Water of crystallization

In chemistry, water(s) of crystallization or water(s) of hydration are water molecules 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

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.

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 particularly common solvent to be found in crystals because it is small and polar. But all solvents can be found in some host crystals. 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.[7][8]

Hydrated metal halides
and their formulas		Coordination sphere
of the metal		Equivalents of water of crystallization
that are not bound to M		Remarks
Calcium chloride
CaCl2(H2O)6		[Ca(μ-H2O)6(H2O)3]2+noneexample of water as a bridging ligand[9]
Titanium(III) chloride
TiCl3(H2O)6		trans-[TiCl2(H2O)4]+[10]twoisomorphous with VCl3(H2O)6
Titanium(III) chloride
TiCl3(H2O)6		[Ti(H2O)6]3+[10]noneisomeric with [TiCl2(H2O)4]Cl.2H2O[11]
Zirconium(IV) fluoride
ZrF4(H2O)3		(μ−F)2[ZrF3(H2O)3]2nonerare case where Hf and Zr differ[12]
Hafnium tetrafluoride
HfF4(H2O)3		(μ−F)2[HfF2(H2O)2]n(H2O)nonerare case where Hf and Zr differ[12]
Vanadium(III) chloride
VCl3(H2O)6		trans-[VCl2(H2O)4]+[10]two
Vanadium(III) bromide
VBr3(H2O)6		trans-[VBr2(H2O)4]+[10]two
Vanadium(III) iodide
VI3(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]four
Chromium(III) chloride
CrCl3(H2O)6		trans-[CrCl2(H2O)4]+twodark green isomer, aka "Bjerrums's salt"
Chromium(III) chloride
CrCl3(H2O)6		[CrCl(H2O)5]2+oneblue-green isomer
Chromium(II) chloride
CrCl2(H2O)4		trans-[CrCl2(H2O)4]nonesquare planar/tetragonal distortion
Chromium(III) chloride
CrCl3(H2O)6		[Cr(H2O)6]3+noneviolet isomer. isostructural with aluminium compound[13]
Aluminum trichloride
AlCl3(H2O)6		[Al(H2O)6]3+noneisostructural with the Cr(III) compound
Manganese(II) chloride
MnCl2(H2O)6		trans-[MnCl2(H2O)4]two
Manganese(II) chloride
MnCl2(H2O)4		cis-[MnCl2(H2O)4]nonecis molecular, the unstable trans isomer has also been detected[14]
Manganese(II) bromide
MnBr2(H2O)4		cis-[MnBr2(H2O)4]nonecis, molecular
Manganese(II) iodide
MnI2(H2O)4		trans-[MnI2(H2O)4]nonemolecular, isostructural with FeCl2(H2O)4.[15]
Manganese(II) chloride
MnCl2(H2O)2		trans-[MnCl4(H2O)2]nonepolymeric with bridging chloride
Manganese(II) bromide
MnBr2(H2O)2		trans-[MnBr4(H2O)2]nonepolymeric with bridging bromide
Iron(II) chloride
FeCl2(H2O)6		trans-[FeCl2(H2O)4]two
Iron(II) chloride
FeCl2(H2O)4		trans-[FeCl2(H2O)4]nonemolecular
Iron(II) bromide
FeBr2(H2O)4		trans-[FeBr2(H2O)4]nonemolecular,[16] hydrates of FeI2 are not known
Iron(II) chloride
FeCl2(H2O)2		trans-[FeCl4(H2O)2]nonepolymeric with bridging chloride
Iron(III) chloride
FeCl3(H2O)6		trans-[FeCl2(H2O)4]+twoone of four hydrates of ferric chloride,[17] isostructural with Cr analogue
Iron(III) chloride
FeCl3(H2O)2.5		cis-[FeCl2(H2O)4]+twothe dihydrate has a similar structure, both contain FeCl−4 anions.[17]
Cobalt(II) chloride
CoCl2(H2O)6		trans-[CoCl2(H2O)4]two
Cobalt(II) bromide
CoBr2(H2O)6		trans-[CoBr2(H2O)4]two
Cobalt(II) iodide
CoI2(H2O)6		[Co(H2O)6]2+none[18]iodide competes poorly with water
Cobalt(II) bromide
CoBr2(H2O)4		trans-[CoBr2(H2O)4]nonemolecular[16]
Cobalt(II) chloride
CoCl2(H2O)4		cis-[CoCl2(H2O)4]nonenote: cis molecular
Cobalt(II) chloride
CoCl2(H2O)2		trans-[CoCl4(H2O)2]nonepolymeric with bridging chloride
Cobalt(II) chloride
CoBr2(H2O)2		trans-[CoBr4(H2O)2]nonepolymeric with bridging bromide
Nickel(II) chloride
NiCl2(H2O)6		trans-[NiCl2(H2O)4]two
Nickel(II) chloride
NiCl2(H2O)4		cis-[NiCl2(H2O)4]nonenote: cis molecular[16]
Nickel(II) bromide
NiBr2(H2O)6		trans-[NiBr2(H2O)4]two
Nickel(II) iodide
NiI2(H2O)6		[Ni(H2O)6]2+none[18]iodide competes poorly with water
Nickel(II) chloride
NiCl2(H2O)2		trans-[NiCl4(H2O)2]nonepolymeric with bridging chloride
Platinum(IV) chloride
[Pt(H2O)2Cl4](H2O)3[19]		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[20]		fac-[PtCl3(H2O)3]+0.5octahedral Pt centers; rare example of non-first row chloride-aquo complex
Copper(II) chloride
CuCl2(H2O)2		[CuCl4(H2O)2]2nonetetragonally distorted
two long Cu-Cl distances
Copper(II) bromide
CuBr2(H2O)4		[CuBr4(H2O)2]ntwotetragonally distorted
two long Cu-Br distances[16]
Zinc(II) chloride
ZnCl2(H2O)1.33[21]		2 ZnCl2 + ZnCl2(H2O)4nonecoordination polymer with both tetrahedral and octahedral Zn centers
Zinc(II) chloride
ZnCl2(H2O)2.5[22]		Cl3Zn(μ-Cl)Zn(H2O)5nonetetrahedral and octahedral Zn centers
Zinc(II) chloride
ZnCl2(H2O)3[21]		[ZnCl4]2− + Zn(H2O)6]2+nonetetrahedral and octahedral Zn centers
Zinc(II) chloride
ZnCl2(H2O)4.5[21]		[ZnCl4]2− + [Zn(H2O)6]2+threetetrahedral and octahedral Zn centers

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.[23] Many of the metal sulfates occur in nature, being the result of weathering of mineral sulfides.[24][25] Many monohydrates are known.[26]

Formula of
hydrated metal ion sulfate		Coordination
sphere of the metal ion		Equivalents of water of crystallization
that are not bound to M		mineral nameRemarks
MgSO4(H2O)[Mn(μ-H2O)(μ4,-κ1-SO4)4][26]nonekieseritesee Mn, Fe, Co, Ni, Zn analogues
MgSO4(H2O)4[Mg(H2O)4(κ′,κ1-SO4)]2nonesulfate is bridging ligand, 8-membered Mg2O4S2 rings[27]
MgSO4(H2O)6[Mg(H2O)6]nonehexahydratecommon motif[24]
MgSO4(H2O)7[Mg(H2O)6]oneepsomitecommon motif[24]
TiOSO4(H2O)[Ti(μ-O)2(H2O)(κ1-SO4)3]nonefurther hydration gives gels
VSO4(H2O)6[V(H2O)6]noneAdopts the hexahydrite motif[28]
VOSO4(H2O)5[VO(H2O)4(κ1-SO4)4]one
Cr(SO4)(H2O)3[Cr(H2O)3(κ1-SO4)]noneresembles Cu(SO4)(H2O)3[29]
Cr(SO4)(H2O)5[CR(H2O)4(κ1-SO4)2]oneresembles Cu(SO4)(H2O)5[30]
Cr2(SO4)3(H2O)18[Cr(H2O)6]sixOne of several chromium(III) sulfates
MnSO4(H2O)[Mn(μ-H2O)(μ4,-κ1-SO4)4][26]noneszmikitesee Fe, Co, Ni, Zn analogues
MnSO4(H2O)4[Mn(μ-SO4)2(H2O)4][31]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[25]see Mg analogue
FeSO4(H2O)[Fe(μ-H2O)(μ4-κ1-SO4)4][26]nonesee Mn, Co, Ni, Zn analogues
FeSO4(H2O)7[Fe(H2O)6]onemelanterite[25]see Mg analogue
FeSO4(H2O)4[Fe(H2O)4(κ′,κ1-SO4)]2nonesulfate is bridging ligand, 8-membered Fe2O4S2 rings[27]
FeII(FeIII)2(SO4)4(H2O)14[FeII(H2O)6]2+[FeIII(H2O)4(κ1-SO4)2]−
2		nonesulfates are terminal ligands on Fe(III)[32]
CoSO4(H2O)[Co(μ-H2O)(μ4-κ1-SO4)4][26]nonesee Mn, Fe, Ni, Zn analogues
CoSO4(H2O)6[Co(H2O)6]nonemoorhouseitesee Mg analogue
CoSO4(H2O)7[Co(H2O)6]onebieberite[25]see Fe, Mg analogues
NiSO4(H2O)[Ni(μ-H2O)(μ4-κ1-SO4)4][26]nonesee Mn, Fe, Co, Zn analogues
NiSO4(H2O)6[Ni(H2O)6]noneretgersiteOne of several nickel sulfate hydrates[33]
NiSO4(H2O)7[Ni(H2O)6]morenosite[25]
(NH4)2[Pt2(SO4)4(H2O)2][Pt2(SO4)4(H2O)2]2-nonePt-Pt bonded Chinese lantern structure[34]
CuSO4(H2O)5[Cu(H2O)4(κ1-SO4)2]onechalcantitesulfate is bridging ligand[35]
CuSO4(H2O)7[Cu(H2O)6]oneboothite[25]
ZnSO4(H2O)[Zn(μ-H2O)(μ4-κ1-SO4)4][26]nonesee Mn, Fe, Co, Ni analogues
ZnSO4(H2O)4[Zn(H2O)4(κ′,κ1-SO4)]2nonesulfate is bridging ligand, 8-membered Zn2O4S2 rings[27][36]
ZnSO4(H2O)6[Zn(H2O)6]nonesee Mg analogue[37]
ZnSO4(H2O)7[Zn(H2O)6]onegoslarite[25]see Mg analogue
CdSO4(H2O)[Cd(μ-H2O)2(κ1-SO4)4]nonebridging water ligand[38]

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 nitrate		Coordination
sphere of the metal ion		Equivalents of water of crystallization
that are not bound to M		Remarks
Cr(NO3)3(H2O)9[Cr(H2O)6]3+threeoctahedral configuration[39] 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[40]
Fe(NO3)3(H2O)9[Fe(H2O)6]3+threeoctahedral configuration[41] isostructural with Cr(NO3)3(H2O)9
Fe(NO3)3)(H2O)4[Fe(H2O)3(κ2-O2NO)2]+onepentagonal bipyramid[42]
Fe(NO3)3(H2O)5[Fe(H2O)5(κ1-ONO2)]2+noneoctahedral configuration[42]
Fe(NO3)3(H2O)6[Fe(H2O)6]3+noneoctahedral configuration[42]
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.[43]
α-Ni(NO3)2(H2O)4cis-[Ni(H2O)4(κ1-ONO2)2]noneoctahedral configuration.[44]
β-Ni(NO3)2(H2O)4trans-[Ni(H2O)4(κ1-ONO2)2]noneoctahedral configuration.[45]
Pd(NO3)2(H2O)2trans-[Pd(H2O)2(κ1-ONO2)2]nonesquare planar coordination geometry[46]
Cu(NO3)2(H2O)[Cu(H2O)(κ2-ONO2)2]noneoctahedral configuration.
Cu(NO3)2(H2O)1.5uncertainuncertainuncertain[47]
Cu(NO3)2(H2O)2.5[Cu(H2O)2(κ1-ONO2)2]onesquare planar[48]
Cu(NO3)2(H2O)3uncertainuncertainuncertain [49]
Cu(NO3)2(H2O)6[Cu(H2O)6]2+noneoctahedral configuration[50]
Zn(NO3)2(H2O)4cis-[Zn(H2O)4(κ1-ONO2)2]noneoctahedral configuration.
Hg2(NO3)2(H2O)2[H2O–Hg–Hg–OH2]2+linear[51]

Photos
  • Hydrated copper(II) sulfate is bright blue.
  • Anhydrous copper(II) sulfate has a light turquoise tint.

See also

References
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