Plastic Sulfur — Making and Watching an Unstable Allotrope

How Can a Brittle Yellow Solid Become Rubbery?

Imagine showing a student a sample of sulfur.

It is yellow, solid and brittle. It looks thoroughly unpromising as a material for anything that needs to bend.

Now imagine transforming it into a dark, rubbery strand that can briefly stretch.

Then leave it alone.

Over time, that flexibility disappears and the material becomes brittle again.

The element has remained sulfur throughout. What has changed is its structure.

Plastic sulfur is a particularly striking demonstration because the story continues after the heating has finished. The freshly prepared material is only a temporary state, and watching it change provides an opportunity to explore allotropy, polymers, crystallisation and stability.

It also poses a useful scientific question:

If a material is solid, does that mean it has finished changing?

The Same Element Can Have Different Structures

Different structural forms of the same element are called allotropes.

Carbon provides the familiar examples: diamond and graphite contain carbon atoms, yet their structures give them very different properties.

Sulfur offers another route into this idea.

Ordinary yellow sulfur consists mainly of molecules containing eight sulfur atoms arranged in puckered rings. We write the molecular formula using ordinary text characters:

S8

These rings are often described as crown-shaped. They are not flat octagons.

In crystalline sulfur, the molecules pack into an ordered arrangement. Different crystal forms can contain the same S8 molecules packed differently.

That gives students two levels of structure to consider:

• How are the atoms joined within each molecule?

• How are those molecules arranged throughout the solid?

Plastic sulfur introduces a further possibility: long chains of sulfur atoms, rather than a material dominated by small rings.

Before the Demonstration: A Proper Laboratory Setting

This is a demonstration for a competent adult in a suitably equipped laboratory with a functioning fume cupboard. It is unsuitable as a kitchen or unsupervised home experiment.

The important hazards include hot, sticky molten sulfur, hot apparatus, splashing during transfer and ignition. Burning sulfur produces sulfur dioxide, a harmful respiratory irritant.

A written risk assessment and an established educational procedure should determine the apparatus, scale, heating method, protective equipment and emergency arrangements. University demonstration guidance specifically identifies extraction, temperature control and careful handling as important.

The description below explains what students observe and why. It does not replace a practical protocol.

For my teaching, a close-up camera would be particularly useful here. Students could watch the colour and movement of the liquid on screen while remaining well clear of the apparatus.

First It Melts — Then Something More Interesting Happens

The demonstrator begins with yellow sulfur and heats it under controlled conditions.

Initially, the solid melts to form a relatively mobile yellow or amber liquid.

At this stage, students may reasonably predict that further heating will make it flow more easily. That is what happens with many familiar liquids.

Sulfur challenges that prediction.

Above roughly 159 degrees C, ring-opening polymerisation becomes important. Sulfur atoms begin forming long chains, and the liquid becomes much more viscous. Its colour also darkens.

In relatively pure sulfur, viscosity rises dramatically and reaches a maximum around 187 degrees C. At still higher temperatures, it decreases again as the balance of chain formation and breaking changes. The whole story is more interesting than “hotter means thicker”.

What does “viscous” mean?

Viscosity describes a fluid’s resistance to flow.

Water has a low viscosity. Honey has a much higher viscosity.

Students should distinguish this from density:

A liquid can resist flowing without being especially dense.

The useful observation is how readily the liquid moves under comparable conditions. Appearance alone cannot provide a precise viscosity measurement.

From Small Rings to Long Chains

A simple molecular model helps explain the change.

Imagine a tray containing many small, closed loops of string. The loops can move around one another relatively easily.

Now imagine a tray containing long lengths of tangled string.

Movement becomes more restricted because the long strands interfere with one another.

The analogy is imperfect, but it gives students a way to picture why chain length and entanglement matter.

In sulfur, heating allows some S8 rings to open. The resulting reactive chain ends can participate in further chain growth.

The crucial point is that melting and polymerisation are different processes:

• Melting changes the physical state.

• Polymerisation changes the molecular structures present.

Simply melting sulfur does not guarantee the same result as preparing a melt containing a substantial proportion of long sulfur chains.

Rapid Cooling Captures a Temporary Structure

In the established demonstration, suitably heated sulfur is carefully transferred into cold water.

Rapid cooling is called quenching.

It restricts the opportunity for the hot material to reorganise immediately into ordinary crystalline sulfur. A freshly prepared sample can form dark, flexible strands with a rubber-like character. Educational demonstrations describe the resulting material as capable of bending and stretching.

This material is traditionally called plastic sulfur.

Here, “plastic” refers to its capacity to be shaped or deformed. It does not mean that it has become a conventional carbon-based plastic such as polythene.

The sample is still elemental sulfur.

There is another useful qualification: plastic sulfur is not necessarily a pure collection of identical long chains. Quenched sulfur can contain both polymeric sulfur and S8 rings in an amorphous material.

Amorphous means that it lacks the long-range ordered structure of a crystal. It does not mean that its atoms have no organisation at all.

Why Can It Stretch?

Long molecular chains can change their arrangement when a material is pulled.

Some chains become more aligned, and parts of the tangled structure straighten. This helps explain why freshly prepared plastic sulfur behaves so differently from a brittle sulfur crystal.

However, its behaviour should not be oversold.

A particular sample may stretch, deform permanently or snap, depending on its preparation, temperature and age. It should not be expected to behave like a manufactured elastic band.

That variation is part of the teaching opportunity.

Rather than asking only, “Did it work?”, I would ask:

“How flexible was it, when did we test it, and what evidence have we recorded?”

Those questions turn a memorable demonstration into an investigation.

The Experiment Continues After the Apparatus Is Put Away

Plastic sulfur gradually loses its flexibility.

Its molecular structures reorganise, and crystalline sulfur develops. At ordinary room conditions, orthorhombic sulfur built from S8 rings is the stable crystalline form towards which other modifications tend to change.

The material may become harder, more opaque and more yellow as it ages.

The timing varies. Some changes may be apparent within hours; observations over the following day or two can reveal more. Preparation history, storage temperature and sample dimensions all matter.

This is an example of metastability: a material can persist temporarily in a state that is not its most stable state under the surrounding conditions.

“Unstable” here does not mean explosive. It means that the structure changes towards a more stable arrangement over time.

A Follow-Up Investigation: How Quickly Does Flexibility Disappear?

Once the demonstrator has confirmed that the material is cool and suitable for examination under the risk assessment, students can record its changing properties.

I would prepare several comparable pieces, using a fresh piece for each mechanical test. Repeatedly stretching the same strand would change the sample and make later comparisons less meaningful.

A useful observation schedule might be:

Observation time	What to record
As soon as safely cooled	Colour, appearance, flexibility and initial length
After 15 minutes	Any visible change; response to the agreed gentle test
After 1 hour	Comparison with the initial photograph and observations
After several hours	Evidence of hardening, cracking or colour change
The following day	Comparison with fresh plastic sulfur and ordinary sulfur

These are proposed observation times, not a prediction of exactly when each change will occur.

Keep the comparisons fair

Use similar sample dimensions, consistent storage conditions and the same gentle testing method.

If extension can be measured reliably:

Extension = stretched length - original length

Percentage extension = (extension / original length) x 100

For example, a strand extending from 40 mm to 50 mm has:

Percentage extension = (10 / 40) x 100 = 25%

That is an illustrative calculation, not an expected experimental result.

Students should also distinguish stretching from elastic recovery. A strand that becomes longer has deformed; to demonstrate recovery, it must shorten again after the force is removed.

Where samples are too irregular for useful measurements, photographs and a clearly defined flexibility scale may produce more honest evidence than precise-looking numbers.

Watching Crystals Return

A microscope adds another dimension.

Students could compare ordinary sulfur crystals with fresh and aged samples of plastic sulfur. Photographs taken with consistent lighting and magnification may reveal changes in surface texture and visible crystalline regions.

However, the limits of the equipment matter.

A classroom digital microscope cannot resolve individual sulfur chains or S8 molecules.

It can show larger-scale changes consistent with the structural explanation. It cannot directly prove the molecular mechanism.

That distinction is valuable:

What we observe and how we explain it are connected, but they are not the same thing.

Is This a Physical Change or a Chemical Change?

Students often expect every change to fit neatly into one of two boxes.

Sulfur shows why the reasoning matters more than the label.

Melting is a physical change. Crystallisation concerns the development of an ordered solid structure. Ring-opening polymerisation involves breaking and forming covalent bonds, even though the material remains an element.

The fact that no second element has been added does not mean that nothing has happened chemically.

I would ask students to identify the particular process they are discussing and explain what happens to the particles and bonds.

That produces a much stronger answer than simply declaring the whole demonstration “physical” or “chemical”.

Why This Matters Beyond Sulfur

Plastic sulfur illustrates a principle that runs throughout materials science:

A material’s properties depend on its structure and processing history, as well as its composition.

For students, that opens several useful questions:

• Why can cooling rate affect a material’s properties?

• Why do long-chain molecules behave differently from small molecules?

• Why can a manufactured material change during storage?

• How could we test whether an apparent improvement lasts?

It also challenges the assumption that every polymer must be carbon-based. Sulfur can form a chain backbone of its own.

Why I Would Include This in My Teaching

What appeals to me is the opportunity to return to the sample.

The heating and quenching provide the immediate visual interest. The ageing provides the deeper question.

A student who sees only the fresh material might conclude that sulfur has been permanently transformed into something rubbery. A student who examines it again the following day has to revise that explanation.

At Hemel Private Tuition, I want practical science to encourage that habit: observe carefully, make a prediction, collect evidence and be willing to change your mind.

This demonstration can also connect different levels of understanding. One student may focus on the visible properties; another may explore molecular chains; a more advanced student may consider the relationship between stability and the rate of structural change.

There is plenty to discuss without losing sight of the sample in front of us.

The Most Interesting Result May Come Tomorrow

Plastic sulfur begins with a surprising transformation: a brittle yellow solid becomes a dark, flexible material.

Its gradual loss of flexibility makes the lesson more powerful.

The sample reminds us that a solid can still be changing, that cooling history matters, and that knowing which element we have is only the beginning of understanding its properties.

Sometimes the most revealing part of an experiment happens after we think it has finished.