Talk:Copper(II) nitrate

message: This page appears to have been moved from its correct place. Wikipedia encourages the use of correct Stock nomenclature in the title pages of articles on chemical compounds (see Wikipedia:Naming conventions (chemistry)): however, there is no space between the name of the element or ion and the parenthesis indicationg the oxidation number, as a quick look through :Category:Chemical compounds and its subsections will confirm.  See also Inorganic nomenclature, Wikipedia talk:WikiProject Chemicals and . Physchim62 13:21, 24 May 2005 (UTC)
replies: text: I've gone ahead and corrected this. - UtherSRG 13:40, May 246, 2005 (UTC)
It's not exactly encyclopedia-like. It does make it a little more entertaining, though, which isn't a bad thing.
What joke!!!??? 71.168.108.66 18:24, 15 January 2007 (UTC)

message: The attached MSDS makes this stuff look like the ultimate oxidizer. Cu(I)NOx may be, but.....PLEASE check asap74.108.139.186 (talk) 21:07, 15 October 2009 (UTC)
thread_title:  Wrong MSDS is attached --REALLY WRONG! 

message: The caption for the photo of the aqueous solution says "Aqueous solution of copper(II) nitrate, which contains [Cu(H2O)6]2+ ions." The solution looks green. Isn't [Cu(H2O)6]2+ blue? It is my understanding that concentrated solutions of copper nitrate look green because they still have ions with nitrate coordinated to the copper, while dilute solutions look blue because the nitrate is replaced by water. Now, I suppose it is true that even a concentrated solution contains some [Cu(H2O)6]2+, but the real question is what is useful to say in such a caption without misleading or confusing the reader. I'd just say "Aqueous solution of copper(II) nitrate", which is more or less what the caption used to say until recently. --Itub (talk) 03:52, 15 January 2012 (UTC)
replies: text: I was the one expanding the caption.  Not sure what the sample really was made from, since the contributor didn't say.  I suspect it is from dissolving copper metal in nitric acid, in which case it would contain some NO2.  --Smokefoot (talk) 13:41, 15 January 2012 (UTC)
replies: text: I think I remember once dissolving copper nitrate in water, and was fascinated by how it's green when you add a little water but then it turns blue when you add more water. So I know the phenomenon firsthand. :) I say "I think", however, because now that I've been trying to look for a reference to back that up, I find plenty of sources describing that behavior for copper chloride (even the WP article shows it), but none for copper nitrate. So maybe I misremembered the anion! (It was maybe 20 years ago.) But if any of you have some copper nitrate close at hand, perhaps you can try it (yes, I know, no original research, but I just want to know.) --Itub (talk) 14:25, 15 January 2012 (UTC)

text: I'm starting to think that you are right that the photo may be of copper recently dissolved in nitric acid. --Itub (talk) 14:42, 15 January 2012 (UTC)
thread_title:  Caption 

message: I've seen a bit of activity on this article today. Based on some of the comments on talk pages, we need clarification of the crystal structures of anhydrous and hydrated copper(II) nitrates. I've looked up and found structures for the alpha and beta forms of anhydrous Cu(NO3)2 and for Cu(NO3)2·nH2O, n = 1, 1.5, 2.5, 3, and 6. Who wants to know what? --Ben (talk) 15:25, 15 January 2012 (UTC)
replies: text: Well, for me, the main message would be that nitrate is coordinated less as the degree of hydration increases.  Although that trend might be obvious to an inorganic chemist, it would not be to a usual reader. We should mention the five hydrates and then describe the structure of the most common one, which is probably the trihydrate.  I couldn't figure out how to search for the entire set - what did you do? (I was searching Acta Cryst). If you are feeling energetic, you could enter the individual members and the refs in water of hydration, which is kind of a nifty compilation. Maybe explodonerd would be interested in helping out, kind of a project...--Smokefoot (talk) 15:56, 15 January 2012 (UTC)

text: Great stuff.  I also noticed that hexaaquo paper described no Jahn-Teller attributed to the effects of hydrogen-bonding.  If you don't get around to inserting this material, I or someone else will.  The main thing is that there are many hydrates, and a similar situation probably applies to the nitrates of other aquated divalent metals - Ni, Co, Fe, Mn, but nitrate might not be compatible with the early reducing metals.  I will look around because it would be helpful to have a similar blurb for several articles.--Smokefoot (talk) 16:50, 15 January 2012 (UTC)
thread_title:  Crystal structures of anhydrous and hydrated copper(II) nitrates 

message: Sorry, I'm just preparing an exam and I noticed the equation Cu + 4 HNO3 → Cu(NO3)2 + 2 H2O + 2 NO2 is not balanced. Actually I tried to read what it's written above here, but to be honest i don't understand. Pleasemake some reference in order to let people (like me) know if the the equation is right for some reason.
Thank you in advance, Marco79.1.219.82 (talk) 11:31, 22 February 2012 (UTC)
replies: text: The equation is balanced.  Explodo-nerd (talk) 01:10, 23 February 2012 (UTC)
thread_title:  Balanced Chemical Equation? 

message: Does the Menke nitration require anhydrous copper nitrate or is the acetic anhydride used to remove the water?150.227.15.253 (talk) 17:33, 3 January 2022 (UTC)
thread_title:  Menke nitration requirement?