# The Polymerization of Ethene


This module guides you through the mechanism for the polymerisation of ethene by a free radical addition reaction. We are going to talk through this mechanism in a very detailed way so that you get a feel for what is going on.

You will remember that 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.

## 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: $$Ra ^{\bullet}$$

## 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 bond called a sigma bond. The other pair is more loosely held in an orbital above and below the plane of the molecule known as a $$\pi$$ bond.

##### Note

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 $$\pi$$ bond in ethene.

##### Note

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 $$\pi$$ 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 $$\pi$$ bond to help to form a new bond between itself and the left hand carbon atom. The other electron returns to the right hand carbon. You can show this using "curly arrow" notation if you want to:

##### Note

This is energetically worth doing because the new bond between the radical and the carbon is stronger than the $$\pi$$ 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.

## Summary

• Chain initiation: The chain is initiated by free radicals, Ra, produced by reaction between some of the ethene and the oxygen initiator.
• Chain propagation: Each time a free radical hits an ethene molecule a new longer free radical is formed (e.g.,

• Chain termination: Eventually two free radicals hit each other producing a final molecule. The process stops here because no new free radicals are formed.

Because chain termination is a random process, poly(ethene) will be made up of chains of different lengths.

## Contributors

Jim Clark (Chemguide.co.uk)

The Polymerization of Ethene is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts.