Talk:Dichloromethane

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NFPA[edit]

I think the NFPA symbol is wrong. If I'm not mistaken it should be 3 health, 1 flammability and 2 reactivity. It's not very nice stuff to deal with.

Au contraire, relative to other chlorocarbons and most organics, CH2Cl2 is remarkably benign. It does scare alarmists who are unfamiliar with chemistry. I confirmed that the NFPA listing is current: Health Hazard of 2 and ZERO for fire and reactivity. Great stuff compared to the seriously dangerous materials with less threatening names - say, phthalates.--Smokefoot (talk) 22:36, 17 July 2008 (UTC)

Unless I am mistaking, in the last revision of NFPA coding, it is 2 for toxicity 1 for fire and 0 for reactivity. —Preceding unsigned comment added by Process engineer france (talkcontribs) 14:45, 16 March 2009 (UTC)

Flash Point[edit]

you should list flash point for all chemicals

  • Actually DCM is a non flammable liquid thus I understand it does not have a flash point. Maybe we could put "Not Flammable" rather than "none" in the infobox? Berserker79 08:27, 12 December 2005 (UTC)

is it dangerous[edit]

i deal with dichloromethane at work and also have a friend who is pregenant and has come in contact with it, what health risks does it pose for herand is it safe to use.

__Please read the MSDS sheet for water (H2O and dicloromethane)__


Is this vandalism?[edit]

What is the meaning of this line? Does it belong in this article? If so, please rewrite in English.

"Dichloromethane is quite often used as a farming tool in Eastern and Central America as a gene adaptation tool."

RastaKins 03:28, 30 August 2007 (UTC)

Small Dichloromethane Spill[edit]

Hello,

I realize this is a talk section, but I am concerned about a small spill at my workplace. I purchased a toy drinking bird which contains this chemical (http://www.thinkgeek.com/geektoys/science/981b/), which was knocked over by a coworker, broken and spilled onto my desk. I cleaned up the area with some water and white board cleaner, and washed my hands thoroughly with soap. I just want to know if, based on the amount seen in the picture, if there is any concern for inhilation or prolonged exposure. —Preceding unsigned comment added by 207.45.240.18 (talk) 20:21, 30 July 2008 (UTC)

Wikipedia is not an appropriate place to seek advice for health and safety matters such as this. See Category:Wikipedia disclaimers.
If you are worried, the best thing to do is consult any information that came with the product. If that doesn't help, or if there isn't any information available, you could ring the manufacturer. MSDSs for dichloromethane are available online - here's one. That may give some indication of likely problems.
If you're concerned about your health, see a doctor.
Ben (talk) 21:06, 30 July 2008 (UTC)

NFPA rating?[edit]

Depending on where you look, you'll find conflicting NFPA ratings.

  • Health: 3, Fire: 1, Reactivity: 0 [1]
  • Health: 2, Fire: 1, Reactivity: 0 [2]
  • Health: 2, Fire: 0, Reactivity: 0 (current article)

Can someone straighten this out, once and for all? Fuzzform (talk) 21:53, 11 November 2008 (UTC)

Do NFPA ratings actually come from the NFPA, or are they made up by the manufacturers? (I have no idea.) I suspect the later because I often see inconsistencies between different manufacturers and different MSDSs. --Itub (talk) 07:11, 12 November 2008 (UTC)

NFPA rating are coming from NFPA. It is responsability of the manufacturers to report it correctly and update it on their MSDSs. —Preceding unsigned comment added by Process engineer france (talkcontribs) 14:48, 16 March 2009 (UTC)

Useful as Plastic cement[edit]

Should be mentioned as a cement solvent for polycarbonate plastic though it must be carefully handled. —Preceding unsigned comment added by 69.150.170.13 (talk) 05:30, 6 May 2009 (UTC)

Naming[edit]

Shouldn't the title of the article be 'Methylene chloride' rather than 'Dichloromethane'? According to IUPAC naming nomenclature, the former is correct. John 07:31, 16 December 2009 (UTC)

Titles for Wikipedia's chemistry articles are based on commonly used terms rather than IUPAC nomenclature (see Wikipedia:Manual_of_Style_(chemistry) for details). -- Ed (Edgar181) 12:50, 16 December 2009 (UTC)

Methanol as propellant gas[edit]

The vapor pressure of methanol at room temperature is less than that of the substance it would be propelling.

Revision as of 11:22, 1 May 2009 Also used in the garment printing industry for removal of heat-sealed garment transfers. Usually sold in cans with Methanol as the propellant gas.

—Preceding unsigned comment added by 63.100.100.5 (talk) 23:39, 4 January 2010 (UTC)


Normal or Standard?[edit]

Hi, does anyone know if the boiling point listed for DCM or other solvents is the standard bp or the normal bp? I know they are about the same, but sometimes it makes a difference. Thank you. El Zarco 08:07, 27 November 2011 (UTC) — Preceding unsigned comment added by ElZarco (talkcontribs)

Free Radical Substitution[edit]

There is a fundamental difference between using heat and UV light to make dichloromethane. UV light is much easier to use and is less dangerous than heat. SchicagoS (talk) 18:20, 10 April 2012 (UTC)

If you want to claim that this is an easier way to make dichloromethane, you will need to find a reliable source that reports this. Please have a look at WP:RS and WP:V. Thank you. ChemNerd (talk) 18:23, 10 April 2012 (UTC)
You're going to claim that heating up methane gas in the presence of chlorine gas to 500 degrees celcius is easier than shining blue or UV light on the two gases? You don't need a reliable source, but rather COMMON SENSE to prove that this is true. http://www.chemhelper.com/frhalog.html PROOF. SchicagoS (talk) 18:33, 10 April 2012 (UTC)
Yes, that's exactly what I'm claiming. And that is why the thermal process is used industrially, not shining light on the two gases (see the cited reference in the article). The link you provide does nothing to support your claim. ChemNerd (talk) 18:39, 10 April 2012 (UTC)
Yes, INDUSTRIAL chemistry *can* use that method... but ORGANIC chemists use this method. Ya know why? because you dont risk BLOWING UP YOUR LAB if there is a leak. It's insane to think that an individual would ever use that method in an organic chemistry lab. It's safer to use the method that I described. Free Radical Halogenation is a much more elegant solution and it uses less energy. http://www.cengagebrain.com/shop/en/US/storefront/US;CMGTJSESSIONID=n69CPGBNRNk2k1w4DzMs8QHBSwqgChZr5Gb9TwXGTBqJBsYDbG70!-170442550!466608370?cmd=catProductDetail&gclid=CLeVgvD5qq8CFSQCQAodFBylaQ&entryPoint=storefront&ISBN=9780840054449&cid=GS&messageType=catProductDetail P. 188 Organic Chemistry, 8th Edition McMurry ISBN10: 0-8400-5444-0, ISBN13: 978-0-8400-5444-9 SchicagoS (talk) 18:53, 10 April 2012 (UTC)
The photochemical method is not used industrially, it is done thermally from methyl chloride and chlorine according to Ullmann's Encyclopedia of Industrial Chem. That source mentions that the photochemical route is feasible, but it is not not practiced nonetheless. Photochem routes are probably not practical given the scale of the production.--Smokefoot (talk) 22:22, 10 April 2012 (UTC)

Why would anyone ever make dichloromethane in the lab? It's a solvent you can buy in bulk for very little money. Even the deuterated version CD2Cl2 is widely available, if a little more expensive. Ben (talk) 08:03, 14 April 2012 (UTC)