symboom - 17-3-2017 at 18:19
Im in that part of chemistry the hard to find rarely performed chemistry
So I have guanidine nitrate
I havent be able to find any soubliity information
I have read that guanidine nitrate
Can form nitroguanidine
Then reduced to aminoguanidide
Then added to nitric acid to form
Aminoguanidine nitrate
Then converted to nitroaminoguanidine by dehydration
I chose nickel because
Hexamine nickel perchlorate is insouble in water
I figure maybe other compounds are also insouble
Many copper complexes require ethanol or other solvent to precipitate
Is nickel guanidine nitrate
Nickel guanidine perchlorate
How would those be formed
Nickel nitroguanidine perchlorate?
Possible if so what are the properties
[Edited on 18-3-2017 by symboom]
[Edited on 18-3-2017 by symboom]
JJay - 17-3-2017 at 21:32
It is often hard to find good solubility information for organic compounds. I remember seeing a searchable database that also showed model predictions
for solubility somewhere....
NeonPulse - 19-3-2017 at 22:34
Perhaps some answers may be found in this document. i dont really have the time to browse through it thoroughly but is is a useful reference for this
material and may have the answers you are searching for either way i found it quite interesting.
Attachment: Chemistry_of_Aminoguanidine_And_Related_Substances.pdf (975kB)
This file has been downloaded 364 times
tsathoggua1 - 19-3-2017 at 22:44
MOST but nit ALL nitrates are soluble ALTHOUGH this was derived from A-level exam material. And is untrue, some nitrate complexes are AQ insoluble,
symboom - 7-4-2017 at 21:36
Update on a couple of attempts with complex salts
Synthesis: Hexamine nickel guanidine nitrate
A ammonia nickel complex was added to guanidine nitrate no insoluble precipitate forms
Synthesis: Guanidine perchlorate
Ammonium perchlorate and guanidine nitrate were mixed then chilled until half frozen still no percipitate
Synthesis: guanidine hydroxide
Ammonium hydroxide and guanidine nitrate no precipitate forms
Cant seem to figure out how to complex with guanidine
Yes I know if processed further to aminoguanidine forms a complex
guanidine primary
Hey Buddy - 30-11-2022 at 23:34
On a long lonely journey of finding "a" primary that isn't azide. of course that probably means the journey will end with an azide. (thinking about
Bi). Anyways, now I'm here.
I started with nitriminotetrazole salts, passed by aminonitroguanidine "laser ignitable primaries", then rounded the corner to aminoguanidine metal
perchlorates. Now I have parsed it down to guanidine. If that doesnt pan out im going to lay down with SA-DS and Azide or aminoguanidine salts.
Guanidine salt can be had where Im at via guanidine nitrate. I already buy this (a lot) for nitroguanidine. I have learned that Guanidine is a very
labile molecule for coordination with oxidizer and metal moieties, it is used all the time in pharma, crazy metal organic coordination complexes in
medicine are all over search results. For some reason, Guanidine complexes are practically unexplored in energetics.
Simple Guanidine perchlorate is already sensitive without any complex of metal moieties. Picric acid is a respective 85 cm drop to guanCLO4's 50 cm.
Vd of 6-7.15 m/s. It seems like guanidine should behave very similarly to the aminoguanidine metal perchlorates which are already appreciated here.
The aminoguanidine metal perchlorates look perfect, but they have only one problem for me. In theory, they are two steps further-away from a
hypothetically equivalent guanidium compound. Thats enough to make me consider guanidine.
It seems that people have encountered difficulty in preparing guanidium perchlorate from anything other than HCLO4. possibly issues with
precipitation? Obviously a meta reaction would be much more convenient than HCLO4.
Id like to look for a guanidine perchlorate primary.
What can I do/ should I do to test out and locate a basic guanidium perchlorate based primary explosive?
My gut tells me to begin with aminoguanidine diperchlorate hydrate methods but supplement guanidine nitrate for the aminoguanidine.
At disposal, I currently have: NH4CLO4, KCLO4, NH4NO3, (NH2)2CNH.NO3.
For metals Ive got:
Cu, Mn, Ti, V, Sb, Pb, Ag, Bi, Sr, Ba, Ni, Zn
I have no perchloric acid and have never made perchloric acid (for some reason), so I am unfamiliar with its behavior.
There must be a guanidine perchlorate primary, it only makes sense. What is the best metathesis reaction for metal perchlorates from NH4CLO4? Also,
Most of the metals are in oxide form.
I think the obvious Target to begin with is Ni/Ag Guanidine Perchlorate, perhaps coordination with amines? No amines? What do you think? I could use
advice. I dont even know what I'm doing.
[Edited on 1-12-2022 by Hey Buddy]