Polymer molecules

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Common polymers

Polyethylene – Cheap plastic bags

Polyethylene.png


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Polypropylene – Labware, dishwasher safe!

Polypropene.png Polypropylene2.png

So what is it about polypropylene that makes products dishwasher safe?

The issue with a dishwasher is that it is a very extreme environment. There is high heat, strong chemicals, and high pressure water. Materials need to be able to cope with all three in order to be deemed 'dishwasher' safe. Often time with hard plastics, you'll see that they get brittle after a few washings and micro-cracks begin to form.

Polypropylene is particularly well suited to deal well with these issues because its melting point is high compated to other plastic materials. (It is 320°F) This allows the container to not crack or warp due to the high temperature of the water. This is the main advantage it has over another popular plastic, polyethylene. It is also water resistant and highly resistant to cracking. The desired properties are achieved through synthesizing the polymer using a catalyst such as Ziegler-Natta or Kaminsky. These offer a level of control over the tacticity of the polymer by controlling the orientation of the monomers. Commercial polypropylene tends to be isotactic with the methyl group on one side allowing the molecules to coil into a helical shape. It's this shape that allows the formation of the crystals that provide the desired properties.


http://askville.amazon.com/SimilarQuestions.do?req=BabyBjorn-Plate-shatterproof-dishwasher-safe http://www.wisegeek.com/what-is-polypropylene.htm http://en.wikipedia.org/wiki/Polypropylene


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Polystyrene – Plastic cups and Styrofoam

Polystyrene.PNG


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Polyisoprene – Natural rubber

Polyisoprene.png

When samples of rubber first arrived in England, it was observed by Joseph Priestley, in 1770, that a piece of the material was extremely good for rubbing out pencil marks on paper, hence the name "rubber".[1]

This can also be made surprisingly well with an organic reaction using the Ziegler-Natta catalyst.

Ziegler.png

Polybutadiene – Synthetic rubber

Polybutadiene.PNG

Polybutadiene was one of the first synthetic elastomers (rubbers) every made. It's glass transition temperature is much lower than that of other polymers, making it an ideal material for winter tires.


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Polyethylene oxide

Water soluble, used in paper making process. A commonly used reagent in biological studies is PEG, a low molecular weight polyethylene oxide, used in osmotic pressure experiments and as a means of concentrating virus particles.

PEG.png


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Polydimethylsiloxanes

Silicones, PDMS~ used in soft lithography in making microfluidic devices, also part of Silly Putty Polydimethylsiloxanes.png


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Polyesters

Polyester is a category of polymers that involves the ester functional group in their main chain (see below). Polyesters include naturally-occurring chemicals, such as in the cutin of plant cuticles, as well as synthetics such as polycarbonate and polybutyrate.

Ester group.gif

Polyesters can be manufactured in many forms such as sheets and three-dimensional shapes. Polyesters as thermoplastics are able to change shape as you apply heat to it. Even though they are combustible at high temperatures, polyesters tend to shrink away from flames and self-extinguish upon ignition.

Polyesters are also used to produce bottles, synthetic fibers, canoes, holograms, filters, films, dielectric film for capacitors, film insulation for wire, insulating tapes and toners. Polyester fibers have high Bulk modulus as well as low water absorption and minimal shrinkage in comparison with other industrial fibers.

Synthesis of polyesters is generally achieved by a polycondensation reaction. Most general equation for the reaction of a diol with a diacid is in production of polyesters is:

(n+1) R(OH)2 + n R´(COOH)2 ---> HO[ROOCR´COO]nROH + 2n H2O

Some examples of polyesters are shown below:

Polyester resin.jpeg

Polyester Resin

Polyester fabric.jpeg

Polyester Fabric

Polyester fibers.jpeg

Polyester Fibers

Recently, a new extremely water-repellant polyester fabric has been developed. The polyester fibers are coated in silicone filaments, which are extremely hydrophobic [2].

Drop.jpg


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Polypeptides

Polypeptides are defined to be chains of amino acids. Proteins are made out of one or more polypeptide chains. In order to form a polypeptide chain, amino acids are connected together using peptide bonds. For example, we can see a tripeptide molecule in the image below.

Tripeptide.jpg [Reference: http://users.rcn.com/jkimball.ma.ultranet/BiologyPages/P/Polypeptides.html]

Proteins exhibit four levels of structure. Primary structure is considered to be the chain of amino acids that create a polypeptide chain. Secondary structure is the ordered arrangement of amino acids in localized regions of a polypeptide molecule. Hydrogen bonding plays important role in stabilizing these patterns. Tertiary structure of a polypeptide is a three-dimensional arrangement of the atoms within one single polypeptide chain. Finally, quaternary structure is used to describe proteins made of multiple polypeptides. Hydrophobic interaction is the primary force responsible for stabilizing subunits (polypeptides) in quaternary structure.

Polypeptide have to be terminated in a specific manner. One end has to be amino-terminal (ends in nitrogen group), whereas the other has to be carboxyl-terminal (ends in carbon group). An example is shown below.

Peptide.jpg [Reference: http://users.rcn.com/jkimball.ma.ultranet/BiologyPages/P/Polypeptides.html]



Polyamide

A polyamide is a polymer containing monomers of amides joined by peptide bonds. They can occur both naturally, examples being proteins, such as wool and silk, and can be made artificially, examples being nylons, aramids, and sodium poly(aspartate). The amide link is produced from the condensation reaction of an amino group and a carboxylic acid or acid chloride group. A small molecule, usually water, or hydrogen chloride, is eliminated. The amino group and the carboxylic acid group can be on the same monomer, or the polymer can be constituted of two different bifunctional monomers, one with two amino groups, the other with two carboxylic acid or acid chloride groups. Amino acids can be taken as examples of single monomer (if the difference between R groups is ignored) reacting with identical molecules to form a polyamide:

Picture 21.png

Aramid is made from two different monomers which continuously alternate to form the polymer and is an aromatic polyamide:

Picture 22.png

Proteins as polymers – Hemoglobin as an example

As seen above, Nature came up with the idea of polymers long before we did, and since they are so common in biology, many of them are just termed "biopolymers". Common examples, which are widely studied, include actin, fibrin, microtubules, collagen and various intermediate filaments such as vimentin. While proteins often self-assemble into networks of long filaments in normal physiological conditions, here is one very interesting and different example:

Hemoglobin is a protein essential to our life, as it is what allows us to take in oxygen from the air, transport it safely in our bloodstream, pass it on to cells in our body and use it for daily functions. More precisely, hemoglobin is found in our red blood cells, which are normally disc-like cells, without a nucleus. Red blood cells transport the oxygen from the air that we breathe in our blood; oxygen being a highly-reactive species, it cannot just remain in a dissolved gaseous state in our blood, which is why red blood cells specialize in its transport.

The structure of hemoglobin is important in how it interacts with oxygen. Hemoglobin contains an iron ion that binds oxygen molecules to it and keeps them in a stable state during transport. But interestingly, the presence or absence of oxygen has a strong effect on the structure and ability to polymerize of hemoglobin; in normal conditions, hemoglobin molecules are present in large numbers in each red blood cell, but cannot polymerize. However, when a minor mutation is present, things can change dramatically: this is the case in sickle cell anemia.

In sickle cell anemia, a mutation in the hemoglobin causes it to polymerize into long and stiff rods when low levels of oxygen are present - which can often be the case in the veins. When hemoglobin polymerizes, it pushes the membranes of the red blood cells outwards and causes them to lose their characteristic disc-like shape. This, in turn, can have some drastic effects on the ability of red blood cells to deform and pass through thin capillaries at the extreme points of our circulation pathway.

The biology and genetics of hemoglobin and sickle cell anemia are fascinating, especially when seen in the light of evolution. If you're interested, you can always read the wikipedia (http://en.wikipedia.org) page on hemoglobin and sickle cell anemia, or just go and talk to Maha here at SEAS (http://www.seas.harvard.edu/softmat/index.html).


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Isomerism

Isomers are chemical compounds with the same chemical formula, but different structural formulas. Specifically, isomers have the same number of each element, but they are topologically or geometrically distinct.

For a topological example, consider the following three molecules I,II,III:

Structural isomers.png

Each of these are isomers, however we can see that they are topologically distinct, in the sense that neither can be deformed into the other (without breaking bonds). For example, I has an O atom connected to a C atom which is connected to 2 H atoms, II has an O atom connected to a C atom that is connected to 2 other C atoms, and III has an O atom connected to 2 C atoms. Each of these properties is distinct to that isomer.

When two compounds are topologically identical but geometrically distinct, they are called stereoisomers. As an example of what this means, consider the following molecules:

375px-Cis-2-butene.svg.png
375px-Trans-2-butene.svg.png

The top and bottom molecules can clearly be deformed into each other by simply rotating the C=C double bond. Thus we would call these stereoisomers, because they are spatially different, even though they have the same connectivity. Because double-bonds can be considered rigid, these are chemically distinct molecules. Stereoisomers can have radically different chemical properties, largely due to the fact that spatial arrangement can change the dipole moment of the molecule significantly. For example, he two stereoisomers of 2-butenedioic acid are so different that they are given different names: maleic acid fumaric acid.

Isomerism is important in polymers. For example, if the monomers in a polymer are not symmetric, then head-to-tail is different than tail to head.

  • Atatic polymers
Witten
  • Syndiotatic polymers
Witten
  • Isotatic polymers
Witten
  • Copolymers
    • Random
    • Diblock and triblock coploymers
      • Coplymers of ethylene and propylene are disordered enough to remain liquid at lower temperatures than either homopolymer.
      • Diblock and triblock copolymers can (partially) self-associate



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Types of Polymerization

(Witten p.45-46)

-Addition polymerization: a catalyst initiates polymerization in a solution of monomers; each chain has a single active end that reacts only with monomers --> molecular uniformity (example: polypeptides and polysaccharides)

Addpol.jpg

Free radical polymerization is the most common type of addition polymerization. A free radical is a molecule with an unpaired electron. Free radicals are often created by the division of a molecule (initiator) into two fragments along a single bond. The unpaired electron makes the free radical highly reactive. The free radical will look for an additional electron to form a pair. This is achieved by breaking the bond on another molecule.


There are three more types of initiating species for addition polymerization besides free radicals. They are cations, anions, and coordination (stereospecific) catalysts. Some monomers can use two or more of the initiation processes but others can use only one process.


Addition polymerization process takes place in three distinct steps: 1. chain initiation, usually by means of an initiator which starts the chemical process. 2. chain propagation, in which the reactive end-groups of a polymer chain react in each propagation step with a new monomer molecule transferring the reactive group to that last unit. 3. chain termination, which occurs either by combination or disproportionation. Termination, in radical polymerisation, is when the free radicals combine and is the end of the polymerisation process.


-Condensation polymerization: many chains may react with one another (example: polyamide nylon)

During condensation polymerization, a small molecule such as water will be condensed out by the chemical reaction. One major drawback of utilizing condensation polymerization is the tendency for the reaction to cease before the chain grows to a sufficient length. This is due to the decreased mobility of the chains and reactant chemical species as polymerization progresses. This result in short chains.

Condpol.jpg


-Living polymerization: various chains are free to exchange monomers amongst themselves--> broad distribution of chain lengths (worm-like micelles)

Living polymerization is similar to addition polymerization without the chain termination. The process continues until the monomer supply has been exhausted. When this happens, the free radicals become less active due to interactions with solvent molecules. If more monomers are added to the solution, the polymerization will resume.


The result is that the polymer chains grow at a more constant rate than seen in traditional chain polymerization and their lengths remain very similar


Uniform molecular weights are characteristic of living polymerization. Because the supply of monomers is controlled, the chain length can be manipulated to serve the needs of a specific application.



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Polymer dimensionality and structure

  • Distinctiveness – Length & flexibility?
    • Polymers are ordered and inflexible in 1D
    • Polymers are random and flexible in 2 and 3 D
    • Polymers are tenuous in 2 and 3 D
    • Polymers “self-avoid” in 2 and 3 D
  • Some are constrained – DNA and RNA
  • Scaling with molecular weight
  • Scaling with structure – more difficult
  • Scaling of diffusion and flow



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Kinks and rings in confined polymer structures

Some polymers naturally tend to form filamentous structures rather than blobs. Many of the biological polymers (or biopolymers) follow that behavior: actin, fibrin, collagen, tubulin, DNA, RNA and others. Carbon nanotubes can also form very strong linear structures, one of their most promising and applicable properties.

Like many filaments, those just mentioned have a finite bending stiffness, which means that they have a characteristic length-scale over which they will appear rigid or straight: the persistence length. Segments shorter than the persistence length will behave like rigid beams, while longer segments will appear more floppy. In the limit of very long segments, the filament can fold on itself and behave more like a blob.

An interesting question arises when these (bio)polymers are forced to grow in a confined space, smaller than their persistence length. This question comes naturally for biological systems like mammalian cells, where the cytoskeleton is comprised of polymeric filaments whose persistence length is on the order of the cell size (e.g. actin) or much larger than the cell (e.g. tubulin). Another example of this is given in an interesting applied math paper by Cohen and Mahadevan (PNAS 2002)[3], where they talk about growing carbon nanotubes confined in air bubbles. A common phenomenon observed with cytoskeletal proteins and nanotubes, is that they tend to form rings or kinks when growing in a confined space; even more interesting is the fact that the angles of the kinks they form typically take discrete values rather than a broad continuous spectrum.

A very simple explanation for a discrete kink-angle lies in the fact that these filamentous structures are composed of multiple thin single chains of monomers and that the interaction between these monomers causes them to want to be spaced out (laterally and longitudinally) at very specific length-scales. The longitudinal spacing is obviously the same or close to the size of the monomer and the lateral spacing between single chains is determined by the monomer size and the strength of the attraction between chains. It is clear that when we introduce bending into these multi-chain filaments, some of the chains will have a greater curvature than others and this will tend to create an offset in the monomer positions and how they fit together. Because there is an energy associated with creating local curvature in a filament, it is better to create one point of high curvature than to create many points of low curvature. This will follow a similar behavior to that described by the Frenkel-Kontorova model, which provides a microscopic explanation for the formation of certain dislocations in solids.

Polymers kinks.jpg

So because these polymers have strong inter-chain interactions and are formed of discrete monomer units, they tend to prefer a rigid rod state locally and will sharply kink to maintain some level of straightness. The paper by Cohen and Mahadevan provides some additional examples of kinks and rings in filamentous structures.


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Renormalization and scaling - The random walk polymer

Probability that the end-to-end vector has some, r , for n segments: <math>p\left( n,r \right)</math> is a probability per volume
The chain must have some length <math>\int{p\left( n,r \right)}d^{3}r=1</math>

If <math>p\left( n,r \right)</math> be known, what be known about <math>p\left( n+1,r \right)</math>?

Assume segment is flexible, but no self-avoidance. Probability depends on magnitude only. <math>p_{0}\left( r_{1} \right)</math>
Probability is the product <math>p\left( n,\vec{r}-\vec{r}_{1} \right)p_{0}\left( \vec{r}_{1} \right)=p\left( n,\vec{r}-\vec{r}_{1} \right)p_{0}\left( r_{1} \right)</math>
For all possible <math>\vec{r}_{1}</math> that have <math>\vec{r}_{{}}-\vec{r}_{1}</math> is <math>p\left( n+1,r \right)=\int{p_{0}\left( r_{1} \right)}p\left( n,\vec{r}-\vec{r}_{1} \right)d^{3}r_{1}</math>

Consider the case of large 'n'.

This difference should be small: <math>p\left( n+1,r \right)-p\left( n,r \right)=\int{p_{0}\left( r_{1} \right)}\left[ p\left( n,\vec{r}-\vec{r}_{1} \right)-p\left( n,r \right) \right]d^{3}r_{1}</math>
A Taylor expansion around <math>\vec{r}_{1}</math> is: <math>p\left( n,\vec{r}-\vec{r}_{1} \right)=p\left( n,r \right)-\vec{r}_{1}\cdot \nabla _{r}p\left( n,r \right)+\frac{1}{6}r_{1}^{2}\nabla _{r}^{2}p\left( n,r \right)+\cdots </math>
If <math>\Delta n=1</math> the RHS remains the same but the LHS is: <math>\underset{n\to \infty }{\mathop{\lim }}\,\frac{p\left( n+\Delta n,r \right)-p\left( n,r \right)}{\Delta n}\to \frac{dp}{dn}</math>
And we have: <math>\frac{dp}{dn}=-\nabla _{r}p\left( n,r \right)\cdot \int{\vec{r}_{1}p_{0}\left( r_{1} \right)d^{3}r_{1}}+\frac{1}{6}\nabla _{r}^{2}p\left( n,r \right)\int{r_{1}^{2}p_{0}\left( r_{1} \right)d^{3}r_{1}}+\cdots </math>
All odd integrals are zero, therefore: <math>\frac{dp}{dn}\cong \frac{1}{6}\nabla _{r}^{2}p\left( n,r \right)\int{r_{1}^{2}p_{0}\left( r_{1} \right)d^{3}r_{1}}+constant\cdot \nabla _{r}^{4}p+\cdots </math>
The integral is <math>\left\langle r^{2} \right\rangle _{1}</math>, therefore: <math>\frac{dp}{dn}\cong \frac{1}{6}\left\langle r^{2} \right\rangle _{1}\nabla _{r}^{2}p\left( n,r \right)+constant\cdot \nabla _{r}^{4}p+\cdots </math>


Now the first scaling idea is introduced.

The “shape” of the distribution should be independent of n.

<math>\begin{align}

 & p\left( n,r \right)=\eta p\left( \lambda n,\mu r \right) \\ 
& p\left( n,r \right)=\tilde{p}\left( \tilde{n},\tilde{r} \right) \\ 

\end{align}</math>

Where: <math>\tilde{p}=\eta p,\text{ }\tilde{n}=\lambda n\text{ and }\tilde{r}=\mu r</math>
Hence: <math>\begin{align}
 & \frac{d}{dn}=\lambda \frac{d}{d\tilde{n}} \\ 
& \nabla _{r}^{2}=\mu ^{2}\nabla _{{\tilde{r}}}^{2}\text{  and  }\nabla _{r}^{4}=\mu ^{4}\nabla _{{\tilde{r}}}^{4} \\ 

\end{align}</math>

Or: <math>\frac{d\tilde{p}}{d\tilde{n}}\cong \frac{1}{6}\frac{\mu ^{2}}{\lambda }\left\langle r^{2} \right\rangle _{1}\nabla _{{\tilde{r}}}^{2}\tilde{p}\left( \tilde{n},\tilde{r} \right)+\text{C}\frac{\mu ^{4}}{\lambda }\nabla _{{\tilde{r}}}^{4}\tilde{p}+\cdots </math>

Now the second scaling idea is introduced.

If n can be arbitrarily large: <math>\mu =\lambda ^{{1}/{2}\;}</math>
Consider the normalization:

<math>\begin{align}

 & \int{p\left( n,r \right)}d^{3}r=1 \\ 
& \int{\eta p\left( \lambda n,\mu r \right)}d^{3}r=1 \\ 
& \frac{\eta }{\mu ^{3}}\int{p\left( \lambda n,\mu r \right)}d^{3}\left( \mu r \right)=1 \\ 
& \therefore \text{ }\frac{\eta }{\mu ^{3}}=1 \\ 

\end{align}</math>

Or:

<math>\eta =\lambda ^{{3}/{2}\;}</math>

Since <math>\lambda </math> is arbitrary, it can be set to <math>{1}/{n}\;</math> and: <math>\tilde{p}=n^{{-3}/{2}\;}p,\text{ }\tilde{n}=1\text{ and }\tilde{r}=n^{{-1}/{2}\;}r</math>
The distribution <math>p\left( n,r \right)=n^{-{3}/{2}\;}p\left( \tilde{n},\tilde{r} \right)_{\tilde{n}=1,\tilde{r}=rn^{-{1}/{2}\;}}</math>
is now: <math>p\left( n,r \right)=n^{-{3}/{2}\;}f\left( rn^{-{1}/{2}\;} \right)</math>
The moments of the distribution are: <math>\begin{align}
 & \left\langle r^{p} \right\rangle _{n}=\int{r^{p}\cdot n^{-{3}/{2}\;}}f\left( rn^{-{1}/{2}\;} \right)d^{3}r \\ 
& \text{        }=n^{{p}/{2}\;}n^{-{3}/{2}\;}n^{{3}/{2}\;}\int{\left( rn^{-{1}/{2}\;} \right)^{p}\cdot }f\left( rn^{-{1}/{2}\;} \right)d^{3}\left( rn^{-{1}/{2}\;} \right) \\ 
& \text{        }=n^{{p}/{2}\;}\int{\left( {\hat{r}} \right)^{p}\cdot }f\left( {\hat{r}} \right)d^{3}\hat{r} \\ 

\end{align}</math>

Since the integral is a constant:

<math>\left[ \left\langle r^{p} \right\rangle _{n} \right]^{{1}/{p}\;}=K_{p}n^{{1}/{2}\;}</math>

Now the solution to <math>\frac{dp}{dn}=\frac{1}{6}\left\langle r^{2} \right\rangle _{1}\nabla _{{}}^{2}p\left( n,r \right)</math>
is: <math>p\left( n,r \right)=\left[ {2\pi n\left\langle r^{2} \right\rangle _{1}}/{3}\; \right]^{-{3}/{2}\;}\exp \left[ -\frac{3r^{2}}{2n\left\langle r^{2} \right\rangle _{1}} \right]</math>



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What is the energy to stretch a polymer from random packing to fully extended?

The only component is entropy, hence _{initial}^{final}=\frac{3}{2}kT\frac{r^{2}}{\left\langle r^{2} \right\rangle }</math>




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How dense is the polymer?

Remember - No liquid has been mentioned!!

What is the "size" of a polymer?

Take any moment of the end-to-end distance: <math>\left[ \left\langle r^{p} \right\rangle _{n} \right]^{{1}/{p}\;}=K_{p}n^{{1}/{2}\;}\sim n^{{1}/{2}\;}</math>

What's the number density? <math>\bar{\rho }\sim \frac{n}{\left\langle r \right\rangle _{n}^{3}}\sim \frac{n}{n^{{3}/{2}\;}}\sim n^{-{1}/{2}\;}</math>

The greater the molecular weight, the more tenuous the polymer.





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How does density vary within the polymer chain?

Random polymer chain.png
Probability of each segment at r: <math>\left\langle \rho \left( r \right) \right\rangle _{0}=2\int\limits_{0}^{\infty }{i^{-{3}/{2}\;}}f\left( ri^{-{1}/{2}\;} \right)di</math>
Define a scaled variable: <math>\tilde{i}=i^{{1}/{2}\;}r^{-1}</math> <math>\left\langle \rho \left( r \right) \right\rangle _{0}=2r^{2}r^{-3}\int\limits_{0}^{\infty }{\tilde{i}^{-{3}/{2}\;}}f\left( \tilde{i}^{-1} \right)d\tilde{i}</math>
The integral is the local density: <math>\left\langle \rho \left( r \right) \right\rangle _{0}={\text{constant}}/{r}\;</math>
The average density is: <math>\left\langle M\left( r \right) \right\rangle =\int\limits_{{r}'<r}{\left\langle \rho \left( {{r}'} \right) \right\rangle _{0}}d^{3}{r}'=\int\limits_{{r}'<r}{{r}'^{2}\left\langle \rho \left( {{r}'} \right) \right\rangle _{0}}d{r}'=\left( \text{constant} \right)r^{2}</math>




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Therefore the random walk polymer has a fractal dimension of D = 2.

Self-avoidance - Flory theory

Purely locally or global models do not change the scaling of density.

Assume that self-avoidance occurs on all length scales.

On each and every length scale the polymer is expanded by a factor b.

Replace: <math>p\left( n,r \right)=n^{-{3}/{2}\;}f\left( rn^{-{1}/{2}\;} \right)</math> with: <math>p\left( n,r \right)=n^{-\nu d}f\left( rn^{-\nu } \right)</math>

This preserves the normalization and the end-to-end distance as <math>n^{-\nu }</math>

And the previous results are similar: <math>\left\langle \rho \left( r \right) \right\rangle _{0}=\left( \text{constant} \right)r^{{1}/{\nu -3}\;}</math>

and <math>\left\langle M\left( r \right) \right\rangle =\left( \text{constant} \right)r^{{1}/{v}\;}</math>


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Universal Ratios

In the previous discussion, we have seen that a polymer has a single asymptotic probability distribution function p(n,r) for any random walk. This is true for all polymers, irregardless of the specific details of how the random walk was created. Furthermore, we have explored the fact that all self-repelling polymers exhibit common behavior, independent of the specifics of the repulsion. Since the aforementioned characteristics are seen for any polymer, we call them universal. Still, even in these universal functions, there is still room for choosing an arbitrary scaling coefficients e.g. <math>\mu</math> or <math>\lambda</math>. Therefore, some quantities are not going to be dependent only on p(n,r). But quantity like <math><r^4>/<r^2>^2</math> has both <math><r^4></math> and <math><r^2></math> scaling as <math>\mu^4</math> which cancels out so we can conclude <math><r^4>/<r^2>^2</math> is only dependent on prabability distribution function, and not on any scaling properties. These kinds of ratios independent of scaling are referred to as universal ratios.

[For more information, see Witten p. 72-73]


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Estimating the fractal dimension D

Consider the work to expand a polymer from the “ideal” state.

<math>U\sim kT\frac{r^{2}}{\left\langle r^{2} \right\rangle }\sim kT\frac{r^{2}}{n}</math>

Think of self-avoiding polymers as ones with slightly repulsive interactions.
The number of (non-local) contacts n times the probability that a monomer has a contact: <math>V\simeq n\left( {\nu \cdot n}/{r^{3}}\; \right)U^{contact}\sim U^{contact}\frac{n^{2}}{r^{3}}</math>
Equating the energies and re-arranging:

<math>\begin{align}

 & kT\frac{r^{2}}{n}\sim U^{contact}\frac{n^{2}}{r^{3}} \\ 
& n\sim r^{{5}/{3}\;} \\ 

\end{align}</math>

Therefore the self-avoiding polymer has a fractal dimension of D = 5/3


What is a fractal dimension, anyway? This is the wikipedia page for it (since we all know that that is a fantastically reliable resource): Fractal Dimension

For a biological reference, I found this article on the fractal analysis of lysozyme interesting; I had never heard of fractals in bio polymers, so this was a neat one to read through. Here is the reference, since I'm not sure how GNU this is (you can snag it through the Harvard library system, though):

Rigid structure of fractal aggregates of lysozyme G. C. Fadda et al 2000 Europhys. Lett. 52 712-718

Abstract: The aggregation of hen egg-white lysozyme upon salt addition was studied by quasi-elastic light scattering. Our results agree with the fractal structure of the aggregates already reported in the literature. However, we also demonstrate that these aggregates are rigid, since they do not display any fluctuation of internal concentration. Such a rigid internal structure is a key point to reconcile the fractal structure of the aggregates and their colloid-like ordering. Furthermore, this result has to be considered for understanding crystal nucleation.

--BPappas 22:09, 25 October 2008 (UTC)



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Polymer degradation

Polymer degradation is a change in the properties—tensile strength, colour, shape, etc.—of a polymer or polymer-based product under the influence of one or more environmental factors, such as heat, light or chemicals. It is often due to the hydrolysis of the bonds connecting the polymer chain, which in turn leads to a decrease in the molecular mass of the polymer. These changes may be undesirable, such as changes during use, or desirable, as in biodegradation or deliberately lowering the molecular mass of a polymer. Such changes occur primarily because of the effect of these factors on the chemical composition of the polymer. Ozone cracking and UV degradation are specific failure modes for certain polymers.

Ozone cracks

The degradation of polymers to form smaller molecules may proceed by random scission or specific scission. The degradation of polyethylene occurs by random scission—a random breakage of the linkages (bonds) that hold the atoms of the polymer together. When heated above 450°C it degrades to form a mixture of hydrocarbons. Other polymers—like polyalphamethylstyrene—undergo specific chain scission with breakage occurring only at the ends. They literally unzip or depolymerize to become the constituent monomer.

However, the degradation process can be useful from the viewpoints of understanding the structure of a polymer or recycling/reusing the polymer waste to prevent or reduce environmental pollution. Polylactic acid and polyglycolic acid, for example, are two polymers that are useful for their ability to degrade under aqueous conditions. A copolymer of these polymers is used for biomedical applications, such as hydrolysable stitches that degrade over time after they are applied to a wound. These materials can also be used for plastics that will degrade over time after they are used and will therefore not remain as litter.


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Polyelectrolytes

Polyelectrolytes are polymers which have electrolyte units. When polyelectrolytes are put into an aqueous solution they become charged. A polyelectrolyte can be simply thought of as a charged chain, which, in solution, conduct electricity, are often viscous, and have complex but interesting physics associated with their structure and conformation. They play major roles in biochemistry; perhaps the most famous electrolyte in the world is DNA. A normal, uncharged linear polymer in solution takes on a random conformation that is close to an approximation given by a self-avoiding three-dimensional random walk theory. This is not true for polyelectrolytes. Because of their charge, the electrolytic units on a polyelectrolyte repel each other, causing the chain to form expand into a rigid-rod conformation. In the presence of multivalent (2+, 3+, etc) salt, however, the charges on the polyelectrolytes get screened, and at a critical point (when the net charge on the polyelectrolyte equals the net charge of the salt), the polyelectrolyte becomes essentially neutral. At this point, the chain is free to conform in a similar way to a neutral chain. After this point, however, the positive ions 'attached' to the polyelectrolyte dominate, and there becomes an effectively positive charge on the system, causing the chain to repel itself again and become rigid and elongated. However, how polyelectrolytes being packaged into a small space in the presence of multi-valent salts is a different question, which I recently explored.

Understanding how polymers behave when constrained into tight spaces is a problem whose relevance stretches well beyond the field of polymer physics. Besides the several industrial applications in which this phenomenon plays a crucial role: colloidal stabilization, filtration, drug-delivery and flow injection; the confinement of bio-polymers is also a ubiquitous phenomenon in nature. Numerous biological processes rely on confinement to perform a diverse set of fundamental tasks, including the release of DNA pre-packaged by molecular-motors inside virus capsids, bacterial gene swapping, and the re-folding of proteins inside double-barreled Chaperonins. The free energy barrier required to insert a flexible neutral chain with radius of gyration RG into a spherical cavity of radius R (< R_G) can be obtained by a simple scaling argument that accounts for the chain loss of entropy. The expression you get is correct in the dilute limit, but becomes inaccurate at large densities, where excluded volume interactions between the monomers dominate over the chain entropy loss, thus causing the free energy penalty to increase at a much steeper rate. Although the physics concerning the confinement of neutral flexible polymers is well understood, such a claim cannot be made for charged chains. While the bulk properties of a charged chain in the presence of monovalent salt can be properly described within the framework of the Poisson-Boltzmann theory--the interaction between the charged monomers can be encoded into an effective chain bending rigidity, kappa, whose value decreases as the electrostatic interactions are screened by addition of salt in solution--the phenomenology is much more complex when the chain is either confined within a small region or when multivalent salt is present in solution. For instance, it is known that the size of a charged chain in the presence of multivalent salt presents a non-monotonic behavior as a function of salt concentration ro, resulting in a conformational collapse when multivalent counterions neutralize the bare charge of the chain, and a subsequent re-expansion, due to the inversion of the chain net charge, at larger values of ro. In a project I recently finished I ran molecular dynamics simulations to account for the role of salt valency and concentration on the packaging of a charged chain into a small, spherical cavity. The results can be summed up as follows: Our goal was not to provide a quantitative estimate for the DNA packaging energy, but to sort out the relevant energy scales dominating the process, and to elucidate the physical mechanisms behind the break-down of the Poisson-Boltzmann treatment of the salt. What we find can be summarized in two points. (1) In the presence of multi-valent counterions, it is easier to confine a charged chainthan a neutral flexible chain, and there exists a threshold salt concentration above which the addition of extra salt does not affect the packaging energy. (2) In the presence of monovalent counterions, the insertion energy is completely independent of salt concentration.

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Glass Transition

For each polymer, there exists a glass transition temperature below which the polymer becomes rigid and brittle. A glass transition is different from melting because the polymers do not solidify into a regular structure but rather harden into an amorphous polymer. Polymers that may move around each other generally have lower glass transition temperatures.

The temperature at which a polymer undergoes a glass transition depends on several factors about its structure: flexibility of the polymer backbone and pendant groups on the molecules. Backbone flexibility is by far the more important of the two factors. A flexible backbone permits the polymers to bend and twist to move around each other more easily. Polydimethylsiloxane is a silicon polymer that is particularly flexible. As a result, its glass transition temperature is -127 degrees C. Wow, that is a very low temperature! It is primarily used in shampoos as a thickener. In contrast, poly(phenylene sulfone) is a very stiff polymer since it has a carbon ring in it. It's transition temperature of 500 degrees C. The presence of pendant groups on an end of the polymer can raise the transition temperature because they can catch on nearby polymers, lowering an individual polymer's mobility. Sometimes pendant groups, including adamantane, can also make a polymer heavier, making it more difficult for it to move. Larger pendant groups make polymers more bulky preventing polymers from being closely packed together. Such groups can lower the glass transition temperature. For example, see the figure below:

Polymers.gif

As addition pendant groups are added, the glass transition temperature decreases.

More information may be found at http://pslc.ws/macrog/tg.htm#high