Sciencemadness Discussion Board
Not logged in [Login - Register]
Go To Bottom

Printable Version  
 Pages:  1  ..  17    19
Author: Subject: Exotic Primaries - Complex Salts
symboom
National Hazard
****




Posts: 453
Registered: 11-11-2010
Member Is Offline

Mood: Feeling Ascaridole

[*] posted on 26-6-2017 at 08:34


Does anyone know the soubility and extraction of hexamine cobalt chlorate and nitrate
https://m.youtube.com/watch?v=PsdJ99qiCRs

[Edited on 26-6-2017 by symboom]




Natures Intellectual Organic Peroxide. >>Ascaridole <<

Oxone
Used for the production of --> CH2O/Cl2/ClO2/Br2/I2

------------------------------------->>Hydrogen Peroxide << -------------------------------------------- >> Acetylene <<
Peroxide Salts
Zinc Peroxide <\> Copper Peroxide <\>Silver Peroxide <\>Lithium Peroxide <\>Magnesium Peroxide <\>Calcium Peroxide to Calcium Superoxide
CoO2. \\ NiO2 \\ Ti/V/Cr peroxy complex \\ Triamine chromium peroxide \\ LiH \\SiO2-H2SO4 (SSA) \\ [Ni(NH3)6]

Exotic reducing agents
Ga2O TiCl2 GeCl2 && Na2S2O4
View user's profile View All Posts By User
PHILOU Zrealone
International Hazard
*****




Posts: 2803
Registered: 20-5-2002
Location: Brussel
Member Is Offline

Mood: Bis-diazo-dinitro-hydroquinonic

[*] posted on 26-6-2017 at 15:58


HACo(II)N is quite soluble and red like Co(NO3)2.
Extraction and synthesis similar to TACuN and HANi(II)N.

I guess HACo(II)C is similar to HACo(II)N in solubility and synthesis.

But here maybe it is the Co(III) that is concerned...thereover I have no clue or info.

The video is no proof of anything...only claims that are dubious:
*Odorless...and NH3 is it odorless?

*Not detectable by any means? And spectrometry? All complexes display specific absorption and emission spectra...

*Vod 7500m/s...really...hard to believe...proof of oscilloscopic or high speed camera measurement? No.

*Several order of power magnitude stronger than peroxyde explosive...HMTD...is quite powerful and I doubt a dead weight metalic holding molecule can beat a purely CHNO explosive material onto energetic content.

*Any molecule holding NH3 and ClO3 onto a catalytic metallic core can't be an unsensitive safe ternary explosive...it must by definition perform easy D2D...and as such is a primary or at best a secondary




PH Z (PHILOU Zrealone)

"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
View user's profile View All Posts By User
greenlight
National Hazard
****




Posts: 498
Registered: 3-11-2014
Member Is Offline

Mood: Energetic

[*] posted on 15-7-2017 at 06:46
Strontium picrate


I was inspired by neonpulse experiment with cesium picrate on the previous page that I decided to try and make strontium picrate.

I made a thick slurry of strontium carbonate due to the insolubility problems and added it with a dropper to boiling hot picric acid solution until neutral.
Nothing crystallised when room temperature was reached and still nothing after chilling in the freezer. Strangely, I poured the strontium picrate solution into a fresh evaporating dish and it instantly started crystallising on the sides and was filtered soonafter.

Its looks very similar to potassium picrate with the crystals needle-like structure but slightly darker in colour (see uploaded photos).
I was unable to intiate it with shock or friction at all.
When ignited it burns similarly to potassium picrate very fast with a slight crack leaving black residue behind. It emits a deep red colour when ignited or exploded which proves the existence of the strontium cation. When confined in foil and heated in flame it explodes with a loud report.
I will have to try the barium version.

It doesnt take fire from a fuse really at all though or only partially burns if it does.
If this was not an issue, considering the low sensitivity I think it would be a suitable more colourful replacement for the colored Mg flash compositions for firecrackers which usually get washed out.

Photo on bottom shows about 50mg strontium picrate confined in foil and heated with a flame exploding.


[Edited on 15-7-2017 by greenlight]

20170715_123557.jpg - 1.6MB Screenshot_2017-07-15-12-37-18.png - 3.6MB Screenshot_2017-07-15-20-05-47.png - 1.9MB

[Edited on 15-7-2017 by greenlight]

[Edited on 15-7-2017 by greenlight]

[Edited on 15-7-2017 by greenlight]

[Edited on 15-7-2017 by greenlight]




The only use for an atomic bomb is to keep somebody else from using one.
George Wald
View user's profile View All Posts By User
Laboratory of Liptakov
International Hazard
*****




Posts: 565
Registered: 2-9-2014
Member Is Offline


[*] posted on 15-7-2017 at 08:51


Beautiful. In foil exploded ? That's a good message....:cool:........LL



Safety explosive Alfred Nobel 1867. Safely ecologic detonator Dr. Liptakov 2015.
View user's profile View All Posts By User
symboom
National Hazard
****




Posts: 453
Registered: 11-11-2010
Member Is Offline

Mood: Feeling Ascaridole

[*] posted on 15-7-2017 at 23:37


I want to add a couple more energetic complex salts
Perticularly

Diamine zinc perchlorate
They dissolve in alcohol. Salvadori has obtained the hydrates Zn(ClO4)2.6H2O and Zn(ClO4)2.4H2O, and the compound Zn(ClO4)2. 4NH4. Both hydrates are strongly hygroscopic, and decompose on heating before all water is eliminated. The ammonia compound is not very stable.

Diamine zinc iodate
3Zn(IO3)2. 8NH4, are obtained by dissolving zinc iodate in concentrated ammonia solution, and either adding alcohol or allowing the solution to evaporate spontaneously. Another compound with ammonia, insoluble in water and stable in air, has been obtained by slow evaporation of an ammoniacal solution of zinc iodate. It decomposes explosively at 150° C. Dry powdered zinc iodate absorbs ammonia gas to form Zn(IO3)2.4NH4.

Less stable diamine zinc bromate
Deliquescent, unstable crystals of Zn(BrO3)2. 3H2O.2NH4 were obtained by adding ammonia to a solution of the salt. Zinc bromate is soluble in its own weight of water at 15° C.

Zinc hexamethylenetetramine (hexamine)nitrite ZHN
Colourless prismatic crystals of Zn(NO2)2.2H2O.C6H12N4 are obtained by adding sodium nitrite to the solution of a zinc salt containing hexamethylenetetramine. Zinc nitrite also occurs in the hygroscopic yellow crystalline double salt, 3KNO2.Zn(NO2)2.3H2O, obtained by acting with nitrous acid on zinc hydroxide suspended in potassium nitrite solution, and in the similar salt, 2KNO2.Zn(NO2 )2.H2O, prepared by mixing solutions of potassium nitrite and zinc chloride

Update sucess made ZHN its a dark yellow compound
Once sodium nitrite was added to the solution the yellow color
ZHN is insouble in water settled to the bottom it seems like a fine percipitate small bubbles are forming not sure if it is decomposing in water or its stability
all reagents are soluble in alcohol so a reaction could take place in alcohol then precipitated slowly with water to cause bigger crystals to form havnt done any flame tests

Excerpt from atomistry.com/zinc
This website is great shows many exotic compounds such as sodium aluminum perchlorate , sodium hypoborate, and diamine silver bromate

[Edited on 16-7-2017 by symboom]

[Edited on 16-7-2017 by symboom]




Natures Intellectual Organic Peroxide. >>Ascaridole <<

Oxone
Used for the production of --> CH2O/Cl2/ClO2/Br2/I2

------------------------------------->>Hydrogen Peroxide << -------------------------------------------- >> Acetylene <<
Peroxide Salts
Zinc Peroxide <\> Copper Peroxide <\>Silver Peroxide <\>Lithium Peroxide <\>Magnesium Peroxide <\>Calcium Peroxide to Calcium Superoxide
CoO2. \\ NiO2 \\ Ti/V/Cr peroxy complex \\ Triamine chromium peroxide \\ LiH \\SiO2-H2SO4 (SSA) \\ [Ni(NH3)6]

Exotic reducing agents
Ga2O TiCl2 GeCl2 && Na2S2O4
View user's profile View All Posts By User
PHILOU Zrealone
International Hazard
*****




Posts: 2803
Registered: 20-5-2002
Location: Brussel
Member Is Offline

Mood: Bis-diazo-dinitro-hydroquinonic

[*] posted on 17-7-2017 at 03:56


Quote: Originally posted by greenlight  
I was inspired by neonpulse experiment with cesium picrate on the previous page that I decided to try and make strontium picrate.

I made a thick slurry of strontium carbonate due to the insolubility problems and added it with a dropper to boiling hot picric acid solution until neutral.
Nothing crystallised when room temperature was reached and still nothing after chilling in the freezer. Strangely, I poured the strontium picrate solution into a fresh evaporating dish and it instantly started crystallising on the sides and was filtered soonafter.

Its looks very similar to potassium picrate with the crystals needle-like structure but slightly darker in colour (see uploaded photos).
I was unable to intiate it with shock or friction at all.
When ignited it burns similarly to potassium picrate very fast with a slight crack leaving black residue behind. It emits a deep red colour when ignited or exploded which proves the existence of the strontium cation. When confined in foil and heated in flame it explodes with a loud report.
I will have to try the barium version.

It doesnt take fire from a fuse really at all though or only partially burns if it does.
If this was not an issue, considering the low sensitivity I think it would be a suitable more colourful replacement for the colored Mg flash compositions for firecrackers which usually get washed out.

Photo on bottom shows about 50mg strontium picrate confined in foil and heated with a flame exploding.


[Edited on 15-7-2017 by greenlight]

Nice...Greenlight that makes RED Lights :D;):):P:cool:
Great info for picrate lovers and picrate information, thank you...
Lithium may also find uses for the red color...

You experienced the overfusion effect...the compound is into sursaturation state...and a sudden temperature change or a scratch/dust into a glas recipient may induce fast crystalization...

Instead of carbonate you could also have used the hydroxyde....what must be slightly more soluble...but the advantage of the carbonate is that it fizzes showing there is stil some picric acid...and the excess carbonate is easy to observe and to separate from the picrate salt.




PH Z (PHILOU Zrealone)

"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
View user's profile View All Posts By User
PHILOU Zrealone
International Hazard
*****




Posts: 2803
Registered: 20-5-2002
Location: Brussel
Member Is Offline

Mood: Bis-diazo-dinitro-hydroquinonic

[*] posted on 17-7-2017 at 04:01


Quote: Originally posted by symboom  
I want to add a couple more energetic complex salts
Perticularly

Diamine zinc perchlorate
They dissolve in alcohol. Salvadori has obtained the hydrates Zn(ClO4)2.6H2O and Zn(ClO4)2.4H2O, and the compound Zn(ClO4)2. 4NH4. Both hydrates are strongly hygroscopic, and decompose on heating before all water is eliminated. The ammonia compound is not very stable.

Diamine zinc iodate
3Zn(IO3)2. 8NH4, are obtained by dissolving zinc iodate in concentrated ammonia solution, and either adding alcohol or allowing the solution to evaporate spontaneously. Another compound with ammonia, insoluble in water and stable in air, has been obtained by slow evaporation of an ammoniacal solution of zinc iodate. It decomposes explosively at 150° C. Dry powdered zinc iodate absorbs ammonia gas to form Zn(IO3)2.4NH4.

Less stable diamine zinc bromate
Deliquescent, unstable crystals of Zn(BrO3)2. 3H2O.2NH4 were obtained by adding ammonia to a solution of the salt. Zinc bromate is soluble in its own weight of water at 15° C.

Zinc hexamethylenetetramine (hexamine)nitrite ZHN
Colourless prismatic crystals of Zn(NO2)2.2H2O.C6H12N4 are obtained by adding sodium nitrite to the solution of a zinc salt containing hexamethylenetetramine. Zinc nitrite also occurs in the hygroscopic yellow crystalline double salt, 3KNO2.Zn(NO2)2.3H2O, obtained by acting with nitrous acid on zinc hydroxide suspended in potassium nitrite solution, and in the similar salt, 2KNO2.Zn(NO2 )2.H2O, prepared by mixing solutions of potassium nitrite and zinc chloride

Update sucess made ZHN its a dark yellow compound
Once sodium nitrite was added to the solution the yellow color
ZHN is insouble in water settled to the bottom it seems like a fine percipitate small bubbles are forming not sure if it is decomposing in water or its stability
all reagents are soluble in alcohol so a reaction could take place in alcohol then precipitated slowly with water to cause bigger crystals to form havnt done any flame tests

Excerpt from atomistry.com/zinc
This website is great shows many exotic compounds such as sodium aluminum perchlorate , sodium hypoborate, and diamine silver bromate

[Edited on 16-7-2017 by symboom]

[Edited on 16-7-2017 by symboom]

Thank you for the informations....;)




PH Z (PHILOU Zrealone)

"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
View user's profile View All Posts By User
greenlight
National Hazard
****




Posts: 498
Registered: 3-11-2014
Member Is Offline

Mood: Energetic

[*] posted on 18-7-2017 at 05:20
Barium picrate


Thanks LL and Philou

[/rquote]
Nice...Greenlight that makes RED Lights :D;):):P:cool:
[/rquote]

Here I will try make the green light haha:D:)

I used the same synthesis method as for the strontium picrate and the same overfusion effect happened when I crystallised it.
The crystals are much finer smaller needles than the Sr salt and leave the same black soot behind after being burnt which seems to be common for picrates.

It is insensitive to friction and shock the same as the strontium picrate.

Although the green colour is not as strong as the Sr picrate it makes up for it in power and brisance when confined.
Unlike the strontium picrate, the top crystals of a small pile first melt and then initiate the whole pile with a loud whooomp when ignited with a flame.
It cannot be initiated without first going through a melt-phase of the surface.
It takes longer to explode when confined in foil because of this as well.

The report is louder than Sr and the foil is reduced to smaller pieces even under slight confinement by making a small Al foil cup it explodes loudly blowing a hole in the bottom and unravelling the whole top.
The amounts used were the same as the tests with Sr picrate.
The left picture is confinement in foil under the same conditions as the Sr salt and the right picture is burning of an small unconfined pile

[Edited on 18-7-2017 by greenlight]

20170717_134506.jpg - 1.9MB 20170718_203712.jpg - 2.9MB Screenshot_2017-07-18-20-14-00.png - 1.2MB Screenshot_2017-07-18-20-27-05.png - 1.2MB

[Edited on 18-7-2017 by greenlight]

[Edited on 18-7-2017 by greenlight]




The only use for an atomic bomb is to keep somebody else from using one.
George Wald
View user's profile View All Posts By User
symboom
National Hazard
****




Posts: 453
Registered: 11-11-2010
Member Is Offline

Mood: Feeling Ascaridole

[*] posted on 20-7-2017 at 21:25
Exotic silver amine complexes


Exotic silver complexes
Diamine silver nitrite
Silver nitrate to sodium nitrite form Silver nitrite
Double compounds with ammonia of the formula
AgNO2,NH3; AgNO2,2NH3; and AgN

Diamine silver bromate
Potassium bromate precipitates silver bromate from Silver nitrate.Its solution in ammonium hydroxide yields crystals of the formula Ag(NH3)2BrO3.

Diamine Silver chlorate
The Silver chlorate, AgClO3, can be prepared by dissolving the monoxide in chloric acid, or by passing chlorine through a suspension of the monoxide in water, the hypochlorite being an intermediate product.produces shock-sensitive dark crystals. A use for silver oxide batteries unfortunatly the silver oxide is very stubborn to desolve in chlorine water due to calcination.
Its solution in ammonium hydroxide yields prismatic crystals, Ag(NH3)2ClO3, melting at 100° C.


And mercury
Trimercury chlorate acetylide
Mercuric nitrate; sodium chlorate; acetylene or calcium carbide

And copper
Tetraaminecopper chlorate
ammonium hydroxide, copper sulfate, sodium chlorate, alcohol

Exotic amine nickel
Nickel Bromate, Ni(BrO3)2.6H2O, may be prepared by double decomposition of barium bromate and nickel sulphate solutions. It crystallises in unstable octahedra which are green in colour. From its solution in aqueous ammonia, alcohol precipitates the diammoniate, Ni(BrO3)2.2NH3.

Popular hexamine nickel perchlorate
If a piece of blotting or filter paper is moistened with a solution of nickel perchlorate and introduced into the tip of a Bunsen flame, a series of small detonations ensues.

the hexammoniate, Ni(ClO4)2.6NH3.

Also never understood the zinc amine complexes are never very stable and decompose such as the diamone zinc permangante and diamine zinc perchlorate

Too bad alumunum chlorate doesnt form a complex but aluminum perchlorate does form a double salt

Aluminium perchlorate, Al(ClO4)3.6H2O, is a colourless, crystalline salt, soluble in water. Its aqueous solution gives, with sodium perchlorate, a crystalline precipitate of aluminium sodium perchlorate, AlNa(ClO4)4.12H2

Info on the chlorate
Kind of off topic but it does produce chlorine dioxide
Aluminium chlorate, Al(ClO3)3.9H2O, prepared by mixing aluminium sulphate and barium chlorate, removing the barium sulphate, and evaporating the cold solution over sulphuric acid, is very soluble in water. From a hot solution it separates as the hexahydrate. The salt is easily decomposed by heat, and explodes when slowly heated.

Im guessing due to chlorine dioxide gas being produced

[Edited on 21-7-2017 by symboom]




Natures Intellectual Organic Peroxide. >>Ascaridole <<

Oxone
Used for the production of --> CH2O/Cl2/ClO2/Br2/I2

------------------------------------->>Hydrogen Peroxide << -------------------------------------------- >> Acetylene <<
Peroxide Salts
Zinc Peroxide <\> Copper Peroxide <\>Silver Peroxide <\>Lithium Peroxide <\>Magnesium Peroxide <\>Calcium Peroxide to Calcium Superoxide
CoO2. \\ NiO2 \\ Ti/V/Cr peroxy complex \\ Triamine chromium peroxide \\ LiH \\SiO2-H2SO4 (SSA) \\ [Ni(NH3)6]

Exotic reducing agents
Ga2O TiCl2 GeCl2 && Na2S2O4
View user's profile View All Posts By User
symboom
National Hazard
****




Posts: 453
Registered: 11-11-2010
Member Is Offline

Mood: Feeling Ascaridole

[*] posted on 22-7-2017 at 21:10


Persulfates of Divalent Metals.
From google books


From this apparently pyridine and hexamine (Hexamethylenetetrammine) can form complexes with persulfates also makes me think of other combinations with pyridine perchlorate or chlorate I have been trying to form stable chlorate complexes no luck oh well so heres a list of persulfate complexes


Crystaline persulfates of the divalent metals are difficult to obtain because of their great solubility and instability.

Tetrammine-zinc persulfate,
large transparent prisms, precipitates only from very concentrated solutions formed by double decomposition between a concentrated solution of ammonium persulfate and a concentrated NH3 solution of the metal sulfate the corresponding NH3 compound separates as a crystaline percipitate

Hexammine-cadmium persulfate, CdS208.6NH3, forms white microscopic crystals, less soluble than the zinc analog Strong NH3 odor, decomposes on standing in moist atmosphere

Hexammine-nickel persulfate, NiS208.6NH3, clear blue-violet crystals, strong NH, odor. Becomes black in moist air; H20 soln. is blue, turns cloudy, percipitates NiO When dried over CaCl, it turns gray, then green, with loss of ammonia and oxygen and forms a double sulfate. In vacuum over H2SO4 it turns dirty yellow.

Tetrammine-copper persulfate dark blue-violet needles, more stable than the precededing. All the above compoinds luae ammonia and oxygen on standing some time, and explode when strongly heated or when struck.

---------------------------------------

By replacing amine with pyridine one obtains stable compounds

The Pyridine compounds are similarly prepared using 8-10 mol. Pyridine to 1 mol. metal sulfate.

Tetrapyridine-zinc persulfate glittering prisms, forms slowly from very concentrated solution Decomp. readily, turning yellow.

Tetrapyridine-cadmium persulfate, sharp glittering needles, less soluble than the Zn salt.

Tetrapyridine-nickel persulfate, thin, clear, blue microscopic needles, forms only from very concentrated solution

Tetrapyridine-copper persulfate, masses of blueviolet microscopic needles, insoluble in presence of excess Pyridine and ammonium persulfate
------------------------------------
Hexamethylenetetrammine compds. were similarly prepd., using 2 mol. Hexamethylenetetrammine to 1 mol. metal sulfate. The compounds obtained should be quickly separated. and washed with ethanol since they decompose rapidly when moist but are more stable when dry.

BisHexamethylenetetramine-magnesium persulfate-octahydrate forms colorless silky scales.

BisHexamethylenetetramine-manganese persulfate-octahydrate - colorless scales.

BisHexamethylenetetramine-cobalt persulfate-octahydrate rose-colored scales.

BisHexamethylenetetramine-nickel persulfate-octahydrate, green scales.
The above 4 compounds are all isomorphous.


[Edited on 23-7-2017 by symboom]
View user's profile View All Posts By User
 Pages:  1  ..  17    19

  Go To Top