which is more reactive 1-chloropropane or 1-iodopropane?
445447
1-chloropropane, because chlorine has a higher value of electronegativity.
585856
The bond energy is closely related to electronegativity.  It is well known in chemistry that covalent bonds involving fluorine, oxygen, and nitrogen (FON or phone) are the strongest possible bonds (in that order).  Following that within the halogens, is chlorine, bromine, and iodine.  Again, as the electronegativity is lower, the bond energy is lower and that bond is easier to break.  \n\nThis is why HI is much more reactive than HF; the bond involving iodine is weaker (lower bond energy) than that of fluorine.  \n\nSo strongest fluorine:\nF>Cl>Br>I
901121
If the cyclopentane is in excess, then that will tend to limit the reaction to one H being replaced by a Br atom.\nIf the proportion of Br is increased, then more H atoms can be substituted.
857379
Nitrogen triiodide is a feisty one:\n\nhttp://en.wikipedia.org/wiki/Nitrogen_triiodide
445656
I think it's 'gammexane' instead. It's also referred to as BHC (benzene hexachloride)\n\nEDIT: Referring to Supertramp_82's answer, hexachlorocyclohexane (HCH) as C6H6Cl6, gammexane and benzene hexachloride (BHC) are the same. Crude BHC or gammexane is a chlorinated hydrocarbon which exists in at least 5 isomeric forms - it doesn't matter which one you write, it's still the same compound.
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
546423
Bromocyclohexane. You don't need to add the "1-" because it's assumed to be 1 by IUPAC convention.
668649
mono-\ndi-\ntri-\ntetra-\n-chloromethane\n\nnb. replace chloro with bromo or iodo (for Br or I) :)
1141478
I don't know about chloroform but acetone works well
480669
Refrigerant 123 is more correctly known as 2,2-dichloro-1,1,1-trifluoroethane.  Density is 1.4638 g/cm3
440959
Below is a link to the MSDS (Material Safety Data Sheet) for this compound, which is actually 2,4-Dihydroxy-5-iodopyrimidine, but curiously it does not list the density.\n\nHave you looked in the Merck Index?
139959
They are both members of the halogen group, which is the column they are in on the periodic table.  All elements in a group have similar chemical properties, as their outer electrons are the same.  Halogens all have 7 electrons, so they need 1 to have a complete shell.  Therefore, they usually like to take an electron from another atom and carry a -1 charge.\n\nHowever, as you move down a group, the atoms get progressively larger.  Therefore, iodide is larger than chloride.
561048
Some oxide of chlorine. No idea about which one would be stable at those conditions, though.
858619
The easiest way to approach problems like these, my friend, is to look at your alkyl halide first and then look at your nucleophile or base.\n\nT-butyl bromide is a tertiary halide.  Tertiary halides undergo E1 and SN1 reactions because of their ability to form a stable carbocation intermediate.  If you recall, tertiary carbocations are more stable than primary and secondary.\n\nYour -OCH3 is a strong base known as methoxide, the conjugate base of methanol.  Strong bases favor elimination reactions and thus the elimination product is your answer.
108256
More than likely a chlorine gas I would rec. NOT experimenting with the two. I work in the water treatment field. Trust me
193729
most of the chemical properties of alkyl halides are related to the polar bond.  this bond strengthens with decreased length.  therefore, as fluorine is the smallest halogen, the carbon-fluorine bond will be the shortest and strongest.  the boiling points of alkyl halides are generally higher than those of the corresponding alkane, and the boiling point rise with with increasing size of the halogen as a result of greater London dispersion forces.\n\ni have studied alkyl halides in respect to their ability to undergo both nucleophilic subsititution and elimination reactions.\n\nhope that helps!
743385
Cl2 + 2 KI → I2 + 2 KCl