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Transition Metal Perchlorate Complexes
class=skin-invert, 300px, Titanium(IV) perchlorate is a transition metal perchlorate complex. Transition metal perchlorate complexes are coordination complexes with one or more perchlorate ligand In coordination chemistry, a ligand is an ion or molecule with a functional group that binds to a central metal atom to form a coordination complex. The bonding with the metal generally involves formal donation of one or more of the ligand's el ...s. Perchlorate can bind to metals through one, two, three, or all four oxygen atoms. Usually however, perchlorate is a counterion, not a ligand. Homoleptic complexes Homoleptic complexes, i.e. complexes where all the ligands are the same (in this case perchlorate), are of fundamental interest because of their simple stoichiometries. Several anhydrous metal diperchlorate complexes are known but most are not molecular (and hence, not complexes). For example, many compounds with the formula are coordination polymers (M = Mn, Fe, Co, Ni, C ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Ferrous Perchlorate
Iron(II) perchlorate is the inorganic compound with the formula . A green, water-soluble solid, it is produced by the reaction of iron metal with dilute perchloric acid followed by evaporation of the solution: : Although the ferrous cation is a reductant and the perchlorate anion is a strong oxidant, in the absence of atmospheric oxygen, dissolved ferrous perchlorate is stable in aqueous solution because the electron transfer between both species is hindered by severe kinetic limitations. Being a weak Lewis base, the perchlorate anion is a poor ligand for the aqueous and does not contribute to the electron transfer by favoring the formation of an inner sphere complex giving rise to a possible reorganisation of the activated complex. The resulting high activation energy prohibits a thermodynamically spontaneous redox reaction (∆''G''r < 0). However, in aqueous solution, and under air, iron(II) perchlorate slowly [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Ligands
In coordination chemistry, a ligand is an ion or molecule with a functional group that binds to a central metal atom to form a coordination complex. The bonding with the metal generally involves formal donation of one or more of the ligand's electron pairs, often through Lewis bases. The nature of metal–ligand bonding can range from covalent to ionic. Furthermore, the metal–ligand bond order can range from one to three. Ligands are viewed as Lewis bases, although rare cases are known to involve Lewis acidic "ligands". Metals and metalloids are bound to ligands in almost all circumstances, although gaseous "naked" metal ions can be generated in a high vacuum. Ligands in a complex dictate the reactivity of the central atom, including ligand substitution rates, the reactivity of the ligands themselves, and redox. Ligand selection requires critical consideration in many practical areas, including bioinorganic and medicinal chemistry, homogeneous catalysis, and environme ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Silver Perchlorate
Silver perchlorate is the chemical compound with the formula AgClO4. This white solid forms a monohydrate and is mildly deliquescent. It is a useful source of the Ag+ ion, although the presence of perchlorate presents risks. It is used as a catalyst in organic chemistry. Production Silver perchlorate is created by heating a mixture of perchloric acid with silver nitrate. Alternatively, it can be prepared by the reaction between barium perchlorate and silver sulfate, or from the reaction of perchloric acid with silver oxide. Solubility Silver perchlorate is noteworthy for its solubility in aromatic solvents such as benzene (52.8 g/L) and toluene (1010 g/L). In these solvents, the silver cation binds to the arene, as has been demonstrated by X-ray crystallographic studies on crystals obtained from such solutions. Its solubility in water is extremely high, up to 500 g per 100 mL water. X-ray diffraction experiments show that aqueous solutions contain g(H2O)2sup>+ with Ag-O d ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Vanadium Pentoxide
Vanadium(V) oxide (''vanadia'') is the inorganic compound with the formula V2 O5. Commonly known as vanadium pentoxide, it is a dark yellow solid, although when freshly precipitated from aqueous solution, its colour is deep orange. Because of its high oxidation state, it is both an amphoteric oxide and an oxidizing agent. From the industrial perspective, it is the most important compound of vanadium, being the principal precursor to alloys of vanadium and is a widely used industrial catalyst. The mineral form of this compound, shcherbinaite, is extremely rare, almost always found among fumaroles. A mineral trihydrate, V2O5·3H2O, is also known under the name of navajoite. Chemical properties Reduction to lower oxides Upon heating a mixture of vanadium(V) oxide and vanadium(III) oxide, comproportionation occurs to give vanadium(IV) oxide, as a deep-blue solid: :V2O5 + V2O3 → 4 VO2 The reduction can also be effected by oxalic acid, carbon monoxide, and sulfur ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chlorine Trioxide
Dichlorine hexoxide is the chemical compound with the molecular formula or , which is correct for its gaseous state. However, in liquid or solid form, this chlorine oxide ionizes into the dark red ionic compound chloryl perchlorate or dioxochloronium(V) perchlorate , which may be thought of as the mixed anhydride of chloric and perchloric acids. This compound is a notable perchlorating agent. It is produced by reaction between chlorine dioxide and excess ozone: : Molecular structure It was originally reported to exist as the monomeric chlorine trioxide in gas phase, but was later shown to remain an oxygen-bridged dimer after evaporation and until thermal decomposition into chlorine perchlorate, , and oxygen. The compound was then rediscovered. It is a dark red fuming liquid at room temperature that crystallizes as a red ionic compound, chloryl perchlorate, . The red color shows the presence of chloryl ions. Thus, chlorine's formal oxidation state in this compound remains ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Weakly Coordinating Anion
Anions that interact weakly with cations are termed non-coordinating anions, although a more accurate term is weakly coordinating anion. Non-coordinating anions are useful in studying the reactivity of electrophilic cations. They are commonly found as counterions for cationic metal complexes with an unsaturated coordination sphere. These special anions are essential components of homogeneous alkene polymerisation catalysts, where the active catalyst is a coordinatively unsaturated, cationic transition metal complex. For example, they are employed as counterions for the 14 valence electron cations C5H5)2ZrRsup>+ (R = methyl or a growing polyethylene chain). Complexes derived from non-coordinating anions have been used to catalyze hydrogenation, hydrosilylation, oligomerization, and the living polymerization of alkenes. The popularization of non-coordinating anions has contributed to increased understanding of agostic complexes wherein hydrocarbons and hydrogen serve as ligand ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Copper(II) Perchlorate
Copper(II) perchlorate is an inorganic compound with the chemical formula . It forms hydrates with the formula . The anhydrous solid is rarely encountered but several hydrates are known. Most important is the perchlorate salt of the copper aquo complex copper(II) perchlorate hexahydrate, . Infrared spectroscopic studies of anhydrous copper(II) perchlorate provided some of the first evidence for the binding of perchlorate anion to a metal ion. The structure of this compound was eventually deduced by X-ray crystallography. Copper resides in a distorted octahedral environment and the perchlorate ligands bridge between the Cu(II) centers. Safety Like other perchlorates, copper(II) perchlorate is a strong oxidant An oxidizing agent (also known as an oxidant, oxidizer, electron recipient, or electron acceptor) is a substance in a redox chemical reaction that gains or "Electron acceptor, accepts"/"receives" an electron from a (called the , , or ''electr .... References Co ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Nickel(II) Perchlorate
Nickel(II) perchlorate is a collection of inorganic compounds with the chemical formula of . Its colors of these solids vary with the degree of hydration. For example, the hydrate forms cyan crystals, the pentahydrate forms green crystals, but the hexahydrate (Ni(ClO4)2·6H2O) forms blue crystals. Nickel(II) perchlorate hexahydrate is highly soluble in water and soluble in some polar organic solvents. Preparation Aqueous solutions of nickel(II) perchlorate can be obtained by treating nickel(II) hydroxide, nickel(II) chloride or nickel(II) carbonate with perchloric acid. :Ni(OH)2 + 2HClO4 + 4H2O → Ni(ClO4)2·6H2O Two hydrates have been characterized by X-ray crystallography: the hexahydrate and the octahydrate. Several other hydrates are mentioned including the pentahydrate, which is claimed to crystallize at room temperature, the nonahydrate, which is claimed to crystallize at −21.3 °C, a tetrahydrate, and a monohydrate. The yellow anhydrous product is obtained by ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Manganese(II) Perchlorate
Manganese(II) perchlorate is an inorganic chemical compound with the formula Mn(ClO4)2. It forms a white-colored anhydrous and a rose-colored hexahydrate, both of which are hygroscopic. As a perchlorate, it is a strong oxidizing agent. Production and reactions The hexahydrate can be produced by reacting manganese metal or manganese(II) carbonate with perchloric acid, followed by the evaporation of the solution. The hexahydrate does not dehydrate when heating but instead oxidizes to manganese dioxide at 150 °C. To produce the anhydrous form, manganese(II) nitrate is reacted with dichlorine hexoxide at 5 °C: :Mn(NO3)2 + 4 Cl2O6 → NO2Mn(ClO4)3 + NO2ClO4 + 4 ClO2 + O2 The resulting nitryl salt is subsequently heated at 105 °C in a vacuum to produce the anhydrous perchlorate. :NO2Mn(ClO4)3 → Mn(ClO4)2 + NO2ClO4 Structure The anhydrous form is predicted to be isostructural with cobalt(II) perchlorate, based on the IR spectrum and the Raman spectrum of the compound. The hexa ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Chromium(III) Perchlorate
Chromium(III) perchlorate is an inorganic compound, a salt with the chemical formula Cr(ClO4)3. It's hexahydrate Cr(ClO4)3·6H2O is a cyan solid that dissolves in water. Preparation Chromium perchlorate can prepared by reacting chromium(III) oxide or chromium(III) hydroxide with perchloric acid: :Cr2O3 + 6HClO4 → 2Cr(ClO4)3 + 3H2O Hydrates Chromium perchlorate has many hydrates, such as the hexahydrate Cr(ClO4)3·6H2O and a nonahydrate Cr(ClO4)3·9H2O. All of them are cyan substances that are soluble in water. Related compounds *Cr(ClO4)3 will react with NH3 in suitable conditions to form an orange hexammine complex Cr(ClO4)3·6NH3. Other compounds with the general formula Cr(ClO4)3(NH3)x are also known. When x = 3, this compound is red, when x = 4 or 5, it is orange. The hexammine complex will explode. *Cr(ClO4)3 can also form complexes with N2H4, such as purple Cr(ClO4)3·2N2H4. *Cr(ClO4)3 can also form complexes with urea Urea, also called carbamide (because it is ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
Cobalt(II) Perchlorate
Cobalt(II) perchlorate is an inorganic chemical compound with the formula Co(ClO4)2·''n''H2O (''n'' = 0,6). The pink anhydrous and red hexahydrate forms are both hygroscopic solids. Preparation and reactions Cobalt(II) perchlorate hexahydrate is produced by reacting cobalt metal or cobalt(II) carbonate with perchloric acid, followed by the evaporation of the solution: :CoCO3 + 2 HClO4 → Co(ClO4)2 + H2O + CO2 The anhydrous form cannot be produced from the hexahydrate by heating, as it instead decomposes to cobalt(II,III) oxide at 170 °C. Instead, anhydrous cobalt(II) perchlorate is produced from the reaction of dichlorine hexoxide and cobalt(II) chloride, followed by heating in a vacuum at 75 °C. Structure The anhydrous form consists of octahedral Co(ClO4)6 centers, with tridentate perchlorate ligands. On the other hand, the orthorhombic hexahydrate consists of isolated o(H2O)6sup>2+ octahedrons and perchlorate A perchlorate is a chemical compound containing the perchlorat ... [...More Info...] [...Related Items...] OR: [Wikipedia] [Google] [Baidu] |
