AFm phases

An AFm phase is an "alumina, ferric oxide, monosubstituted" phase, or aluminate ferrite monosubstituted, or Al2O3, Fe2O3 mono, in cement chemist notation (CCN). AFm phases are important hydration products in the hydration of Portland cements and hydraulic cements.

They are crystalline hydrates with generic, simplified, formula 3CaO·(Al,Fe)2O3·CaXy·nH2O,
where:

  • CaO, Al2O3, Fe2O3 represent calcium oxide, aluminium oxide, and ferric oxide, respectively;
  • CaX represents a calcium salt, where X replaces an oxide ion;
  • X is the substituted anion in CaX:
    – divalent  (SO2−4, CO2−3…) with y = 1, or;
    – monovalent (OH−, Cl−…) with y = 2.
  • n represents the number of water molecules in the hydrate and may be comprised between 13 and 19.[1]

AFm form inter alia when tricalcium aluminate 3CaO·Al2O3, or C3A in CCN, reacts with dissolved calcium sulfate (CaSO4), or calcium carbonate (CaCO3). As the sulfate form is the dominant one in AFm phases in the hardened cement paste (HCP) in concrete, AFm is often simply referred to as Aluminate Ferrite monosulfate or calcium aluminate monosulfate. However, carbonate-AFm phases also exist (monocarbonate and hemicarbonate) and are thermodynamically more stable than the sulfate-AFm phase. During concrete carbonation by the atmospheric CO2, sulfate-AFm phase is also slowly transformed into carbonate-AFm phases.

Different AFm phases

AFm phases belong to the class of layered double hydroxides (LDH). LDHs are hydroxides with a double layer structure. The main cation is divalent (M2+) and its electrical charge is compensated by 2 OH− anions: M(OH)2. Some M2+ cations are replaced by a trivalent one (N3+). This creates an excess of positive electrical charges which needs to be compensated by the same number of negative electrical charges born by anions. These anions are located in the space present in between adjacent hydroxide layers. The interlayers in LDHs are also occupied by water molecules accompanying the anions counterbalancing the excess of positive charges created by the cation isomorphic substitution in the hydroxides sheets.

In the most studied class of LDHs, the positive layer (c), consisting of divalent M2+ and trivalent N3+ cations, can be represented by the generic formula:

[M2+
1-xN3+
x(OH−
)2]x+ [(Xn−)x/n · yH
2O]x-
where Xn− is the intercalating anion.

In AFm, the divalent cation is a calcium ion (Ca2+), while the substituting trivalent cation is an aluminium ion (Al3+). The nature of the counterbalancing anion (Xn−) can be very diverse: OH−, Cl−, SO2−4, CO2−3, NO−3, NO−2.[2][3][4] The thickness of the interlayer is sufficient to host a variety of relatively large anions often present as impurities: B(OH)−4, SeO2−4, SeO2−3...[5][6] As other LDHs, AFm can incorporate in their structure toxic elements such as boron[5] and selenium.[6] Some AFm phases are presented in the table here below as a function of the nature of the anion counterbalancing the excess of positive charges in the Ca(OH)2 hydroxide sheets. As in portlandite (Ca(OH)2), the hydroxide sheets of AFm are made of hexa-coordinated octahedral cations located in a same plane, but due to the excess of positive electrical charges, the hydroxide sheets are distorted.

Different AFm phases as a function of the nature of the counterbalancing anion in the LDH structure and its stoichiometry
n AnionAFm nameOxide notationLDH formulaReference
AFm-generic3CaO·Al2O3·CaXy·nH2OCa4Al2Xy(OH)12·(n− 6)H2O—
AFm-monohydrate3CaO·Al2O3·Ca(OH)2·10H2OCa4Al2(OH)14·4H2OHydrocalumite (HBM)[7] (Mindat)[8]
AFm-monosulfate3CaO·Al2O3·CaSO4·12H2OCa4Al2(SO4)(OH)12·6H2ODivet (2000)[9]
AFm-monocarbonate3CaO·Al2O3·CaCO3·11H2OCa4Al2(CO3)(OH)12·5H2ODivet (2000)[9]
AFm-hemicarbonate3CaO·Al2O3·½CaCO3·½Ca(OH)2·11.5H2OCa4Al2(CO3)½(OH)13·5.5H2ODivet (2000)[9]
Friedel's salt3CaO·Al2O3·CaCl2·10H2OCa4Al2Cl2(OH)12·4H2OFriedel (1897)[2]
Kuzel's salts3CaO·Al2O3·½CaSO4·½CaCl2·11H2OCa4Al2(SO4)½Cl(OH)12·5H2OGlasser (1999)[3]
AFm-nitrate3CaO·Al2O3·Ca(NO3)2·10H2OCa4Al2(NO3)2(OH)12·4H2OBalonis & Glasser (2011)[4]
AFm-nitrite3CaO·Al2O3·Ca(NO2)2·10H2OCa4Al2(NO2)2(OH)12·4H2OBalonis & Glasser (2011)[4]

To convert the oxide notation in LDH formula, the mass balance in the system has to respect the principle of the conservation of matter. Oxide ions (O2−) and water are transformed into 2 hydroxide anions (OH−) according to the acid-base reaction between H2O and O2− (a strong base) as typically exemplified by the quicklime (CaO) slaking process:

H2O + O2− ⇌ OH− + OH−,
A1 + B2 ⇌ B1 + A2
or simply,
O2− + H2O ⇌ 2 OH−

AFm structure

AFm phases encompass a class of calcium aluminate hydrates (C-A-H) whose structure derives from that of hydrocalumite:[7][8] 4CaO·Al2O3·13–19H2O, in which OH− anions are partly replaced by SO2−4 or CO2−3 anions.[8] The different mineral phases resulting from these anionic substitutions do not easily form solid solutions but behave as independent phases. The replacement of hydroxide ions by sulfate ions does not exceed 50 mol %. So, AFm does not refer to a single pure mineralogical phase but rather to a mix of several AFm phases co-existing in hydrated cement paste (HCP).[1]

Considering a monovalent anion X, the chemical formula can be rearranged and expressed as 2[Ca2(Al,Fe)(OH)6]·X·nH2O (or Ca4(Al,Fe)2(OH)12·X·nH2O, as presented in the table in the former section). The Me(OH)6 octahedral ions are located in a plane as for calcium or magnesium hydroxides in portlandite or brucite hexagonal sheets respectively. The replacement of one divalent Ca2+ cation by a trivalent Al3+ cation, or to a lesser extent by a Fe3+ cation, with a Ca:Al ratio of 2:1 (one Al substituted for every 3 cations) causes an excess of positive charge in the sheet: 2[2Ca(OH)2·(Al,Fe)(OH)2]+ to be compensated by 2 negative charges X–. The anions X– counterbalancing the positive charge imbalance born by the sheet are located in the interlayer whose spacing is much larger than in the layered structure of brucite or portlandite. This allows the AFm structure to accommodate larger anionic species along with water molecules.[1]

The crystal structure of AFm phases is that of layered double hydroxide (LDH) and AFm phases also exhibit the same anion exchange properties. The carbonate anion (CO2−3) occupies the interlayer space in a privileged way with the highest selectivity coefficient and is more retained in the interlayer than other divalent or monovalent anions such as SO2−4 or OH−.

According to Miyata (1983),[10] the equilibrium constant (selectivity coefficient) for anion exchange varies in the order CO2−3 > HPO2−4 > SO2−4 for divalent anions, and OH− > F− > Cl− > Br− > NO−3 > I− for monovalent anions, but this order is not universal and varies with the nature of the LDH.

Thermodynamic stability

The thermodynamic stability of AFm phases studied at 25 °C depends on the nature of the anion present in the interlayer: CO2−3 stabilises AFm and displaces OH− and SO2−4 anions at their concentrations typically found in hardened cement paste (HCP).[1] Different sources of carbonate can contribute to the carbonation of AFm phases:[1] Addition of limestone filler finely ground, atmospheric CO2, carbonate present as impurity in the gypsum interground with the clinker to avoid cement flash setting, and "alkali sulfates" condensed onto clinker during its cooling, or from added clinker kiln dust.[1] Carbonation can rapidly occur within the fresh concrete during its setting and hardening (internal carbonate sources), or slowly continue in the long-term in the hardened cement paste in concrete exposed to external sources of carbonate: CO2 from the air, or bicarbonate anion (HCO−3) present in groundwater (immersed structures) or clay porewater (foundations and underground structures).

When the carbonate concentration increases in the hardened cement paste (HCP), hydroxy-AFm are progressively replaced, first by hemicarboaluminate and then by monocarboaluminate. The stability of AFm phases increases with their carbonate content as shown by Damidot and Glasser (1995) by means of their thermodynamic calculations of the CaO-Al2O3-SiO2-H2O system at 25 °C.[1][11]

When carbonate displaces sulfate from AFm, the sulfate released in the concrete pore water may react with portlandite (Ca(OH)2) to form ettringite (3CaO·Al2O3·3CaSO4·32H2O), the main AFt phase present in the hydrated cement system.[1]

As stressed by Matschei et al. (2007), the impact of small amounts of carbonate on the nature and stability of the AFm phases is noteworthy.[1] Divet (2000) also notes that micromolar amount of carbonate can inhibit the formation of AFm sulfate, favoring so the crystallisation of ettringite (AFt sulfate).[9]

See also

References
  1. Matschei, T.; Lothenbach, B.; Glasser, F. P. (2007-02-01). "The AFm phase in Portland cement". Cement and Concrete Research. 37 (2): 118–130. doi:10.1016/j.cemconres.2006.10.010. ISSN 0008-8846. Retrieved 2022-02-10.
  2. Friedel, Georges (1897). "Sur un chloro-aluminate de calcium hydraté se maclant par compression". Bulletin de la Société Française de Minéralogie et de Cristallographie. 19: 122–136.
  3. Glasser, F.P.; Kindness, A.; Stronach, S.A. (June 1999). "Stability and solubility relationships in AFm phases". Cement and Concrete Research. 29 (6): 861–866. doi:10.1016/S0008-8846(99)00055-1. ISSN 0008-8846.
  4. Balonis, Magdalena; Mędala, Marta; Glasser, Fredrik P. (July 2011). "Influence of calcium nitrate and nitrite on the constitution of AFm and AFt cement hydrates". Advances in Cement Research. 23 (3): 129–143. doi:10.1680/adcr.10.00002. eISSN 1751-7605. ISSN 0951-7197.
  5. Champenois, Jean-Baptiste; Mesbah, Adel; Cau Dit Coumes, Céline; Renaudin, Guillaume; Leroux, Fabrice; Mercier, Cyrille; Revel, Bertrand; Damidot, Denis (October 2012). "Crystal structures of Boro-AFm and sBoro-AFt phases". Cement and Concrete Research. 42 (10): 1362–1370. doi:10.1016/j.cemconres.2012.06.003. ISSN 0008-8846.
  6. Baur, Isabel; Johnson, C. Annette (November 2003). "The solubility of selenate-AFt (3CaO·Al2O3·3CaSeO4·37.5H2O) and selenate-AFm (3CaO·Al2O3·CaSeO4·xH2O)". Cement and Concrete Research. 33 (11): 1741–1748. doi:10.1016/S0008-8846(03)00151-0. ISSN 0008-8846.
  7. Handbook of mineralogy (2005). "Hydrocalumite" (PDF). handbookofmineralogy.org. Retrieved 19 April 2023.
  8. Mindat (3 April 2023). "Hydrocalumite". mindat.org. Retrieved 19 April 2023.
  9. Divet, Loïc (2000). "Etat des connaissances sur les causes possibles des réactions sulfatiques internes au béton" (PDF). Bulletin de Liaison des Laboratoires des Ponts et Chaussées. 227: 71–84.
  10. Miyata, Shigeo (1983-08-01). "Anion-exchange properties of hydrotalcite-like compounds". Clays and Clay Minerals. 31 (4): 305–311. Bibcode:1983CCM....31..305M. doi:10.1346/CCMN.1983.0310409. ISSN 1552-8367.
  11. Damidot, D.; Glasser, F.P. (January 1995). "Investigation of the CaO-Al2O3-SiO2-H2O system at 25 °C by thermodynamic calculations". Cement and Concrete Research. 25 (1): 22–28. doi:10.1016/0008-8846(94)00108-B. ISSN 0008-8846.

Further reading


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