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Ettringite is a hydrous calciumaluminiumsulfate mineral with formula: Ca6Al2(SO4)3(OH)12·26H2O. It is a colorless to yellow mineral crystallizing in the trigonalsystem. The prismatic crystals are typically colorless, turning white on partial dehydration.[3][4] It is part of the ettringite-group which includes other sulfates such as thaumasite and bentorite.[5]
Ettringite was first described in 1874 by J. Lehmann,[6] for an occurrence near the Ettringer Bellerberg Volcano, Ettringen, Rheinland-Pfalz, Germany.[3][4] It occurs within metamorphically altered limestone adjacent to igneous intrusive rocks or within xenoliths. It also occurs as weathering crusts on larnite in the Hatrurim Formation of Israel.[3] It occurs associated with portlandite, afwillite and hydrocalumite at Scawt Hill, Ireland and with afwillite, hydrocalumite, mayenite and gypsum in the Hatrurim Formation.[3] It has also been reported from the Zeilberg quarry, Maroldsweisach, Bavaria; at Boisséjour, near Clermont-Ferrand, Puy-de-Dôme, Auvergne, France; the N’Chwaning mine, Kuruman district, Cape Province, South Africa; in the US, occurrences were found in spurrite-merwinite-gehleniteskarn at the 910 level of the Commercial quarry, Crestmore, Riverside County, California[7] and in the Lucky Cuss mine, Tombstone, Arizona.[3][4]
Ettringite is also sometimes referred in the ancient French literature as Candelot salt, or Candlot salt.[8]
In concrete chemistry, ettringite is a hexacalcium aluminate trisulfate hydrate, of general formula when noted as oxides:
or
Ettringite is formed in the hydrated Portland cement system as a result of the reaction of tricalcium aluminate (C3A) with calcium sulfate, both present in Portland cement.[9]
The addition of gypsum (CaSO4·2H2O) to clinker during the grinding operation to obtain the crushed powder of Portland cement is essential to avoid the flash setting of concrete during its early hydration. Indeed, the tricalcium aluminate (C3A) is the most reactive phase of the four main mineral phases present in Portland cement (C3S, C2S, C3A, and C4AF). C3A hydration is very exothermic and also occurs very fast in the fresh concrete mix as the temperature quickly increases with the progress of the hydration reaction. The effect of gypsum addition is to promote the formation of a thin impervious film of ettringite at the surface of the C3A grains, passivating their surface, and so slowing down their hydration.[10] The addition of gypsum to Portland cement is needed to control the concrete setting.[10]
Ettringite, the most prominent representative of AFt phases or (Al2O3 − Fe2O3 − tri), can also be synthesized in aqueous solution by reacting stoichiometric amounts of calcium oxide, aluminium oxide, and sulfate.
In the cement system, the presence of ettringite depends on the ratio of calcium sulfate to tri-calcium aluminate (C3A); when this ratio is low, ettringite forms during early hydration and then converts to the calcium aluminate monosulfate (AFm phases or (Al2O3 − Fe2O3 − mono)). When the ratio is intermediate, only a portion of the ettringite converts to AFm and both can coexist, while ettringite is unlikely to convert to AFm at high ratios.
The following standard abbreviations are used to designate the different oxide phases in the cement chemist notation (CCN):[11]
The mineral ettringite has a structure that runs parallel to the c axis – the needle axis – in the middle of these two lie the sulfate ions and H2O molecules, the space group is P31c. Ettringite crystal system is trigonal, crystals are elongated and in a needle like shape, occurrence of disorder or twining is common, which affects the intercolumn material.[12] The first X-ray diffraction crystallographic study was done by Bannister, Hey and Bernal (1936), which found that the crystal unit cell is of a hexagonal form with a = 11.26 and c = 21.48 with space group P63/mmc and Z = 2, where Z is a number of formula units per unit cell. From observations on dehydration and chemical formulas there were suggestions of the structure being composed of Ca2+ and Al(OH)3−6, were between them lie SO2−4 ions and H2O molecules. Further X-ray studies ensued; namely Wellin (1956) which determined the crystal structure of thaumasite, and Besjak and Jelenic (1966) which gave confirmation of the structure nature of ettringite.[12]
An ettringite sample extracted from Scawt Hill was analysed by C. E. Tilley, the crystal was 1.1 × 0.8 × 0.5 mm, with specific gravity of 1.772±0.002, possessed five prism faces of the form m{1010} and a small face a{1120}, with no pyramidal or basal faces. Upon X-ray diffraction a Laue diagram along the c-axis revealed a hexagonal axis with vertical planes of symmetry, this study showed that the structure has a hexagonal and not a rhombohedral lattice.[13] Further studies conducted on synthetic ettringite by use of X-ray and powder diffraction confirmed earlier assumptions and analyses.[14]
Upon analyzing the structure of both ettringite and thaumasite, it was deduced that both minerals have hexagonal structures, but different space groups.
Ettringite crystals have a P31c with a = 11.224 Å, c = 21,108 Å, while thaumasite crystals fall into space group P63 with a=11.04 Å, c=10.39 Å While these two minerals form a solid solution, the difference in space groups lead to discontinuities in unit cell parameters Differences between structures of ettringite and thaumasite arise from the columns of cations and anions Ettringite cation columns are composed of Ca3[Al(OH)6·12H2O]3+, which run parallel to the c axis, and the other columns of sulfate anions and water molecules in channels parallel to these columns In contrast, thaumasite containing a hexacoordinated silicon complex of Si(OH)2–6 (a rare octahedral configuration for Si) consists of a cylindrical column of Ca3[Si(OH)6·12H2O]4+ in the c axis, with sulfate and carbonate anions in channels between these columns which contain water molecules as well.[15]
Ongoing research on ettringite and cement phase minerals is performed to find new ways to immobilize toxic anions (e.g., borate, selenate and arsenate) and heavy metals to avoid their dispersion in soils and the environment; this can be achieved by using the proper cement phases whose crystal lattice can accommodate these elements. For example, copper immobilization at high pH can be achieved through the formation of C-S-H/C-A-H and ettringite.[16] The crystal structure of ettringite Ca6Al2(SO4)3(OH)12·26H2O can incorporate a variety of divalent ions: Cu2+, Pb2+, Cd2+ and Zn2+, which can substitute for Ca2+.[16]