Water of crystallization

In chemistry, water(s) of crystallization or water(s) of hydration are watermolecules that are present inside crystals. Water is often incorporated in the formation of crystals from aqueous solutions.[1] In some contexts, water of crystallization is the total mass of water in a substance at a given temperature and is mostly present in a definite (stoichiometric) ratio. Classically, "water of crystallization" refers to water that is found in the crystalline framework of a metal complex or a salt, which is not directly bonded to the metal cation.

Upon crystallization from water, or water-containing solvents, many compounds incorporate water molecules in their crystalline frameworks. Water of crystallization can generally be removed by heating a sample but the crystalline properties are often lost.

Compared to inorganic salts, proteins crystallize with large amounts of water in the crystal lattice. A water content of 50% is not uncommon for proteins.

Applications

Knowledge of hydration is essential for calculating the masses for many compounds. The reactivity of many salt-like solids is sensitive to the presence of water. The hydration and dehydration of salts is central to the use of phase-change materials for energy storage.[2]

Position in the crystal structure

Some hydrogen-bonding contacts in FeSO4·7H2O. This metal aquo complex crystallizes with water of hydration, which interacts with the sulfate and with the [Fe(H2O)6]2+ centers.

A salt with associated water of crystallization is known as a hydrate. The structure of hydrates can be quite elaborate, because of the existence of hydrogen bonds that define polymeric structures.[3][4] Historically, the structures of many hydrates were unknown, and the dot in the formula of a hydrate was employed to specify the composition without indicating how the water is bound. Per IUPAC's recommendations, the middle dot is not surrounded by spaces when indicating a chemical adduct.[5] Examples:

  • CuSO4·5H2O – copper(II) sulfate pentahydrate
  • CoCl2·6H2O – cobalt(II) chloride hexahydrate
  • SnCl2·2H2O – tin(II) (or stannous) chloride dihydrate

For many salts, the exact bonding of the water is unimportant because the water molecules are made labile upon dissolution. For example, an aqueous solution prepared from CuSO4·5H2O and anhydrous CuSO4 behave identically. Therefore, knowledge of the degree of hydration is important only for determining the equivalent weight: one mole of CuSO4·5H2O weighs more than one mole of CuSO4. In some cases, the degree of hydration can be critical to the resulting chemical properties. For example, anhydrous RhCl3 is not soluble in water and is relatively useless in organometallic chemistry whereas RhCl3·3H2O is versatile. Similarly, hydrated AlCl3 is a poor Lewis acid and thus inactive as a catalyst for Friedel-Crafts reactions. Samples of AlCl3 must therefore be protected from atmospheric moisture to preclude the formation of hydrates.

Structure of the polymeric [Ca(H2O)6]2+ center in crystalline calcium chloride hexahydrate. Three water ligands are terminal, three bridge. Two aspects of metal aquo complexes are illustrated: the high coordination number typical for Ca2+ and the role of water as a bridging ligand.

Crystals of hydrated copper(II) sulfate consist of [Cu(H2O)4]2+ centers linked to SO2−4 ions. Copper is surrounded by six oxygen atoms, provided by two different sulfate groups and four molecules of water. A fifth water resides elsewhere in the framework but does not bind directly to copper.[6] The cobalt chloride mentioned above occurs as [Co(H2O)6]2+ and Cl−. In tin chloride, each Sn(II) center is pyramidal (mean O/Cl−Sn−O/Cl angle is 83°) being bound to two chloride ions and one water. The second water in the formula unit is hydrogen-bonded to the chloride and to the coordinated water molecule. Water of crystallization is stabilized by electrostatic attractions, consequently hydrates are common for salts that contain +2 and +3 cations as well as −2 anions. In some cases, the majority of the weight of a compound arises from water. Glauber's salt, Na2SO4(H2O)10, is a white crystalline solid with greater than 50% water by weight.

Consider the case of nickel(II) chloride hexahydrate. This species has the formula NiCl2(H2O)6. Crystallographic analysis reveals that the solid consists of [trans-NiCl2(H2O)4] subunits that are hydrogen bonded to each other as well as two additional molecules of H2O. Thus one third of the water molecules in the crystal are not directly bonded to Ni2+, and these might be termed "water of crystallization".

Analysis

The water content of most compounds can be determined with a knowledge of its formula. An unknown sample can be determined through thermogravimetric analysis (TGA) where the sample is heated strongly, and the accurate weight of a sample is plotted against the temperature. The amount of water driven off is then divided by the molar mass of water to obtain the number of molecules of water bound to the salt.

Other solvents of crystallization

Water is a particularly common solvent to be found in crystals because it is small and polar. But many other solvents can be hosted in crystals, known as solvates.[7][8] Water is noteworthy because it is reactive, whereas other solvents such as benzene are considered to be chemically innocuous. Occasionally more than one solvent is found in a crystal, and often the stoichiometry is variable, reflected in the crystallographic concept of "partial occupancy". It is common and conventional for a chemist to "dry" a sample with a combination of vacuum and heat "to constant weight".

For other solvents of crystallization, analysis is conveniently accomplished by dissolving the sample in a deuterated solvent and analyzing the sample for solvent signals by NMR spectroscopy. Single crystal X-ray crystallography is often able to detect the presence of these solvents of crystallization as well. Other methods may be currently available.

Table of crystallization water in some inorganic halides

In the table below are indicated the number of molecules of water per metal in various salts.[9][10]

Hydrated metal halidesand their formulasCoordination sphereof the metalEquivalents of water of crystallization that are not bound to MRemarks
Calcium chlorideCaCl2(H2O)6[Ca(μ-H2O)6(H2O)3]2+0 example of water as a bridging ligand[11]
Calcium bromideCaBr2(H2O)9[Ca(H2O)8]2+1the most hydrated calcium halide[12]
Calcium iodideCaI2(H2O)7[Ca(H2O)8]2+[12]0bridging water ligands
Calcium iodideCaI2(H2O)8[Ca(H2O)8]2+[12]0
Calcium iodideCaI2(H2O)6.5[Ca(H2O)8]2+[12]0bridging water ligands
Titanium(III) chlorideTiCl3(H2O)6trans-[TiCl2(H2O)4]+[13]2isomorphous with VCl3(H2O)6
Titanium(III) chlorideTiCl3(H2O)6[Ti(H2O)6]3+[13]noneisomeric with [TiCl2(H2O)4]Cl.2H2O[14]
Zirconium(IV) fluorideZrF4(H2O)3(μ−F)2[ZrF3(H2O)3]2nonerare case where Hf and Zr differ[15]
Hafnium tetrafluorideHfF4(H2O)3(μ−F)2[HfF2(H2O)2]n(H2O)n1rare case where Hf and Zr differ[15]
Vanadium(III) chlorideVCl3(H2O)6trans-[VCl2(H2O)4]+[13]2
Vanadium(III) bromideVBr3(H2O)6trans-[VBr2(H2O)4]+[13]2
Vanadium(III) iodideVI3(H2O)6[V(H2O)6]3+nonerelative to Cl− and Br−, I− competes poorly with water as a ligand for V(III)
Nb6Cl14(H2O)8[Nb6Cl14(H2O)2]4
Chromium(III) chlorideCrCl3(H2O)6trans-[CrCl2(H2O)4]+2dark green isomer, aka "Bjerrums's salt"
Chromium(III) chlorideCrCl3(H2O)6[CrCl(H2O)5]2+1blue-green isomer
Chromium(II) chlorideCrCl2(H2O)4trans-[CrCl2(H2O)4]nonesquare planar/tetragonal distortion
Chromium(III) chlorideCrCl3(H2O)6[Cr(H2O)6]3+noneviolet isomer. isostructural with aluminium compound[16]
Manganese(II) chlorideMnCl2(H2O)6trans-[MnCl2(H2O)4]2
Manganese(II) chlorideMnCl2(H2O)4cis-[MnCl2(H2O)4]nonecis molecular, the unstable trans isomer has also been detected[17]
Manganese(II) bromideMnBr2(H2O)4cis-[MnBr2(H2O)4]nonecis, molecular
Manganese(II) iodideMnI2(H2O)4trans-[MnI2(H2O)4]nonemolecular, isostructural with FeCl2(H2O)4.[18]
Manganese(II) chlorideMnCl2(H2O)2trans-[MnCl4(H2O)2]nonepolymeric with bridging chloride
Manganese(II) bromideMnBr2(H2O)2trans-[MnBr4(H2O)2]nonepolymeric with bridging bromide
Rhenium(III) chlorideRe3Cl9(H2O)4triangulo-[Re3Cl9(H2O)3]noneheavy early metals form M-M bonds[19]
Iron(II) chlorideFeCl2(H2O)6trans-[FeCl2(H2O)4]two
Iron(II) chlorideFeCl2(H2O)4trans-[FeCl2(H2O)4]nonemolecular
Iron(II) bromideFeBr2(H2O)4trans-[FeBr2(H2O)4]nonemolecular,[20] hydrates of FeI2 are not known
Iron(II) chlorideFeCl2(H2O)2trans-[FeCl4(H2O)2]nonepolymeric with bridging chloride
Iron(III) chlorideFeCl3(H2O)6trans-[FeCl2(H2O)4]+twoone of four hydrates of ferric chloride,[21] isostructural with Cr analogue
Iron(III) chlorideFeCl3(H2O)2.5cis-[FeCl2(H2O)4]+twothe dihydrate has a similar structure, both contain FeCl−4 anions.[21]
Cobalt(II) chlorideCoCl2(H2O)6trans-[CoCl2(H2O)4]two
Cobalt(II) bromideCoBr2(H2O)6trans-[CoBr2(H2O)4]two
Cobalt(II) iodideCoI2(H2O)6[Co(H2O)6]2+none[22]iodide competes poorly with water
Cobalt(II) bromideCoBr2(H2O)4trans-[CoBr2(H2O)4]nonemolecular[20]
Cobalt(II) chlorideCoCl2(H2O)4cis-[CoCl2(H2O)4]nonenote: cis molecular
Cobalt(II) chlorideCoCl2(H2O)2trans-[CoCl4(H2O)2]nonepolymeric with bridging chloride
Cobalt(II) bromideCoBr2(H2O)2trans-[CoBr4(H2O)2]nonepolymeric with bridging bromide
Nickel(II) chlorideNiCl2(H2O)6trans-[NiCl2(H2O)4]two
Nickel(II) chlorideNiCl2(H2O)4cis-[NiCl2(H2O)4]nonenote: cis molecular[20]
Nickel(II) bromideNiBr2(H2O)6trans-[NiBr2(H2O)4]two
Nickel(II) iodideNiI2(H2O)6[Ni(H2O)6]2+none[22]iodide competes poorly with water
Nickel(II) chlorideNiCl2(H2O)2trans-[NiCl4(H2O)2]nonepolymeric with bridging chloride
Platinum(IV) chloride[Pt(H2O)2Cl4](H2O)3[23]trans-[PtCl4(H2O)2]3octahedral Pt centers; rare example of non-first row chloride-aquo complex
Platinum(IV) chloride[Pt(H2O)3Cl3]Cl(H2O)0.5[24]fac-[PtCl3(H2O)3]+0.5octahedral Pt centers; rare example of non-first row chloride-aquo complex
Copper(II) chlorideCuCl2(H2O)2[CuCl4(H2O)2]2nonetetragonally distorted two long Cu-Cl distances
Copper(II) bromideCuBr2(H2O)4[CuBr4(H2O)2]ntwotetragonally distorted two long Cu-Br distances[20]
Zinc(II) chlorideZnCl2(H2O)1.33[25]2 ZnCl2 + ZnCl2(H2O)4nonecoordination polymer with both tetrahedral and octahedral Zn centers
Zinc(II) chlorideZnCl2(H2O)2.5[26][27]Cl3Zn(μ-Cl)Zn(H2O)5nonetetrahedral and octahedral Zn centers
Zinc(II) chlorideZnCl2(H2O)3[25][26][ZnCl4]2− & [Zn(H2O)6]2+nonetetrahedral and octahedral Zn centers
Zinc(II) chlorideZnCl2(H2O)4.5[ZnCl4]2− & [Zn(H2O)6]2+threetetrahedral and octahedral Zn centers[26][25]
Cadmium chlorideCdCl2·H2O[28]nonewater of crystallization is rare for heavy metal halides
Cadmium chlorideCdCl2·2.5H2O[29]CdCl5(H2O) & CdCl4(H2O)2none
Cadmium chlorideCdCl2·4H2O[30]CdCl4(H2O)4twooctahedral, doubly bridging chlorides
Cadmium bromideCdBr2(H2O)4[31][CdBr4(H2O)2twooctahedral Cd centers
Aluminum trichlorideAlCl3(H2O)6[Al(H2O)6]3+noneisostructural with the Cr(III) compound
Aluminum triiodideAlI3(H2O)6[Al(H2O)6]3+noneother hydrates are known[32]
Aluminum triiodideAlI3(H2O)15[Al(H2O)6]3+9other hydrates are known[32]
Aluminum triiodideAlI3(H2O)17[Al(H2O)6]3+11the highest hydrate crystallized[32]

Hydrates of metal sulfates

Transition metal sulfates form a variety of hydrates, each of which crystallizes in only one form. The sulfate group often binds to the metal, especially for those salts with fewer than six aquo ligands. The heptahydrates, which are often the most common salts, crystallize as monoclinic and the less common orthorhombic forms. In the heptahydrates, one water is in the lattice and the other six are coordinated to the ferrous center.[33] Many of the metal sulfates occur in nature, being the result of weathering of mineral sulfides.[34][35] Many monohydrates are known.[36]

Formula of hydrated metal ion sulfateCoordinationsphere of the metal ionEquivalents of water of crystallization that are not bound to Mmineral nameRemarks
MgSO4(H2O)[Mn(μ-H2O)(μ4,-κ1-SO4)4][36]nonekieseritesee Mn, Fe, Co, Ni, Zn analogues
Substructure of MSO4(H2O), illustrating presence of bridging water and bridging sulfate (M = Mg, Mn, Fe, Co, Ni, Zn).
MgSO4(H2O)4[Mg(H2O)4(κ′,κ1-SO4)]2nonesulfate is bridging ligand, 8-membered Mg2O4S2 rings[37]
MgSO4(H2O)6[Mg(H2O)6]nonehexahydratecommon motif[34]
MgSO4(H2O)7[Mg(H2O)6]oneepsomitecommon motif[34]
TiOSO4(H2O)[Ti(μ-O)2(H2O)(κ1-SO4)3]nonefurther hydration gives gels
VSO4(H2O)6[V(H2O)6]noneAdopts the hexahydrite motif[38]
VSO4(H2O)7[V(H2O)6]onehexaaquo[39]
VOSO4(H2O)5[VO(H2O)4(κ1-SO4)4]one
Cr(SO4)(H2O)3[Cr(H2O)3(κ1-SO4)]noneresembles Cu(SO4)(H2O)3[40]
Cr(SO4)(H2O)5[Cr(H2O)4(κ1-SO4)2]oneresembles Cu(SO4)(H2O)5[41]
Cr2(SO4)3(H2O)18[Cr(H2O)6]sixOne of several chromium(III) sulfates
MnSO4(H2O)[Mn(μ-H2O)(μ4,-κ1-SO4)4][36]noneszmikitesee Fe, Co, Ni, Zn analogues
MnSO4(H2O)4[Mn(μ-SO4)2(H2O)4][42]noneIlesitepentahydrate is called jôkokuite; the hexahydrate, the most rare, is called chvaleticeitewith 8-membered ring Mn2(SO4)2 core
MnSO4(H2O)5?jôkokuite
MnSO4(H2O)6?Chvaleticeite
MnSO4(H2O)7[Mn(H2O)6]onemallardite[35]see Mg analogue
FeSO4(H2O)[Fe(μ-H2O)(μ4-κ1-SO4)4][36]nonesee Mn, Co, Ni, Zn analogues
FeSO4(H2O)7[Fe(H2O)6]onemelanterite[35]see Mg analogue
FeSO4(H2O)4[Fe(H2O)4(κ′,κ1-SO4)]2nonesulfate is bridging ligand, 8-membered Fe2O4S2 rings[37]
FeII(FeIII)2(SO4)4(H2O)14[FeII(H2O)6]2+[FeIII(H2O)4(κ1-SO4)2]−2nonesulfates are terminal ligands on Fe(III)[43]
CoSO4(H2O)[Co(μ-H2O)(μ4-κ1-SO4)4][36]nonesee Mn, Fe, Ni, Zn analogues
CoSO4(H2O)6[Co(H2O)6]nonemoorhouseitesee Mg analogue
CoSO4(H2O)7[Co(H2O)6]onebieberite[35]see Fe, Mg analogues
NiSO4(H2O)[Ni(μ-H2O)(μ4-κ1-SO4)4][36]nonesee Mn, Fe, Co, Zn analogues
NiSO4(H2O)6[Ni(H2O)6]noneretgersiteOne of several nickel sulfate hydrates[44]
NiSO4(H2O)7[Ni(H2O)6]morenosite[35]
(NH4)2[Pt2(SO4)4(H2O)2][Pt2(SO4)4(H2O)2]2−nonePt-Pt bonded Chinese lantern structure[45]
CuSO4(H2O)5[Cu(H2O)4(κ1-SO4)2]onechalcantitesulfate is bridging ligand[46]
CuSO4(H2O)7[Cu(H2O)6]oneboothite[35]
ZnSO4(H2O)[Zn(μ-H2O)(μ4-κ1-SO4)4][36]nonesee Mn, Fe, Co, Ni analogues
ZnSO4(H2O)4[Zn(H2O)4(κ′,κ1-SO4)]2nonesulfate is bridging ligand, 8-membered Zn2O4S2 rings[37][47]
ZnSO4(H2O)6[Zn(H2O)6]nonesee Mg analogue[48]
ZnSO4(H2O)7[Zn(H2O)6]onegoslarite[35]see Mg analogue
CdSO4(H2O)[Cd(μ-H2O)2(κ1-SO4)4]nonebridging water ligand[49]

Hydrates of metal nitrates

Transition metal nitrates form a variety of hydrates. The nitrate anion often binds to the metal, especially for those salts with fewer than six aquo ligands. Nitrates are uncommon in nature, so few minerals are represented here. Hydrated ferrous nitrate has not been characterized crystallographically.

Formula of hydrated metal ion nitrateCoordinationsphere of the metal ionEquivalents of water of crystallization that are not bound to MRemarks
Cr(NO3)3(H2O)9[Cr(H2O)6]3+threeoctahedral configuration[50] isostructural with Fe(NO3)3(H2O)9
Mn(NO3)2(H2O)4cis-[Mn(H2O)4(κ1-ONO2)2]noneoctahedral configuration
Mn(NO3)2(H2O)[Mn(H2O)(μ-ONO2)5]noneoctahedral configuration
Mn(NO3)2(H2O)6[Mn(H2O)6]noneoctahedral configuration[51]
Fe(NO3)3(H2O)9[Fe(H2O)6]3+threeoctahedral configuration[52] isostructural with Cr(NO3)3(H2O)9
Fe(NO3)3)(H2O)4[Fe(H2O)3(κ2-O2NO)2]+onepentagonal bipyramid[53]
Fe(NO3)3(H2O)5[Fe(H2O)5(κ1-ONO2)]2+noneoctahedral configuration[53]
Fe(NO3)3(H2O)6[Fe(H2O)6]3+noneoctahedral configuration[53]
Co(NO3)2(H2O)2[Co(H2O)2(κ1-ONO2)2]noneoctahedral configuration
Co(NO3)2(H2O)4[Co(H2O)4(κ1-ONO2)2noneoctahedral configuration
Co(NO3)2(H2O)6[Co(H2O)6]2+noneoctahedral configuration.[54]
α-Ni(NO3)2(H2O)4cis-[Ni(H2O)4(κ1-ONO2)2]noneoctahedral configuration.[55]
β-Ni(NO3)2(H2O)4trans-[Ni(H2O)4(κ1-ONO2)2]noneoctahedral configuration.[56]
Pd(NO3)2(H2O)2trans-[Pd(H2O)2(κ1-ONO2)2]nonesquare planar coordination geometry[57]
Cu(NO3)2(H2O)[Cu(H2O)(κ2-ONO2)2]noneoctahedral configuration.
Cu(NO3)2(H2O)1.5uncertainuncertainuncertain[58]
Cu(NO3)2(H2O)2.5[Cu(H2O)2(κ1-ONO2)2]onesquare planar[59]
Cu(NO3)2(H2O)3uncertainuncertainuncertain[60]
Cu(NO3)2(H2O)6[Cu(H2O)6]2+noneoctahedral configuration[61]
Zn(NO3)2(H2O)4cis-[Zn(H2O)4(κ1-ONO2)2]noneoctahedral configuration.
Hg2(NO3)2(H2O)2[H2O–Hg–Hg–OH2]2+linear[62]
  • Hydrated copper(II) sulfate is bright blue.
    Hydrated copper(II) sulfate is bright blue.
  • Anhydrous copper(II) sulfate has a light turquoise tint.
    Anhydrous copper(II) sulfate has a light turquoise tint.

See also

References

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