning insensitive.
How stupid of me to not immediately check the sensitivity of a substance that I have been using for years. Anyway the detos seem to work relatively
well, even after months of storage, but I would like to change the LNP to something more powerful and maybe even less sensitive. Although senitivity
has not been a problem in the caps.
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DeAdFX
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I tried making a complex Triethanolamine(TEA) of my own. I first made copper (II) nitrate by reacting copper sulfate and potassium nitrate in 30mL
of water(1/10 mol scale). I fucked up though and added half as much KNO3 as I should have(christ this is the 2nd time I have neglected the fact that
SO4 is a -2 ion). Well anywho I added in 20mL of TEA into the CuSO4/Cu(NO3)2 solution. The solution turned a dark turquiose(SP) color. After
swirling the solution for a few seconds the color intensity went down a bit. I added 30mL of ethanol and a blue/turquiose perciptate formed. The
perciptate is really fine. I assume its about >200 mesh easy. Right now the perciptate is drying off in the air.
I wonder if Copper (II) Nitrate would form a complex with nitrosoamines like NitrosoEthanolamine or Dinitrosoethanol amine. These complexes would
probably be more energetic due better OB.
Anywho Copper(II) Nitrate TEA complex should be more stable* than the tetramine variant. By stable I mean the complex won't fume off ammonia and
become useless after a few days. TEA has a much higher boiling point.
[Edited on 23-12-2006 by DeAdFX]
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DeAdFX
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UPDATE:
The complex has dried off and still has the same turquiose color. I burned a small sample of the complex. The sample turned from a turquiose color
to a black color indicating the complex decomposed to copper(II) oxide. The decompisition was not violent nor was there any flame. To verify that I
had a copper complex I burned the sample with some Ammonium Perchlorate in a paper cup. The resulting flame was a very pretty blue.
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quicksilver
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Copper (II) nitrate is SO hygroscopic that there would be some water in the crystals unless special efforts were taken and that would effect the
outcome to a degree that it would deflagrate. Under other circumstances it may well detonate but the water would present a problem. Copper (II)
nitrate has often had this as a stumbeling block. The issue has arisen with many primaries. Even lead-based materials, if water still existed within
the final product, they did not respond well. Really -=DRY=- material often tests far differently. Determine if any water existed before making a
final assesment.
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Zinc
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| Quote: | Originally posted by quicksilver
Copper (II) nitrate is SO hygroscopic that there would be some water in the crystals unless special efforts were taken and that would effect the
outcome to a degree that it would deflagrate. Under other circumstances it may well detonate but the water would present a problem.
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You mean that copper (II) nitrate can detonate?
If yes do you know anything about its properties(stability,VOD and how to dehidrate it)?
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quicksilver
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No it does not. It is a nitrate salt that is very hygroscopic but that in use, it brings with it so much water that unless steps are taken to deal
with the water - the compound / resultant will have that issue. Some primaries are desensitized by water to a greater degree than others., etc.
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chemoleo
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DeadFX what I really wonder is why you think TEA is an appropriate complexing agent. I mean, for one Cu ion there are two molecules of TEA, and 2x
NO3. If you calculate the oxygen balance, you'll note it is appalling. No way this will ever make it into some sort of energetic material.
Try hydrazine, hydroxylamine (although I think that I tried that before, and it doesn't work-> decomposition in solution), guanidine, and other
small nitrogen containing bases, these are feasible targets! Or even tetrazole, I think Nick F may have tested that.
Never Stop to Begin, and Never Begin to Stop...
Tolerance is good. But not with the intolerant! (Wilhelm Busch)
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halogen
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Would it not be one molecule of TEA per copper atom?
F. de Lalande and M. Prud'homme showed that a mixture of boric oxide and sodium chloride is decomposed in a stream of dry air or oxygen at a red heat
with the evolution of chlorine.
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DeAdFX
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| Quote: | Originally posted by chemoleo
DeadFX what I really wonder is why you think TEA is an appropriate complexing agent. I mean, for one Cu ion there are two molecules of TEA, and 2x
NO3. If you calculate the oxygen balance, you'll note it is appalling. No way this will ever make it into some sort of energetic material.
Try hydrazine, hydroxylamine (although I think that I tried that before, and it doesn't work-> decomposition in solution), guanidine, and other
small nitrogen containing bases, these are feasible targets! Or even tetrazole, I think Nick F may have tested that. |
The reason I thought TEA would be a more suitable complexing agent is because it has a way higher boiling point than ammonia[liquid vs gas]. The TEA
complex should be more stable in the sense of having a somewhat longer shelf life with a major sacrifice in power. However my experiment was a
failure because I had a miscalculation so the power is yet to be determined. The perchlorate variant would probably show more promise.
The nitrogen bases that I posses are urea and hexamine[yeah yeah big molecule..]. Technically I could also posess ammonia, guanidine and methyl amine
if I weren't so god damn lazy/bogged with work. I also have azide however my time is limited in my home lab so I can't synthesize tetrazole and even
then my knowledge in high explosives is rather limited.
Even if the compound is only capable of a simple burn it will still be of practical use for me atleast. Somewhat off topic but I am working on a blue
star composition involving Ammonium Nitrate( I hear it burns a lot cooler than Perchlorates] as the primary oxidizer. So far I have very little
success.
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quicksilver
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OT remark:
Blue is a tough color to get right. However I have had some success. The problem is that metal fuels (other than copper) will drown it out very fast.
Ammonium nitrate could work just fine if you used something like: ammonium nirate 33% nickle or cupric nitrate 20% copper powder (325 mesh) 13%
chlorine doner 20%, burn rate enhanser 7% binder 6% - The burn rate enhancer is needed due to ammonium nirate's slower burn and less O than the
perchlorate. It's a problem and a good thing as well.
[Edited on 15-2-2007 by quicksilver]
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nitro-genes
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Haven't seen any mention of nitrato/nitrito-metal complexes for energetic complex salts in this thread (or I have overlooked them  ). Some would be pretty promissing, like the hexanitritocobaltate(III) ion. The sodium
salt is one of the few well soluble salts, while it readily precipitates with K+ or even NH4+...
Forming a salt with methylamine, urea, hexamine, etc could give interesting results, no idea what it's properties, or how stable they would be, as
most NO or NO2 ligand metal complexes are not very stable...
Are there even any known nitrito/nitrato complexes that have been reported to have primary explosive properties? I seem to remember this
nitrato-Hg(II) aldehyde complex, though it was a rather feeble explosive IIRC...
[Edited on by nitro-genes]
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Rosco Bodine
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Joeychemist got this file from solo ,
and hasn't posted it here so I will .
Attachment: Explosive Properties of Metal Ammines.pdf (273kB)
This file has been downloaded 3161 times
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nitro-genes
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Thanks for posting that article!
Ammonium hexanitrocobaltate(III) goes out the window as it seems concerning it's potential as a primary. Hydrazine hexanitrocobalate still seems
pretty spicy though, if it would exist that is...
Most of the used oxidizers seem to stable to accellerate fast enough to behave like a primary, like the perchlorates or nitrates. On the other hand
the chlorates are capable of doing so, but are not very storage stable. For that matter would the peroxo chromates Woelen posted about be a good
starting point, since it was pretty obvious that it is a very powerfull oxizer, but seemingly stable in storage...
[Edited on by nitro-genes]
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Ballermatz
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[Edited on 24-12-2007 by Ballermatz]
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12AX7
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Nitrito-?
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Ballermatz
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[Edited on 24-12-2007 by Ballermatz]
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Nerro
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| Quote: | Originally posted by 12AX7
Nitrito-? |
nitrite as a ligand 
#261501 +(11351)- [X]
the \"bishop\" came to our church today
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12AX7
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Yes; he spelled "nitrato" is all. I wasn't aware NO3- formed ligands, but I've heard of the NO2 cobalt complex.
Tim
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Nerro
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Why shouldn't nitrate form ligands? It does, it even forms reasonably stable eta-2 ligands (bridging ligands with 2 hapticity).
#261501 +(11351)- [X]
the \"bishop\" came to our church today
he was a fucken impostor
never once moved diagonally
courtesy of bash
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JohnWW
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Getting the anions of strong oxy-acids like NO3-, SO4--, ClO4-, BrO4-, IO4-, and similar, and of strong fluoro-acids like PF6-, SbF6-, BF4-, to act as
ligands is very difficult, if not impossible, because of their high symmetry and steric crowding reasons, and, in the case of the oxy-acids, their
resonance-stabilization which results in the negative charge being evenly distributed over the oxygens.
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Nerro
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Which makes it impractical for an amateur chemist but not impossible on the whole.
#261501 +(11351)- [X]
the \"bishop\" came to our church today
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woelen
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I'm almost 100% sure that the yellow material, mentioned here is ammonium hexanitritocobaltate (III). So, nitrite as ligand and not nitrate. I have
the sodium salt of this complex ion and indeed it forms beautul precipitates with ammonium salts and even better results are obtained with potassium
salts. I know of nitrato complexes, e.g. UO2(NO3)2 and also some cerium compounds, such as (NH4)2[Ce(NO3)6].
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Nerro
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Are those the nitrito complexes (-O-N=O) or the nitro complexes (with the bond being made by the lone pair on the N)?
And how feasible is it to make a complex like ferrocene but with N<sub>5</sub><sup>-</sup>? (the structure of which being
similar to that of the cyclopentadienyl ion). Is anything known of such complexes and their stability?
-Edit-
The complex would be called bis-pentazolido iron(II).
| Quote: | source
Abstract : The pentazole anion has been generated from para-hydroxyphenylpentazole and identified by electrospray ionization mass spectrometry.
Whereas at low collision voltages the para-phenoxypentazole anion undergoes stepwise N2 elimination generating the corresponding azide and nitrene, at
high collision voltages the N5(-) anion is formed. Fragmentation of the pentazole anion produces the N3(-) anion as the principal negative ion. These
experiments provide the first experimental proof for the existence of the pentazole anion. They also demonstrate that under suitable reaction
conditions the C-N bond in a phenylpentazole can selectively be broken with conservation of the pentazole ring, thus providing a potential synthetic
route to the pentazole anion. |
Doesn't sound like a very usefull synthesis... I remember synthesizing the cyclopentadienyl ion by letting a saturated solution of KOH with excess KOH
at the bottom react with C<sub>5</sub>H<sub>6</sub>, why shouldn't something similar work on HN<sub>5</sub>? A
stronger base will probably be needed...
Could an oxidizing agent be applied to synthesize N<sub>10</sub> (+2H<sup>+</sup> and two electrons)? Sounds like a pretty
dangerous substance to me but perhaps at -80°C it might be stable enough?
And I also read that phenylpentazole is much more stable than just pentazole. Could para-dipentazolebenzene be synthesized somehow? And how is
phenylpentazole synthesized anyway?
[Edited on 7-8-2007 by Nerro]
[Edited on 7-8-2007 by Nerro]
#261501 +(11351)- [X]
the \"bishop\" came to our church today
he was a fucken impostor
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quicksilver
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Hey Nerro: if find out more stuff about ferrocenes please post 'em! I'm interested also and have had little luck......
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The_Davster
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I have done minor looking into of pentazoles
Phenylpentazole is formed by the reaction of benzenediazonium chloride with sodium azide, this is analogous to the making of tetrazoles by the
reaction of cyanides, 5-phenyl -1H-tetrazole being formed from phenylacetonitrile and sodium azide.
I have seen a paper somewhere about the free pentazoles, it was posted on this site years ago. I forget one very important thing, whether it was
theoretical, or had been done before. It was on a 'pentazolium pentazolate' compound which could cyclize into a nitrogen flavour of buckyballs.
1H,5H-tetrazole can be formed from anhydrous HCN and HN3, problem is finding a nitrogen analogue of HCN that would be substitutable here.
Acetylides/acetylene(forget which exactly) also react with HN3/NaN3 making the triazoles, but no such easy lab analogues exist for N. I wonder if
under extreme conditions nitrogen gas would react with HN3? Some sort of exotic excitation would likely be necessary,and under pressure.
EDIT:
| Quote: |
And how feasible is it to make a complex like ferrocene but with N5-? (the structure of which being similar to that of the cyclopentadienyl ion). Is
anything known of such complexes and their stability? |
There is something close, nitrotetrazolate CN4NO2-, ion would seem to be similar to a substituted cyclopentadiene, but its complexes are not eta5, all
I have seen is eta1. A tetrazolate might make a ferrocene type compound, but I have seen nothing on it as a ligand.
[Edited on 8-8-2007 by The_Davster]
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