Sorel cement

Sorel cement (also known as magnesia cement or magnesium oxychloride) is a non-hydraulic cement first produced by the French chemist Stanislas Sorel in 1867.[1]

In fact, in 1855, before working with magnesium compounds, Stanislas Sorel first developed a two-component cement by mixing zinc oxide powder with a solution of zinc chloride.[2][3] In a few minutes he obtained a dense material harder than limestone.

Only a decade later, Sorel replaced zinc with magnesium in his formula and also obtained a cement with similar favorable properties. This new type of cement was stronger and more elastic than Portland cement, and therefore exhibited a more resilient behavior when submitted to shocks. The material could be easily molded like plaster when freshly prepared, or machined on a lathe after setting and hardening. It was very hard, could be easily bound to many different types of materials (good adhesive properties), and colored with pigments. Therefore, it was used to make mosaics and to mimic marble. After mixing with cotton crushed in powder, it was also used as a surrogate material for ivory to fabricate billiard balls resistant to shock. [4]

Sorel cement is a mixture of magnesium oxide (burnt magnesia) with magnesium chloride with the approximate chemical formula Mg4Cl2(OH)6(H2O)8, or MgCl2·3Mg(OH)2·8H2O, corresponding to a weight ratio of 2.5–3.5 parts MgO to one part MgCl2.[5]

Quite surprisingly, much more recently, another chemist, Charles A. Sorrell (1977, 1980) – whose family name sounds quite similar to that of Stanislas Sorel – also studied the topic and published works on the same family of oxychloride compounds based on zinc and magnesium, just as Sorel had done about 100 years before. The zinc oxychloride cement is prepared from zinc oxide and zinc chloride instead of the magnesium compounds.[6][7]

Composition and structure

The set cement consists chiefly of a mixture of magnesium oxychlorides and magnesium hydroxide in varying proportions, depending on the initial cement formulation, setting time, and other variables. The main stable oxychlorides at ambient temperature are the so-called "phase 3" and "phase 5", whose formulas can be written as 3Mg(OH)
2·MgCl
2·8H
2O and 5Mg(OH)
2·MgCl
2·8H
2O, respectively; or, equivalently, Mg
2(OH)
3Cl·4H
2O and Mg
3(OH)
5Cl·4H
2O.[8]

Phase 5 crystallizes mainly as long needles which are actually rolled-up sheets. These interlocking needles give the cement its strength.[9]

In the long term the oxychlorides absorb and react with carbon dioxide CO
2 from the air to form magnesium chlorocarbonates.[10]

History

These compounds are the primary components of matured Sorel cement, first prepared in 1867 by Stanislas Sorel.[1]

In the late 19th century, several attempts were made to determine the composition of the hardened Sorel's cement, but the results were not conclusive.[11][12][13][14] Phase 3 was properly isolated and described by Robinson and Waggaman (1909),[11] and phase 5 was identified by Lukens (1932).[15]

Properties

Sorel cement can withstand 10,000–12,000 psi (69–83 MPa) of compressive force whereas standard Portland cement can typically only withstand 7,000–8,000 psi (48–55 MPa). It also achieves high strength in a shorter time.[16]

Sorel cement has a remarkable capacity to bond with, and contain, other materials. It also exhibits some elasticity, an interesting property increasing its capacity to resist shocks (better mechanical resilience), particularly useful for billiard balls.

The pore solution in wet Sorel cement is slightly alkaline (pH 8.5 to 9.5), but significantly less so than that of Portland cement (hyperalkaline conditions: pH 12.5 to 13.5).[17]

Other differences between magnesium-based cements and portland cement include water permeability, preservation of plant and animal substances, and corrosion of metals.[18] These differences make different construction applications suitable.[19]

Prolonged exposure of Sorel cement to water leaches out the soluble MgCl
2, leaving hydrated brucite Mg(OH)
2 as the binding phase, which without absorption of CO
2, can result in loss of strength.[17]

Fillers and reinforcement

In use, Sorel cement is usually combined with filler materials such as gravel, sand, marble flour, asbestos, wood particles and expanded clays.[20]

Sorel cement is incompatible with steel reinforcement because the presence of chloride ions in the pore solution and the low alkalinity (pH < 9) of the cement promote steel corrosion (pitting corrosion).[17] However, the low alkalinity makes it more compatible with glass fiber reinforcement.[20] It is also better than Portland cement as a binder for wood composites, since its setting is not retarded by the lignin and other wood chemicals.[20]

The resistance of the cement to water can be improved with the use of additives such as phosphoric acid, soluble phosphates, fly ash, or silica.[17]

Uses

Magnesium oxychloride cement is used to make floor tiles and industrial flooring, in fire protection, wall insulation panels, and as a binder for grinding wheels.[20] Due to its resemblance to marble, it is also used for artificial stones,[20] artificial ivory (e.g. for billiard balls) and other similar purposes.

Sorel cement is also studied as a candidate material for chemical buffers and engineered barriers (drift seals made of salt-concrete) for deep geological repositories of high-level nuclear waste in salt-rock formations (Waste Isolation Pilot Plant (WIPP) in New Mexico, USA; Asse II salt mine, Gorleben and Morsleben in Germany).[21][22][23] Phase 5 of the magnesium oxychloride could be a useful complement, or replacement, for MgO (periclase) presently used as a CO
2 getter in the WIPP disposal chambers to limit the solubility of minor actinides carbonate complexes, while establishing moderately alkaline conditions (pH: 8.5–9.5) still compatible with the undisturbed geochemical conditions initially prevailing in situ in the salt formations. The much more soluble calcium oxide and hydroxide (portlandite) are not authorized in WIPP (New Mexico) because they would impose a too high pH (12.5). As Mg2+
 is the second most-abundant cation present in sea water after Na+
, and that magnesium compounds are less soluble than these of calcium, magnesium-based buffer materials and Sorel cement are considered more appropriate backfil materials for radioactive waste disposal in deep salt formations than common calcium-based cements (Portland cement and their derivatives). Moreover, as magnesium hydroxychloride is also a possible pH buffer in marine evaporite brines, Sorel cement is expected to less disturb initial in situ conditions prevailing in deep salts formations.[24]

Preparation

Sorel cement is usually prepared by mixing finely divided MgO powder with a concentrated solution of MgCl
2.[17]

In theory, the ingredients should be combined in the molar proportions of phase 5, which has the best mechanical properties. However, the chemical reactions that create the oxychlorides may not run to completion, leaving unreacted MgO particles and/or MgCl
2 in pore solution. While the former act as an inert filler, leftover chloride is undesirable since it promotes corrosion of steel in contact with the cement. Excess water may also be necessary to achieve a workable consistency. Therefore, in practice the proportions of magnesium oxide and water in the initial mix are higher than those in pure phase 5.[20] In one study, the best mechanical properties were obtained with a molar ratio MgO:MgCl
2 of 13:1 (instead of the stoichiometry 5:1).[20]

Production

Periclase (MgO) and magnesite (MgCO
3) are not abundant raw materials, so their manufacture into Sorel cement is expensive and limited to specialized niche applications requiring modest materials quantities. China is the dominant supplier of raw materials for the production of magnesium oxide and derivatives. Magnesium-based "green cements" derived from the more abundant dolomite ((Ca,Mg)(CO
3)
2) deposits (dolostone), but also containing 50 wt. % calcium carbonate, have not to be confused with the original Sorel cement, as this later does not contain calcium oxide. Indeed, Sorel cement is a pure magnesium oxychloride.

See also

References
  1. Sorel Stanislas (1867). "Sur un nouveau ciment magnésien". Comptes Rendus Hebdomadaires des Séances de l'Académie des Sciences, volume 65, pages 102–104.
  2. Sorel Stanislas (1856). Procédé pour la formation d'un ciment très-solide par l'action d'un chlorure sur l'oxyde de zinc. Bulletin de la Société d'Encouragement pour l'Industrie Nationale, 55, 51–53.
  3. Souchu, Philippe (2012-04-18). "Le ciment Sorel". Site documentaire du Lerm. Retrieved 2020-07-08.
  4. Chevalier, Michel (1868). "Exposition Universelle de 1867 à Paris. Rapports du Jury international, Tome dixième, Groupe VI, Arts Usuels – Classes 65 – Section I, Chapitre 3 – Matériaux artificiels, § 5 – Ciment d'oxychlorure de magnésium, 80–83". archive.org/. Imprimerie Administrative de Paul Dupont, Paris. Retrieved 2020-07-08.
  5. Holleman, A. F.; Wiberg, E. (2001). "Inorganic Chemistry". Academic Press, San Diego. ISBN 0-12-352651-5.
  6. Sorrell, Charles A. (1977). "Suggested chemistry of zinc oxychloride cements". Journal of the American Ceramic Society. 60 (5–6): 217–220. doi:10.1111/j.1151-2916.1977.tb14109.x. ISSN 0002-7820.
  7. Urwongse, Ladawan; Sorrell, Charles A. (1980). "The system MgO-MgCl2-H2O at 23 °C". Journal of the American Ceramic Society. 63 (9–10): 501–504. doi:10.1111/j.1151-2916.1980.tb10752.x. ISSN 0002-7820.
  8. Isao Kanesaka and Shin Aoyama (2001). "Vibrational spectra of magnesia cement, phase 3". Journal of Raman Spectroscopy, volume 32, issue 5, pages 361-367. doi:10.1002/jrs.706
  9. B. Tooper and L. Cartz (1966). "Structure and Formation of Magnesium Oxychloride Sorel Cements". Nature, volume 211, pages 64–66. doi:10.1038/211064a0
  10. W. F. Cole and T. Demediuk (1955). "X-Ray, thermal, and Dehydration studies on Magnesium oxychlorides". Australian Journal of Chemistry, volume 8, issue 2, pages 234-251. doi:10.1071/CH9550234
  11. W. O. Robinson and W. H. Waggaman (1909): "Basic magnesium chlorides". Journal of Physical Chemistry, volume 13, issue 9, pages 673–678. doi:10.1021/j150108a002
  12. Davis J.W.C. (1872). "Composition of Crystalline Deposit from a Solution of Magnesium and Ammonium Chloride". The Chemical News and Journal of Physical Science, volume 25, page 258.
  13. Otto Krause (1873): "Ueber Magnesiumoxychlorid". Annalen der Chemie und Pharmacie, volume 165, pages 38–44.
  14. André G.M. (1882). "Sur les oxychlorures de magnésium". Comptes Rendus Hebdomadaires des Séances de l'Académie des sciences, volume 94, pages 444–446.
  15. Lukens H.S. (1932). "The composition of magnesium oxychloride". Journal of the American Chemical Society, volume 54, issue 6, pages 2372–2380. doi:10.1021/ja01345a026
  16. Ronan M. Dorrepaal and Aoife A. Gowen (2018). "Identification of magnesium oxychloride cement biomaterial heterogeneity using Raman chemical mapping and NIR hyperspectral chemical imaging". Scientific Reports, volume 8, article number 13034. doi:10.1038/s41598-018-31379-5
  17. Amal Brichni, Halim Hammi, Salima Aggoun, and M'nif Adel (2016). "Optimization of magnesium oxychloride cement properties by silica glass". Advances in Cement Research (Springer conference proceedings). doi:10.1680/jadcr.16.00024
  18. "Karthikeyan N., Sathishkumar A., and Dennis Joseph Raj W. (2014). Effects on setting, strength and water resistance of Sorel cement on mixing fly ash as an additive. International Journal of Mechanical Engineering and Robotics Research, Vol. 3, N° 2, 251–256" (PDF).
  19. Du, Chongjiang (1 December 2005). "A review of magnesium oxide in concrete". Concrete International. 27 (12).
  20. Zongjin Li and C. K. Chau (2007). "Influence of molar ratios on properties of magnesium oxychloride cement". Cement and Concrete Research, volume 37, issue 6, pages 866-870. doi:10.1016/j.cemconres.2007.03.015
  21. Walling, Sam A.; Provis, John L. (2016). "Magnesia-based cements: A journey of 150 years, and cements for the future?". Chemical Reviews. 116 (7): 4170–4204. doi:10.1021/acs.chemrev.5b00463. ISSN 0009-2665. PMID 27002788.
  22. US-DOE (2016). "Proceedings of the 6th US/German Workshop on Salt Repository Research, Design, and Operation, January 11, 2016" (PDF). www.energy.gov/. US-DOE. Retrieved 2020-07-12.
  23. Xiong, Yongliang; Deng, Haoran; Nemer, Martin; Johnsen, Shelly (2010). "Experimental determination of the solubility constant for magnesium chloride hydroxide hydrate (Mg
    3    Cl(OH)
    5    ·4H
    2    O    , phase 5) at room temperature, and its importance to nuclear waste isolation in geological repositories in salt formations". Geochimica et Cosmochimica Acta. 74 (16): 4605–4611. doi:10.1016/j.gca.2010.05.029. ISSN 0016-7037.
  24. Bodine, M. W. Jr. (1976). "Magnesium hydroxychloride: A possible pH buffer in marine evaporite brines?" Geology, volume 4, issue 2, 76–80. doi:10.1130/0091-7613(1976)4<76:MHAPPB>2.0.CO;2
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.