The name was given by Törnebohm in 1897 to a crystal identified in microscopic investigation of Portland cement. Belite is a name in common use in the cement industry, but is not a recognised mineral name. It occurs naturally as the mineral larnite, the name being derived from Larne, Northern Ireland, the closest town to Scawt Hill where it was discovered.
Composition and structure
The belite found in Portland cement differs in composition from pure dicalcium silicate. It is a solid solution and contains minor amounts of other oxides besides CaO and SiO2. A typical composition:
Based on this, the formula can be expressed as Ca1.94Mg0.02Na0.01K0.03Fe0.02Al0.07Si0.90P0.01O3.93. In practice, the composition varies with the bulk composition of the clinker, subject to certain limits. Substitution of calcium ions or orthosilicate ions requires that electric charges be kept in balance. For instance, a limited number of orthosilicate (SiO44−) ions can be replaced with sulfate (SO42−) ions, provided that for each sulfate ion, two aluminate (AlO45−) ions are also substituted.
Dicalcium silicate is stable, and is readily prepared from reactive CaO and SiO2 at 300 °C. The low temperature form is γ-belite, or lime olivine. This form does not hydrate, and is avoided in cement manufacture.
As the temperature rises, it passes through several polymorphic states:
Belite is the mineral in Portland cement responsible for development of "late" strength. The other silicate, alite contributes "early" strength, due to its higher reactivity. Belite reacts with water (roughly) to form calcium silicate hydrates (C-S-H) and portlandite (Ca(OH)2) according to the reaction:
This rapid reaction is "chemically analogue" to the slow natural hydration of forsterite (the magnesium end-member of olivine) leading to the formation of serpentine and brucite in nature, although the kinetic of hydration of poorly crystallized artificial belite is much faster than the slow weathering of well crystallized Mg-olivine under natural conditions.
The hydrate phase, [3 CaO · 2 SiO2 · 3 H2O], is referred to as the "C-S-H" phase. It grows as a mass of interlocking needles that provide the strength of the hydrated cement system. Relatively high belite reactivity is desirable in Portland cement manufacture, and the formation of the unreactive γ-form must be rigorously avoided. This is achieved by rapid cooling, forming crystals that are small, distorted and highly defective. Defects provide sites for initial water attack. Failure to cool the clinker rapidly leads to inversion of belite to the γ-form. The γ-form has a substantially different structure and density, so that inversion leads to degradation of the crystal and its surrounding matrix, and can also trigger decomposition of the neighboring alite. This is observed macroscopically as "dusting": the clinker nodules fall to a fine dust.
The minerals in Portland cement clinker may be observed and quantified by petrographic microscopy. Clinker nodules are cut and ground to a flat, polished surface. The exposed minerals are made visible and identifiable by etching the surface. The surface can then be observed in reflected light by optical microscopy. In the example, a clinker nodule has been polished and etched with hydrogen fluoride vapour. The alite shows as brown, the belite as blue, and the melt phases as white. Electron microscopy can also be used, in which case the minerals may be identified by microprobe analysis. The preferred method to quantify the minerals accurately is X-ray diffraction on the powdered clinker, using the Rietveld analysis technique. Belite is much harder to grind in a cement mill than alite.
- Hydration reaction of forsterite (olivine) in serpentinisation
- CCN, cement chemist notation
- Jean-Pierre Bournazel, Yves Malier, Micheline Moranville Regourd, 1998, Concrete, from Material to Structure RILEM Publications, ISBN 2-912143-04-7.
- Deer, William Alexander; Howie, R. A; Zussman, J (1997-05-01). "Larnite". Disilicates and ring silicates. pp. 248–249. ISBN 9781897799895.
- Taylor H.F.W. (1990), Cement Chemistry, Academic Press, 1990, ISBN 0-12-683900-X, pp. 10-11.