Organic+Halides

=__Organic Halides__= Organic halides (also known as halocarbons) are organic compounds in which one or more carbon atoms are linked by covalent bonds with one or more halogen atoms: fluorine, chlorine, bromine, or iodine. The halogen atoms in organic halides usually take the places of hydrogen atoms in common organic compounds. For this reason, the halogen atoms in halocarbon molecules are often called "substituents."

An organic halide that contains a carbon atom bonded to a chlorine atom (C-Cl) is called an organochloride, an organic halide that contains a carbon atom bonded to a fluorine atom (C-F) is called an organofluoride, and so on. Organochlorides are the most common organic halides. The reactivity of organic halides depends on the halogen atom that is bonded to the carbon atom in the particular compound. Organoiodides are the most reactive and can be converted into many other compounds. Organobromides are less reactive than organoiodides but more reactive than organochlorides. Organofluorides are the least reactive of the organic halides.

__Naming Organic Halides__:

 * 1) Determine the name of the parent chain. This will be the base
 * 2) Identify the halogen(s) that is/are replacing the hydrogen(s) to get the prefix (chloro-, fluoro-, bromo-, or iodo-)
 * 3) Determine how many atoms of each type of halogen there are on the molecule to get the pre-prefix (di-, tri-, tetra-, etc.)
 * 4) Identify the location(s) of the halogen atom(s) on the molecule to get the pre-pre-prefix

So the format for naming halides is:(location of halides)-(halogen prefix)(parent chain)

__Example:__
---H -H CH3-C-C-CH3 ---F -F 1. The parent chain is butane 2. The hydrogen atoms are substituted with fluorine atoms, so the prefix is "fluoro-" 3. There are two fluorines so the pre-prefix is "di-" 4. The fluorines are located in positions 1 and 2 so the pre-pre-prefix is "1,2-"

The name of this compound would be 1,2-difluorobutane

__Boiling points__
Halocarbons are more polar than the hydrocarbon families. Therefore the boiling points will be larger for the same sized molecules. The London Dispersion and the dipole-dipole interactions are the intermolecular forces holding the halocarbon molecules together.

__Water Solubility__
The halocarbons are insoluble in water because there is very little attraction that the halide molecules have for the solvent water. Hydrogen bonding is not present and for that reason most halocarbons are insoluble in water but tend to be soluble in hydrocarbon solvents and other alkyl halide solvents.

__Density__
The densities of halocarbons tend to be greater than that of water because of the relatively massive halogen atoms.

__Production of halocarbons:__
Halocarbons can be produced using two methods:


 * 1. Substitution Reaction:** A halogen is mixed with a saturated hydrocarbon; the halogen atom substitutes hydrogen from the hydrocarbon chain. This reaction can be shown by the general equation:

X2 + R-H → R-X + HX


 * 2. Addition Reaction:** A halogen is mixed with an unsaturated hydrocarbon; a halogen atom adds on to each of the two carbons from the carbon-carbon double bond in the hydrocarbon chain. This reaction can be shown by the general equation:

--X --- X --| | X2 + R-C=C-R' → R-C – C -R'

( R and R' represent alkyl groups)

Sources:
http://en.wikipedia.org/wiki/Organic_halide http://science.jrank.org/pages/3192/Halide-Organic.html http://www.angelfire.com/bc2/OrgChem/halides.html http://hrsbstaff.ednet.ns.ca/dawsonrj/11%20Chem/Chapter%20notes/Chapter%2014%20notes.htm