Sciencemadness Discussion Board - Copper Compound Collection

Copper Compound Collection

nlegaux - 28-11-2014 at 13:44

One of my current goals in home chemistry is to collect as many Copper compounds as possible.
Currently I have the following:
- Chevreul's Salt
- Copper Carbonate
- Copper Sulfate
- Copper Phosphate
- Tetraamminecopper(ii) sulfate
- Copper Aspirinate
- Copper Acetate
- Copper Borate (I think)

These are the compounds I plan on making:
- Copper Hydroxide
- Copper Citrate
- Copper Formate
- Copper(i) Chloride
- Copper (ii) Chloride
- Copper (i) Oxide
- Copper (ii) Oxide
- Copper Nitrate

Can anyone think of any Copper compounds not on either list?

Thank you,

Nick

DraconicAcid - 28-11-2014 at 13:50

Oxalate, sulphide, copper(I) iodide...

[Edited on 28-11-2014 by DraconicAcid]

TheChemistryShack - 28-11-2014 at 13:52

If you are willing to mess with HF you could synthesize CuF2
Of course all of the other cupric halides like CuBr2 and CuI2 (and their cuprous forms as well)
Copper sulfide
Check out this page; it lists a bunch of copper compounds: http://www.webelements.com/copper/compounds.html

DraconicAcid - 28-11-2014 at 13:53

Quote: Originally posted by TheChemistryShack

Of course all of the other cupric halides like CuBr2 and CuI2

Copper(II) iodide isn't stable, and decomposes to copper(I) iodide and iodine.

Zyklon-A - 28-11-2014 at 15:11

I can't think of any others, but my "collection" is:
Copper (II) sulfate (anyhdrous and pentahydrate)
Copper (II) chloride (anyhdrous and dihydrate)
Copper (II) nitrate (unknown hydrate)
Copper (II) bromide (anyhrous)
Copper (II) carbonate (basic)
Copper (II) hydroxide
Copper (II) oxide
Copper (II) aspirinate
Copper (II) acetate
Copper (I) chloride
Copper (I) bromide (not tested)
Copper (I) oxide

I haven't really tried to collect any specifically, it all sortta just happened.

I want to make some anyhydrous copper nitrate, but it's really hard and not too practical.

[Edited on 28-11-2014 by Zyklon-A]

nlegaux - 28-11-2014 at 16:21

Nice list! What is it you used to make your Copper (II) Bromide?

Zyklon-A - 28-11-2014 at 16:28

Thanks. Hydrobromic acid and copper (II) hydroxide or carbonate.
HBr (aq) was made from H₂SO₄ and NaBr I think - not an easy reaction to do, cause it partially oxidizes bromide to bromine.
I ought to find a better way to make such a useful acid.

The Volatile Chemist - 28-11-2014 at 17:31

I can't recall if there is a copper-thiosulfate complex or not, I know there's one of cobalt(ii) and iron(ii & iii).

blargish - 28-11-2014 at 21:54

A good one would be the copper (III) complex with periodate ions. I believe the anion is bis-orthoperiodato dihydroxo cuprate (III). It can be made if you have a periodate salt.

Texium - 28-11-2014 at 22:33

Try the copper(II) dichloroisocyanurate complex. It's extremely purple, unusual for a copper compound. You can make it very easily if you can get some sodium dichloroisocyanurate as a pool chlorination chemical. Simple precipitation reaction between it and copper(II) sulfate.

j_sum1 - 29-11-2014 at 02:34

I have some trichloroisocyanuric acid. I might have a play.

Amos - 29-11-2014 at 06:15

If you're looking to make the chlorides and oxides, including the bright yellow hydrous copper(I) oxide, this might help you:
http://www.reddit.com/r/homechemistry/comments/2ec832/colorf...
Just scroll down to the comments that detail syntheses.

I was wondering, since the common household drug ibuprofen is an acid, if it is possible to make a sodium salt by neutralization, and then to precipitate a "copper ibuprofenate" using a water-soluble copper salt.

Texium - 29-11-2014 at 09:10

Quote: Originally posted by No Tears Only Dreams Now

I was wondering, since the common household drug ibuprofen is an acid, if it is possible to make a sodium salt by neutralization, and then to precipitate a "copper ibuprofenate" using a water-soluble copper salt.

I think that Pinkhippo has successfully accomplished that. The other day I saw it on a list of chemicals that he has. I'd like to try that too, once I recrystallize some ibuprofen.

nlegaux - 29-11-2014 at 09:10

I got some 57% Sodium Dichloroisocyanurate the other day. I guess I will recrystallize it and try making the Copper Complex

nlegaux - 29-11-2014 at 09:16

Could Ibuprofen be separated from the tablets in a similar way to ASA being separated from aspirin? In the past I was able to successfully separate ASA from aspirin; it seems like the properties of Ibuprofen are similar enough to ASA to use the same procedure.

Also, I made some Copper Sulfide yesterday. Is there a way to tell if if it is a mix of the Sulfides or just one? Based on what I read on wikipedia, the copper reacts with Sulfur vapors to form Cu2S, which can react with molten sulfur to produce CuS. Looking at it under a microscope, it looks fairly consistent (black with copper oxide coating some of it).

[Edited on 11-29-2014 by nlegaux]

Hawkguy - 29-11-2014 at 11:03

Try Copper Tetraamine Persulfate, and I think Copper Tetraamine Nitrate can be made too ... Copper complexes are the bomb dot com

blargish - 29-11-2014 at 12:13

Quote: Originally posted by nlegaux

I got some 57% Sodium Dichloroisocyanurate the other day. I guess I will recrystallize it and try making the Copper Complex

Here is a cool document with some information about the complex, and the procedure for making it. Apparently, the complex is of the form, Na₂[Cu(C₃N₃O₃Cl₂)]

Attachment: Transition Metal Dichloroisocyanurate Complexes.pdf (368kB)
This file has been downloaded 647 times

nlegaux - 29-11-2014 at 14:41

Thanks for the document blargish! I couldn't find much information it it anywhere!

Zephyr - 29-11-2014 at 15:37

Quote: Originally posted by nlegaux

Could Ibuprofen be separated from the tablets in a similar way to ASA being separated from aspirin? In the past I was able to successfully separate ASA from aspirin; it seems like the properties of Ibuprofen are similar enough to ASA to use the same procedure.
[Edited on 11-29-2014 by nlegaux]

Yes, I filter and recrystallized twice with ethanol, and received nice large crystals. Here is a picture of the copper Ibuprofenate;

Among other thins I have also made copper stearate, benzoate, nitrite(?), formate, silicate, and what I think is copper chromate.

[Edited on 11-29-2014 by Pinkhippo11]

[Edited on 11-29-2014 by Pinkhippo11]

nlegaux - 29-11-2014 at 15:55

What method did you use to create Copper Silicate? I can't find any clear directions on preparing it...

DraconicAcid - 29-11-2014 at 18:10

Quote: Originally posted by Pinkhippo11

Here is a picture of the copper Ibuprofenate;

Is that soluble in anything? It looks like it could be recrystallized.

bismuthate - 29-11-2014 at 18:16

Is your copper chromate a slightly reddish brown?

Zephyr - 29-11-2014 at 19:57

In order;

1. I created copper silicate by reacting a solution of sodium silicate with a solution of copper chloride, then filtering the blue precipitate. Due to the filtration, the ammount of copper chloride to sodium silicate need not be exact, because any excess with be seperated by the filtration.
Here is a thread on the subject.

2. I tested in water, acetone, and isopropanol; it wasn't soluble in water, it just floated to the top. I acetone a minute amount dissolved, and the rest settle to the bottom. In isopropanol, more dissolved than in the others, but I don't think its soluble enough to enable crystal growing. Let me know if you have any solvents in mind you'd lime me to test.

3. I prepared the copper chromate by adding sodium dichromate to a solution of copper sulfate. Nothing happened, and I was mildly disappointing. But as soon I added a spec of sodium hydroxide, the reddish brown salt converted from copper chromate to copper dichromate, and precipitated out.

[Edited on 11-30-2014 by Pinkhippo11]

blargish - 29-11-2014 at 20:19

Quote: Originally posted by Pinkhippo11

3. I prepared the copper chromate by adding sodium dichromate to aa solution of copper sulfate. Nothing happened, and I was mildly disappointing. But as soon I added a spec of sodium hydroxide, the reddish brown salt converted from copper dichromate to copper chromate, and precipitated out.

Are you sure that that is copper(II) chromate? This website says that copper chromate is a dark green color.
http://www.rsc.org/Education/EiC/issues/2007July/ExhibitionC...

Maybe what you have is a basic form combined with hydroxide ions or something.

nlegaux - 29-11-2014 at 20:38

I went ahead and tried the recrystallization of ibuprofen using IPA (I don't have large enough amounts of the other solvents on hand to use...). The red coating on the tablets also dissolved in the IPA, and i'm not sure how to separate it. I will go ahead and add the water; maybe one will remain in solution while the other drops out. I may be able to separate them after they precipitate out.

j_sum1 - 29-11-2014 at 20:48

Quote: Originally posted by blargish

Quote: Originally posted by nlegaux

I got some 57% Sodium Dichloroisocyanurate the other day. I guess I will recrystallize it and try making the Copper Complex

Here is a cool document with some information about the complex, and the procedure for making it. Apparently, the complex is of the form, Na₂[Cu(C₃N₃O₃Cl₂)]

zts16 has a lovely picture here. http://www.sciencemadness.org/talk/viewthread.php?tid=45845&...

I feel somewhat inspired. The colour is really pretty. I don't have any sodium dichloroisocyanurate though. I do have some TCCA and if I am not mistaken I can make some by reacting with NaOH.
Thanks for the link although I haven't read much of it yet. There are loads of possibilities. I will also substitute NaOH for KOH and see what the potassium variant looks like. And I can substitute Cu for Pb, Ni, Co and possibly Mn. This could be a fun little project.

By the way, in this post, Nicodem reports a molecular formula different from what you have stated above. Apparently there are 4 dichloroisocyanurate ligands.

Quote: Originally posted by Nicodem

The reaction of CuSO₄ and sodium dichloroisocyanurate in water is described in US3055889 and is claimed to give Na2[CuL₄] where L is the dichloroisocyanurate ligand: (C₃N₃O₃Cl₂)^-. Described are also the preparation of analogous Ca, K, Ba and Li tetrakis(dichloroisocyanuro)cuprates (or whatever they are called). Analogous Cd and Ni coordination compounds are also reported.
US3115493 describes the preparation of a lead dichloroisocyanurate and this is then used in the preparation of Pb[CuL₄].
An analogous potassium nickelate dichloroisocyanuric complex is also known (DOI: 10.1016/0022-1902(64)90014-4).

[Edited on 14/3/2014 by Nicodem]

blargish - 29-11-2014 at 21:00

Quote: Originally posted by j_sum1

By the way, in this post, Nicodem reports a molecular formula different from what you have stated above. Apparently there are 4 dichloroisocyanurate ligands.

[Edited on 14/3/2014 by Nicodem][/rquote]

Oops, my bad. There formula given in the document is actually Na₂[Cu(C₃N₃O₃Cl₂)₄], you're right.

Zephyr - 29-11-2014 at 21:09

blargish, I mispoke in my previous post, what I think I have is copper (II) chromate, which is described in the CRC as reddish brown crystals with the formula of CuCrO₄.
nlegaux, the 70% ethanol I used for my recrystallization can be bought cheaply at most pharmacies and works well. Good luck with your isolation.

nlegaux - 30-11-2014 at 08:18

Trying to recrystallize Ibuprofen with IPA failed... No crystals formed when water was added, even when chilled overnight. I guess I will have to go buy some Ethanol

[Edited on 11-30-2014 by nlegaux]

sum - 14-1-2015 at 04:47

Hi,I am new in this.I want to know how to make copper(||)acetoarsanite (Paris green).this is one of copper compound.

The Volatile Chemist - 14-1-2015 at 09:15

I like making Fehling's solution, although you kinda get a mix of compounds if you crystallize it out, it's still pretty enough to 'collect'.
Try copper(II) ferricyanide and copper(II) ferrocyanide, both different brown-like colors.

Amos - 14-1-2015 at 09:51

Quote: Originally posted by sum

Hi,I am new in this.I want to know how to make copper(||)acetoarsanite (Paris green).this is one of copper compound.

So why not look up a preparation for it? Simply google searching it seems to indicate one can just add arsenic trioxide to a copper acetate solution. It might be more complicated, so maybe do some research.

Praxichys - 14-1-2015 at 10:02

Quote: Originally posted by Zyklon-A

Thanks. Hydrobromic acid and copper (II) hydroxide or carbonate.
HBr (aq) was made from H₂SO₄ and NaBr I think - not an easy reaction to do, cause it partially oxidizes bromide to bromine.
I ought to find a better way to make such a useful acid.

There is a better way to make CuBr2, without the acid.

NaBr + CaCl2 <--> NaCl + CaBr2

CaBr2 is about 5 times as soluble as NaCl, so it is easily purified by concentration, filtering most of the NaCl, then fractional crystallization.

CaBr2 + CuSO4 --> CuBr2 + CaSO4

Calcium sulfate is 265 times less soluble than CuBr2 (basically insoluble) and can be filtered out, leaving a solution of CuBr2.

The Volatile Chemist - 14-1-2015 at 16:39

Quote: Originally posted by Praxichys

Quote: Originally posted by Zyklon-A

Yup. Of course, fractional crystallization isn't the easiest, but still.

Squall181 - 14-1-2015 at 18:30

Here's an idea for displaying your copper compounds. I tried to recreate the peg game that you find at Crackle Barrel with copper compounds and it turned out pretty good.
The compounds are sealed in culture tubes and the triangle is machined acrylic. I have since made a new and improved version, but I don't have a picture handy at the moment.

Zyklon-A - 14-1-2015 at 18:46

Thanks for that Praxichys, I'll be sure to use that method next time and save what little HBr(aq) I have left.
Beautiful collection Squall181! I know what most of those are, but could you list them?

bismuthate - 14-1-2015 at 18:57

In my experience copper ferricyanide is a yellow color.

Squall181 - 14-1-2015 at 19:16

The one's visible in the picture from top right are: Copper Acetate, Copper(II) Chloride, Copper(II) Oxide, Copper, Tetraaminecopper(II) sulfate. The rest are copper nitrate, copper carbonate, copper bromide, copper(I) oxide, copper(I) chloride, copper sulfate, copper sulfide, Copper Cyanurate, and copper aspirinate. I believe that all the ones I have.

numos - 14-1-2015 at 22:25

Quote: Originally posted by Squall181

Here's an idea for displaying your copper compounds. I tried to recreate the peg game that you find at Crackle Barrel with copper compounds and it turned out pretty good.
The compounds are sealed in culture tubes and the triangle is machined acrylic. I have since made a new and improved version, but I don't have a picture handy at the moment.

This looks really, nice, I'll have to see what local prices for Plexiglas are. Here is a picture of my collection. Copper benzoate was made after this picture was taken and hence not in it.

From left to right:
Chevreul's salt - Copper I iodide (with water) - Pyridine copper iodide - tetrachlorocopper complex - Copper oxalate - Copper II chloride - Copper stearate - Copper carbonate - Copper acetate - Copper oleate - Copper (durr) - Copper aspirinate - Copper II sulfate - Copper nitrate - Tetraaminecopper II sulfate - Pyridine/Copper nitrate complex - Copper phthalocyanine - Copper sulfate/cyanurate - A mislabeled vial of decomposed copper complex (I have no clue where it came from I found it in a corner of a shelf, but I have no clue what it is.) - Copper bromide - Copper II oxide

nezza - 15-1-2015 at 01:32

Copper (en) perchlorate is fun. Woelen & myself have synthesised this from copper sulphate, ammonium perchlorate and ethylene diamine.

Attachment: Copper.mp4 (1.2MB)
This file has been downloaded 805 times

The Volatile Chemist - 15-1-2015 at 12:33

Quote: Originally posted by bismuthate

In my experience copper ferricyanide is a yellow color.

I've been doing a lot of Iron cyanide indicator experimentation recently, it has always had a yellow brown color, with a tint of green, but I just call it brown. It's kinda brown mustard colored for me. I've seen with coloration for others, it has to do with the concentration of the ferricyanide and the concentration of the iron cyanide, which change crystal size.

Nezza, that does look fun!
Numos, your collection is great!

sasan - 15-1-2015 at 23:43

Hey guys try copper tungstate by treating sodium tungstate and copper sulfate or nitrate solutions to obtain dense copper tungstate precipitate.

sasan - 15-1-2015 at 23:45

and try potassium bisoxalatocuprate dihydrate

[Edited on 16-1-2015 by sasan]

potassium bisoxalatocuprate dihydrate.jpg - 810kB

sasan - 15-1-2015 at 23:50

oh I have forgotten copper tetraiodomercurate

[Edited on 16-1-2015 by sasan]

warteo - 16-1-2015 at 00:04

The mention of an orange Cu(II) complex in this paper Copper(II) Complexes With Lignin Model Compound Vanillin got me interested. The synthesis appeared easy so I gave it a go:

[Cu(C8H7O3)2(H2O)2] (2): [Cu2(O2CCH3)4(H2O)2]
(0.160 g) was dissolved at room temperature in 10.0 mL
of acidified water (one drop of glacial acetic acid). The
solution and solid vanillin (0.244 g) were slowly heated
in two separated flasks. When vanillin had melted, the
acetate solution was put over melted vanillin that turned
red and dissolved in ~5 seconds. Orange crystals of 2
were filtered off next day and dried in air for a day.

However both of my attempts following the above failed. There was obviously a reaction because the blue copper acetate solution instantly turned the most beautiful emerald green upon addition to the molten vanillin. Upon cooling a large crop of pale green needle crystals formed which are quite possibly compound 1.

Anyone else care to try this and see if they can achieve the orange compound? I'd really like to know where I went wrong (currently suspecting not high enough temperature at mixing time). I'll need to make some more copper acetate before making another attempt.

DraconicAcid - 16-1-2015 at 10:14

Quote: Originally posted by warteo

The mention of an orange Cu(II) complex in this paper Copper(II) Complexes With Lignin Model Compound Vanillin got me interested. The synthesis appeared easy so I gave it a go:

[Cu(C8H7O3)2(H2O)2] (2): [Cu2(O2CCH3)4(H2O)2]
(0.160 g) was dissolved at room temperature in 10.0 mL
of acidified water (one drop of glacial acetic acid). The
solution and solid vanillin (0.244 g) were slowly heated
in two separated flasks. When vanillin had melted, the
acetate solution was put over melted vanillin that turned
red and dissolved in ~5 seconds. Orange crystals of 2
were filtered off next day and dried in air for a day.

However both of my attempts following the above failed. There was obviously a reaction because the blue copper acetate solution instantly turned the most beautiful emerald green upon addition to the molten vanillin. Upon cooling a large crop of pale green needle crystals formed which are quite possibly compound 1.

Anyone else care to try this and see if they can achieve the orange compound? I'd really like to know where I went wrong (currently suspecting not high enough temperature at mixing time). I'll need to make some more copper acetate before making another attempt.

That's cool- I didn't think vanillinate would make that good of a ligand. I may have to try that. It strikes me as odd, though, that a change in the hydration (without a change in the coordination) would give such a strong change in colour. I suspect that their formulation of compound 2 was incorrect- I wonder if they ever did get a crystal structure?

ETA: They did get a crystal structure, and it is the cis isomer. Z. Naturforsch. 60b, 1273 – 1277 (2005);

Has anyone ever made KCuCl₃? It's supposed to form ruby-red crystals, but I've never managed to get it to work.

[Edited on 16-1-2015 by DraconicAcid]

blargish - 16-1-2015 at 10:43

Quote: Originally posted by DraconicAcid

Has anyone ever made KCuCl₃? It's supposed to form ruby-red crystals, but I've never managed to get it to work.

I've never done it personally, but I've come across a prep for it online (the source is attached).

Preparation of Potassium Trichlorocuprate (II)
Dissolve 1.0g of Potassium Chloride (KCl) in 3.7 mL of distilled Water. In a fume hood,
dissolve 5.5g of Cupric Chloride Dihydrate (CuCl2•2H2O) in 50 mL of concentrated HCl in a
250 mL Erlenmeyer flask. Stir the mixture until it is dissolved; this may take several minutes.
Do not heat the mixture as this will drive off the HCl. Essentially dropwise, pour the KCl
solution into the CuCl2 solution slowly and with rapid stirring. Place the Erlenmeyer in an Ice
bath for half an hour. Vacuum filter the red, needle-like crystals in a medium porosity sintered
glass crucible. Spread the damp precipitate onto a watch glass and dry them in an oven that is
not any hotter than 85oC. Once dry, weigh the product and then store the sample in a 3 dram vial
flushed with Nitrogen and sealed with Parafilm wax.

Is this the procedure that you attempted?

[Edited on 16-1-2015 by blargish]

Attachment: Two Interesting Copper Compounds.pdf (299kB)
This file has been downloaded 1687 times

DraconicAcid - 16-1-2015 at 10:51

Quote: Originally posted by blargish

Quote: Originally posted by DraconicAcid

Has anyone ever made KCuCl₃? It's supposed to form ruby-red crystals, but I've never managed to get it to work.

Yes, from the same source. No red needles or red precipitate of any kind.

bbartlog - 16-1-2015 at 12:36

I've tried to prepare KCuCl₃ by a different method; according to Atherton Seidell's 1919 book on solubilities (p. 268), a mixed solution of KCl and CuCl₂ at elevated temperatures (above 72 C or so) will precipitate this double salt as it evaporates, if the compounds are present in roughly equimolar amounts. Had difficulties with the temperature control and set the solution aside, though.

At lower temperatures it appears that a different, blue-green double salt is precipitated from aqueous solution: CuCl₂.2KCl.2H₂O. I suppose that the use of concentrated HCl in the prep you mention changes things so that this compound isn't the result.

nlegaux - 17-1-2015 at 07:39

Wow, Those complexes look really nice! If I can get some of the reagents together, I will have to attempt to prepare them.

Where do you buy your Sodium Tungstate? All I have been able to find is a product on amazon (50 grams or so for $100). Since this is the only synthesis for it I would have planned, I am not ready to drop that kind of money on it.

gdflp - 17-1-2015 at 07:59

Try buying tungsten disulfide as "dry lube", some hardware stores have it, but lots of people sell it on eBay rather cheaply. This is then heated to 1250°C in a crucible with a propane torch until the dark green powder has turned canary yellow. This is WO₃ which can be dissolved in sodium hydroxide to yield Na₂WO₄.

EDIT: Fixed incorrect chemical formula

[Edited on 1-17-2015 by gdflp]

nlegaux - 20-1-2015 at 19:09

Thanks for the tip! I will definitely have to check my local hardware store for some.