In this notes sheet...
Broadly, polymers (also known as plastics) are split into three types:
Each type has a specific set of properties that are dictated by its structure and the bonding within the polymer.
All polymers consist of long macromolecules which contain chains of covalently bonded atoms. The process of turning single monomer molecules into long chains of polymers is known as polymerisation:
Polymerisation is a chemical reaction that generally happens at high temperatures with the help of a catalyst (this is to break the double bond between the carbon atoms).
The schematic above shows the polymerisation of ethylene, C₂H₄ into polyethylene (PE).
Chains are typically between 10³ and 10⁵ monomers long.
The molecular weight of the polymer is the product of the chain length and monomer weight.
Chains vary hugely in weight, and so commercial polymers are classified in terms of mean molecular weight:
The chains can be linear, branched, or cross-linked networks:
This is what dictates their properties.
Monomers are bonded as chains with covalent bonds
Chains are connected at branches and cross-links with Van der Waals bonds
Often, hydrogen bonds form here too
As seen above, these can be regular semi-crystalline structures or amorphous (no ordered structure). The more branches there are to a chain, the less regular the structure.
We say semi-crystalline, as no polymers are truly ordered. All thermoplastics contain crystalline and amorphous regions.
The Van der Waals bonds between chains break when heated at lower temperatures than the covalent bonds holding the monomers as chains. This means they easily melt and can be formed into different shapes over and over again.
Some of the most common examples include:
Easy to mould
Generally used in bottles, packaging, pipes
Same properties as PE, but stiffer
Good UV resistance
Used as fibres, outdoor furniture, rope
Excellent temperature and chemical resistance
Good non-stick properties
Used in lubricants, chemical containers & bottles, non-stick surfaces
Common examples are:
Can be expanded into foam
Used for stationary, packaging, food containers, electrical insulation
Stiff but brittle
Can be expanded into foam
Used in window frames, sheeting, artificial leather, fibres
Used for windows, laminates, surgical instruments
Thermosets are highly crosslinked and amorphous. They are generally formed by mixing two compounds which undergo a chemical reaction.
This reaction is irreversible, forming strong crosslinks between chains. Therefore, they do not soften or melt when heated, and cannot be reformed.
Uses for thermosets are specialist:
Epoxies are used as a matrix for fibres in composites and adhesives
Phenolics are used in motor housing, telephones, and electrical fixtures
Thermosetting polyesters are used for composites, helmets, and automotive bodies
Many double carbon bonds remain intact in elastomers, so there are few crosslinks between chains. This makes them extremely elastic.
The more cross links there are, the more brittle and less elastic the elastomer becomes. Elastomers do not soften or melt. They burn.
Examples of Elastomers
Natural Rubber (polyisoprene)
Harvested from the sap of the Hevea tree
Used in erasers and for latex
Synthetic Rubber (polybutadiene)
Synthesised via polymerisation
Used in car tyres
Used in oil resistant seals
Tensile Properties of Polymers
When a load is applied to a polymer:
Bonds may rotate
Chains may slip & disentangle
Chains may stretch
The slipping and disentanglement of chains is very easy in elastomers and thermoplastics, giving both very low stiffness and fairly low strength.
The crosslinks in thermosets, however, provide more stiffness, but at the cost of reduced toughness.
Tangent & Secant Modulus
Polymers rarely have linear sections on a stress-strain curve. As a result, the modulus cannot easily be measured as the gradient. Instead, there are two methods used:
Polymers & Temperature
The tensile properties of polymers are often hugely dependent on temperature. Take this graph of PMMA (amorphous thermoplastic), for example:
The change in properties occurs because as temperature increases, there is a change in specific volume:
At the glass transition temperature, secondary bonds between chains break apart allowing molecules to rotate (movement of side groups)
In an amorphous solid, there is free space in which the molecules can rotate, leading to a change in physical properties. Throughout the transition region, it is soft and rubbery.
Crystalline structures are incredibly dense, with little free space. The molecules have nowhere to rotate, so properties do not change in the transition region.
Semi-crystalline solids show a slight change.
Amorphous solids show a change in properties at glass transition, crystalline solids do not.