Radical Polymerization of Alkenes, Polymers

Radical Polymerization of Alkenes, Polymers

Prior to the early 1920’s, chemists doubted the existence of molecules having molecular weights greater than a few thousand. This limiting view was challenged by Hermann Staudinger, a German chemist with experience in studying natural compounds such as rubber and cellulose. In contrast to the prevailing rationalization of these substances as aggregates of small molecules, Staudinger proposed they were made up of macromolecules composed of 10,000 or more atoms. He formulated a polymeric structure for rubber, based on a repeating isoprene unit (referred to as a monomer). For his contributions to chemistry, Staudinger received the 1953 Nobel Prize. The terms polymer and monomer were derived from the Greek roots poly (many), mono (one) and meros (part).

Recognition that polymeric macromolecules make up many important natural materials was followed by the creation of synthetic analogs having a variety of properties. Indeed, applications of these materials as fibers, flexible films, adhesives, resistant paints and tough but light solids have transformed modern society. Some important examples of these substances are discussed in the following sections.There are two general types of polymerization reactions: addition polymerization and condensation polymerization. In addition polymerization, the monomers add to one another in such a way that the polymer contains all the atoms of the starting monomers. Ethylene molecules are joined together in long chains.

Strictly speaking, this chapter is on radical reactions, which include most addition polymerization processes. However, in order to cover the topic of polymers properly, we are including a brief section on condensation polymerization (usually based on substitution chemistry) here as well.

Many natural materials—such as proteins, cellulose and starch, and complex silicate minerals—are polymers. Artificial fibers, films, plastics, semisolid resins, and rubbers are also polymers. More than half the compounds produced by the chemical industry are synthetic polymers.

Chain-Reaction (Addition) Polymerization

The polymerization can be represented by the reaction of a few monomer units:

The bond lines extending at the ends in the formula of the product indicate that the structure extends for many units in each direction. Notice that all the atoms—two carbon atoms and four hydrogen atoms—of each monomer molecule are incorporated into the polymer structure. Because displays such as the one above are cumbersome, the polymerization is often abbreviated as follows:

nCH₂=CH₂ → [ CH₂CH₂ ] _n

During the polymeriation of ethene, thousands of ethene molecules join together to make poly(ethene) – commonly called polythene. The reaction is done at high pressures in the presence of a trace of oxygen as an initiator.

Some common addition polymers are listed in the Table below . Note that all the monomers have carbon-to-carbon double bonds. Many polymers are mundane (e.g., plastic bags, food wrap, toys, and tableware), but there are also polymers that conduct electricity, have amazing adhesive properties, or are stronger than steel but much lighter in weight.

**Table** *: Some Addition Polymers*
Monomer	Polymer	Polymer Name	Some Uses
CH₂=CH₂	~CH₂CH₂CH₂CH₂CH₂CH₂~	polyethylene	plastic bags, bottles, toys, electrical insulation
CH₂=CHCH₃		polypropylene	carpeting, bottles, luggage, exercise clothing
CH₂=CHCl		polyvinyl chloride	bags for intravenous solutions, pipes, tubing, floor coverings
CF₂=CF₂	~CF₂CF₂CF₂CF₂CF₂CF₂~	polytetrafluoroethylene	nonstick coatings, electrical insulation

Step 1: Chain Initiation

The oxygen reacts with some of the ethene to give an organic peroxide. Organic peroxides are very reactive molecules containing oxygen-oxygen single bonds which are quite weak and which break easily to give free radicals. You can short-cut the process by adding other organic peroxides directly to the ethene instead of using oxygen if you want to. The type of the free radicals that start the reaction off vary depending on their source. For simplicity we give them a general formula: Ra∙

Step 2: Chain Propagation

In an ethene molecule, CH₂=CH₂, the two pairs of electrons which make up the double bond aren’t the same. One pair is held securely on the line between the two carbon nuclei in a sigma bond. The other pair is more loosely held in an orbital above and below the plane of the molecule in a π

bond.

It would be helpful – but not essential – if you read about the structure of ethene before you went on. If the diagram above is unfamiliar to you, then you certainly ought to read this background material.

Imagine what happens if a free radical approaches the π bond in ethene.

Don’t worry that we’ve gone back to a simpler diagram. As long as you realise that the pair of electrons shown between the two carbon atoms is in a π bond – and therefore vulnerable – that’s all that really matters for this mechanism.

The sigma bond between the carbon atoms isn’t affected by any of this. The free radical, Ra

, uses one of the electrons in the π bond to help to form a new bond between itself and the left hand carbon atom – a radical addition step. The other electron returns to the right hand carbon. You can show this using curved arrow notation (with single-headed “fish-hook” arrows) if you want to:

This is energetically worth doing because the new bond between the radical and the carbon is stronger than the π bond which is broken. You would get more energy out when the new bond is made than was used to break the old one. The more energy that is given out, the more stable the system becomes. What we’ve now got is a bigger free radical – lengthened by CH₂CH₂. That can react with another ethene molecule in the same way:

So now the radical is even bigger. That can react with another ethene – and so on and so on. The polymer chain gets longer and longer.

Step 3: Chain Termination

The chain does not, however, grow indefinitely. Sooner or later two free radicals will collide together.

That immediately stops the growth of two chains and produces one of the final molecules in the poly(ethene). It is important to realise that the poly(ethene) is going to be a mixture of molecules of different sizes, made in this sort of random way. Because chain termination is a random process, poly(ethene) will be made up of chains of different lengths.

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