Experiment 9

The Formation of the Wonder Polymer: Nylon, an Amide

Objectives

The objective of this experiment is to see how a polymer, nylon is made. This experiment is referred to as a "Condensation Polymerization Reaction" where smaller components are combined in a specific order to produce the wonder polymer nylon. You will create a form of nylon referred to as Nylon 6-6 (both building-block components contain six carbons. As a contest, your Instructor might give extra points for the group producing the longest continuous piece of nylon. Can you beat 79 feet?

Background

The word "nylon" is used to represent synthetic polyamides. The various nylons are described by a numbering system that indicates the number of carbon atoms in the monomer chains. Nylons from diamines and dicarboxylic acids are designated by two numbers, the first representing the diamine and the second the dicarboxylic acid. Thus nylon 6-10 is formed by the reaction of hexamethylenediamine and sebacic acid. In this demonstration the acid chloride, sebacyl (or Sebacoyl) chloride, is used instead of sebacic acid. The equation is:

Many diamines and diacids (or diacid chlorides) can be reacted to make other condensation products that are described by the generic name "nylon." One such product is an important commercial polyamide, nylon 6-6 (because there are six carbons in both organic compounds), which can be prepared by substituting adipoyl chloride for Sebacoyl chloride in the procedure described here. The equation is:

Experimental Procedure

Time: About 30-45 minutes of class time.

Safety Guidelines

Part I: Synthesis of Nylon 6-6

  1. Wearing gloves (if you do not have gloves be sure to wash your hands frequently), pour about 25-30 mL of the hexameylenediamine solution into a 100-125-mL beaker or crystallizing dish. (You could add one drop of phenolphthalein solution to the beaker prior to the addition of the diamine solution.)
  2. Slowly pour the Sebacoyl chloride solution down the side of the beaker to establish a second layer on top of the diamine solution, taking care to minimize agitation at the interface. (Tilt the beaker and slowly pour the Sebacoyl chloride solution down the inside of the beaker.)
  3. With forceps, grasp the polymer film that forms at the interface of the two solutions and pull it carefully from the center of the beaker.
  4. Wind the polymer read on a stirring rod or a small windlass (a piece of paper towel rolled on itself works fine).
  5. Wash the polymer thoroughly with water or ethanol before handling.

The phenolphthalein dye, which can be added to the lower (aqueous) phase, will enhance the visibility of the liquid interface. The upper phase can also be colored with dyes such as azobenzene, but observation of the polymer film at the interface is somewhat obscured. Some of the dye will be taken up with the polymer, but can be removed by washing with water.

Disposal

  1. Any remaining reactants should be mixed thoroughly to produce nylon. The solid nylon should be washed before being discarded in a solid waste container.
  2. Any remaining liquid should be discarded in a solvent waste container or should be neutralized with either sodium bisulfate (if basic) or sodium carbonate (if acidic) and flushed down the drain with water.


Part II: Solubility of amines

During this part of the experiment, you will determine what makes amines soluble.  Most organic chemicals that contain more than about four carbons, generally are not soluble in water.  Many drugs fit into this category.  Some of these drugs, for example, contain the term "hydrochloride" in their names.  For example, morphine might be listed as "morphine hydrochloride" instead of just "morphine."  To produce a compound in the "hydrochloride" form, you smiply add some hydrochloric acid (HCl) to the compound, and then isolate the resulting compound.

What is the purpose for is addition of HCl to the compound?  There are actually two purposes.  The first is to help make the compound soluble, when it might not dissolve in water. The second consideration is that adding HCl will convert the compound into an ionic compound that does not vaporize.

To do the experiment today, you will take two large test tubes containing:

After the tubes have cooled, make observations and answer the following questions.

After you are finished with this part of the experiment, dispose of the contents from each tube into the liquid waste container and wash your tubes with soap and water.


Materials and Supplies (some items prepared by stockroom):

 


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Copyright © Donald L. Robertson (Modified: 11/19/2012)