User talk:Chemicalinterest/Archive 1

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Welcome!

Hello, Chemicalinterest, and welcome to Wikipedia! Thank you for your contributions, especially what you did for Wikipedia:Reference desk/Science‎. I hope you like the place and decide to stay. Here are some pages that you might find helpful:

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I hope you enjoy editing here and being a Wikipedian! Please sign your messages on discussion pages using four tildes (~~~~); this will automatically insert your username and the date. If you need help, check out Wikipedia:Questions, ask me on my talk page, or ask your question on this page and then place {{helpme}} before the question. Again, welcome! The High Fin Sperm Whale 00:40, 30 April 2010 (UTC)[reply]

Death

Hello, sorry i wasn't signed in before, i replied to your question on my talk page User talk:Vespine#Death Vespine (talk) 01:33, 30 April 2010 (UTC)[reply]

Talkback

Hello, Chemicalinterest. You have new messages at Wikipedia:Reference desk/Science.
Message added 02:15, 8 May 2010 (UTC). You can remove this notice at any time by removing the {{Talkback}} or {{Tb}} template.

By the way, when you write a chemical formula, when writing numbers, add NUMBER, as in H2SO4, to get H₂SO₄. The High Fin Sperm Whale 02:15, 8 May 2010 (UTC)[reply]

Barnstar

		The Chemistry Star
		For your contributions to the science reference desk. --The High Fin Sperm Whale 20:47, 8 May 2010 (UTC)[reply]

Reliable sources

Hi Chemicalinterest.

I saw your recent good work on several articles in my watchlist, including this edit to Bismuth(III) iodide. When you add such information, please provide a reference to the source of the information, otherwise it's hard to check if it's true or not.

See the official guidlines on referencing:

If you need any help, feel free to contact me or anyone else from WP:CHEMISTRY.

Cheers,

Ben (talk) 01:40, 11 May 2010 (UTC)[reply]

You replied at User talk:Benjah-bmm27#Chemicalinterest, Bismuth triiodide:

I added that uncited example in bismuth triiodide because I thought that all metal oxides react with acids to form the corresponding metal salts. --Chemicalinterest (talk) 14:33, 11 May 2010 (UTC)

You can't just add things to Wikipedia that you think you know. The reasons for this are given at Wikipedia:Verifiability and Wikipedia:No original research. In my time here at Wikipedia, I've found that there are almost always exceptions to general rules, especially in chemistry.

I strongly advise you to find a reliable source for any information you add to articles.

By way of example, in the case of bismuth triiodide, if you couldn't easily find a source that says Bi₂O₃(s) + 6HI(aq) → 2BiI₃(s) + 3H₂O(l), then at the very least, cite the book that told you "all metal oxides react with acids to form the corresponding metal salts".

In this case, I've done it for you :)

If you need any help identifying good places to find reliable information, just ask.

Cheers

Ben (talk) 17:29, 11 May 2010 (UTC)[reply]

Thanks. I just wanted to contribute vital data that is missing in various pages. Some don't have preparation data, some don't have safety data, some don't have properties. I did add safety data from [1] for the safety data. Would I need to put a source on it? You can see an example on cobalt carbonate#safety. Thanks. --Chemicalinterest (talk) 20:26, 11 May 2010 (UTC)[reply]

Get involved with WP:CHEMS. We're always looking for people to contribute content.

We don't really like too much safety data, mainly because the purpose of Wikipedia is not to be a safety manual or MSDS.

Cobalt carbonate#Safety looks reasonable. The main problem we have is with campaigners who are very bad at writing from a neutral point of view. I don't think this applies to you, you seem to just be genuinely interested in chemistry. If you want to see some classic examples of ridiculous POV writing from editors with a bee in their bonnet, try the histories and talk pages of e.g. Uranium trioxide (depleted uranium campaigners) or Fluoride (water fluoridation campaigners).

As a rule of thumb, always provide a source. You always get your information from somewhere, so just state where alongside your additions. It's not that hard, and we can help you with formatting if you need it.

Ben (talk) 13:10, 12 May 2010 (UTC)[reply]

I needed a source for the work I did on sodium hydroxide (that was the article needing improvement on WP:CHEMS). I wrote in a reaction that I saw in a science kit and a chemistry textbook that sodium carbonate reacts with calcium hydroxide to produce sodium hydroxide and calcium carbonate. Can I use my chemistry textbook as a source for it? Thanks. --Chemicalinterest (talk) 14:05, 12 May 2010 (UTC)[reply]

Yes. A chemistry textbook is the best kind of source for this sort of information. The science kit probably wouldn't be, as it is unlikely to be peer reviewed.

Ben (talk) 14:36, 12 May 2010 (UTC)[reply]

Thanks. --Chemicalinterest (talk) 14:37, 12 May 2010 (UTC)[reply]

Before I created an account, I edited copper(II) chloride with [edit]. I have a source to back up the equilibrium (it is in my science book), but I don't have any available for the reaction with aluminum. Can you help find a source for the first reaction? I have limited access at this time, so directing to a google search may not work. Thanks. --Chemicalinterest (talk) 10:54, 20 May 2010 (UTC)[reply]

If you don't have a source for the reaction with Al, how do you know it's true?

I'll look for these reactions in my inorganic textbooks, I'll get back to you ASAP.

Cheers,

Ben (talk) 17:42, 20 May 2010 (UTC)[reply]

I once saw something about it online as a science demonstration. But I (before i knew about WP:NOR) also did some experiments about it and wrote them in.--Chemicalinterest (talk) 17:45, 20 May 2010 (UTC)[reply]

No problem, I'll look it up for you.

Ben (talk) 13:25, 21 May 2010 (UTC)[reply]

magnet

Added something to an old question of yours..http://wiki.riteme.site/wiki/Wikipedia:Reference_desk/Archives/Science/2010_May_15#Magnetic_powder Sf5xeplus (talk) 13:03, 18 May 2010 (UTC)[reply]

(edit conflict)Thanks. Feel free to contact me if you have any questions or answers. I have some of both. --Chemicalinterest (talk) 13:04, 18 May 2010 (UTC)[reply]

You were editing the same time I did, that's what the edit conflict means. --Chemicalinterest (talk) 13:05, 18 May 2010 (UTC)[reply]

Peer review

Peer review To add a nomination -->

Add {{subst:PR}} to the top of the article's talk page and save it, creating a peer review
Within the notice, click where instructed to open a new peer review discussion page. If there is no such link in the notice, see this.
Complete the new page as instructed. Remember to note the kind of comments/contributions you want, and/or the sections of the article you think need reviewing.
Save the page with the four tildes (~~~~) at the end of your request to sign it. Your peer review will be listed automatically on this page within an hour.
Consult the volunteers list for assistance. An excellent way to get reviews is to review a few other requests without responses and ask for reviews in return.

....... See -->Wikipedia:Peer review for more info!!....Moxy (talk) 20:32, 20 May 2010 (UTC)[reply]

Thanks. --Chemicalinterest (talk) 20:36, 20 May 2010 (UTC)[reply]

Barnstar

Thank you! --Rifleman 82 (talk) 16:06, 22 May 2010 (UTC)[reply]

I monitor edit history of iron, and I saw that you contributed much to the article. All additions are appreciated. --Chemicalinterest (talk) 16:17, 22 May 2010 (UTC)[reply]

Lithium

People touch alkali metals all the time with dry hands. Just don't stick them in your eyes afterward. No, it's not recommended, but yes, it's often done. In any case, you can still get a very good feel for the heft of metals while wearing shear plastic food-handler-type gloves. S B H arris 05:53, 23 May 2010 (UTC)[reply]

I saw your edit summary when I was scanning the Recent Changes to the Elements. I thought handling lithium might be something not good to do, but after I sent the message, I deleted it because I thought "Oh just use gloves". Thanks. --Chemicalinterest (talk) 11:15, 23 May 2010 (UTC)[reply]

Because it is a very strong reducing agent, make sure it doesn't reduce you to tears, itself being oxidized to lithium ions.--Chemicalinterest (talk) 11:16, 23 May 2010 (UTC)[reply]

File:CuCl2_equilibrium.JPG

Nice. You'll need a better "permission" - check the templates for one which is appropriate. --Rifleman 82 (talk) 15:26, 24 May 2010 (UTC)[reply]

Which templates? --Chemicalinterest (talk) 15:30, 24 May 2010 (UTC)[reply]

See Wikipedia:Image_copyright_tags. The preferred license is of course public domain. If you choose, there are other licenses available as well. --Rifleman 82 (talk) 15:35, 24 May 2010 (UTC)[reply]

Got it. Thanks. --Chemicalinterest (talk) 15:47, 24 May 2010 (UTC)[reply]

Polonides

I've written you an article about polonides, just so you know that I'm not making this up! I think you confusion about their stability is that you are basing your ideas on electrode potentials, ie solution behavior, and not taking into account the lattice energy that stabilizes the solids. Best wishes, Physchim62 (talk) 15:40, 26 May 2010 (UTC)[reply]

Taking a look at it now. Thanks. --Chemicalinterest (talk) 17:31, 26 May 2010 (UTC)[reply]

I was wondering how all of that just "appeared", but then I saw your conversation with User:Rifleman 82 on your talk page. BTW, I'm still in high school so I may not understand all terminology fully. --Chemicalinterest (talk) 17:35, 26 May 2010 (UTC)[reply]

My real issue was that polonides would (according to periodicity) be very strong reducing agents. But if their lattice energy is very high, then that may prevent them from being oxidized easily. Maybe there is a thin film of polonium on them that prevents further oxidation. --Chemicalinterest (talk) 17:38, 26 May 2010 (UTC)[reply]

There's a quirk of periodicity (called the lanthanide contraction) which means that polonides are not much more reducing than tellurides, but about the same. Now sodium telluride will readily oxidize in air to give tellurium, and I would imagine that sodium polonide (and the other ioinc polonides) would do the same. But that assumes that you are letting them in contact with air! I didn't put it in the article because the papers I've seen are not clear on the point, but I believe that all the ionic polonides were prepared and studied under nitrogen: this would be logical, because they are prepared from the elements and the electropositive metals will simply oxidize if you heat them in air! In fact, even polonium will slowly oxidize in air, on a time-scale of days, so it too needs to be stored under nitrogen. The lanthanide polonides, on the other hand, are amazingly air-stable (that's their technological interest): that's because they don't actually contain Po²⁻ ions! You can think of them as more like covalent structures, a bit like silicon dioxide: there are many, many sulfides, selenides and tellurides with the same type of "intermediate" bonding. Physchim62 (talk) 08:12, 27 May 2010 (UTC)[reply]

That was just my curiosity, whether polonium is the same or different from the trend. Since I cannot experiment on polonium and its compounds, then I can't determine their properties very well. Thanks for answering my question. --Chemicalinterest (talk) 10:39, 27 May 2010 (UTC)[reply]

Chromium(VI) peroxide

Sorry about that, I assumed that you were still following the thread at WP:Requests for feedback#User:Chemicalinterest/Chromium(VI) peroxide. – ukexpat (talk) 16:11, 27 May 2010 (UTC)[reply]

Oh I forgot to monitor it. My problem. --Chemicalinterest (talk) 16:14, 27 May 2010 (UTC)[reply]

If you have any amyl alcohol handy, you can use it it extract the chromium peroxide into an organic layer to give you a lovely blue colour. You just need a few drops in the test-tube scale reaction that you've already carried out ;) Physchim62 (talk) 16:41, 27 May 2010 (UTC)[reply]

You can get the etherate... --Rifleman 82 (talk) 16:48, 27 May 2010 (UTC)[reply]

I don't have any advanced chemicals like that: the only chemical I got from a chemical supply shop was copper(II) sulfate: the rest are homemade. I might need to take a better picture of chromium(VI) peroxide, but it always comes out blurry. --Chemicalinterest (talk) 18:24, 27 May 2010 (UTC)[reply]

Feel free to give some to me: leave it on the shore of Oakeys Brook. Thank you. --Chemicalinterest (talk) 18:26, 27 May 2010 (UTC)[reply]

A lovely blue color also exists with cuprammonium sulfate (without the carcinogenic chromium(VI)). --Chemicalinterest (talk) 18:27, 27 May 2010 (UTC)[reply]

Oakeys Brook (New Jersey)

I'm happy that the WikiProject Rivers liked your article. Obviously, I guessed wrong, but at least I sent you to the right place :)--SPhilbrick T 22:48, 28 May 2010 (UTC)[reply]

Marx

Yes, I really felt I should remove User:SteveBakers comment since one editor had already complained and rightly so - since the response had little to to with the question asked and was well into the territory of WP:SOAPBOX , I removed your comment too in the interests of fairness since it was along the same lines.77.86.47.199 (talk) 22:50, 28 May 2010 (UTC)[reply]

I also removed this [2] which you added, for the same reasons. I think you know why this comment has been removed. It definately doesn't have anything to do with the answer, and is vaguely inflammatory.77.86.47.199 (talk) 22:54, 28 May 2010 (UTC)[reply]

Yeah sometimes I add those to rile people on purpose. BTW, why don't you create an account for yourself? You can make pages, have a user page like this one for myself, and be identified more easily by people who have a hard time remembering an IP. --Chemicalinterest (talk) 00:17, 29 May 2010 (UTC)[reply]

Well anyway stevebaker reinstated his comment, so the topic is now up for discussion on the reference desk talk page if you want to comment. I really can't see how he can describe what he wrote as anything but "gas" but we'll see :)

77.86.47.199 (talk) 00:22, 29 May 2010 (UTC)[reply]

He's a staunch atheist, but he doesn't tend to be confrontational. He likes best attacking an anonymous enemy, i.e. creationists in general. --Chemicalinterest (talk) 00:24, 29 May 2010 (UTC)[reply]

By the way I do have a user name User:sf5xeplus - but I don't usually sign in because I keep getting signed out again 77.86.47.199 (talk) 00:35, 29 May 2010 (UTC)[reply]

When you log in, select "remember me for 30 days". That way it stores your information as a cookie in your computer. You are automatically logged in every time you go on for 30 days. That's what I do. Note: You may have to change the cookie setting on your browser (On internet explorer it is under tools menu→internet options→privacy→set the bar lower and try again)

Feedback archived

Hi there.

A while ago, you requested feedback in WP:FEED. Because it has been a while, and you'd received at least some response there, I have now archived the replies in Wikipedia:Requests for feedback/Archive/27. Please do not edit that page though; if you require further feedback, add a new request on WP:FEED.

I am trying to clear the backlogs; it would help us a lot if you could look at the requests from other users on WP:FEED and add any comments to help them out. Anyone can respond there, so please do take a look, and comment on the articles from other people.

If you want help with anything at all, you could either;

Leave a message on my own talk page; OR
Use a {{helpme}} - please create a new section at the end of your own talk page, put {{helpme}}, and ask your question - remember to 'sign' your name by putting ~~~~ at the end; OR
Talk to us live, with this or this.

The last of those is particularly useful - please try it; pop in now and say hello. Best, Chzz ► 02:36, 29 May 2010 (UTC)[reply]

Sorry, but I cannot access that. Thank you. --Chemicalinterest (talk) 14:24, 29 May 2010 (UTC)[reply]

Nine Mile Run

I added some additional info to your article on the Nine Mile Run, including the GNIS coordinates listed for the source and mouth. Also made some tweaks to the wording in the Course description. Let me know what you think.

Additionally, would be good to add an infobox. The same should be done for Six Mile Run (maybe you can get a picture for it?).

-Lithium6ion (talk) 22:55, 30 May 2010 (UTC)[reply]

Yes I can get some pictures for the Six Mile Run. I live at 40.45078°N, 74.53574°W so I have easy access. Also you can take a look at Oakeys Brook (New Jersey). --Chemicalinterest (talk) 00:51, 31 May 2010 (UTC)[reply]

I plan to take 2 more pictures (fill up the gallery) of the Nine Mile Run: where it crosses Rt. 27 and its source marsh tomorrow. I may take pictures of the Six Mile Run crossing Rt. 27, South Middlebush Road, etc. I would like to know if the stream crossing Cozzens Lane is considered the Six Mile Run; or is its official source at the hidden lake at Hidden Lake Park? --Chemicalinterest (talk) 00:59, 31 May 2010 (UTC)[reply]

According to GNIS, the official source of the Six Mile Run is at 40.4598272 N -74.4862644 W, near Corporate Road. So yes, the stream crossing Cozzens Lane is in fact the Six Mile Run. I'll take a look at Oakeys at some point tomorrow or later in the week. I can tell you that Oakeys does have a GNIS listing, with a source listed at 40.4323277 N -74.5440438 W, near Augustine Drive/Beekman Road (consistent with the article). For reference, Oakeys' GNIS ID is 878917. I'll see if I can dig up some history on either of the streams.

-Lithium6ion (talk) 06:28, 31 May 2010 (UTC)[reply]

I tried to find the source but I couldn't: maybe there is just a huge spring bubbling out of the ground. So the branch draining the hidden lake at Parkside Ave is just another tributary. Thank you for finding the information. --Chemicalinterest (talk) 11:19, 31 May 2010 (UTC)[reply]

BTW, if the source data confused you for the Nine Mile Run, it was because I was talking about minor source, not the official source. The source I was talking about was at 40.41947°N 74.55580°W. --Chemicalinterest (talk) 18:20, 1 June 2010 (UTC)[reply]

"normal" oxidized copper

appears too dark in the right image File:Copper wire comparison.JPG. Are you sure it is clean copper? Materialscientist (talk) 01:08, 2 June 2010 (UTC)[reply]

I put the caption on copper article: the picture is the comparison of clean with oxidized copper (people tend to think of the oxidized color as "copper". You may edit the description. (I am typing this holding a test tube of iron(III) chloride, which I just took a picture of). --Chemicalinterest (talk) 01:18, 2 June 2010 (UTC)[reply]

You've got not enough light for keeping right brightness in the camera, or the auto-brightness meter of the camera didn't work well. It is best to try fixing it in the camera itself (increase the exposure time somehow, change meter settings from spot to area, focus on a slightly different object, increase the AV setting from default zero to +1 or even +2, etc). If nothing works, I post process with GIMP, which is free to download. It allows fixing many camera problems, but only to a certain degree.Materialscientist (talk) 11:18, 2 June 2010 (UTC)[reply]

Meter settings are spot to area, and I used the flash so it might be dim. Maybe I can try not using the flash. --Chemicalinterest (talk) 11:31, 2 June 2010 (UTC)[reply]

Thank you

Hello! Thank you for helping me, now I also have a lab as you but the chemical is very limited, consisting only of: Axid Nitric (HNO3), axid sulfuric (H2SO4), axid Chlohydric (HCl), axid nitrua (HNO2), and some salts of the metals such as Copper, Nickel, Iron, Zinc, Sodium, Potassium, Calcium. My goal is just want to be general elements in the periodic table, but now only isolated Copper, Zinc, Sodium, Magnesium and Potassium. you know how to isolate boron from borax, and melting Tungsten, then please just help me!
Also I will give you a pretty interesting experiment, you probably already know or not know: First, use white Phosphorus (Red Phosphorus baked in a vacuum, to evaporate the collected white P) in test tubes containing KOH (potassium hydroxide) heated tube, the ball will have small air escape from the test tube , leave the lid open test tube and you should turn off their lights in the room, it will be strange phenomenon occurs

Gas escape intense smell, you should wear a mask!

--I love chemistry (talk) 07:50, 6 June 2010 (UTC)[reply]

Wow you have some chemicals I don't have! I just have household chemicals (no sulfuric acid, no nitric acid, no nitrous acid, just "boring" chemicals). I do have metal salts though.

On a note of correction, "axid" is normally spelled "acid". HCl is known as hydrochloric acid, and HNO2 is known as nitrous acid. You can also put double brackets around chemicals which links to the wiki article for them. Like [[boron]] would make boron.

I tried to isolate boron by electrolysis of a boric acid solution, but the reduction potential for hydrogen is easier than the reduction potential for boron. You could try reacting boron trioxide with aluminum powder at high temperature in a vacuum. Dissolve the aluminum oxide produced in an acid, preferably hydrochloric acid.

Melting tungsten is hard without an electric arc welder; maybe an oxyhydrogen torch would work. It also would probably oxidize (without a flux) to tungsten(VI) oxide, which is the smoke you see coming out when you smash an incandescent bulb (not damaging the filament) and turn it on. (Be careful though, the two wires holding the filament are electrically live).

I do not have any burner other than a cooking stove, so I cannot perform molten salt electrolysis, the method to produce sodium, magnesium, calcium, potassium, lithium, and some other alkali metals and alkaline earth metals.

I do not own any phosphorus other than a 20 microgram quantity from several cap gun pellets. Red phosphorus, that is. Is the ball you are referring too a ball of white phosphorus? The potassium hydroxide, I assume, stabilizes the white phosphorus so it does not self ignite, a quality known as pyrophoricity. The light is from a slow oxidation reaction going on in the phosphorus. Is the gas flammable? If so then it is phosphine. If it is, then the phosphorus is not being oxidized. Otherwise it could be a smoke of phosphorus trioxide or phosphorus pentoxide. The former is very toxic, as well as is phosphorus. --Chemicalinterest (talk) 11:33, 6 June 2010 (UTC)[reply]

See my user page for photos of my lab. --Chemicalinterest (talk) 18:10, 6 June 2010 (UTC)[reply]

As I come out of the gas that is hidrogen phosphua reaction, at room temperature (24⁰C), it can also burn and shine with a blue flame hovering mid-air (provided you light switches) , this highly toxic gas, i did once hospitalized for because Inflammatory respiratory! Also the preparation of nitrous acid (HNO₂) and nitric acid (HNO₃), you can do with simple liturgy follows:

Tools needed: Two Iron ingots approximately 6 cm, a key plug, a strand of wire about 20cm long, the power (which may be DC or AC), a test tube or a glass bottle
The implementation process:

Connect the two bars with two Iron with Copper wire attached directly to the keyboard plugged in, note: no keyboard plugged in to the mains before connecting.
Set the two electrodes Iron tank, sealed glass tube, then plug the keyboard connected to the mains
Reporter arc with two poles into the air in the bottle, the air is modified by the following equation:

NO ----> N₂ + O₂ (gas, colorless, anesthetic effect)

Open the cap for air in the average exposure to outdoor air, quickly close the lid:

O₂ ----> NO + NO₂ (gas, brown, red)

For NO2 reacts with water:

H₂O + NO₂ ----> HNO₂

Use the residual effects of NO2 with oxygen again for the N₂O₇ (solid white, not durable) then reacts with water:

NSmall Text2O₇ + H₂O ----> HNO₃

Beware of power lines !!!!--I love chemistry (talk) 03:37, 7 June 2010 (UTC)[reply]

Where does the hydrogen come out. If it burns readily, it is phosphine; click the blue colored font to go to a wikipedia article (if it is red there is no article). Does it have a fishy smell? That's what phosphine's supposed to have.

Liturgy means the system of public worship in a church; process would be a better word. Hidrogen phosphua is normally known as hydrogen phosphide or phosphorus hydride or phosphine. But I don't speak that good Vietmanese either.

What is the keyboard in your process? Is it some kind of plug to plug into your power source? I would also assume you need high voltage, which I don't have; nothing but a grill lighter (press the button and the sparks fly).

NO, also known as nitric oxide, is not the gas with an anaesthetic effect. The one they use in dentist offices is N2O, known as nitrous oxide. Nitric oxide is toxic, and it is easily oxidized to the brown NO2, also known as nitrogen dioxide. N2O5 (not N2O7), is known as nitrogen pentoxide, is the anhydride of nitric acid. It may be formed by dehydrating nitric acid with phosphorus pentoxide, a powerful dessicant. --Chemicalinterest (talk) 11:02, 7 June 2010 (UTC)[reply]

Your process seems similar to the Ostwald process in its later steps. It is used in the commerical preparation of nitric acid. --Chemicalinterest (talk) 11:17, 7 June 2010 (UTC)[reply]

This would be my version:

N₂ + O₂ → (see the bar below the save button, has some scientific figures on it) 2 NO (nitric oxide gas, colorless, toxic)

2 NO + O₂ → 2 NO₂ (nitrogen dioxide, brown, toxic gas)

3 NO₂ + H₂O → 2 HNO₃ + NO (nitric acid plus nitric oxide gas, which may be reoxidized to produce more nitric acid.)

Nitrous acid would be produced by the absorption of a mixture of NO and NO₂ onto NaOH (or any other "OH") to produce the metal nitrite salt. Adding this to an acid will produce a solution of the unstable nitrous acid. --Chemicalinterest (talk) 11:32, 7 June 2010 (UTC)[reply]

Your reaction for the formation of nitrous acid will never balance. NO2 (+4 oxidation state) is being reduced to NO2(-) (+3 oxidation state), but nothing is being oxidized. In my reaction the NO (+2) is being oxidized to NO2(-) (+3). See redox for more details about oxidation and reduction.

When NO2 is pressurized it forms the colorless nitrogen tetroxide, N2O4, a connection of two NO2 molecules. --Chemicalinterest (talk) 11:54, 7 June 2010 (UTC)[reply]

Oh I saw your process to form nitrous acid in the nitrous acid#decomposition wiki article. It forms nitrous and nitric acid by a disproportionation reaction. --Chemicalinterest (talk) 11:57, 7 June 2010 (UTC)[reply]

See User:Chemicalinterest/List of chemicals. --Chemicalinterest (talk) 01:31, 8 June 2010 (UTC)[reply]

Fe acetate

You are in over your head on this one. Transition metal chemistry is a dumping ground for unreliable rsch and few scientists would take a paper from that journal to overturn a lot of verified work. Your work in filling in chemboxes is very helpful. Keep it up.--Smokefoot (talk) 13:14, 7 June 2010 (UTC)[reply]

To my understanding, there is iron(III) acetate Fe(OAc)3, and basic iron(III) acetate FeOH(OAc)2. There is reference to the former in qualitative inorganic analysis. I also have created it. It is a blood red solution, which, upon heating, releases acetic acid and turns into basic iron(III) acetate, which is an insoluble red-brown chemical. But it looks like you have replaced the content in iron(III) acetate with the chembox for basic iron(III) acetate. I need to create a chembox for iron(III) acetate, mentioning its decomp. before melting, molar mass, no boiling point, appearance, etc. --Chemicalinterest (talk) 14:29, 7 June 2010 (UTC)[reply]

If you deleted all the info for iron(III) acetate, delete the page for basic iron(III) acetate. --Chemicalinterest (talk) 14:37, 7 June 2010 (UTC)[reply]

The problem is that either:

Fe³⁺ + 3Ac⁻ should be colourless in dilute aqueous solution and violet as a solid; or
[FeAc₃] should be insoluble in water and not strongly coloured.

So the simple explanation is that the old formulations of "iron(III) acetate" refer to a more complicated compound. We have no obligation to perpetuate old information which now appears to be wrong. Physchim62 (talk) 14:39, 7 June 2010 (UTC)[reply]

It definitely isn't colorless, its one of the most brightly colored compounds. What is it though... --Chemicalinterest (talk) 14:41, 7 June 2010 (UTC)[reply]

Don't know, to give you an honest answer! Why not try leaving the solution to slowly evaporate, and see if you can get any crystals... Physchim62 (talk) 15:02, 7 June 2010 (UTC)[reply]

That's what I can try. I was impatient and boiled it, getting the basic iron(III) acetate. BTW, if you are an admin, you can delete basic iron(III) acetate. --Chemicalinterest (talk) 15:03, 7 June 2010 (UTC)[reply]

Ac = acetate is really archaic nomenclature... Ac = CH3CO; AcO = CH3COO --Rifleman 82 (talk) 15:33, 7 June 2010 (UTC)[reply]

I can see you deleted it. I just used the Ac as an abbrev. instead of writing CH₃COO each time. What is the proper abbreviation for acetate (if there is any)? --Chemicalinterest (talk) 15:36, 7 June 2010 (UTC)[reply]

I didn't delete it, someone else did. See my last comment: Ac = acetyl, CH₃CO; AcO or OAc.

PC: what were you hoping, that he'd have access to a diffractometer? --Rifleman 82 (talk) 15:47, 7 June 2010 (UTC)[reply]

No... just hoping that he would know what the obscure useless compound is. --Chemicalinterest (talk) 15:53, 7 June 2010 (UTC)[reply]

@RM82: Chemicalinterest doesn't need access to to a diffractometer if he can get his unknown compound to crystallize! I bet it will just go to the basic acetate on simple evaporation, but It's always worth a try... Physchim62 (talk) 22:08, 7 June 2010 (UTC)[reply]

I'll try it now, may get results in several days. --Chemicalinterest (talk) 22:41, 7 June 2010 (UTC)[reply]

(ec, also known as edit conflict) :::I'm not expert in organic chemistry, so I don't really know the different isomers and molecules that are functional groups that well. --Chemicalinterest (talk) 15:49, 7 June 2010 (UTC)[reply]

Which one is acetyl, CH3O or CH3CO? --Chemicalinterest (talk) 15:50, 7 June 2010 (UTC)[reply]

Acetyl is CH₃CO, i.e. H₃C-C=O. Acetate is often abbreviated to AcO or OAc, so acetate esters become ROAc or AcOR, and acetate salts contain AcO⁻ or ⁻OAc. For example, ethyl acetate can be written EtOAc, and sodium acetate can be written NaOAc.

Ben (talk) 20:14, 7 June 2010 (UTC)[reply]

All right, I never knew which was the right abbreviation. --Chemicalinterest (talk) 20:16, 7 June 2010 (UTC)[reply]

Not a problem, now you know!

)

Ben (talk) 21:40, 7 June 2010 (UTC)[reply]

June 2010

Thank you for your contributions to Wikipedia. When using certain templates on talk pages, as you did to User talk:87.102.13.111, don't forget to substitute with text by adding subst: to the template tag. For example, use {{subst:uw-test1}} instead of {{uw-test1}}. This reduces server load and prevents accidental blanking of the template. Thank you. -- Rick Van Tassel ^{user|talk|contribs} 16:58, 9 June 2010 (UTC)[reply]

I always wondered what it was for. So instead of accessing the template every time you look at the page, it just converts the template to text and you just view the text? --Chemicalinterest (talk) 17:13, 9 June 2010 (UTC)[reply]

Yes, and my understanding of the reson behind this policy is as follows: If every template on a user page is subst'd, every userpage has high text contents, so they just take up more space. The other extreme is that a lot of user pages all reference the same templates very frequently. In particular, WP:WARNING templates. This would make the server(s) need to access the same files very frequently which would result in a lot of slowdown. The reason that this policy doesn't apply for articles is that consistency is frequently more important in articles than in user space, where the consistency is not important as long as the message is clear. This is just my understanding of the policy. I'll look for official statements sometime. —Preceding unsigned comment added by Ruzihm (talk • contribs) 17:22, 9 June 2010 (UTC)[reply]

Your pictures

Hello, Chemicalinterest. I saw you uploaded some pictures from your home lab to Wikipedia. Could you please upload them here instead? If you do, then your pictures can also be used on different language wikis and also on Commons. Thanks. Also, you can remove File:Ferric acetate.JPG from User:Chemicalinterest/Unused pictures, I added it to the Iron(III) acetate article. Best, --The High Fin Sperm Whale 20:41, 10 June 2010 (UTC)[reply]

I cannot upload them now, but possibly in the near future. Thank you. --Chemicalinterest (talk) 20:52, 10 June 2010 (UTC)[reply]

Silicon

How to split Silicon [Si] from Silicon Dioxide [SiO2], although I know that Silicon [Si] is an active-metals, splitting it in pure form is extremely difficult !!--אנונימי גבר (talk) 01:10, 15 June 2010 (UTC)[reply]

There is one way that is difficult to do. Heat a mixture of silicon dioxide and carbon to 2000C in an electric arc furnace (or welder). Liquid silicon will be produced. --Chemicalinterest (talk) 01:14, 15 June 2010 (UTC)[reply]

Fluorine can use [F] instead of carbon [C] it?--אנונימי גבר (talk) 01:22, 15 June 2010 (UTC)[reply]

When you use spaces instead of colons on wikipedia, it makes a box around your post. Just a note.

Fluorine cannot reduce silicon dioxide to silicon because it is an oxidizing agent (an extremely powerful one). Carbon is a reducing agent (very strong at high temperatures). I seemed to have produced silicon once by electrolysis of a silicic acid solution. It plated a gray coating on a screw that was very corrosion-resistant. You might be able to use aluminum instead though.

I will be away for about 10 hours so I will not respond readily to your next post. Thanks for the conversation. Feel free to keep it up. --Chemicalinterest (talk) 01:31, 15 June 2010 (UTC)[reply]

Inox

I can rip metal Chromium [Cr] pure from stainless steel alloy is not? (In this steel contains about 12.5% prime Chromium) I know that this type of steel is dissolved in nitric acid, with a slow speed (20g steel nitric acid is boiled in a special day that has just been dissolved 0.2 g) but for the of strength Cards the others it dissolves quickly!--אנונימי גבר (talk) 01:42, 15 June 2010 (UTC)[reply]

Difficult to. Stainless steel dissolves slowly in hydrochloric acid to produce a mixture of chromium, nickel, and ferrous chlorides. You could use the procuess listed below to separate the chromium out but the nickel and the iron salts will stay together. --Chemicalinterest (talk) 11:06, 15 June 2010 (UTC)[reply]

Chromium and Nickel from Nichrome

Can separate the two metals Nickel [Ni] and Chromium [Cr] alloy from Nichrome is not?

My opinion is, we can for this alloy in a solution of hydrochloric acid [HCl], we will create a battery element in which the role Nickel (extreme -) (dissolves) and Chromium close the role (pole +) then separating and purifying mixtures of metal.
Or we can let the air flow carbon dioxide (CO2) into the alloy effects Nichrome, nickel in the alloy reacts with carbon dioxide to create Nickel cacbonate , white liquid, then baked to obtain the pure Nickel and gas CO2 exit.

These are only my personal opinion, it looks like you have Nichrome alloy must, you can check to help me?--אנונימי גבר (talk) 10:01, 15 June 2010 (UTC)[reply]

I see one problem with your air flow use. What I think you are thinking of is the reaction of carbon monoxide (a poisonous gas only present in very trace amounts in the atmosphere) with nickel to form nickel carbonyl, which can be a liquid or a gas. Carbon dioxide doesn't actually react with metals except for very active ones such as magnesium at high temperatures. And that to form carbon and the metal oxide, not the carbonate.

Yes; I do have it; and it is difficult to separate the nickel and the chromium. I am thinking of separation by dissolution in base. Nickel(II) oxide, part of the precipitate formed when you react nichrome with hydrochloric acid and then precipitate the hydroxides with alkali. It only reacts with alkali at high temperatures (700C). It seems that chromium(III) oxide, the other component, reacts with concentrated alkali easily. So:

React nichrome with hydrochloric acid. You will get a green solution. NiCr + 5 HCl → NiCl₂ + CrCl₃
React that with an alkali until you get a green precipitate of NiO or Ni(OH)₂ and Cr₂O₃. NiCl₂ + 2 NaOH → Ni(OH)₂ + 2 NaCl; 2 CrCl₃ + 6 NaOH → Cr₂O₃ + 3 H₂O + 6 NaCl (Note:If you let it sit though, it may turn brown-yellow, meaning that it was oxidized by air to form nickel chromate.4 NiO + 2 Cr₂O₃ + 3 O₂ → 4 NiCrO₄)
React the precipitate with excess concentrated alkali and warm to help it dissolve. The chromium oxide should dissolve to form chromite salts. The nickel oxide should stay in precipitation. Cr₂O₃ + 6 NaOH + 3 H₂O → 2Na₃Cr(OH)₆
Filter the solution and repeat the procedure with the alkali.Cr₂O₃ + 6 NaOH + 3 H₂O → 2Na₃Cr(OH)₆ (Each time you repeat it, the NiO gets purer.) After you have done it as many times as you want, you have more or less pure nickel oxide (just NiO).
React that with aluminum powder at a high temperature to produce a thermite reaction. Pure molten nickel should be produced. (3 NiO + 2 Al → 3 Ni + Al₂O₃)

The chromite solution may be reacted with hydrochloric acid to produce chromium(III) chloride (Na₃[Cr(OH)₆] + 6 HCl → 3 NaCl + CrCl₃ + 6 H₂O), and reacted with alkali (not concentrated) to produce chromium(III) oxide precipitate (2 CrCl₃ + 6 NaOH → Cr₂O₃ + 3 H₂O + 6 NaCl). React that with aluminum powder to get a thermite reaction and molten chromium metal again(Cr₂O₃ + 2 Al → Al₂O₃ + 2 Cr) . (This latter procedure is used commercially, see chromium).

Your battery element will not work because both nickel and chromium dissolve easily in acids.

Sources for pure nickel would be: a US nickel (it is made from 75% copper which doesn't dissolve in acids and 25% nickel which does); a nickel electrode from a scientific supply company; and some others. I don't know where you live but you can look up your coins to see if you have any composed of pure nickel or a mixture of nickel and copper; either will do. --Chemicalinterest (talk) 11:03, 15 June 2010 (UTC)[reply]

Can you please record the above reactions using chemical equations are not? I am not very fluent in English, I only learn this subject fairly, so I do not understand you? Thank you much!--אנונימי גבר (talk) 12:45, 15 June 2010 (UTC)[reply]

No problem! :) --Chemicalinterest (talk) 12:47, 15 June 2010 (UTC)[reply]

You can make a compound of titanium and cobalt with high concentrations where?--אנונימי גבר (talk) 12:56, 15 June 2010 (UTC)[reply]

Simple. It is alloy, not compound. Just heat titanium metal and cobalt metal in vacuum until liquid. Mix and you will have alloy. (Tried to make this simple English). --Chemicalinterest (talk) 13:07, 15 June 2010 (UTC)[reply]

In the experiment you mentioned above, I can use carbon [C] to replace the aluminum powder [Al] is not? And let me ask Bo [B] can react with chlorine [Cl] or not?--אנונימי גבר (talk) 12:40, 15 June 2010 (UTC)[reply]

~~Carbon may not be a strong enough reducing agent to reduce chromium~~Carbon can be used. In the chromium article is mentions aluminum; so I know aluminum works. I cannot actually experiment to see whether it works since I do not have the equipment necessary (you can see on User:Chemicalinterest/Chemistry Lab the pictures of my lab, very simple]]). Carbon can reduce nickel though.

Boron does not easily react with chlorine; as you see in the boron trichloride article, it is formed by a reaction between boron trioxide, carbon, and chlorine. --Chemicalinterest (talk) 12:45, 15 June 2010 (UTC)[reply]

soy

are the estrogen's in soy; fat or water soluble ? —Preceding unsigned comment added by Alexsmith44 (talk • contribs) 11:26, 15 June 2010 (UTC)[reply]

A simpler question would be that whether estrogens in general are fat or water soluble. I'm only in high school and not expert in organic chemistry, but I wouldn't think they are water-soluble. --Chemicalinterest (talk) 11:28, 15 June 2010 (UTC)[reply]

I don't see it in any article; the articles have very little chemical quantitative data (solubility, properties). --Chemicalinterest (talk) 11:31, 15 June 2010 (UTC)[reply]

yes but arent the estrogen's in soy synthetic estrogen's ? is there solubility different ? —Preceding unsigned comment added by Alexsmith44 (talk • contribs) 13:47, 15 June 2010 (UTC)[reply]

They should have the same properties whether they are synthetic or not. The chemical properties should not change. --Chemicalinterest (talk) 13:50, 15 June 2010 (UTC)[reply]

so does soybean oil contain estrogen's ? —Preceding unsigned comment added by Alexsmith44 (talk • contribs) 21:46, 15 June 2010 (UTC)[reply]

It probably does, unless they are thermally unstable and are ruined when the soybean oil is processed. --Chemicalinterest (talk) 22:08, 15 June 2010 (UTC)[reply]