Water of crystallization

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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.

Contents

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 .mw-parser-output .template-chem2-su{display:inline-block;font-size:80%;line-height:1;vertical-align:-0.35em}.mw-parser-output .template-chem2-su>span{display:block;text-align:left}.mw-parser-output sub.template-chem2-sub{font-size:80%;vertical-align:-0.35em}.mw-parser-output sup.template-chem2-sup{font-size:80%;vertical-align:0.65em} FeSO4*7H2O. This metal aquo complex crystallizes with water of hydration, which interacts with the sulfate and with the [Fe(H2O)6] centers. H-bondingFeSO47aq.tif
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] 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:

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] 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 Ca and the role of water as a bridging ligand. Ca(aq)6 improved image.tif
Structure of the polymeric [Ca(H2O)6] 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 Ca 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 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] none isomeric 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

Substructure of MSO4(H2O), illustrating presence of bridging water and bridging sulfate (M = Mg, Mn, Fe, Co, Ni, Zn). ICSD CollCode71346.png
Substructure of MSO4(H2O), illustrating presence of bridging water and bridging sulfate (M = Mg, Mn, Fe, Co, Ni, Zn).

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]none bridging 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+three octahedral configuration [39] isostructural with Fe(NO3)3(H2O)9
Mn(NO3)2(H2O)4 cis-[Mn(H2O)4(κ1-ONO2)2]none octahedral configuration
Mn(NO3)2(H2O) [Mn(H2O)(μ-ONO2)5]none octahedral configuration
Mn(NO3)2(H2O)6 [Mn(H2O)6]none octahedral configuration [40]
Fe(NO3)3(H2O)9 [Fe(H2O)6]3+three octahedral configuration [41] isostructural with Cr(NO3)3(H2O)9
Fe(NO3)3)(H2O)4 [Fe(H2O)3(κ2-O2NO)2]+one pentagonal bipyramid [42]
Fe(NO3)3(H2O)5 [Fe(H2O)5(κ1-ONO2)]2+none octahedral configuration [42]
Fe(NO3)3(H2O)6 [Fe(H2O)6]3+none octahedral configuration [42]
Co(NO3)2(H2O)2 [Co(H2O)2(κ1-ONO2)2]none octahedral configuration
Co(NO3)2(H2O)4 [Co(H2O)4(κ1-ONO2)2none octahedral configuration
Co(NO3)2(H2O)6 [Co(H2O)6]2+none octahedral configuration. [43]
α-Ni(NO3)2(H2O)4 cis-[Ni(H2O)4(κ1-ONO2)2]none octahedral configuration. [44]
β-Ni(NO3)2(H2O)4 trans-[Ni(H2O)4(κ1-ONO2)2]none octahedral configuration. [45]
Pd(NO3)2(H2O)2 trans-[Pd(H2O)2(κ1-ONO2)2]none square planar coordination geometry [46]
Cu(NO3)2(H2O) [Cu(H2O)(κ2-ONO2)2]none octahedral configuration.
Cu(NO3)2(H2O)1.5 uncertainuncertainuncertain [47]
Cu(NO3)2(H2O)2.5 [Cu(H2O)2(κ1-ONO2)2]one square planar [48]
Cu(NO3)2(H2O)3 uncertainuncertainuncertain [49]
Cu(NO3)2(H2O)6 [Cu(H2O)6]2+none octahedral configuration [50]
Zn(NO3)2(H2O)4 cis-[Zn(H2O)4(κ1-ONO2)2]none octahedral configuration.
Hg2(NO3)2(H2O)2 [H2O–Hg–Hg–OH2]2+linear [51]

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See also

Related Research Articles

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<span class="mw-page-title-main">Magnesium sulfate</span> Chemical compound with formula MgSO4

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<span class="mw-page-title-main">Copper(II) nitrate</span> Chemical compound

Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO3)2(H2O)x. The hydrates are blue solids. Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C. Common hydrates are the hemipentahydrate and trihydrate.

<span class="mw-page-title-main">Nickel(II) chloride</span> Chemical compound

Nickel(II) chloride (or just nickel chloride) is the chemical compound NiCl2. The anhydrous salt is yellow, but the more familiar hydrate NiCl2·6H2O is green. Nickel(II) chloride, in various forms, is the most important source of nickel for chemical synthesis. The nickel chlorides are deliquescent, absorbing moisture from the air to form a solution. Nickel salts have been shown to be carcinogenic to the lungs and nasal passages in cases of long-term inhalation exposure.

<span class="mw-page-title-main">Cadmium chloride</span> Chemical compound

Cadmium chloride is a white crystalline compound of cadmium and chloride, with the formula CdCl2. This salt is a hygroscopic solid that is highly soluble in water and slightly soluble in alcohol. The crystal structure of cadmium chloride (described below), is a reference for describing other crystal structures. Also known are CdCl2•H2O and the hemipentahydrate CdCl2•2.5H2O.

<span class="mw-page-title-main">Uranyl chloride</span> Chemical compound

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<span class="mw-page-title-main">Nickel(II) nitrate</span> Chemical compound

Nickel nitrate is the inorganic compound Ni(NO3)2 or any hydrate thereof. The anhydrous form is not commonly encountered, thus "nickel nitrate" usually refers to nickel(II) nitrate hexahydrate. The formula for this species is written in two ways: Ni(NO3)2.6H2O and, more descriptively [Ni(H2O)6](NO3)2. The latter formula indicates that the nickel(II) center is surrounded by six water molecules in this hydrated salt. In the hexahydrate, the nitrate anions are not bonded to nickel. Also known are three other hydrates: Ni(NO3)2.9H2O, Ni(NO3)2.4H2O, and Ni(NO3)2.2H2O. Anhydrous Ni(NO3)2 is also known.

<span class="mw-page-title-main">Manganese(II) sulfate</span> Chemical compound

Manganese(II) sulfate usually refers to the inorganic compound with the formula MnSO4·H2O. This pale pink deliquescent solid is a commercially significant manganese(II) salt. Approximately 260,000 tonnes of manganese(II) sulfate were produced worldwide in 2005. It is the precursor to manganese metal and many other chemical compounds. Manganese-deficient soil is remediated with this salt.

<span class="mw-page-title-main">Cobalt(II) sulfate</span> Inorganic compound

Cobalt(II) sulfate is any of the inorganic compounds with the formula CoSO4(H2O)x. Usually cobalt sulfate refers to the hexa- or heptahydrates CoSO4.6H2O or CoSO4.7H2O, respectively. The heptahydrate is a red solid that is soluble in water and methanol. Since cobalt(II) has an odd number of electrons, its salts are paramagnetic.

<span class="mw-page-title-main">Cobalt(II) bromide</span> Chemical compound

Cobalt(II) bromide (CoBr2) is an inorganic compound. In its anhydrous form, it is a green solid that is soluble in water, used primarily as a catalyst in some processes.

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Beryllium sulfate normally encountered as the tetrahydrate, [Be(H2O)4]SO4 is a white crystalline solid. It was first isolated in 1815 by Jons Jakob Berzelius. Beryllium sulfate may be prepared by treating an aqueous solution of many beryllium salts with sulfuric acid, followed by evaporation of the solution and crystallization. The hydrated product may be converted to anhydrous salt by heating at 400 °C.

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Manganese(II) nitrate refers to the inorganic compounds with formula Mn(NO3)2·(H2O)n. These compounds are nitrate salts containing varying amounts of water. A common derivative is the tetrahydrate, Mn(NO3)2·4H2O, but mono- and hexahydrates are also known as well as the anhydrous compound. Some of these compounds are useful precursors to the oxides of manganese. Typical of a manganese(II) compound, it is a paramagnetic pale pink solid.

<span class="mw-page-title-main">Thorium(IV) nitrate</span> Chemical compound

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Vanadium(II) sulfate describes a family of inorganic compounds with the formula VSO4(H2O)x where 0 ≤ x ≤ 7. The hexahydrate is most commonly encountered. It is a violet solid that dissolves in water to give air-sensitive solutions of the aquo complex. The salt is isomorphous with [Mg(H2O)6]SO4. Compared to the V–O bond length of 191 pm in [V(H2O)6]3+, the V–O distance is 212 pm in the [V(H2O)6]SO4. This nearly 10% elongation reflects the effect of the lower charge, hence weakened electrostatic attraction.

Copper(II) chlorate is a chemical compound of the transition metal copper and the chlorate anion with basic formula Cu(ClO3)2. Copper chlorate is an oxidiser. It commonly forms the tetrahydrate, Cu(ClO3)2·4H2O.

Nickel is one of the metals that can form Tutton's salts. The singly charged ion can be any of the full range of potassium, rubidium, cesium, ammonium (), or thallium. As a mineral the ammonium nickel salt, (NH4)2Ni(SO4)2 · 6 H2O, can be called nickelboussingaultite. With sodium, the double sulfate is nickelblödite Na2Ni(SO4)2 · 4 H2O from the blödite family. Nickel can be substituted by other divalent metals of similar sized to make mixtures that crystallise in the same form.

<span class="mw-page-title-main">Transition metal nitrate complex</span> Compound of nitrate ligands

A transition metal nitrate complex is a coordination compound containing one or more nitrate ligands. Such complexes are common starting reagents for the preparation of other compounds.

<span class="mw-page-title-main">Nickel(II) perchlorate</span> Compound of nickel

Nickel(II) perchlorate is a inorganic compound with the chemical formula of Ni(ClO4)2, and it is a strong oxidizing agent. Its colours are different depending on water. For example, the hydrate forms cyan crystals, the pentahydrate forms green crystals, but the hexahydrate (Ni(ClO4)2·6H2O) forms blue crystals.

References

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  3. ↑ Wang, Yonghui; Feng, Liyun; Li, Yangguang; Hu, Changwen; Wang, Enbo; Hu, Ninghai; Jia, Hengqing (2002). "Novel Hydrogen-Bonded Three-Dimensional Networks Encapsulating One-Dimensional Covalent Chains: [M(4,4′-bipy)(H2O)4](4-abs)2·nH2O (4,4′-bipy = 4,4′-Bipyridine; 4-abs = 4-Aminobenzenesulfonate) (M = Co, n = 1; M = Mn, n = 2)". Inorganic Chemistry. 41 (24): 6351–6357. doi:10.1021/ic025915o. PMID   12444778.
  4. ↑ Maldonado, Carmen R.; Quirós, Miguel; Salas, J.M. (2010). "Formation of 2D water morphologies in the lattice of the salt with [Cu2(OH)2(H2O)2(phen)2]2+ as cation and 4,6-dimethyl-1,2,3-triazolo[4,5-d]pyrimidin-5,7-dionato as anion". Inorganic Chemistry Communications. 13 (3): 399–403. doi:10.1016/j.inoche.2009.12.033.
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