AS Organic Chemistry - Haloalkanes
Haloalkanes - Nomenclature
(i) Position number -
Count the number of carbon atoms from the nearest chain end to where the halogen is attached.
(ii) Prefix -
Second comes the prefix based on which halogen element is present,
(iii) Suffix -
Simply add the normal unchanged alkane (or alkene) name onto the suffix (see naming alkanes in the alkanes page).
Exemplar compounds -
Some examples to try out -back to top
Haloalkanes - Reactions
(1) Reactions of Bromoethane :
(i) Hydrolysis -
This is the direct replacement of the bromine atom in the molecule with a hydroxide (-OH) group, giving a bromide ion.
This can be achieved in a variety of ways. Water is the main reactant needed, to provide the -OH group. Some sort of acidic catalyst is also needed to help remove the halogen atom -
(i) either an alkali (NaOH, KOH, etc.), which provides extra -OH ions (very common)
(ii) or silver nitrate solution, which reacts with the halide ions produced, removing them from solution, as a silver halide precipitate, and pushing the reaction equilm over to the products.
CH3CH2Br + -OH → CH3CH2OH + Br-
(ii) Reaction with cyanide ions -
This is the direct replacement of the bromine atom with a nitrile group (-CN), giving a bromide ion.
The reactant is either hydrogen cyanide (HCN) or more likely an acidified solution of an alkali metal cyanide salt (e.g. NaCN, KCN ) in an alcoholic solvent.
CH3CH2Br + -CN → CH3CH2CN + Br-
(iii) Reaction with ammonia -
This is the direct replacement of the bromine atom with an amine group (-NH2) (see amines in chains and rings and spectroscopy), giving hydrogen bromide.
The reactant is ammonia at high pressure in sealed vessel.
CH3CH2Br + NH3 → CH3CH2NH2 + HBr
(2) Reactions of 2-Bromopropane :
This type of reaction involves the removal of a group of atoms from a compound, giving two neutral compounds.
In this case it is the removal of hydrogen bromide (HBr).
The reactants are virtually the same as with the hydrolysis of bromoethane, i.e. alcoholic alkali(aq) - with the added condition of reflux (i.e. heat to boiling).
CH3CHBrCH3 → CH3CH=CH2 + HBr
There is always a competition between the substitution and elimination reactions. The refluxing pushes the reaction over to elimination.back to top
Haloalkanes - Reactions mechanisms
There are only two reaction mechanisms that concern us here. They are both variants on the theme of nucleophilic substitution -
nucleo = nucleus, centre of +ve charge, region of low electron density
philic = attraction
substitution = the direct replacement of an atom, or group of atoms, with another atom or group of atoms
There is one mechanism for 1° haloalkanes and another slightly different one for 3° haloalkanes. They both depend on the polarisation of the carbon-halogen bond present in the molecule.
(1) 1° haloalkanes :
This mechanism involves only one stage - the simultaneous attacking by the nucleophile and expulsion of the halogen atom from the molecule.
e.g. hydrolysis and reaction of cyanide ions and ammonia with bromoethane.
Two molecules are involved in the rate determining step (in fact the only step in the reaction) and therefore the mechanism is called SubstitutionNucleophilic2 or SN2.
(2) 3° haloalkanes :
This variant mechanism involves two separate parts. Firstly, the breaking of the C-X bond and then the formation of a new C-Nu bond.
e.g. hydrolysis and reaction of cyanide ions and ammonia with 2-bromo-2-methylpropane.
One molecule is involved in the rate determining step and therefore the mechanism is labeled SN1. (SubstitutionNucleophilic1).back to top
Haloalkanes - Reaction rates
(1) 1° vs. 2° vs. 3° haloalkanes :
The rate of reaction of 1°, 2° and 3° haloalkanes depends on the mechanism followed by the particular compound.
The rate of any reaction can depend on a number of factors including heat and pressure. Another important factor is the ability for molecules to collide with one another in order to start a reaction.
With 1° haloalkanes the mechanism followed is SN2, because the carbon-halogen bond can be attacked by the hydroxide ion,
With the 3° haloalkane the central carbon atom is hidden by the surrounding methyl groups,
this prevents the hydroxide ion from attacking directly.
As previously mentioned SN2 depends on two molecules colliding with one another before any reaction can occur. This is inherently a slow process and depends on a chance occurrence.
3° haloalkanes on the other hand follow an SN1 pathway since the carbocation formed is stabilised by the alkyl groups attached to the central carbon atom. The 1° haloalkane does not form a stable carbocation so does not follow SN1.
SN1 relies on the spontaneous splitting apart of a single molecule. Whilst this itself is not particularly fast it is a lot faster than the chance collision of two molecules in SN2.
Therefore, 3° haloalkanes react a lot faster than 1° haloalkanes.
2° halo compounds follow a mixture of the two reaction mechanisms and therefore are faster than the 1° compounds but slower than the 3° compounds.
(2) -F vs. -Cl vs. -Br vs. -I :
The relative rate of reaction of the various halogen compounds depends on the strength and polarisation of the C-halogen bond.
The average bond energies for the four types of C-halogen bond are -
|C-F =||467 kJmol-1|
|C-Cl =||346 kJmol-1|
|C-Br =||290 kJmol-1|
|C-I =||228 kJmol-1|
The change in the bond energies is due partly to the increased size of the halogen down the group leading to poorer orbital overlap forming the C-X bond.
The relative reactivities follow these energies with the weaker C-I bonds being the easiest to break and the stronger C-F bond being the hardest.
(3) 2° chloroalkanes vs chlorobenzene :
Whilst technically chlorobenzene is a 2° halo compound, because there are two carbon atoms attached to the C-Cl group, it reacts in a totally different manner.
The aromatic benzene ring prevents the normal substitution reactions that would occur with normal 2° haloalkanes. The C-Cl bond is a lot stronger than normal partly because of the increased overlap with the p-orbitals of the ring.
Therefore chloroform will not undergo hydrolysis or react with ammonia or cyanide ions as any other 2° haloalkane will.back to top
Haloalkanes - Uses
(1) Fluoroalkanes and Fluorohaloalkanes :
Haloalkenes make up a number of addition polymers including poly(chloroethene) and poly(tetrafluroethene).
(2) CFC's :
Many chlorofluorocarbons (CFCs) were used in the past as refrigerant and general propellant gases. These have been replaced by small chain alkanes which don't harm the ozone layer but are a lot more flammable.
(3) Anaesthetics :
Haloalkanes can be used for anaesthetics. These include chloroform, CHCl3 (which was one of the first widely used anaesthetics) and chloral hydrate, CCl3C(OH)2H (aka "a Mickey Finn"). A modern anaesthetic is halothane, CF3CHBrCl.back to top
written by Dr Richard Clarkson : © Saturday, 1 November 1997
Updated : Saturday, 25th August, 2012
mail to: chemistryrules
Created with the aid of,
The haloalkanes (also known as halogenoalkanes or alkyl halides) are a group of chemical compounds derived from alkanes containing one or more halogens. They are a subset of the general class of halocarbons, although the distinction is not often made. Haloalkanes are widely used commercially and, consequently, are known under many chemical and commercial names. They are used as flame retardants, fire extinguishants, refrigerants, propellants, solvents, and pharmaceuticals. Subsequent to the widespread use in commerce, many halocarbons have also been shown to be serious pollutants and toxins. For example, the chlorofluorocarbons have been shown to lead to ozone depletion. Methyl bromide is a controversial fumigant. Only haloalkanes which contain chlorine, bromine, and iodine are a threat to the ozone layer, but fluorinated volatile haloalkanes in theory may have activity as greenhouse gases. Methyl iodide, a naturally occurring substance, however, does not have ozone-depleting properties and the United States Environmental Protection Agency has designated the compound a non-ozone layer depleter. For more information, see Halomethane. Haloalkane or alkyl halides are the compounds which have the general formula "RX" where R is an alkyl or substituted alkyl group and X is a halogen (F, Cl, Br, I).
Haloalkanes have been known for centuries. Chloroethane was produced synthetically in the 15th century. The systematic synthesis of such compounds developed in the 19th century in step with the development of organic chemistry and the understanding of the structure of alkanes. Methods were developed for the selective formation of C-halogen bonds. Especially versatile methods included the addition of halogens to alkenes, hydrohalogenation of alkenes, and the conversion of alcohols to alkyl halides. These methods are so reliable and so easily implemented that haloalkanes became cheaply available for use in industrial chemistry because the halide could be further replaced by other functional groups.
While most haloalkanes are human-produced, non-artificial-source haloalkanes do occur on Earth, mostly through enzyme-mediated synthesis by bacteria, fungi, and especially sea macroalgae (seaweeds). More than 1600 halogenated organics have been identified, with bromoalkanes being the most common haloalkanes. Brominated organics in biology range from biologically produced methyl bromide to non-alkane aromatics and unsaturates (indoles, terpenes, acetogenins, and phenols). Halogenated alkanes in land plants are more rare, but do occur, as for example the fluoroacetate produced as a toxin by at least 40 species of known plants. Specific dehalogenase enzymes in bacteria which remove halogens from haloalkanes, are also known.
From the structural perspective, haloalkanes can be classified according to the connectivity of the carbon atom to which the halogen is attached. In primary (1°) haloalkanes, the carbon that carries the halogen atom is only attached to one other alkyl group. An example is chloroethane (CH
2Cl). In secondary (2°) haloalkanes, the carbon that carries the halogen atom has two C–C bonds. In tertiary (3°) haloalkanes, the carbon that carries the halogen atom has three C–C bonds.
Haloalkanes can also be classified according to the type of halogen on group 7 responding to a specific halogenoalkane. Haloalkanes containing carbon bonded to fluorine, chlorine, bromine, and iodine results in organofluorine, organochlorine, organobromine and organoiodine compounds, respectively. Compounds containing more than one kind of halogen are also possible. Several classes of widely used haloalkanes are classified in this way chlorofluorocarbons (CFCs), hydrochlorofluorocarbons (HCFCs) and hydrofluorocarbons (HFCs). These abbreviations are particularly common in discussions of the environmental impact of haloalkanes.
Haloalkanes generally resemble the parent alkanes in being colorless, relatively odorless, and hydrophobic. Their boiling points are higher than the corresponding alkanes and scale with the atomic weight and number of halides. This is due to the increased strength of the intermolecular forces—from London dispersion to dipole-dipole interaction because of the increased polarity. Thus carbon tetraiodide (CI
4) is a solid whereas carbon tetrafluoride (CF
4) is a gas. As they contain fewer C–H bonds, halocarbons are less flammable than alkanes, and some are used in fire extinguishers. Haloalkanes are better solvents than the corresponding alkanes because of their increased polarity. Haloalkanes containing halogens other than fluorine are more reactive than the parent alkanes—it is this reactivity that is the basis of most controversies. Many are alkylating agents, with primary haloalkanes and those containing heavier halogens being the most active (fluoroalkanes do not act as alkylating agents under normal conditions). The ozone-depleting abilities of the CFCs arises from the photolability of the C–Cl bond.
Haloalkanes are of wide interest because they are widespread and have diverse beneficial and detrimental impacts. The oceans are estimated to release 1-2 million tons of bromomethane annually.
A large number of pharmaceuticals contain halogens, especially fluorine. An estimated one fifth of pharmaceuticals contain fluorine, including several of the most widely used drugs. Examples include 5-fluorouracil, fluoxetine (Prozac), paroxetine (Paxil), ciprofloxacin (Cipro), mefloquine, and fluconazole. The beneficial effects arise because the C-F bond is relatively unreactive. Fluorine-substituted ethers are volatile anesthetics, including the commercial products methoxyflurane, enflurane, isoflurane, sevoflurane and desflurane. Fluorocarbon anesthetics reduce the hazard of flammability with diethyl ether and cyclopropane. Perfluorinated alkanes are used as blood substitutes.
Chlorinated or fluorinated alkenes undergo polymerization. Important halogenated polymers include polyvinyl chloride (PVC), and polytetrafluoroethene (PTFE, or Teflon). The production of these materials releases substantial amounts of wastes.
The formal naming of haloalkanes should follow IUPAC nomenclature, which put the halogen as a prefix to the alkane. For example, ethane with bromine becomes bromoethane, methane with four chlorine groups becomes tetrachloromethane. However, many of these compounds have already an established trivial name, which is endorsed by the IUPAC nomenclature, for example chloroform (trichloromethane) and methylene chloride (dichloromethane). For unambiguity, this article follows the systematic naming scheme throughout.
Haloalkanes can be produced from virtually all organic precursors. From the perspective of industry, the most important ones are alkanes and alkenes.
Main article: Free radical halogenation
Alkanes react with halogens by free radical halogenation. In this reaction a hydrogen atom is removed from the alkane, then replaced by a halogen atom by reaction with a diatomic halogen molecule. The reactive intermediate in this reaction is a free radical and the reaction is called a radical chain reaction.
Free radical halogenation typically produces a mixture of compounds mono- or multihalogenated at various positions. It is possible to predict the results of a halogenation reaction based on bond dissociation energies and the relative stabilities of the radical intermediates. Another factor to consider is the probability of reaction at each carbon atom, from a statistical point of view.
Due to the different dipole moments of the product mixture, it may be possible to separate them by distillation.
From alkenes and alkynes
In hydrohalogenation, an alkene reacts with a dry hydrogen halide (HX) like hydrogen chloride (HCl) or hydrogen bromide (HBr) to form a mono-haloalkane. The double bond of the alkene is replaced by two new bonds, one with the halogen and one with the hydrogen atom of the hydrohalic acid. Markovnikov's rule states that in this reaction, the halogen is more likely to become attached to the more substituted carbon. This is an electrophilic addition reaction. Water must be absent otherwise there will be a side product of a halohydrin. The reaction is necessarily to be carried out in a dry inert solvent such as CCl
4 or directly in the gaseous phase. The reaction of alkynes are similar, with the product being a geminal dihalide; once again, Markovnikov's rule is followed.
Alkenes also react with halogens (X2) to form haloalkanes with two neighboring halogen atoms in a halogen addition reaction. Alkynes react similarly, forming the tetrahalo compounds. This is sometimes known as "decolorizing" the halogen, since the reagent X2 is colored and the product is usually colorless and odorless.
Alcohol undergoes nucleophilic substitution reaction by halogen acid to give Haloalkanes.Tertiary alkanol reacts with hydrochloric acid directly to produce tertiary choloroalkane(alkyl chloride), but if primary or secondary alcohol is used, an activator such as zinc chloride is needed. This reaction is exploited in the Lucas test.
The most popular conversion is effected by reacting the alcohol with thionyl chloride (SOCl
2) in the "Darzens halogenation", which is one of the most convenient laboratory methods because the byproducts are gaseous. Both phosphorus pentachloride (PCl
5) and phosphorus trichloride (PCl
3) also convert the hydroxyl group to the chloride.
Alcohols may likewise be converted to bromoalkanes using hydrobromic acid or phosphorus tribromide (PBr3). A catalytic amount of PBr
3 may be used for the transformation using phosphorus and bromine; PBr
3 is formed in situ.
Iodoalkanes may similarly be prepared using red phosphorus and iodine (equivalent to phosphorus triiodide). The Appel reaction is also useful for preparing alkyl halides. The reagent is tetrahalomethane and triphenylphosphine; the co-products are haloform and triphenylphosphine oxide.
From carboxylic acids
Two methods for the synthesis of haloalkanes from carboxylic acids are the Hunsdiecker reaction and the Kochi reaction.
Many chloro and bromolkanes are formed naturally. The principal pathways involve the enzymes chloroperoxidase and bromoperoxidase.
By Rydons method
An alcohol on heating with halogen in presence of triphenyl phosphate produces haloalkanes or alkyl halides.
Haloalkanes are reactive towards nucleophiles. They are polar molecules: the carbon to which the halogen is attached is slightly electropositive where the halogen is slightly electronegative. This results in an electron deficient (electrophilic) carbon which, inevitably, attracts nucleophiles.
Substitution reactions involve the replacement of the halogen with another molecule—thus leaving saturated hydrocarbons, as well as the halogenated product. Haloalkanes behave as the R+synthon, and readily react with nucleophiles.
Hydrolysis, a reaction in which water breaks a bond, is a good example of the nucleophilic nature of haloalkanes. The polar bond attracts a hydroxide ion, OH− (NaOH(aq) being a common source of this ion). This OH− is a nucleophile with a clearly negative charge, as it has excess electrons it donates them to the carbon, which results in a covalent bond between the two. Thus C–X is broken by heterolytic fission resulting in a halide ion, X−. As can be seen, the OH is now attached to the alkyl group, creating an alcohol. (Hydrolysis of bromoethane, for example, yields ethanol). Reaction with ammonia give primary amines.
Chloro- and bromoalkanes are readily substituted by iodide in the Finkelstein reaction. The iodoalkanes produced easily undergo further reaction. Sodium iodide is used thus as a catalyst.
Haloalkanes react with ionic nucleophiles (e.g. cyanide, thiocyanate, azide); the halogen is replaced by the respective group. This is of great synthetic utility: chloroalkanes are often inexpensively available. For example, after undergoing substitution reactions, cyanoalkanes may be hydrolyzed to carboxylic acids, or reduced to primary amines using lithium aluminium hydride. Azoalkanes may be reduced to primary amines by the Staudinger reduction or lithium aluminium hydride. Amines may also be prepared from alkyl halides in amine alkylation, the Gabriel synthesis and Delepine reaction, by undergoing nucleophilic substitution with potassium phthalimide or hexamine respectively, followed by hydrolysis.
In the presence of a base, haloalkanes alkylate alcohols, amines, and thiols to obtain ethers, N-substituted amines, and thioethers respectively. They are substituted by Grignard reagents to give magnesium salts and an extended alkyl compound.
Where the rate-determining step of a nucleophilic substitution reaction is unimolecular, it is known as an SN1 reaction. In this case, the slowest (thus rate-determining step) is the heterolysis of a carbon-halogen bond to give a carbocation and the halide anion. The nucleophile (electron donor) attacks the carbocation to give the product.
SN1 reactions are associated with the racemization of the compound, as the trigonal planar carbocation may be attacked from either face. They are favored mechanism for tertiary haloalkanes, due to the stabilization of the positive charge on the carbocation by three electron-donating alkyl groups. They are also preferred where the substituents are sterically bulky, hindering the SN2 mechanism.
Main article: Dehydrohalogenation
Rather than creating a molecule with the halogen substituted with something else, one can completely eliminate both the halogen and a nearby hydrogen, thus forming an alkene by dehydrohalogenation. For example, with bromoethane and sodium hydroxide (NaOH) in ethanol, the hydroxide ion HO− abstracts a hydrogen atom. Bromide ion is then lost, resulting in ethylene, H2O and NaBr. Thus, haloalkanes can be converted to alkenes. Similarly, dihaloalkanes can be converted to alkynes.
In related reactions, 1,2-dibromocompounds are debrominated by zinc dust to give alkenes and geminal dihalides can react with strong bases to give carbenes.
Haloalkanes undergo free-radical reactions with elemental magnesium to give alkylmagnesium compounds: Grignard reagents. Haloalkanes also react with lithium metal to give organolithium compounds. Both Grignard reagents and organolithium compounds behave as the R− synthon. Alkali metals such as sodium and lithium are able to cause haloalkanes to couple in the Wurtz reaction, giving symmetrical alkanes. Haloalkanes, especially iodoalkanes, also undergo oxidative addition reactions to give organometallic compounds.
Haloalkanes are widely used as synthon equivalents to alkyl cation (R+) in organic synthesis. They can also participate in a wide variety of other organic reactions.
Short chain haloalkanes such as dichloromethane, trichloromethane (chloroform) and tetrachloromethane are commonly used as hydrophobic solvents in chemistry. They were formerly very common in industry; however, their use has been greatly curtailed due to their toxicity and harmful environmental effects.
Chlorofluorocarbons were used almost universally as refrigerants and propellants due to their relatively low toxicity and high heat of vaporization. Starting in the 1980s, as their contribution to ozone depletion became known, their use was increasingly restricted, and they have now largely been replaced by HFCs.
Bromochlorodifluoromethane (Halon 1211), and Bromotrifluoromethane (Halon 1301), as well as others are used in fire extinguishers. Due to their high ozone depletion potential, production has ended as of April 6, 1998 cost is high, and they are primarily used for critical applications such as aviation and military.