trihalomethanes? what are they from (for)?
488906
The most obvious one is chloroform, CHCl3.\nIt is created by reacting methane with chlorine free radicals.  I think its a UV light thats used to create the radical, but im not certain.\n\nIt can be used as an anaesthetic, administered orally. Whenever you see someone on a film pass out when a hankie is helt to their mouth its meant to have chloroform on it. More recently it has been used more as a solvent by chemistry labs. Although its main use is in the  production of freon, the thing in fridges that help to keep them cold.
405453
If you do the above reaction, you can get the following compounds: (chloromethyl)benzene, (dichloromethyl)benzene, and (trichloromethyl)benzene.
921311
Bromine is the only non-metal that is a liquid at room temperature and is a highly volatile and unstable compound.  The reason for this is due to the fact that it has 7 valence electrons, 1 away from being a stable noble gas.  Therefore, bromine is highly reactive in order to obtain the extra electron it needs to be happy.  \n\nPlus it smells terrible.  Another reason why it must be unstable.
516493
a) Toluene and Cl2 form p-chlorotoluene and HCl in presence of AlCl3\nb) nitrobenzene + Cl2 -(AlCl3)-> m-chloro-nitrobenzene\nc) chlorobenzene + Cl2 -(AlCl3)-> p-dichlorobenzene\nd) 1-(3-chlorophenyl)ethanone\ne) 3-chlorophenyl acetate\nf) methyl 3-chlorobenzoate\n\nOrganic Chem rocks!
488563
Bromine (from Gr. βρωμος (brómos), meaning "stench"; pronounced [ˈbɹomin]), is a chemical element in the periodic table that has the symbol Br and atomic number 35. A halogen element, bromine is a red volatile liquid at standard room temperature which has a reactivity between chlorine and iodine. This element is corrosive to human tissue in a liquid state and its vapors irritate eyes and throat. Bromine vapors are very toxic upon inhalation.\n\nNotable characteristics\nBromine is the only liquid nonmetallic element at room temperature and one of only two liquid elements on the periodic table (the other is mercury). The pure chemical element has the physical form of a diatomic molecule, Br2. It is a heavy, mobile, reddish-brown liquid, that evaporates easily at standard temperature and pressures in a red vapor (its color resembles nitrogen dioxide) that has a strong disagreeable odor resembling that of chlorine. A halogen, bromine resembles chlorine chemically but is less active. It is more active than iodine, however. Bromine is slightly soluble in water, and highly soluble in carbon disulfide, aliphatic alcohols (such as methanol), and acetic acid. It bonds easily with many elements and has a strong bleaching action.\n\nBromine is highly reactive and is a powerful oxidizing agent in the presence of water. It reacts vigorously with amines, alkenes and phenols as well as aliphatic and aromatic hydrocarbons, ketones and acids (these are brominated by either addition or substitution reactions). With many of the metals and elements, anhydrous bromine is less reactive than wet bromine; however, dry bromine reacts vigorously with aluminium, titanium, mercury as well as alkaline earth metals and alkaline metals.
403761
An organochloride is an organic compound containing at least one covalently bonded chlorine atom. Their wide structural variety and divergent chemical properties lead to a broad range of uses.\n\nThe simplest form of organochlorides are chlorinated hydrocarbons. These consist of simple hydrocarbons in which one or more hydrogen atoms have been replaced with chlorine. Most low molecular weight chlorinated hydrocarbons such as chloroform, dichloromethane, dichloroethene and trichloroethane are useful as solvents.\n\nMany organochlorides have significant biological activities. For example, many powerful and effective insecticides are organochlorides. Common examples include dioxin, DDT, dicofol, heptachlor, endosulfan, chlordane, mirex and pentachlorophenol.\n\nPolychlorinated biphenyls were once commonly used electrical insulators and heat transfer agents. Their use has generally been phased out due to health concerns.\n\nChlorinated alkenes are useful monomers used in the preparation of a variety of materials. For example, vinyl chloride is polymerized to form the plastic polyvinyl chloride (PVC).\n\nMany organochlorides have significant toxicity. Insecticides such as dioxin and DDT are persistent organic pollutants which pose dangers to the environment. Chlorinated solvents, when not handled and disposed of properly, present problems with groundwater pollution. Some organochlorides such as phosgene have even been used as Chemical warfare agents. However, the presence of chlorine in an organic compound, does not insure toxicity. Some organochlorides are safe enough for consumption in foods, such as the sweetener sucralose (Splenda).\n\n\n\nSplenda
124921
CH4 is given to the abreviated name methene, (methanol). It is actually metholethaline. or as we like to cll it on the Hazmat squad, methandeathanol.  Very leathal in large quantities.
1077307
not all of them..\n\nH2O, CH3CL, CH3COONa are weak.. (also any organic substance eg. CH3COOH)\nNaOH, KF are categorized as strong ones due to the formation of ionic bond bet. them, + they're inorganic..
635418
CH3CH2CH2CH3 + CL2 -hV--> \nCH3CH2(CL)CHCH3 + HCL ..\n\nwhat are the ways to get the CL at the end of the chain..so that\n\nCH3CH2CH2CH2CL + 2NA + CLCH2CH2CH2CH3\n--->CH3--------CH3\n\nThat's a radical reaction, the chlorination of an alkane with chlorine in UV light. The intermediate is a carbon radical and secondary radicals are more stable than primary. There are also more secondary carbons on this molecule. So probability and reaction kinetics dictates that the primary alkyl halide will be a minor product.\n\nI guess, if this were my synthesis, I'd:\n\n1. Put the glucose in HCl to cleave the anomers it likes to make.\n\n2. Esterify the carboxlic acid with whatever's available (Fisher esterification with MeOH, for example)\n\n3. Reduce the ester with Diisobutyl aluminium hydride (DIBALH)\n\n4. React the aldehyde with 1 equivalent of Ethyl Magnesium Bromide (Grignard)\n\n5. Reduce the hydroxy groups with a Barton-McCombie deoxygenation, although I've never seen it done in a case like this.\n\nThen again:\n\nI'd go to the stockroom and save my research advisor a lot of money. :)
226789
I would say because the molecules are too big to be effectively dissolved by chloroform. Or the oils are not polar where chloroform would be polar (remember like disolves like).
618652
.........CH3\n..........|\nCH3 - C  - CH2 - CH2 - CH2 - CH3\n.........      |\n........      CH3\n\nPlease ignore the full stops in the above image (which i had to insert to get the correct spacing).\n\nI hope that this helps you.
892054
Is Hydrorogen chloride a solid? I've only ever thought of it as Hydrochloric Acid (get it out of a bottle!) which, of course, liberates See-oh-2 from See-ay-2-see-oh-3.\n\nPS. I asked about the solid 'cos on a practical level be careful of Toluene - it's nasty stuff. It's not used to make HCl, but I can't remember how you do make it. Sorry.
884486
you have one group of CH3 and hence its methylamine....\n\ndimethylamine-----> (CH3)2NH\ntrimethylamine-----> (CH3)3N\n\nCorrect me if i am wrong please....
804029
Trimethylamine, because there are three methyl groups attached to the nitrogen.  (I'm not sure why nitrogen compunds are called amines.)
100646
Trichloromethane (CHCl3) as a) it is asymmetrical & b) the electronegativity of the Cl 'pulls' the eletron density away from the C-H bond
932300
Methane\nsulfur dihydride\nchlorofluorocarbon
38135
Well, I can give you three nonflammable liquids that are mutually immiscible...\n\nwater\ncarbon tetrachloride\nmercury\n\nMost things that are immiscible with water tend to be nonhalogenated solvents and therefore flammable.