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Decomposition is the breaking of inter-molecule bonds during melting in the kiln. To understand it we need to understand elements, oxides, compounds, solutions and mixtures (from the chemistry jargon point-of-view).

"Elements" are one kind of atom which cannot be broken down any further (except by nuclear reactions). Atoms are a nucleus with varying numbers of electrons in orbit. Oxygen, silicon, carbon, etc. are among the 100+ elements.

"Compounds" are atoms of more than one element bound together chemically. How? Atoms share electrons or electro-statically attract others having opposite charges. An "oxide" is a compound containing oxygen. A molecule of SiO2 is one atom of silicon and two of oxygen, thus is it an oxide (there are about ten that are important in glazes). Oxides are bonded together really well.

"Solutions" are mixtures of molecules in a liquid. In salt water, for example, the NaCl molecules move independently. But as the water evaporates the mobility of the water enables them to bond in a preferred orientation: crystalline.

Theoretical soda feldspar is a compound of oxides: molecules of sodium (Na2O), alumina (Al2O3) and silica (SiO2) are bonded chemically to form a crystaline solid.

A bucket of glaze made of feldspar, kaolin and silica powders is a "mixture", the particles are not chemically bonded and they are not dissolved. Rather, they float freely in "suspension" in the water.

Now, if we dry a glaze and subject it to increasing heat in a kiln, the bonds holding oxides together (in their compounds) will be broken (weakest first, strongest later). An increasingly liquid "melt" will form as temperature rises. This melt is a "solution", particles are dissolving into it.

Since glaze melts are much more viscous than water solutions, the opportunities for orientation of particles into crystals during cooling of the melt in the kiln are dramatically less. So they freeze as a "glass". A glass is a compound, but a rather novel one: a solid solution.

The above is the theoretical process. In practice a variety of other things are also occurring as the kiln fires.

Remaining water is driven off during early stages of firing. It is not decomposition because no molecular bonds are broken. However many materials are compounds that have water molecules bonded into their chemical structure (e.g. clays). These are called "hydrates" and they can account for up to 12% or better of the weight. Relatively low temperatures (e.g. red heat) are sufficient to break these water molecules away (sometimes called "water smoking"). The product of decomposition: steam.

There is another class of 'volatiles' or gases that are driven off: Carbon and sulphur. Carbon is integral in the crystal structure in some materials (e.g. calcium carbonate, dolomite, barium carbonate). Clays contain sulphates and organic carbon. Red heat is sufficient to burn away the organic carbon as CO2 but it takes higher temperatures (varying by material) to decompose and liberate CO2 and SO3 from the carbonates and sulphates (e.g. calcium carbonate loses 45% it is weight).

Some materials experience decompositions that disqualify them for use in glazes. For example, hydrated lime is a good source of CaO, but 25% of its weight is converted to water at 500C. To say this would be an inconvenient event in a firing would be an understatement! Other materials that do generate significant gases during decomposition may not be an issue because the host glaze and firing method can tolerate this. Soluble materials are no-nos in glazes, they concentrate on the surface was water evaporates.

The perfect storm of high surface tension and high LOI: Blisters.

The perfect storm of high surface tension and high LOI: Blisters.

An example of how calcium carbonate can cause blistering as it decomposes during firing. This is a cone 6 Ferro Frit 3249 based transparent (G2867) with 15% CaO added (there is no blistering without the CaO). Calcium carbonate has a very high loss on ignition (LOI) and for this glaze, the gases of its decomposition are coming out at the wrong time. While there likely exists a firing schedule that takes this into account and could mature it to a perfect surface, the glaze is high in MgO, it has a high surface tension. That is likely enabling bubbles to form and hold better.

Calcium carbonate and glaze bubbles

Calcium carbonate and glaze bubbles

The two cone 04 glazes on the right have the same chemistry but the center one sources it's CaO from 12% calcium carbonate and ulexite (the other from Gerstley Borate). The glaze on the far left? It is almost bubble free yet it has 27% calcium carbonate. Why? It is fired to cone 6. At lower temperatures carbonates and hydrates (in body and glaze) are more likely to form gas bubbles because that is where they are decomposing (into the oxides that stay around and build the glass and the ones that are escaping as a gas). By cone 6 the bubbles have had lots of time to clear.

Carbonate gassing can cause glaze blisters

Carbonate gassing can cause glaze blisters

An example of how a carbonate can cause blistering. Carbonates produce gases during decomposition. This glaze (G2415B) contains 10% lithium carbonate, which likely pushes the initial melting temperature down toward the most active decomposition temperatures.

The difference between these low fire transparents: Gerstley Borate vs. Ulexite

The difference between these low fire transparents: Gerstley Borate vs. Ulexite

Left: Worthington Clear cone 04 glaze (A) uses Gerstley Borate to supply the B2O3 and CaO. Right: A substitute using Ulexite and 12% calcium carbonate (B). The degree of melting is the same but the gassing of the calcium carbonate has disrupted the flow of B. Gerstley Borate gasses also, but does so at a stage in the firing that does not disrupt this recipe. However, as a glaze, B does not gel and produces a clearer glass. A further adjustment to source CaO from non-gassing wollastonite would likely improve it.

Let me count the reasons this glossy white cone 6 glaze is pinholing

Let me count the reasons this glossy white cone 6 glaze is pinholing

First, the layer is very thick. Second, the body was only bisque fired to cone 06 and it is a raw brown burning stoneware with lots of coarser particles that generate gases as they are heated. Third, the glaze contains zircopax, it stiffens the melt and makes it less able to heal disruptions in the surface. Fourth, the glaze is high in B2O3, so it starts melting early (around 1450F) and seals the surface so the gases must bubble up through. Fifth, the firing was soaked at the end rather than dropping the temperature a little first (e.g. 100F) and soaking there instead.

White spots and blisters in a high zircon glaze at cone 6

White spots and blisters in a high zircon glaze at cone 6

This is also a common problem at low fire on earthenware clay (but can also appear on a buff stonewares). Those white spots you see on the beetle also cover the entire glaze surface (although not visible). They are sites of gas escaping (from particles decomposing in the body). The spots likely percolate during soaking at top temperate. Some of them, notably on the almost vertical inner walls of this bowl, having not smoothed over during cool down. What can you do? Use the highest possible bisque temperature, even cone 02 (make the glaze thixotropic so it will hang on to the denser body, see the link below about this). Adjust the glaze chemistry to melt later after gassing has finished (more zinc, less boron). Apply a thinner glaze layer (more thixotropy and lower specific gravity will enable a more even coverage with less thickness). Instead of soaking at temperature, drop 100 degrees and soak there instead (gassing is much less and the increasing viscosity of the melt overcomes the surface tension). Use a body not having any large particles that decompose (and gas) on firing. Use cones to verify the temperature your electronic controller reports.

Out Bound Links

  • (URLs) Milestone temperatures during firing


  • (URLs) A study of the cmparative decompositions of MgCO3, CaCO3, SrCO3 and BaCO3


  • (Glossary) Oxide

    An oxide is a combination of oxygen and another element. There are only about ten common oxides that we need to learn about (most glazes have half that number). CaO (a flux), SiO2 (a glass former) and Al2O3 (an intermediate) are examples of oxides. CaO (calcium oxide or calcia), for example, is cont...

  • (Glossary) Glass vs. Crystalline

    In ceramic technology the term 'glass' is contrasted with the crystalline state, it is seen as a "super-cooled liquid". When crystalline materials solidify the molecules have opportunity to orient themselves in the preferred pattern during freezing whereas in a glass the random orientation of molecu...

  • (Glossary) Volatiles

    Compounds with clays or glazes that burn away during firing. For example, calcium carbonate decomposes during firing to produce CO2 gas and loses almost half its weight. Other common volatiles are sulphur, carbon, water, fluorine, nitrogen. The term "volatilization" refers to the burning off of vola...

In Bound Links

  • (Project) Temperatures

    Many ceramic problems relate to a lack of understanding about what is happening at each stage of a firing, there are just so many materials that are doing so many things. This part of the database wil...

  • (Tests) DTMP - Decomposition Temperature
  • (Glossary) Water

    There is a need to discuss water in ceramic production as it related to a number of natural phenomena and production processes: Plasticity: Clays are plastic because water glues and lubricates the particles. The micro-dynamics of this are complex. Rheology: Suspensions (solids:water systems) e...

  • (Glossary) Water Smoking

    Refers to the period in a kiln firing where the last of the mechanical water in body (and glaze if on second firing) are being released. Firing can normally proceed quickly after this water has been ejected (750C/hour or more is common in industry but potters would typically proceed at half of that)...

  • (Glossary) Blisters

    Glaze blisters are a surface defect in fired ceramic glazes. They have caused every potter and company grief at one time or another. The problem can be erratic. The blisters trace their origins to the generation of gases as particles in the body and glaze itself decompose during firing (loosing H2O,...

  • (Articles) Where Do I Start?

    Break your addiction to online recipes that don't work. Get control. Learn why glazes fire as they do. Why each material is used. Some chemistry. How to create perfect dipping and drying properties. Be empowered. Adjust recipes with issues rather than sta

  • (Glossary) Glaze Chemistry

    Glaze chemistry is learning what each oxide does in a fired glaze and the relative advantages and disadvantages of each material supplying it. The chemistry of a glaze is expressed in a manner similar to its recipe, except that the items are oxides and the amounts can be by weight (an analysis) or n...

By Tony Hansen

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