


Colour in Glass
Entry 06 / 15
12 min read
Colour in glass is chemistry. The same metal can turn glass blue or red depending on the flame, and the same glass can be clear while hot and coloured once it is reheated. This entry explains why, and how to work with it at the torch.
It covers the four ways glass gets its colour, a metal-by-metal guide, why glass is transparent and how it is made colourless, the colour techniques of the torch, and finally what is particular about colour in borosilicate, how to test colours and how to use them safely.
How glass gets its colour
When we add metals to glass, the metal atoms have electrons that can absorb energy from light. White light contains every colour: red, orange, yellow, green, blue, violet. Each colour corresponds to a different energy. When metals absorb some colours, they remove them from the light passing through the glass. What remains is the colour we see. Cobalt glass, for example, absorbs mainly yellow, orange and red light, so what reaches your eye is blue.
Metals are the most common way to colour glass, but not the only one. There are four main mechanisms.
1. Dissolved metal ions
Transition metals such as cobalt, copper, iron, chromium, manganese and nickel have electrons that absorb particular energies of visible light. For example: Co²⁺ gives blue, Cr³⁺ green, Mn³⁺ purple. These colours are usually transparent because the ions are fully dissolved in the glass network. The exact shade depends on the ion's oxidation state (how many electrons it has lost) and its surroundings in the glass, which is why one metal can give different colours in different recipes and flames.
2. Metallic nanoparticles
In some glasses, the metal doesn't stay dissolved as an ion but forms tiny metallic particles, a few to a few tens of nanometres across. These interact with light through surface plasmon resonance: the free electrons on the particle's surface oscillate together when light hits them, and the frequency of that oscillation decides which wavelengths are absorbed and scattered. The particles form when metal ions are reduced to neutral atoms, which group together into nuclei that grow.
The colour depends on the metal, the particle size and the concentration. Gold is the classic case: small particles absorb green light, so the glass looks ruby red; as they grow, the absorption shifts to longer wavelengths and the colour moves towards purple and blue, and very large particles scatter light and make the glass cloudy or brownish. Silver particles absorb blue-violet instead, giving yellows and ambers. So there is no universal rule that smaller particles mean cooler tones: for gold it is the opposite.
3. Crystals in the glass
Here microscopic crystals do the work, in two different ways. Cadmium sulphide (CdS) and cadmium sulphoselenide (CdSSe) absorb all light above a certain energy: CdS cuts out blue and looks yellow, and adding selenium moves the cut-off through orange to red. When these crystals are very small the glass can be transparent (the red of old traffic-light lenses); larger crystals, or an added opacifier, make it opaque. Other crystals, such as tin oxide, absorb nothing but scatter all light, making the glass white and opaque.
4. Colour centres (structural defects)
A less familiar mechanism. Sometimes colour comes not from a pigment but from defects in the glass structure that trap electrons. High-energy radiation such as X-rays or gamma rays creates these colour centres and can turn clear glass brown, which is why cerium is added to glass meant for radiation environments.
A metal-by-metal guide
"Oxidised" and "reduced" describe the chemistry; at the torch, an oxygen-rich flame pushes towards the first and a fuel-rich flame towards the second.
| Colourant | Form in the glass and colour | Notes |
|---|---|---|
| Cobalt | Co²⁺: intense blue, even at around 0.1% | Very stable in the flame. Tiny amounts balance decolourisers. |
| Chromium | Cr³⁺: green. Cr⁶⁺ (oxidised, chromate): yellow | Oxidising conditions give yellow-greens. High levels give near-black, or chromium oxide crystals (chrome aventurine). |
| Manganese | Mn³⁺ (oxidised): violet, purple. Mn²⁺ (reduced): almost colourless | The historic decolouriser (see below). |
| Iron | Fe³⁺ (oxidised): pale yellow to yellow-brown. Fe²⁺ (reduced): blue-green. Both: bottle green | The green tint of ordinary glass comes from iron in the sand. Amber bottle glass is iron combined with sulphur. |
| Copper | Cu²⁺ (oxidised): blue, turquoise, green. Cu⁺: colourless. Cu⁰ nanoparticles: ruby red. Cu₂O crystals: opaque red-orange | Reduction can bring a red or metallic copper surface. Copper crystals give goldstone its sparkle. |
| Nickel | Ni²⁺: brown, yellow-brown, grey; violet in some potash and lead glasses | Used with other oxides for greys and blacks. Strong reduction gives grey or metallic surfaces. |
| Gold | Dissolved gold: nearly colourless. Au⁰ nanoparticles: ruby, pink, cranberry, purple | Around 0.001% gold is enough for ruby glass. The colour develops on striking. |
| Silver | Ag⁺: colourless. Ag⁰ nanoparticles: yellow, amber, orange | Silver-rich art glasses strike to many colours and reduce to a silvery lustre. |
| Selenium | Oxidised selenium: colourless. Se⁰ nanoparticles: pink to red | A trace decolourises; more gives pink. With cadmium sulphide it forms selenium ruby. |
| Cadmium | Cd²⁺ alone: colourless. CdS crystals: yellow. CdSSe crystals: orange to red | The bright yellows, oranges and reds. Overheating can dull or brown them. Toxic: see safety below. |
Transparency, opacity and clear glass
Glass is transparent because its structure lets light through: it scatters very little of it and barely absorbs it.
Glass is made mostly of silicon and oxygen. The electrons in these atoms absorb ultraviolet and infrared, but not visible light. And because glass has no grains or crystal boundaries inside it, there is nothing for light to bounce off. So visible light simply passes through.
Glass can be made opaque by adding special compounds to the molten glass.
Tin oxide (SnO₂) is the classic example; fluorides and calcium phosphate are others. They form microscopic crystals as the glass cools, and the crystals scatter light in every direction, so the glass looks milky or opaque.
Transparent = everything is mixed at the atomic level.
Opaque = there are tiny "solid things" inside that scatter the light.
The manganese story
Since at least Roman times, manganese has been used (alongside antimony) to decolourise glass, neutralising the greenish tint of the iron in sand. It works in two ways. Chemically, it turns strongly coloured blue-green Fe²⁺ into much paler Fe³⁺. Visually, a little purple Mn³⁺ sits opposite green on the colour wheel, so the remaining tints cancel out. The result: glass that looks colourless.
There is a side effect. Years of ultraviolet light from the sun turn the nearly colourless Mn²⁺ back into purple Mn³⁺, and clear glass slowly goes lavender. This is solarisation, and collectors call the result "sun-purpled" or "sun-coloured amethyst" glass.
In American bottle making, manganese was the standard decolouriser from around the 1870s–1880s until about 1920. The First World War disrupted supply: Germany is often named as the source, though research shows much of it came from India and Brazil. The bigger reason was technological: manganese worked well in the pots of hand production but poorly in the large tanks feeding the new automatic bottle machines, and selenium was cheaper. That is why purple-tinted bottles and windows usually date from before the 1920s.
Selenium and cerium
Selenium decolourises the same visual way: a trace of pink, often balanced with a little cobalt, masks the green. Cerium oxide works chemically, oxidising Fe²⁺ to Fe³⁺, and also resists radiation browning. Today, purer, low-iron raw materials do much of the work.
Colour techniques at the torch
Striking
Some glasses look transparent or pale while hot, but colour appears when they are gently reheated. The colour depends on particles that haven't formed yet. When the glass is very hot, the metals are dissolved as ions. As it cools, tiny nuclei form; reheated to a moderate temperature, these grow into particles large enough to colour the glass. Striking glasses usually contain gold, silver, copper, selenium or cadmium.
Step by step: let the piece cool until the glow has gone. Reheat it gently (in the kiln, or in a cooler part of the flame) without bringing it back to a glow. Nanoparticles form. The colour appears. Stop when you like it: overstriking can make some colours dark, muddy or opaque, and reheating to a full glow can dissolve the particles so you have to start again.
Reduction
When the flame has little oxygen, some metals are reduced. This can produce metallic surfaces, iridescent colours and darker tones. It is very common with silver-rich glasses, and with gold and copper glasses. Reduction effects sit on the surface, so an oxidising flame can burn them off again.
Fuming
Fuming means vaporising fine silver or pure (22–24 carat) gold in the flame so that its vapour settles as a microscopically thin film on hot glass. A small piece of metal, usually stuck to the end of a glass rod, is held in a hot, oxidising flame, and the piece is held downstream so the vapour washes over it. Encased in clear, the film gives soft colours.
The thickness of the film decides the result. Light silver fuming looks pale yellow to amber when you look through it, and over a dark background heavier silver often reads as blue. Gold gives soft pinks that deepen to rose and magenta, and heavy gold looks metallic or mirror-like. Both keep developing in the kiln, so judge the colour after annealing.
The variables that control the result:
- Glass temperature: warm enough for the vapour to stick, not so hot that it softens; many lampworkers fume just below a visible glow.
- Distance from the metal along the flame: a few centimetres is typical; closer generally deposits more.
- Angle to the vapour stream: square-on gives an even layer, oblique a gradient.
- Speed and number of passes: slower passes deposit more, and each extra pass adds depth.
- Flame: hot and oxidising to vaporise the metal (gold needs more heat than silver), then neutral to encase. Strong reheating of unencased fume can burn it off.
Encased fuming: fume an inner layer, encase it in clear glass, then add more layers. The result is dimensional, almost holographic. You can also layer silver over gold for unusual hues.
Reactive glasses
Some glasses react with each other where they touch. The classic examples involve sulphur: a sulphur-bearing glass meeting one that contains copper, silver or lead forms dark metal sulphide at the boundary, seen as a dark line or halo. A well-known soft-glass pairing is ivory with copper turquoise. Used on purpose, these reactions draw fine outlines; by accident, they muddy a design.
Dichroic glass
Dichroic glass carries a coating of many very thin layers of metal oxides and silica, evaporated by an electron beam in a vacuum chamber: often 30 to 50 layers, less than a thousandth of a millimetre in total. Light reflecting from the layer boundaries interferes, so one band of colours is reflected while the complementary colours pass through, and both shift with the viewing angle. It is optical interference, the same physics as a soap bubble. Modern coatings grew out of NASA-related research into optical filters. For lampworking, use dichroic made for your glass type, encase it, and avoid overheating, which can dull or break up the coating.
Working with colour at the torch
- Overlay transparent colours: a base colour with a different transparent hue on top creates colour that seems to shift with the light.
- Gradients: vary the heat across a piece to create colour gradients, especially in sculptural work and with striking colours.
- Preheat colour: keep colour rods warm in a cooler part of the flame before adding them, for even colour and less thermal shock.
- Mind the thickness: transparents look far lighter in a thin stringer than in a thick gather, and cobalt can look almost black in a heavy piece.
Colour in borosilicate, testing and safety
Why the borosilicate palette is different
Borosilicate began as laboratory glass, so coloured boro rod for studio artists is recent compared with the long tradition of coloured soft glass. It is also harder to colour: boro is high in silica and boron, low in alkali and worked much hotter, so colourants dissolve and behave differently; volatile ingredients such as sulphur, selenium and cadmium are harder to hold; and every colour must match the low expansion of clear boro (COE around 33). For a long time boro offered fewer and paler colours, with bright reds and yellows especially difficult. The gap has narrowed: silver- and gold-rich striking colours became a boro strength, and brighter cadmium-based opaques followed. The range is still smaller than soft glass, and more dependent on heat and flame. More on the glass itself in What Glass Is: Structure, Types and Borosilicate.
Testing colours
- Make a labelled test piece for every new colour, with maker, name and batch number: batches can vary.
- Test it as you will use it: thin and thick, encased and on the surface, struck and unstruck, neutral and reducing flame. Note what you did.
- Anneal before judging, since many colours shift in the kiln.
- Look in different light: daylight and indoors, against white and dark, with light passing through and reflecting off.
- Test combinations for reactions and compatibility before a finished piece.
Safety with colour
These add to the studio basics in The Studio: Workspace, Safety and Equipment.
- Cadmium and selenium colours: cadmium compounds are toxic and carcinogenic, and selenium compounds are toxic too. In finished glass they are bound in, but overheating these colours can release fumes. Work with good ventilation, don't boil or burn them, read the supplier's safety data sheet, and keep such glass away from food use.
- Fuming: metal fumes are hazardous to breathe. Fume only with strong local extraction that carries vapour out of the studio. Use only fine silver and pure gold: never sterling, plated metal, solder or unknown metal, which can contain copper, zinc, lead or cadmium.
- Dust and hygiene: grind coloured glass wet, wipe dust with a damp cloth, wash your hands after handling rods and frit, and don't eat or drink at the bench.
Always follow your suppliers' safety data and local regulations.
With colour understood, the next step is the finished piece: Finishing, Combining and Troubleshooting.
Test yourself10 questions
Choose one answer for each question, then check your results at the end.
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01Why does cobalt glass look blue?
What reaches your eye is the light that was not absorbed.
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02What makes gold ruby glass red?
This is surface plasmon resonance: the particles' surface electrons oscillate and absorb green light.
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03As gold particles grow larger, the colour moves:
There is no universal rule that smaller means cooler: for gold it is the opposite.
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04How does tin oxide make glass opaque?
Transparent means mixed at the atomic level; opaque means tiny solid things inside scatter the light.
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05What was manganese historically used for in glass?
It turns blue-green Fe²⁺ into paler Fe³⁺, and a touch of purple masks what is left.
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06Why does some old clear glass turn lavender in the sun?
Collectors call it sun-purpled glass. It helps date bottles made before the 1920s.
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07What is striking?
Stop when you like the colour: overstriking can make some colours dark or muddy.
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08Which metals should be used for fuming?
Never sterling, plated metal or solder, which can contain copper, zinc, lead or cadmium. Always fume under strong extraction.
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09Where does dichroic glass get its colour?
The same physics as a soap bubble: colours shift with the viewing angle.
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10Why is the borosilicate colour palette smaller than soft glass?
The gap has narrowed: silver and gold striking colours became a boro strength.
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