lflage/wiki-talks huggingface dataset:
Talk:Magnesium perchlorate

message: Magnesium perchlorate was used as a constituent of a water activated (magnesium-magnesium perchlorate) battery during the vietnam war. It was used to partially passivate the magnesium anode plates during the working life of the primary battery pack.WFPM (talk) 02:20, 6 March 2013 (UTC)

message: The right sidebar claims 251°C as the MP...  but it's supposed to be dried at 250 according to the article text and also decomposes at it.
https://cameochemicals.noaa.gov/chemical/1011 says:
"Decomposes at 185-190°C [Hawley]. Noncombustible but accelerates the burning of combustible materials. If large quantities are involved in the fire or the combustible material is finely divided an explosion may result. Avoid contact with mineral acids because of the danger of explosion. In the preparation of anhydrous dimethyl sulfoxide by vacuum distillation from anhydrous magnesium perchlorate, an explosion occurred [MCA Case History 1187, 1966]. Drying ethylene oxide with magnesium perchlorate resulted in an explosion [NSC Newsletter. Chem. Soc. 1959]. Magnesium perchlorate used in drying hydrocarbons exploded when heated to 220°C [Ind. & Eng. News 17:70. 1939]. As soon as trimethyl phosphite contacted a small amount of magnesium perchlorate in a flask, there was a flash and an explosion that shattered the flask [Allison 1968]."
...they later list 250°C as decomposition point and no given melting point which makes sense given that explosive decomposition seems to be a common theme at variable temperatures depending on what residues were left near it.  They Terk Err Jerbs (talk) 13:57, 19 May 2016 (UTC)
thread_title:  Oddity in listed decomposition point and drying temperature 

message: The article originally stated Magnesium perchlorate "appear[s] especially abundant and/or hydrated in locations where active flows are observed." This was the conclusion of a 2015 paper by Ojha et al., but later shown by Leask, et al. (2018) to be an artifact in the instrument and not a true detection of magnesium perchlorate in those regions.  — Preceding unsigned comment added by Andrew Shumway (talk • contribs) 18:19, 9 July 2020 (UTC)
thread_title:  Magnesium perchlorate on Mars
Talk:Mercury(II) thiocyanate

message: Perhaps a brief explanation of the phenomenon (why / how it occurs, as opposed to other minerals where it does not) or a link to a page describing it would b76.65.21.198 (talk) 04:41, 4 June 2010 (UTC)
replies: text: I found two references with the information.  We should certainly include the chemical reactions and discussion.  -- ke4roh (talk) 17:03, 11 May 2013 (UTC)
thread_title:  Pharaoh's Serpent 

message: Thiocyanate ions are of rather low toxicity, so the high toxicity of mercury(II)-thiocyanate just depends on its mercury content. --FK1954 (talk) 19:08, 1 October 2010 (UTC)
thread_title:  Toxicity
Talk:Molybdate

message: The pictures of the molybdate ion , especially the second, suggest that the oxygens are inequivalent, but I believe molybdate is symmetrically tetrahedral like sulfate and chromate, with all bond lengths and angles equal.  A figure like the one used to illustrate chromate might better indicate this.CharlesHBennett (talk) 15:54, 15 January 2019 (UTC)
thread_title:  Structure of molybdate anion
Talk:Monopotassium phosphate

message: a search for Monobasic Potassium Phosphate doesn't lead to this page, but I don't know how to fix that.
:Redirect created. Tomj (talk) 02:40, 6 December 2007 (UTC)
thread_title: Untitled

message: I don't believe KH2PO4 is deliquescent- it is used as a primary standard for phosphate determination, and deliquescent compounds are not generally used as primary standards because their water content tends to vary after the bottle has been opened a few times. Google "phosphate primary standard" and you will get half a dozen links referring to KH2PO4 as the primary standard for phosphate. K2HPO4 is deliquescent. Eaberry (talk) 05:59, 14 January 2023 (UTC)
replies: text: I've worked with KH2PO4 and as far as I know it is not even noticeably hygroscopic. I will remove the assertion until a source is provided. Regmolar (talk) 10:51, 19 January 2023 (UTC)
thread_title:  Properties: NOT deliquescent?
Talk:Palladium hydride

message: PdH is a potential Room-temperature superconductor. How did this manage to go unmentioned?  —Preceding unsigned comment added by 166.70.80.198 (talk) 02:02, 16 January 2010 (UTC)
thread_title:  Room-temperature superconductor 

message: A "CANR", Chemically Assisted Nuclear Reaction' would, like any other nuclear reaction, produce nuclear reaction products, high energy particles and maybe X-rays. So far these do not appear to be reported. Such a reaction and its associated products would be a major discovery, it would not be hidden for long. --Damorbel (talk) 21:34, 3 February 2022 (UTC)
thread_title:  "CANR", Chemically Assisted Nuclear Reactions
Talk:Palladium(II) nitrate

message: I removed the following statement from the article:
"This chemical is noticeable not only for its cucumber like smell and dark blue complexion, it is a proposed cure for skitzophrenia when combined with Martini."
It seems to be clear vandalism.  --Pyrochem 01:26, 9 May 2007 (UTC)
thread_title:  Vandalism
Talk:Perchloryl fluoride

message: What measurement unit has the molar enthalpy of formation which is given as -5.7 in the article? Is it -5.7 kJ/mol or -5.7 kcal/mol or even something else? --79.243.248.247 (talk) 20:23, 2 September 2013 (UTC)
thread_title:  ΔHf = -5.7 

message: Why is perchloryl fluoride considered being flammable (due to the hazard diamond)? It is a strong oxidizer but not a combustible. And strong oxidizers are normally marked as 'highly reactive' but not as 'flammable'... --79.243.248.162 (talk) 16:52, 5 September 2013 (UTC)
thread_title:  Combustible??
Talk:Permanganic acid

message: I propose to merge this skeleton of an article with the well developed article on the anhydride Mn2O7.  If we accumulate enough material on HMnO4 later, we can split the Mn2O7 report in the future.  Mainly, we want readers to find something substantive.  Thus, this article will be converted into a "redirect". Objections and suggestions are welcome here.--Smokefoot 22:29, 29 March 2007 (UTC)
thread_title: Merge proposal
Talk:Peroxydisulfuric acid

message: I have left this as a stub. As for notability this is like so many other compounds not of great "importance" in itself but wikipedia is an encyclopedia. I have left it tagged hoping someone can come up with some suitable gloss  to add to the opening words.Axiosaurus 14:05, 25 October 2007 (UTC)
thread_title: If I build it, will you come (edit)?
Talk:Phosphonium

message: Phosphonium salt should probably merged here – compare ammonium salt and sulfonium salt. However, I'm not sure how to deal with the langlinks of Phosphonium salt; at least two of them (de, nl) refer specifically to quaternary phosphonium compounds, and only dewiki has separate articles on quaternary phosphonium salts and phosphonium anions (substituted and unsubstituted in one article). --ἀνυπόδητος (talk) 18:22, 8 November 2016 (UTC)
replies: text: support. --Smokefoot (talk) 18:23, 8 November 2016 (UTC)
replies: text: , copyedit pending. --ἀνυπόδητος (talk) 12:37, 12 November 2016 (UTC)
thread_title:  Merge proposal
Talk:Phosphorus trioxide

message: Why isn't this compound called tetraphosphorus hexoxide?? Georgia guy 23:14, 17 April 2007 (UTC)
thread_title:  Name 

message: The article lists a pKa of 9.2 without any reference -- presumably this is copied from arsenic trioxide. Maybe we should put a link to phosphorous acid there instead. Zhieaanm (talk) 02:33, 22 January 2011 (UTC)
thread_title:  Acidity
Talk:Polyoxometalate

message: I suppose this is due to later additions, but the 'structure' paragraph says that "The Lindqvist ion is an iso-polyoxometalate, the other three are hetero-polyoxometalates" while 11 structures are shown. 46.116.123.106 (talk) 12:03, 9 June 2012 (UTC)
thread_title:  Structure paragraph is not clear 

message: The expression "closed 3-dimensional framework" doesn't make much sense for a chemist. If you talk about dimensionality in chemistry it usually refers to polymers or coordination polymers, e.g. 1D string, 2D sheet, 3D framework (MOFs for example). Finite Clusters are even called zero dimensional in this respect, although this term tends to confuse more people than it should. Calling polyoxometalates "closed 3D frameworks" is wrong in my opinoin --Zwischenrufer (talk) 21:59, 19 August 2013 (UTC)
thread_title:  3 dimensional 

message: Based on my edits of the article, here are some humble suggestions (only suggestions, I dont make rules!):
*for a big topic like POMs, it is probably best to rely on reviews and textbooks, per WP:SECONDARY, not primary journal references.
*mention of people and institutions might be avoided unless some compelling reason exists.  Just impossible to mention people/places that for every factoid within Wiki-chemistry.
*Real applications = some company is making money, usually.  Extremely few supramolecular, crystal engineered, molecular capsuley, molecular magnetic, luminescent POMs are the basis of any real application, despite good intentions and dreams.  POMs are actually used in commercial oxidation catalysis, I think.  They are also central to manipulating these Mo-W oxides in aqueous soln, which is an application. --Smokefoot (talk) 03:03, 4 May 2015 (UTC)
thread_title: Couple of suggestions
Talk:Potassium cyanate

message: Hey, the structure drawn is wrong. It should be KOCN, not KNCO.  That's potassium ISOcyanate  — Preceding unsigned comment added by 192.12.78.250 (talk) 15:35, 5 July 2011 (UTC)
replies: text: Some editor will eventually upload an image based on crystal coordinates, but this material adopts a polymeric structure, like related species.  Its structure is probably similar to that the corresponding azide.  We are just behind gathering such data and converting those data to images. The real question will likely center on whether the structure is ordered (O's vs N's), but the distinction between KNCO and KOCN is probably not very relevant to anything. --Smokefoot (talk) 05:04, 11 August 2015 (UTC)
thread_title: Structure is incorrect?

message: I note that some sources indicate that Potassium Cyanate reacts with water to produce Potassium Carbonate and Ammonium Carbonate.  This would mean that the Potassium Cyanate would likely taste bitter (due to the Potassium ions or Potassium Carbonate).  Ammonium Carbonate is meant to be a component of smelling salts, which induce an inhaling reflex and would be quite distinctive (presumably inducing a reflex not entirely dissimilar to Menthol sweets).  
Are these assertions true?
ASavantDude (talk) 18:40, 29 April 2018 (UTC)
thread_title: Smell and Taste of Potassium Cyanate

message: What is under "Properties" should be part of "Preparation and Reactions".
Colo(u)r: "white" is a color. "Clear" is colo(u)rless. Potassium cyanate is a white powder. Perhaps large, single crystals are clear?  — Preceding unsigned comment added by 69.2.26.130 (talk) 01:06, 1 August 2023 (UTC)
thread_title: Properties
Talk:Potassium hypomanganate

message: Old text books refer to potassium manganite being the formulated as K2MnO3, salt of the hypothetical manganous acid  Axiosaurus (talk) 16:39, 1 May 2008 (UTC)
replies: text: I vaguely remember seeing similar things in the past: however, Cotton & Wilkinson is quite formal that there is disproportionation when MnO2 dissolves in concentrated alkali. There are also lithium and sodium manganites, MMnO2 (that is manganese(III), ), but these are probably best considered as mixed oxides. Physchim62 (talk) 16:14, 26 June 2010 (UTC)
thread_title:  potassium manganite
Talk:Potassium silicate

message: The 3D-image shows Sodium silicate, not Potassium silicate  —Preceding unsigned comment added by 130.237.216.122 (talk) 08:40, 10 July 2009 (UTC)

message: Problem with some content of the chembox:
| SystematicName = Dipotassium oxosilanebis(olate)
In organic chemistry, the suffix "olate" commonly refers to an alcoholate, not to the conjugated base of an inorganic acid. Dipotassium oxosilanebis(olate) is very misleading for the reader. The conjugated base of the metasilicic acid has to follow the same rules as for these of other inorganic acids whose base is also an oxyanion: e.g.
* sulfuric acid: sulfate and not sulfonate;
* phosphoric acid: phosphate and not phosphonate.
All the rules of organic chemistry nomenclature are not directly transposable to inorganic compounds. The analogy with the carbon atom has its limits, even for silicon a close cousin of carbon. Shinkolobwe (talk) 00:35, 9 January 2011 (UTC)
thread_title:  Dipotassium oxosilanebis(olate) = inappropriate SystematicName 

message: Article was moved from Stub to Start status because it has a significant amount of information and multiple references. Compared to numerous other "Stub" articles in Chemicals and Glass and had greater content than most.  In addition, the main article Stub tags were removed. Araesmojo (talk) 22:00, 23 October 2020 (UTC)
thread_title:  Stub to Start
Talk:Potassium sulfide

message: The way I read it, this sentence seems to contradict itself:
:In the laboratory, this synthesis is usually conducted in a solution of anhydrous ammonia.
'solution' means that a solute is dissolved in water, unless is it specified that the solvent is not water.
 'anhydrous' means that the substance contains no water.   Could someone please clarify whether the ammonia is solved in water or not?
Nirmos (talk) 01:57, 19 February 2010 (UTC)
thread_title:  Contradiction? 

message: The reaction 2 KMnO4 + S → K2S + 2 MnO2 + 2 O2 seems to be most commonly used for pyrotechnics. Its value as a preparative technique for even technical grade K2S requires citation. There's going to be K2O and SO2 byproducts, at minimum; I don't know how much, though. --Eh9 (talk) 03:47, 13 April 2012 (UTC)
thread_title:  Permanganate + Sulfur 

message: "the small K+ ions" - K+ ions are extremely large among the whole ions known.Eudialytos (talk) 20:02, 7 April 2020 (UTC)
replies: text: You are incorrect.  K atoms are relatively large, but K+ ions are smaller (196 vs 152).  S2- ions have a radius of 170.  units = picometers.  See Ionic radius.--Smokefoot (talk) 00:03, 8 April 2020 (UTC)
thread_title: ERROR
Talk:Potassium thiocyanate

message: I'm concerned about the information that KSCN can be used to resemble fake blood and stigmata; this may encourage some readers of the article to try this on their own hands and skins, yet the article doesn't mention any of the health risks, although the word "harmful" does appear. The article's box gives a 3 for its health rating, which is very high. The MSDS from Flinn Sci. says that KSCN is:
:Moderately toxic by ingestion. Irritating to body tissues. Avoid all body tissue contact.
The MSDS lists eczema as a side effect. It also mentions the dangers of inhaling any vapors that may result from the breakdown of KSCN, particularly if heated or if it comes in contact with an acid. 
Ferric chloride is an acid and contact of KSCN with an acid can release hydrogen cyanide gas.  If the Fx industry uses KSCN, how do they make it safe for body contact? How diluted should it be?
Does anyone know more about these health hazards than just what the MSDS says? Ileanadu (talk) 18:18, 22 March 2011 (UTC)
thread_title:  Health Hazards!
Talk:Red fuming nitric acid

message: I was a little taken aback reading in the Experiments section that HF is added as a corrosion inhibitor.  One of the few factoids I thought I knew about chemistry was that hydrofluoric acid is itself extremely corrosive.  I don't doubt the article, but maybe one of you experts can add a few words of explanation on how the HF has a corrosion inhibiting effect.  --ChetvornoTALK 10:15, 30 May 2014 (UTC)
replies: text: Fluoride, being an anion with a dense charge, might be expected to bind tightly to certain metals.  The situation would be analogous to passivation of metals (Al, Si) by strongly adhering oxides.  Here is a quote from a technical source "Carbon steel is commonly used with liquid or gaseous anhydrous hydrofluoric acid up to 100 – 150 C. Carbon steel is passivated by the formation of a layer of iron(III) fluoride." See .--Smokefoot (talk) 15:32, 30 May 2014 (UTC)
replies: text: Ah, I see.  That makes sense.  Thank you, sir. --ChetvornoTALK 20:46, 30 May 2014 (UTC)
thread_title:  HF as a corrosion inhibitor? 

message: I see no reason to have a separate article for this particular grade of nitric acid. The contents should be merged back into the corresponding section of nitric acid, and some details could be trimmed or factored out.  For example, the details of the resistance of metals to corrosion is too technical for Wikipedia.  --Jorge Stolfi (talk) 17:03, 18 February 2019 (UTC)
replies: text: * My fault.  I did suggest the merge also on Talk:Nitric acid, but forgot to say that here. --Jorge Stolfi (talk) 01:23, 19 February 2019 (UTC)
thread_title:  No reason for a separate article
Talk:Rubidium fluoride

message: When metal compounds are reacted with hydrogen fluoride, the resultant metal fluoride, such as potassium fluoride, normally reacts with the HF to form an adduct, such as KHF2. I thought that rubidium would be no exception. --Cheminterest (talk) 20:59, 24 March 2010 (UTC)
thread_title:  Reaction of Rubidium compounds with hydrogen fluoride
Talk:Ruthenium(IV) oxide

message: How exactly does an oxide that is solid at room temperature have the crystal structure of O=Ru=O, which would be more like a dioxide gas?  This fact seems confusing or misleading to me, and I think it may be incorrect (I couldn't find any reference to molecular RuO2 in the literature).
Mbkatz 20:37, 8 August 2007 (UTC)

message: Is there really a justification for red-linking to an in-exhaustive list of suppliers?--WhirlwindChemist (talk) 14:02, 29 August 2008 (UTC)
thread_title: Suppliers Section
Talk:Scandium(III) sulfide

message: How can Sc2S3 be synthesized at >1550°C if it decomposes above 1100°C? This is only possible if the lower sulfides are formed in the described synthesis process, and then react with further sulfur (or hydrogen sulfide) upon cooling, ultimately producing Sc2S3. But the article also describes that heating scandium and sulfur together only produces ScS and never Sc2S3, implying that Sc2S3 cannot be produced by reacting lower scandium sulfides (like ScS) with further sulfur. --79.243.249.158 (talk) 20:27, 3 September 2013 (UTC)
replies: text: Sorry, I confused scandium oxide with elemental scandium ... but there's still the question how to yield Sc2S3 at temperatures above its decomposition temperature... --79.243.249.158 (talk) 20:32, 3 September 2013 (UTC)
replies: text: Good catch.  The prep gives crappy samples for the reasons that you indicate - it is unstable at 1550 C.  Limiting decomp is the fact that the prep is conducted under flowing H2S.  To obtain good samples, they transported the material at 950 C, well below the decomp temp. --Smokefoot (talk) 23:02, 3 September 2013 (UTC)
thread_title:  Synthesis temperature > decomposition temperature?
Talk:Selenic acid

message: Shouldn't the systematic names read Selenium(X) rather than Selenic(X)? I noticed that the systematic name for Selenic Acid read Selenic (VI) and the name for Selenious Acid read Selenic (IV). A little nitpicky, but still...  —Preceding unsigned comment added by 128.54.201.237 (talk) 23:03, 6 November 2008 (UTC)
replies: text: That's what I thought. JIMp talk·cont 15:39, 13 June 2009 (UTC)
thread_title: Systematic name
Talk:Silicon tetrachloride

message: why is the boiling point of carbon tetra chloride higher then silicon tetra chloride???? 
this is an odd trend in the group 4 chlorides!!!!  —Preceding unsigned comment added by 202.125.143.76 (talk) 11:18, 17 August 2008 (UTC)
thread_title:  boiling point!!! 

message: I am sorry for hitting that link accidentally. Incnis Mrsi (talk) 18:01, 14 April 2010 (UTC)
thread_title:  Reverting at 14 April 2010 was a mistake 

message: http://www.washingtonpost.com/wp-dyn/content/article/2008/03/08/AR2008030802595.html is not accessible anymore?  — Preceding unsigned comment added by UserHuge (talk • contribs) 18:21, 1 October 2019 (UTC)
replies: text: Works fine for me. VQuakr (talk) 18:27, 1 October 2019 (UTC)
thread_title:  Link to leakage into environment? 

message: Or tri valant 2402:3A80:18C1:B67C:A910:43A3:F205:6421 (talk) 07:07, 14 December 2021 (UTC)
thread_title:  Is it di valant? 

message: These terms are used without any description or link. Could someone remedy this? Chemical Engineer (talk) 22:58, 14 March 2024 (UTC)
thread_title:  MCVD and OFD
Talk:World War Veterans

message: The source of this article is the page http://www.marxisthistory.org/subject/usa/eam/worldwarveterans.html
of the Early American Marxist History website. This page contains links to PDF documents created by or about the World War Veterans during its existence. 
:# The original text was not copyrighted.
:# The author was consulted as a courtesy.  The author then granted explicit permission to use these texts. 
DJ Silverfish 18:39, 27 August 2006 (UTC)
thread_title: Untitled
Talk:Silicon tetraiodide

message: As the comparison of the mp of the silicon halide compounds shows, the mp for silicon iodide is 155 C. 
Therefore, if we attempt to make an aqueou solution of KI and etch silicon via formation of silicon iodide, 
the SiI4 product will not be soluble up to the boiling point (~100C) of the aqueous solution. Berkeleybill (talk) 21:00, 28 April 2023 (UTC)
replies: text: My reading is that the article refers to etching Si with SiI4, which would not use water.--Smokefoot (talk) 21:23, 28 April 2023 (UTC)
thread_title:  Reference needed for using KI as an etchant for silicon