symboom
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Help add to the sciencemadness wiki
I hope this question is not too vague
For example I would add
That silica gel can absorb iodine, Bromine, nitrogen dioxide and sulfuric acid
solidified form making it a storage medium for reactions.
Iodine
https://www.sciencemadness.org/whisper/viewthread.php?tid=84...
Nitrogen dioxide
http://www.sciencemadness.org/talk/viewthread.php?tid=61896
I also came across how sodium can be absorbed on silica which is not well known.
Sodium
http://www.sciencemadness.org/talk/viewthread.php?tid=14626
Added to
http://www.sciencemadness.org/smwiki/index.php/Silica_gel
Anyone have any posts of chemical synthesis that is missing on the wiki. From youtube videos such as the poor man's chemist which has many uncommon
chemicals that could be added or from sciencemadness posts.
[Edited on 4-9-2020 by symboom]
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symboom
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Format of the science madness wiki
IUPAC chemical name
Quick information
(Infobox on the right)
Properties
>Chemical
>Physical
Availability
Preparation
Projects
Handling
>Safety
>Storage
>Disposal
References
Relevant Sciencemadness threads
____________________________________
These are chemicals not found on the sciencemadness wiki
Here is from the poormanschemist channel
---
Sodium bismuthate
Chemicals for synthesis
bismuth trioxide
bromine
aqueous sodium hydroxide.
PROPERTIES:
Formula weight 280.0. Fine yellow needles. Variable water content may go as high as 5 H2O. The usual formula is NaBiO3 • 3.5 H3O. Reacts with acids
with partial decomposition and formation of higher bismuth oxides; oxidizes Mn(II) in H2SO4to MnO4 in the cold."
Preparation
"Bi2O3 + 6NaOH + 2 Br2 = 2 NaBiO3 + 4 NaBr + 3 H2O
A suspension of 170 g. of Bi3O3 in 1.5 liters of 40% sodium hydroxide is vigorously stirred and oxidized at the boiling point by gradually added Br3
(300 g.). The brown precipitate formed is filtered off, washed with 40% sodium hydroxide, and suspended in three liters of H3O. The suspension is now
agitated for a while, until the color changes from brown through light brown to yellow. The precipitate is then allowed to settle; it is filtered,
added to 1.5 liters of 53% NaOH, and refluxed for one half hour. The resultant brown precipitate is readily filtered off after settling. It is washed
with 50% sodium hydroxide, placed, while still damp, in three liters of H3O, and briefly agitated. When the yellow precipitate settles, it is
filtered, thoroughly washed with water, and finally dried on clay. The yield is 170 g.
Projects
Oxidative cleavage of glycol, ketol or alpha hydroxy acids
Determine if manganese is present in sample
Handling
>Safety
>Storage
>Disposal
References
The following synthesis is taken from The Handbook of Preparative Inorganic
Chemistry, edited by Georg Brauer. Volume 1 page 627-628. It has been modified slightly for clarity.
https://m.youtube.com/watch?v=Izd4WHqq2Rw&t=73s
___________________________________________
Potassium bromate
Preparation and References
https://www.prepchem.com/synthesis-of-potassium-bromate/
https://m.youtube.com/watch?v=AqFvOeETqjY
---------
Antimony iodide
Preparation and References
http://antimony.atomistry.com/antimony_triiodide.html
https://m.youtube.com/watch?v=72n2ao33yCI
-----------
Indium monoiodide
Preparation and References
https://m.youtube.com/watch?v=OxFCwMCnBhs
http://indium.atomistry.com/indium_mono_iodide.html
http://indium.atomistry.com/indium_tri_iodide.html
https://en.m.wikipedia.org/wiki/Indium_halides#InI
---------
Bismith pentoxide
Preparation and References
https://m.youtube.com/watch?v=UXwMFIHWWlo
---------
Sodium metavanadate
Preparation and References
https://m.youtube.com/watch?v=d7qim9bKI8c
---------
Tellurium iodide
Preparation and References
https://m.youtube.com/watch?v=fHRO8-m0c84
---------
dinitrotetramminenickel(II)
Preparation and References
https://m.youtube.com/watch?v=GNHdWMJ0uak
---------
Reiecke's salt
Preparation and References
https://m.youtube.com/watch?v=81zxZzPecjE
https://m.youtube.com/watch?v=t2ePnoCM-gk
---------
Crystalloluminescence
Light forming crystalization of strontium compound
Crystalloluminescence of strontium bromate
https://youtu.be/QwiWjSK4tfc
Samarium iodide/chloride/ salts??
[Edited on 29-9-2020 by symboom]
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B(a)P
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I am a little confused. Are you looking for assistance to write these up or for more content that people have noticed is missing? I would be happy to
draft up a few if that was of assistance.
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symboom
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I'm adding the link to preparation and the video of synthesis.
add what chemicals are missing that you think the wiki should have. It's more of an example. It doesn't have to be absolute just what ever chemical
and section you can add to. this should help build the wiki. Well I'd be interested in what chemical you want to add put the information here.
Hope that is more clear. Happy to have the assistance.
[Edited on 29-9-2020 by symboom]
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B(a)P
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I am happy to help with any of them. Feel free to send one or two my way and I will send you a write up for review.
I just noticed that nickel perchlorate has an error in the wiki, in the first sentence of the first paragraph it starts nickel nitrate......
It would also be nice to include:
ammonium iodide
cesium fluoride
antimony sulfide
I could make a start on these three or any others that you think are more necessary.
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symboom
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I can't think of any right now just common salts.
That would be great start there is a lot to add.
http://www.sciencemadness.org/smwiki/index.php/Samarium
There is a lot of red links here
Samarium oxide
Samarium chloride
Samarium iodide
I feel like this could be a thread to add compounds and pages to the wiki
And the wiki discussion http://www.sciencemadness.org/talk/viewthread.php?tid=65174 seems to turn in to a thread to declare what needs to be fixed and corrected.
[Edited on 29-9-2020 by symboom]
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symboom
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Samarium oxide
Preparation
thermal decomposition of samarium(III) carbonate, hydroxide, nitrate, oxalate or sulfate:
Sm2(CO3)3 → Sm2O3 + 3 CO2
2. by burning the metal in air or oxygen at a temperature above 150 °C
The oxide can be reduced to metallic samarium by heating with a reducing agent, such as hydrogen or carbon monoxide, at elevated temperatures
Projects
Catalytic properties used in dehydrogenation and dehydration of alcohols and the dehydrogenation of tetralin.
Reference
Bulletin of the Academy of Sciences of the USSR, Division of chemical science
_______________
Samarium trichloride
SmCl3 is prepared by the "ammonium chloride" route, which involves the initial synthesis of (NH4)2[SmCl5]. This material can be prepared from
ammonium chloride and samarium oxide at reaction temperatures of 230 °C from samarium oxide:
10 NH4Cl + Sm2O3 → 2 (NH4)2[SmCl5] + 6 NH3 + 3 H2O
The pentachloride is then heated to 350-400 °C resulting in evolution of ammonium chloride and leaving a residue of the anhydrous samarium
trichloride:
(NH4)2[SmCl5] → 2 NH4Cl + SmCl3
_______________________
Samarium (III) fluoride
Preparation
Aqueous solutions of samarium chloride can be used to prepare samarium trifluoride
SmCl3 + 3 KF → SmF3 + 3 KCl
__________________________
Samarium (II) fluoride
Preparation
Samarium(II) fluoride can be produced by using samarium or hydrogen gas to reduce samarium(III) fluoride
_______________________
Samarium (II) iodide
When employed as a solution for organic synthesis, it is known as Kagan's reagent. Typical reaction conditions use SmI2 in THF in the presence of
catalytic NiI2.
It is a strong one-electron reducing agent that is used in organic synthesis it is a very strong reducing agent. it rapidly reduces water to hydrogen
Preparation
Samarium iodide is easily prepared in nearly quantitative yields from samarium metal and either diiodomethane or 1,2-diiodoethane.
_____________________
Ammonium bromide
Preparation
Ammonium bromide can be prepared by the direct action of hydrogen bromide on ammonia.
NH3 + HBr → NH4Br
It can also be prepared by the reaction of ammonia with iron(II) bromide or iron(III) bromide, which may be obtained by passing aqueous bromine
solution over iron filings.
2 NH3 + FeBr2 + 2 H2O → 2 NH4Br + Fe(OH)2
Modified version of the solvay process
product of the Solvay process used to produce sodium carbonate:[3]
CO2 + 2 NH3 + 2 NaBr + H2O → 2 NH4Br + Na2CO3
Calcium Bromide and ammonium sulfate can also for ammonium bromide due to insoluble calcium sulfate that is formed to drive the reaction forward.
[Edited on 30-9-2020 by symboom]
[Edited on 30-9-2020 by symboom]
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symboom
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Aluminium chlorate
mixing aluminium sulfate 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.
___________________
Phosphorous trioxide
Phosphorous oxide has also been prepared by the action of the trichloride on phosphorous acid, thus
H3PO3 + PCl3 = P2O3 + 3HCl
It is also produced when phosphorus trichloride is used to replace the hydroxyl group of anhydrous acetic acid, thus
-----------------------------
phosphorous acid
white phosphorus is placed in a deep cylinder and covered with water. The element is melted and chlorine is passed in through a tube which dips well
into the phosphorus. Large quantities may be quickly obtained by this method, but the product contains phosphoric acid. Regulated action of PCl3 on
water may be effected by passing a current of dry air through the trichloride kept at 60° C. and then through two wash- bottles containing water. The
action is also much less violent if an acid such as concentrated aqueous hydrochloric acid is used in place of the water. Oxalic acid is most
suitable, since it is dehydrated with decomposition when heated in a flask with phosphorus trichloride. The flask is furnished with a reflux
condenser. Much of the HCl is evolved and a concentrated solution of phosphorous acid remains:—
PCl3 + 3H2C2O4 = H3PO3 + 3CO + 3CO2 + 3HCl
these preparations it is usually necessary to remove the hydrochloric acid which is produced; this may be done by distilling the solution up to a
temperature not exceeding 180° C. A syrupy liquid is then obtained which, after cooling, crystallises quickly, or at any rate within a few hours. The
process may be hastened as usual by seeding
Properties
crystalline acid was found to melt at 70.1° C., 74° C. The density of the liquid supercooled at 21° C. was 1.651. The latent heat of fusion of the
acid was found to be 7.07 Cals. The heat of solution of the acid per mol dissolved in 400 mols or more of water was +233 Cals. The heat of formation
of the crystallised acid has been given as +227.7 Cals.
Sodium phosphite
neutralising phosphorous acid to the appropriate end point with alkali hydroxides and evaporating to crystallisation.
By neutralising a solution of phosphorous acid, or one made from PCl3, with ammonia and adding a salt of the required metal.
By dissolving the hydroxide of the base in phosphorous acid.
phosphites are fairly stable in the absence of oxidising agents and dilute solutions may even be boiled without decomposition. More concentrated
solutions may decompose, giving hydrogen; thus
Na2HPO3 + NaOH = Na3PO4 + H2
------------------------
Sodium perphosphate
Simular to sodium percarbonate it is an adduct with hydrogen peroxide
Peroxymonophosphoric acid
most widely used method of preparation is the hydrolysis of potassium of lithium peroxydiphosphate in a strong acid such as perchloric acid.
can be obtained from the reaction between phosphorus pentoxide and highly-concentrated hydrogen peroxide within an inert solvent like acetonitrile or
carbon tetrachloride
((less vigorous method of preparing peroxyphosphoric acid by introducing the inert solvent acetonitrile instead of by themselves was described by
Gerrit Toennies in 1937. This method was shown to be unsuitable in diethyl ether or isoamyl alcohol.))
---------
Peroxodiphosphates can be obtained by electrolysis of phosphate solutions
---------------
The Sodium hyponitrite
, Na2N2O2, can be prepared by reducing sodium nitrite with sodium-amalgam and precipitating the solid by addition of alcohol to the solution. The
reduction can also be effected by means of sulphur dioxide.
Sodium hyponitrite is readily soluble in water, the concentrated solution being stable in presence of a large proportion of sodium hydroxide. On
crystallization the salt is deposited as pentahydrate, this substance losing its water of crystallization in a desiccator or on exposure to air. The
anhydrous salt is the more stable form; it melts with decomposition at 300° C. The cryoscopic method gives the double molecular formula, Na2N2O2.
------------------------
Hydroxylamine phosphite, (NH2OH)2.H3PO3, was prepared by double decomposition of one mol of Na2HPO3 with two mols of NH2OH.HCl. The sodium chloride
was crystallised out by evaporation in vacuo, and the very soluble hydroxylamine salt crystallised from alcohol. It melts easily, is inflammable and
is a strong reducing agent. Hydrazine phosphite, N2H4.H3PO3, has also been prepared, from barium phosphite and hydrazine sulphate.
[Edited on 20-10-2020 by symboom]
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B(a)P
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For review/inclusion in the wiki
IUPAC chemical name
diantimony trisulfide, antimony(III) sulfide
Quick information
Other names
antimony sulfide, antimonious sulfide, antimony sesquisulfide, antimony vermilion, black antimony, sulphuret of antimony
Antimony trisulfide (Sb2S3) occurs in nature as the mineral stibnite. It is formed as a low temperature deposit from hot solutions often associated
with arsenic minerals and cinnabar.
Significant deposits occur in Algeria, Borneo, Canada, China, Czechoslovakia, the Federal Republic of Germany, France, Italy, Japan, Mexico and Peru
(Pough, 1960; Roberts et al., 1974; Palencia & Mishra, 1986). Antimony trisulfide is a moderately acid soluble antimony source.
Properties
Antimony trisulfide in its mineral form, stibnite, is an orthorhombic-bipyramidal crystalline structure
(Roberts et al., 1974).
Molecular weight: 339.68 g/mol
Appearance: grey / black orthorhombic crystal (stibnite)
Density: 4.562 g/cm3 (Lide, 2001)
Melting point: 550 C (Merck, 2001)
Solubility: H2O 175 ug/100 mL; soluble in alkalies and in concentrated hydrochloric acid and sulfide solutions, and in ethanol (Herbst et al., 1985;
Lewis, 2002; Lide, 2001; Merck, 2001)
Availability
Preparation
Amorphous (red to yellow-orange) antimony trisulfide can be prepared by treating an antimony trichloride solution with hydrogen sulfide or sodium
thiosulfate, or by heating metallic antimony or antimony trioxide with sulfur (Freedman et al., 1992)
Projects
Antimony trisulfide is used in combination with potassium chlorate (along with other compounds) to make friction primers.
Crude commercial antimony trisulfide can be used directly in the manufacture of matches or Bengal lights. For the production of high-quality
pyrotechnics, e.g., electrically ignited detonators, the crude compound must be remelted in a reducing atmosphere at as slow a temperature as
possible. A well-crystallized, readily ground product is obtained (Herbst et al., 1985).
Antimony trisulfide is used in the production of vermilion or yellow pigment and antimony salts such as antimony oxide and chloride, and in the
manufacture of ruby glass (Mannsvle Chemical Products Corp., 1985; Palencia & Mishra, 1986; Hawley, 1981).
Handling
>Safety
Flammable/combustible material; may be ignited by friction, heat, sparks, or flames.
In industry, antimony enters the body almost entirely by inhalation of dust or fumes from processing or packing antimony compounds (McCallum, 1989).
OSHA PEL 0.5 mg/m8 8h TWA
>Storage
Keep container tightly sealed
Store in cool, dry place in tightly closed containers
Ensure good ventilation in storage area
>Disposal
Depends on jurisdiction, not appropriate to dispose to sewer or stormwater, seek advice from local environmental/waste regulator or waste disposal
company
>References
Freedman, L.D., Doak, G.O. & Long, G.G. (1992) Antimony compounds. In: Kroschwitz, J.I. & Howe-Grant, M., eds., Kirk-Othmer Encyclopedia of
Chemical Technology, 3rd ed., Vol. 3, New York, John Wiley & Sons, Inc., pp 382-412
Hawley, G.G. (1981) Condensed Chemical Dictionary, 10th ed., New York, Van Nostrand Reinhold Co., pp. 81–82.
Herbst, K.A., Rose, G., Hanusch, K., Schumann, H.& Wolf, H.U. (1985) Antimony and antimony compounds. In: Elvers, B., Hawkins, S. & Russey,
W., eds., Ullmann’s Encyclopedia of Industrial Chemistry, Vol. A3, VCH Publishers, pp 55-76
Lewis, R.J., ed. (2002) Hawley’s Condensed Chemical Dictionary
Lide, D.R., ed. (2001) CRC Handbook of Chemistry and Physics, 80th ed., (On CD-Rom) Boca Raton, FL, CRC Press
McCallum, R.I. (1989) The industrial toxicology of antimony. J.R. Coll. Physicians Lond
Merck (2001) Antimony trisulfide. The Merck Index, 12.3 ed. (On CD-Rom). Boca Raton, FL, Chapman & Hall
Palencia, C.M. & Mishra, C.P. (1986) Antimony Availability — Market Economy Countries, A Minerals Availability Appraisal (Bureau of Mines
Information Circular 9098), Washington DC, US Department of the Interior
Pough, F.H. (1960), A Field Guide to Rocks and Minerals, 3rd ed., Boston, MA, Houghton Mifflin Co., p. 102
Roberts, W.L., Rapp, G.R., Jr & Weber, J. (1974) Encyclopedia of Minerals, New York, Van Nostrand Reinhold Co., p. 582
Relevant Sciencemadness threads
https://www.sciencemadness.org/whisper/viewthread.php?tid=29...
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B(a)P
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IUPAC chemical name
Caesium fluoride
Quick information
Other names
Cesium fluoride
Caesium fluoride is an inorganic ionic compound usually found as a hygroscopic white solid. It is more soluble and more readily dissociated than
sodium fluoride or potassium fluoride. Caesium has the highest electropositivity of all non-radioactive elements and fluorine has the highest
electronegativity of all elements.
Properties
Caesium fluoride has a cubic crystal structure (Haynes 2011)
Molecular weight: 151.903 g/mol
Appearance: white crystalline solid
Density: 4.62 g/cm3 (Haynes 2011)
Melting point: 550 C (Haynes 2011)
Solubility: H2O 537 g/100 mL (25 C); Insoluble in acetone, diethyl ether, pyridine and ethanol
191 g/100 mL in methanol (Haynes 2011)
Availability
Preparation
Caesium fluoride may be prepared by the action of hydrofluoric acid on caesium hydroxide or caesium carbonate, followed by removal of water.
Projects
Caesium fluoride reacts usually as a source of fluoride ion, F-. It therefore undergoes all of the usual reactions associated with soluble fluorides
such as potassium fluoride (Smith 2002).
Being highly dissociated it is quite reactive as a fluoride source under anhydrous conditions too, and it will react with electron-deficient aryl
chlorides to form aryl fluorides ( halex reaction). Due to the strength of the Si-F bond, fluoride ion is useful for desilylation reactions (removal
of Si groups) in organic chemistry; caesium fluoride is an excellent source of anhydrous fluoride for such reactions (see uses below). As with other
soluble fluorides, CsF is moderately basic, due to the fact that HF is a weak acid. The low nucleophilicity of fluoride means it can be a useful base
in organic chemistry (Friestad 1999).
Caesium fluoride is a useful base in organic chemistry, due the fact that fluoride ion is largely unreactive as a nucleophile. It is reported that CsF
gives higher yields in Knoevenagel condensation reactions than KF or NaF.
Removal of silicon groups (desilylation) is a major application for CsF in the laboratory, as its anhydrous nature allows clean formation of
water-sensitive intermediates. Caesium fluoride in THF or DMF can attack a wide variety of organosilicon compounds to produce an organosilicon
fluoride and a carbanion, which can then react with electrophiles.
Desilylation is also useful for the removal of silyl protecting groups.
Caesium fluoride is also a popular source of fluoride in organofluorine chemistry. For example, CsF reacts with hexafluoroacetone to form a caesium
perfluoroalkoxide salt which is stable up to 60 ° C, unlike the corresponding sodium or potassium salt (Evans 1968)
Single crystals of the salt are transparent into the deep infrared. For this reason it is often used as the windows of cells used for infrared
spectroscopy.
Handling
>Safety
Causes severe skin burns and eye damage.
Fatal if swallowed, in contact with skin or inhaled.
Handle under dry protective gas.
Non-flammable (American Elements 2020)
OSHA PEL 2.5 mg/m3 long term
>Storage
Keep container tightly sealed.
Store in cool and dry place.
Store away from water and moisture, strong bases and oxidising agents. (American Elements 2020)
>Disposal
Depends on jurisdiction, not appropriate to dispose to sewer or stormwater, seek advice from local environmental/waste regulator or waste disposal
company
>References
American Elements, 2020, Safety Data Sheet, Cesium Fluoride
Evans, F. W.; Litt, M. H.; Weidler-Kubanek, A. M.; Avonda, F. P. (1968). "Formation of adducts between fluorinated ketones and metal fluorides".
Journal of Organic Chemistry. 33 (5): 1837–1839
Friestad, G. K.; Branchaud, B. P. (1999). Reich, H. J.; Rigby, J. H. (eds.). Handbook of Reagents for Organic Synthesis: Acidic and Basic Reagents.
New York: Wiley. pp. 99–103
Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics
Smith, Adam P.; Lamba, Jaydeep J. S.; Fraser, Cassandra L. (2002). "Efficient Synthesis of Halomethyl-2,2'-bipyridines:
4,4'-Bis(chloromethyl)-2,2'-bipyridine". Organic Syntheses. 78: 82.; Collective Volume, 10, p. 107
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symboom
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IUPAC chemical name
Indium(III) nitrate
>Properties
Indium nitrate forms colourless, deliquescent needle shaped crystals. One-third of its water of crystalization is decomposed at 100° and it becomes
anhydrous when dessicated with concentrated sulphuric acid. It forms a double salt with ammonium nitrate
>Production
Indium metal reacts with nitric acid and reduces the acid to ammonia gas, due to the reducing nature of indium metal. A more pure product can be
obtained by reacting indium (III) hydroxide with nitric acid it dissolves slowly in dilute nitric acid and more rapidly in concentrated nitric acid.
The indium nitrate crystallises from the nitric acid solution due to its lower soubility in nitric acid due to the common ion effect.
>References
http://indium.atomistry.com/indium_nitrate.html
[Edited on 6-11-2020 by symboom]
[Edited on 6-11-2020 by symboom]
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symboom
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IUPAC name
Iodo nitrate
Iodine nitrate is a chemical with formula INO3. (It differs from iodine nitrite with formula INO2).
The compound was first produced by the reaction of mercury(II) nitrate and iodine in ether.
Iodine nitrate is also prepared by the reaction of silver nitrate and iodine within an acetonitrile, ether, or methanol solution.
References
Hassner, Alfred (15 April 2001). "Iodine Nitrate". Encyclopedia of Reagents for Organic Synthesis: ri016
doi:10.1002/047084289X.ri016
---------
Nickel Bromate
Properties
It crystallises in unstable octahedra which are green in colour.
Preparation
prepared by reaction of barium bromate and nickel sulphate solutions. The barium sulfate precipitates out of the solution leaving nickel bromate
Uses
- make Diammonium Nickel Bromate
From its solution in aqueous ammonia, alcohol precipitates the diammoniate, Ni(BrO3)2.2NH3.
Refrences
http://nickel.atomistry.com/nickel_bromate.html
[Edited on 9-11-2020 by symboom]
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B(a)P
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I wonder if this information should be added to the picric acid wiki page - very helpful for recrystallisation.
Water Solubility (mg/L):
66,670 at 100 °C (quoted, Windholz et al., 1983)
14,000 at 20 °C, 68,000 at 100 °C (quoted, Verschueren, 1983)
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symboom
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I think if this was edited along the way on the wiki as a draft it would have been a smoother collaboration. Just an idea for next year's newsletter.
Especially if a talk page can be added.
http://www.sciencemadness.org/talk/viewthread.php?tid=156605
[Edited on 26-11-2020 by symboom]
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symboom
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cadmium(II) iodide
https://youtu.be/bIBB4LVzJhE
Mercury
Mercurous Nitrate
https://youtu.be/TiCj61u3GfI
Thorium
Thorium Hydroxide
https://youtu.be/o2T5kycQNlE
Thorium chromate
https://youtu.be/kC0KbIQBd_E
Thorium acetate
https://youtu.be/FKuc7Vn8B70
thorium superoxide // tricesium (IV) heptachlorothorium
https://youtu.be/wSDYZp9zJnM
Uranium
Uranyl ferrocyanide
https://youtu.be/GcM1SJKJGgY
Uranyl acetoacetonate
https://youtu.be/WauOvOtJvH4
barium diuranate
https://youtu.be/IRzAuf-FAlM
Uranyl Hypophosphite //Ammonium Peruranate
https://youtu.be/6FDgGGDnBJc
Uranium Trioxide
https://youtu.be/-iC4YAqzlvM
Barium Diuranate
https://youtu.be/IRzAuf-FAlM
Uranyl Sulfate
https://youtu.be/lJBC8eN1U1E
Thallium
Thallium(I) Chlorate
https://youtu.be/hH-nlxB-TSo
thallium(I) carbonate
https://youtu.be/VaZ5xqdrMG4
thallium sulfate
https://youtu.be/r80lKcyt5OI
Gold
potassium tetrabromoaurate(III) // bromoauric acid
https://youtu.be/-9Szck6KtP4
Platnium
Potassium Platinocyanide
https://youtu.be/srewuuN-LmM
Platnium group
platinum triselenide
https://youtu.be/2otuBQ_Th_M
Barium Ruthenate // Barium Iridate
https://youtu.be/gV2N2Jqpo6w
barium osmate
https://youtu.be/M5X_tLinRwo
Source
Written Procedures
http://www.poormanschemist.com/PMC_Notebook/PMC_LabNotebook....
YouTube
Project los alamos
Poormans chemist
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Refractory metal nitrates preparation
http://www.sciencemadness.org/talk/viewthread.php?tid=156511
[Edited on 4-12-2020 by symboom]
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symboom
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Posts: 1143
Registered: 11-11-2010
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Mood: Doing science while it is still legal since 2010
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Here is a old compiled list of some compounds
Hate for this effort another member put go to waste maybe some of this could be added to the wiki
http://www.sciencemadness.org/talk/viewthread.php?tid=27016
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garphield
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For the page on ethylenediamine, can someone put the method RustyShackleford (think that was his username) posted here a few months ago?
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Newton2.0
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Thanks, Symboom, I was looking for that post for a while.
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