Following is an extract from John Sankey's Website with detailed instructions on achieving iron reds.


Red iron oxide Fe2O3 decomposes to iron monoxide FeO above 1000°C even in oxidising environments. Iron red is produced by a surface growth of columnar crystals of Fe2O3. Best reds are obtained by a fast cool through the temperature range above 1000°C, where black FeO tends to form crystals, to about 950°C where growth of red Fe2O3 crystals is optimised. Oxygen is required for this phase. Holding the temperature at 950°C for about an hour produces the maximum coverage of iron crystals and best red colour. The colour deteriorates with holds much longer than that, tending towards rust brown.

The more calcium there is in an iron glaze, the more difficult it is to obtain a good red, however some calcium is required to get red from iron. To get a tomato red also requires phosphorus; the red becomes more orange when magnesium is added to these two. The best iron reds in oxidation firing are obtained with about 0.10 molar CaO, 0.03-0.06 MgO, 0.01-0.02 P2O5 and 0.08-0.12 FeO.


Colours reported
Black, tomato to rust red to muddy brown with green, honey, rust, rarely blue nuances are reported in the literature. I have seen them all in my tests. I have only seen blues as crust-like surface components; if they are crystalline, the crystals are to small to see at 100x. I have never seen yellows or greens as a surface component, only as body. Reds seem to appear solely as a crystalline surface layer.

Thickness of application
This is often mentioned as a major determining factor in colour of red iron glazes. In my own work, I have found that a minumum thickness of about 50 µm is required.

Cooling temperature
Cooling schedule is known to be important. Refiring to cone 04 is often recommended to improve the red. Murrow (Ceramics Monthly Sept 2001) found that shino glazes turned red only below 982°C. Marians (Ceramics Monthly June/July 2007) found that temperature holds between 980°C and 870°C during the cooling cycle were critical to the development of red in her iron glaze. She saw three components, one believed to be iron-rich and two silica-rich, at low magnification. My own work confirms these findings, that holds at 950°C for an hour during cooling produce the best reds.

Colour analysis
Murrow&Vandiver (noted in Ceramics Monthly Sept 2001) found that the red colour of shino glazes came from a surface layer of ferric microcrystals about 20 µm thick. Under this layer, the glaze was white. My collaboration with John Stirling found that in iron glazes the surface is iron sesquioxide (Fe2O3) while deeper iron is iron monoxide (FeO). Park&Lee (J.Ceram.Soc.Japan 113(1314):161-165 2005) found that in high magnesia glazes the red colour is magnesioferrite MgO.Fe2O3.

Cardew (Pioneer Pottery) states that alkali earths must be minimised for an iron red, that even 0.2 calcia will turn an iron glaze brown, and proposes a special frit to this end. My work confirms this for calcia.

Park&Lee (op.cit.) found by X-ray diffraction that in their glazes magnesia forms a red colour as magnesioferrite MgO.Fe2O3, and that magnesioferrite crystal formation is closely related to the presence of whitlockite-type crystals Ca.9(Mg,Fe).(PO4).6(PO3OH). Phosphorus seems to crystallize as whitlockite at 1000-1050°C, magnesioferrite at 900-950°C. Edouard Bastarache (unpublished) considers that the presence of dolomite (Ca,Mg)CO3 in iron red glazes makes better reds.

Hamer&Hamer (The Potter's Dictionary) mention that soda combined with small amounts of iron produce blue, and that soda encourages red with large amounts of iron, but give no details.

Bone ash is reported by many to make more reliable reds; some use ferric phosphate instead of red iron oxide and the bone ash (which contains a lot of calcia).

Hamer&Hamer (The Potter's Dictionary) mention that boron combined with small amounts of iron produce blue, but give no details. Rhodes (Glazes for the Potter) mentions blue from iron and boron; again no details. Obstler (Out of the Earth, Into the Fire) mentions that boron increases green in iron celadons; no details given. Hesselberth&Roy's Waterfall Brown (Mastering Cone 6 Glazes) obtains green from iron; it has 50% more boron than usual formulations, also more soda. True boron iron greens seem to require the near-absence of calcia, which can only be achieved with frits since natural borates are half calcia.

Weyl (Coloured Glasses) notes that iron is green when it is a network-modifier (equivalent of interstitial atoms in crystals), and that titania moves it to brown by shifting it to a network former (the equivalent of taking part in a crystal lattice). 4% titania achieved this in my experiments with the calcium iron glaze below.

Migration of iron
There are two unpublished reports of sub-surface iron migrating to the surface of glazes. Ron Roy has noticed this under strong reduction, but not in oxidation under otherwise identical conditions. Hank Murrow believes that fluorine in a glaze assists migration of iron to the surface and uses a percent or less cryolite in his glazes to achieve this.

Sankey Iron Red
Custer feldspar 44g
silica 16.5g
bone ash 14g
red iron oxide 11g
EPK 10.5g
talc 10g
lithium carbonate 3
Bentonite 2g
COE: 6.8x10-6/K
calcia: 10% molar
Stoneware (Tucker Smooth White)
Source: Kevin Baldwin, adapted to local clays
Painted on bisque, fired cone 6 electric, one hour hold at 950°C. Vase is 7 cm high. A very even colour as long as it is thicker than 50 µm, red crystals on a black ground with visual depth. It tends to black where it is thin. By far the most reliable of the iron reds I've tried, and the one I've chosen for my own dinner set. The expansion is high, but it works perfectly on my clay, which is fairly low expansion (6.64x10-6/K), probably due to the high potash content, which increases both elasticity and tensile strength.

Microphotos are about 60x. X-ray analysis shows that all the crystals are pure iron oxide; Fe2O3 is the red, FeO the black. Red crystals were analysed at three depths. The data shows that the result of the 950°C soak is primarily to oxidize the iron crystals on the surface to red Fe2O3 while the buried iron remains black FeO. This may be done by movement of oxygen to the surface under chemical-strength forces or by surface oxidation. The glaze is far too viscous at 950°C to permit physical sorting of crystals.

one hour hold at 950°C

no hold

scanning electron microscope photo of Fe2O3 crystals
Borate Iron Red:
Gerstley borate 32g
silica 30g
Custer feldspar 20g
red iron oxide 15g
talc 14g
EPK 5g
bone ash 6g
Bentonite 2g
COE: 5.6x10-6/K
calcia: 14% molar
Stoneware (Tucker Smooth White), thrown and trimmed.
Source: published many times under many names
Dipped on bisque, prefire thickness 0.47 mm. Fired cone 6 electric, two hour rise to maximum temperature (1220°C), held there for 10 min, kiln off until soak temperature reached (typically 30 min.), held there for a soak period, kiln off (5 hr to reach 200°C).

I did a series of runs with the same bowl, changing only the soak temperatures. The first involved a long soak to fully develop all crystals that might be formed. The microphoto (about 50x) shows that there are two types of components to this glaze. One group forms very small crystals or crusts on the surface; it forms a rust colour with long soak times. The other component oozes out to the surface without crystalizing and is often yellow, sometimes bright. It is probably ferrosilite (see below). Under certain temperature regimes the ferrosilate is coloured a dull red by the iron. Bright colours always seem associated with surface components; the two other microphotos shown are typical of the variety of colours seen. X-ray analyses show that the surface crusts are thinner than 4 µm, the effective penetration depth of the 20 kV electrons used; reliable analyses could not be obtained.

Black gradually took over the bowl with repeated firings (the 980°C at right was the eighth in the series). So, if you don't get the colour you wish with this glaze, try refirings, but not too many. I obtained the most interesting colours with moderate-length soaks in the 900-980°C range.

X-ray analysis of the final glaze (the 980°C photo) showed considerable fine and medium-scale differentiation in the surface. There were large patches of nearly pure silica (87%). Other patches had double the concentration of iron as the total glaze formulation; all these were low in calcia. There was also evidence of calcium silicate. It was not possible to match the X-ray image to an optically-visible feature of the glaze.

In contrast to some reports, I found this to be a very well-mannered glaze as I mixed it, not at all runny, or even droopy when laid on thickly, as you can see from the lack of problems with the sharp horizontal edges of the 8 cm diameter sugar bowl.

5 hr hold at 870°C
30 min hold at 940°C
30 min hold at 980°C
glaze painted thickly on the outside, thinly on the inside, 1 hr hold at 920°C
scanning electron microscope photo of a 0.7 mm square portion of the surface, showing a typical crust-like differentiation.
Calcium Iron:
Wollastonite 28g
EPK 28g
Fusion F2 frit 23g
silica 17g
red iron oxide 7g
nepheline syenite 4g
Bentonite 2g
cobalt carbonate 2g
COE: 5.5x10-6/K
calcia: 17% molar
Porcelain (Tucker 6-50), thrown and trimmed.
Dipped on bisque, fired cone 6 electric. This began as an attempt at a matte lustre black, but turned out to be a microcrystalline glaze. With the same bowl, a fast cool of this glaze gives a glossy black, then a refire followed by a slow cool converts it to a mottled black and green semi-matte, and vice versa. Green crystal size is dependent upon cooling rate. Cooling from 1200°C at 50C/hr to 800°C produced crystals typically 2 mm in diameter. At 80C/hr the crystals were about 1 mm, at 100C/hr, ½ mm. 150C/hr is required to get a smooth surface, but then it's close to glossy. Unless fired glossy, iron in excess of 7% comes out of solution to form a metallic layer between the green crystals. Bowl is 10 cm diameter.

Besides the individual oxides, possible mineral compositions include Andalusite Al2O3.SiO2, Anorthite CaO.Al2O3.2(SiO2), Wollastonite CaO.SiO2, Fayalite 2(FeO).SiO2, Hedenbergite CaFe.2(SiO3) and Ferrosilite FeO.SiO2. [mineral photos]

The right half of the bowl is the result of a 10 hr soak at 1120°C after firing to 1220°C. X-ray analysis shows that the crystals are FeO; as shown in the microphoto (about 100x), they are mostly long rhombs. The surface is rough to the touch.

The left half of the bowl had a 10 hr soak at 870°C after firing to 1220°C. This produces a surface layer of greenish-yellow crystal needles that grow in six rays from a central point. The colour could match either Hedenbergite or Ferrosilite, but the crystal form is most consistent with Hedenbergite. The crystals are so thin that their X-ray output was mixed with background material output, but it also indicates Hedenbergite.

Not an attractive or useful glaze.

I thank John Stirling of Natural Resources Canada's Geological Survey for making the scanning electron microscope guided X-ray analyses.

Iron Glaze Chemistry

To investigate the interaction of calcia, magnesia and phosphorus with iron in oxidising fired glazes, a series of mixes were made. A base glaze contained none of any of the three oxides under study, and one glaze each was made up similar to the composition of the base glaze, but with a large quantity of each of the oxides in turn. The target analysis for each was 3.5 Seger SiO2, 0.4 Al2O3 and 0.25 B2O3 (B2O3 and FeO omitted from Seger ratios).

mix recipe molar Seger oxide
28 silica
28 potassium carbonate
24 kaolin,EPK
10 iron oxide,red
10 frit,Fusion 367
0.602  3.392  SiO2
0.166 0.935 K2O
0.102 0.575 FeO
0.010 0.059 Na2O
0.072 0.404 Al2O3
0.045 0.253 B2O3
30 silica
25 magnesium sulphate
25 kaolin,EPK
10 iron oxide,red
10 frit,Fusion 367
0.611  3.497  SiO2
0.163 0.935 MgO
0.098 0.562 FeO
0.072 0.411 Al2O3
0.043 0.248 B2O3
0.010 0.058 Na2O
32 silica
26 kaolin,EPK
22 calcium carbonate
10 iron oxide,red
10 frit,Fusion 367
0.615  3.485  SiO2
0.166 0.939 CaO
0.094 0.533 FeO
0.071 0.405 Al2O3
0.041 0.234 B2O3
0.010 0.055 Na2O
27 silica
26 potassium carbonate
23 kaolin,EPK
15 iron phosphate
9 frit,Fusion 367
0.587  3.494  SiO2
0.157 0.936 K2O
0.100 0.596 FeO
0.070 0.418 Al2O3
0.041 0.246 B2O3
0.033 0.197 P2O5
0.010 0.057 Na2O

Since the potassium and magnesium salts are hygroscopic (magnesium sulphate particularly so), each of these was baked at 220°C until anhydrous before weighing. Each glaze mix was then ground in a ball mill until uniformly fine. An attempt was made to use a 200 mesh seive on the dry mixes, but the hygroscopic-powered clumping of the soluble salts made that impractical - lumps had to be taken out after mixing with the oil.

Each tile glaze was made with four 1/4 tsp portions (1 tsp=5 ml) of dry material, using a precision stainless steel measure, then mixed with 3/4 tsp corn oil. (Water could not be used due to the soluble salts required to separate the oxides.) They were fired to 1290°C (cone 10), cooled to 950°C, then held there for 1 hr.

Since the best results were obtained with the maximum amount of phosphorus available from these mixes, and calcium was shown to be required, a supplementary mix was made up using bone ash (which contains calcium) to obtain larger amounts of phosphorus. Finally, the ratio that gave the best colour response was tested with 0-25% added red iron oxide. Some of the 54 test tiles are shown at right. Although not exactly decorative, they show several useful results for oxidation firing above 1000°C:

  1. Although excess calcium is known to turn iron glazes brown, some calcium is required to get red from iron.
  2. To get an intense red also requires phosphorus, but too much phosphorus turns the glaze brown.
  3. The red becomes more orange when magnesium is added to these two, but too much magnesium turns the glaze grey.
  4. The best iron colour responses in this series were obtained with 0.10 molar CaO, 0.03-0.06 MgO, 0.01-0.02 P2O5.
  5. Using a base with these proportions fired to cone 6, the best reds were obtained with 9-14% added red iron oxide.
  6. 1% cryolite (fluorine) may help to brighten the red on the surface a bit, but gives foaming to spitting problems during firing if used even slightly in excess or if insufficiently finely divided.

I have located only one phosphorus-iron mineral that is red: Simferite Li(Mg,Fe+++,Mn+++)2(PO4), which is not a player since none of my test series contained lithia. Park&Lee identified a magnesium-iron compound as their red. However, they seem to have concluded that the role of phosphorus is to tie up calcia so it doesn't interfere with the formation of magnesioferrite. It can't be as simple as that, since I got zero red from any glaze that did not contain calcia, and only a trace of very dark red on glazes that contained calcia but no phosphorus.

My current working hypothesis is that a calcium-phorphorus compound acts as a promotor (perhaps catalyst) for the oxidation of FeO to Fe2O3. It is possible that the two instead tie up something else that inhibits the oxidation, but this seems less likely.

The tests were originaly planned for cone 6 and boron added that is usually sufficient for it. Although the magnesium mix melted at cone 6, all mixtures with it turned viscous and foamy as soon as they melted. Cone 10, the maximum for my kiln, helped with some, but was still inadequate for a few.
Every stray cat in the neighbourhood was attracted to the kiln outside air vent by the smell of the corn oil!


Here is the setup I use to take my microphotos. My microscope is a basic full-size frame - no condenser, fine focus, stage movement or anything else expensive. The objective is a 5x 0.1 NA - low NA gives large depth of field, important for viewing solid objects. The eyepiece is a 10x periplan, selected from a dozen brands in the store for clearest view over the field with this objective.

My camera is a basic Canon PowerShot, set to focus and meter only in a central square that is shown on the LCD in P mode. This is the least expensive camera I've found that gives pictures as sharp as its pixel count. Many made by electronics companies have poor resolution lenses and/or autofocus. Its 3.2 megapixels is ample for web photographs.

In use, the camera is placed on the eyepiece, moved from side to side until all the circle of light from the microscope is visible on the screen, then zoomed until the edge of the circular field just touches the edges of the view. That standardizes the magnification of the photos so only one session with measuring scales is required. The microscope is focussed until the image is sharp on the LCD, then the shutter pressed.

Total cost for microscope plus camera - $340 in Canada (2006). Of course, both microscope and camera can be and are used independently of each other.

If 50x is too high a magnification, remember: a camera works just like a human eye. If you can see it you can photograph it! Try holding magnifying glasses in front of the lens - I find a 4x jewellers' loupe especially useful for photographing small insects.

Author's permission to republish

All materials presented on my site, except those specifically credited to other authors, are Copyright © John Sankey, 1939-2008, under the Berne convention, solely in order to protect the right of all to continue to use them freely. Anyone may copy, link to, or distribute any of them as much as they wish, as long as this notice of copyright and permission to further copy is distributed with all copies. That's the only restriction I put on them - that they remain absolutely free to all. No one may restrict their further use in any way, by collection copyright, physical copy prevention, or any other means. The courtesy of a reference link or credit is always appreciated. John Sankey

Comment by George Lewter on September 25, 2011 at 11:50am

In the March 2011 issue of Ceramics Monthly was great 2-page article about iron compounds, which is viewable online.  It has a chart of different iron sources, variations, characteristics, and uses.  The row concerning red iron had condensed data that I've been looking for.

  • Natural red iron oxide is around 85% pure
  • Spanish red iron oxide ranges from 83-88% purity
  • Synthesized red iron oxide (high purity red iron oxide, Red 4284, brand named Crocus Martis, or Red Iron Precipitate) is very fine 325 mesh, and is 96-99% pure. 

Other iron compounds like black and yellow iron oxides, chromates, sulfates, chlorides, phosphates, siennas, umber, illmenite, rutile are also covered in the chart.  Very interesting stuff if you want to know more about iron.  

Comment by George Lewter on March 16, 2010 at 10:47pm
My experience with C Harris temoku is similar. I like it as a mottled warm red on Laguna b-mix 5, but over Laguna's #80 stoneware which is a darker brown C Harris variegates with stronger red flecked with darker colors of brown, blue, and black, and it breaks the darker colors over rims and edges. I like it better over the darker body.
Comment by George Lewter on March 8, 2010 at 10:07pm
I believe I did the recommended cooling -- rapid cool from max temp down to 950 deg C and 1 hour hold there followed by turning off the kiln.
Comment by George Lewter on March 8, 2010 at 2:36pm
I too got only a slightly reddish brown from the Sankey recipe.
Comment by VicsArt on January 24, 2010 at 5:31pm
Many thanks for your kind response. I will look into the C Harris Temoku recipe you mention. I would be tempted to try stains also as I see so many references to them on american sites, but I have not yet found a UK supplier for them. I am only just beginning to learn to mix glazes so there is a very long learning curve ahead! Thanks again,
Comment by George Lewter on January 24, 2010 at 2:47pm
I think your best bet for an iron red is with the C Harris Temoku recipe that is posted a couple of places on this site. (Use the search box at the upper right of the screen.) That glaze is possibly not a true "saturated" iron red as Sankey speaks of, but I believe it is forming the same red crystals. It is by far the most reliable of 5 or 6 iron reds I have tried, and when it doesn't turn red, it is still a pretty nice, defect-free brown, when compared to the other iron reds that don't turn red. The only way I know to get red consistentently is to use glazes with encapsulated stains. Because of the expense of the stains, I have chosen to pursue the iron reds.

In your situation, the stain based glazes may be the way to go. You can either use mixed glazes or add the stain of your choice to a clear base glaze you mix yourself. It usually takes upwards of 10% stain to get a glaze to have an intense color. Some glaze components are not compatible with some stains and will cause the color to fail, but the stain manufacturers (such as Mason) list the problem materials on their website and with their literature. Good Luck!
Comment by VicsArt on January 19, 2010 at 8:36pm
I love the Sankey Iron Red glaze effect you have here. The technical expertise is also incredible, so much so that I feel I need to apologise in advance for a "dummy question". I only have access to a community kiln - where cone 6 firings are the norm. I have no control over the soak period and am pretty ignorant with regard to firing processes. Any chance that this glaze would hold up and show its wonderful tones in the circumstances? I'm guessing I will be told to test it - but then, the appeal of this site is that just maybe one can reduce the learning curve by benefiting from the experience of others! Also, I assume that all the consituents of the glaze are food safe if you have chosen the glaze for your dinner service - but maybe there is some ambiguity here. Hope you can tolerate the questions from a relative novice - I seem to be having a lot of difficulty in getting glaze results that I like and would really love some way to speed up my learning curve.

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John Post achieves some spectacular glazes with Iron reds and variations of Jen's Juicy Fruit. He has helpful information at;

Firing Schedules and helping you to get your reds to develop.

Several Iron Red Recipes

Juicy Fruit variations

George thanks for this topic. I read through this and benefited heavily. I modified an tenmoku recipe and added a hold at 1742F for an hour and got some really great results I have attached them below.

Just wanted to say thanks for taking the time to post all this information here as I would have never found it.

Enjoyed the article very much.

Joseph, thats a cool glaze you are working on, I hope you continue and perfect it!!

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