Water Of Crystallization

Water of crystallization (alt. Br.E. water of crystallisation) is water that occurs in crystals but is not covalently bonded to a host molecule or ion. The term is archaic and predates modern structural inorganic chemistry, coming from an era when the relationships between stoichiometry and structure were poorly understood. Nonetheless, the concept is pervasive and when employed precisely, the term can be useful. Upon crystallization from water or moist solvents, many compounds incorporate water molecules in their crystalline frameworks. Often, in fact, the species of interest cannot be crystallized in the absence of water, even though no strong bonds to the "guest" water molecules may be apparent. Classically, "water of crystallization" refers to water that is found in a crystalline framework of a metal complex but that is not directly bonded to the metal ion. Obviously the "water of crystallization" is bound or interacting with some other atoms and ions or it would not be included in the crystalline framework. Consider the case of nickel(II) chloride hexahydrate. This species has the formula NiCl2(H2O)6. Examination of its molecular structure reveals that the crystal consists of [trans-NiCl2(H2O)4] subunits that are hydrogen bonded to each other and two isolated molecules of H2O. Thus 1/3 of the water molecules in the crystal are not directly bonded to Ni2+, and these might be termed "water of crystallization". Compared to inorganic salts, proteins crystallize with unusually large amounts of water in the crystal lattice. A water content of 50 % is not uncommon. The extended hydration shell is what allows the protein crystallographer to argue that the conformation in the crystal is not too far from the native conformation in solution. 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. 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. Examples: * CuSO4•5H2O - copper (II) sulphate pentahydrate * CoI2•6H2O - cobalt (II) iodide hexahydrate * SnCl2•2H2O - stannous (tin II) chloride dihydrate Since the latter part of the 20th century, the structures of most common hydrates have been determined by crystallography, so the dot formalism is increasingly obsolete. Another reason for using the dot formalism is simplicity. For many salts, the exact bonding of the water is unimportant because the water molecules are labilized 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 the aforementioned hydrated copper sulphate consists of [Cu(H2O)4]2+ centers linked to SO42- 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. The cobalt iodide mentioned above occurs as [Co(H2O)6]2+ and I-. In the 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 can arises from water. Glauber's salt, a white crystalline solid Na2SO4(H2O)10 is >50% water by weight.