  | |
| Identifiers | |
|---|---|
| ECHA InfoCard | 100.030.635 |
CompTox Dashboard (EPA) | |
| Properties | |
| Cs2SeO4 | |
| Molar mass | 408.77 |
| Appearance | colourless crystals [1] |
| insoluble | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
Caesium selanate is an inorganic compound, with the chemical formula of Cs2SeO4. It can form colourless crystals of the orthorhombic crystal system.
caesium selenate can be obtained from the reaction of caesium carbonate and selenic acid solution: [2]
caesium selenate can also be prepared by the neutralization reaction of selenic acid and caesium hydroxide: [1]
caesium selenate can precipitate compounds such as CsLiSeO4·1⁄2H2O and Cs4LiH3(SeO4)4 in Cs2SeO4-Li2SeO4-H2O and its acidification system. [2] It can also form double salts with other metals, such as Cs2Mg(SeO4)2·6H2O, Cs2Co(SeO4)2·6H2O, etc. [3]
Caesium fluoride or cesium fluoride is an inorganic compound with the formula CsF. A hygroscopic white salt, caesium fluoride is used in the synthesis of organic compounds as a source of the fluoride anion. The compound is noteworthy from the pedagogical perspective as caesium also has the highest electropositivity of all commonly available elements and fluorine has the highest electronegativity.
A permanganate is a chemical compound with the manganate(VII) ion, MnO−
4, the conjugate base of permanganic acid. Because the manganese atom has a +7 oxidation state, the permanganate(VII) ion is a strong oxidising agent. The ion is a transition metal ion with a tetrahedral structure. Permanganate solutions are purple in colour and are stable in neutral or slightly alkaline media. The exact chemical reaction depends on the carbon-containing reactants present and the oxidant used. For example, trichloroethane (C2H3Cl3) is oxidised by permanganate ions to form carbon dioxide (CO2), manganese dioxide (MnO2), hydrogen ions (H+), and chloride ions (Cl−).
Caesium chloride or cesium chloride is the inorganic compound with the formula CsCl. This colorless salt is an important source of caesium ions in a variety of niche applications. Its crystal structure forms a major structural type where each caesium ion is coordinated by 8 chloride ions. Caesium chloride dissolves in water. CsCl changes to NaCl structure on heating. Caesium chloride occurs naturally as impurities in carnallite, sylvite and kainite. Less than 20 tonnes of CsCl is produced annually worldwide, mostly from a caesium-bearing mineral pollucite.
Selenic acid is the inorganic compound with the formula H2SeO4. It is an oxoacid of selenium, and its structure is more accurately described as O2Se(OH)2. It is a colorless compound. Although it has few uses, one of its salts, sodium selenate is used in the production of glass and animal feeds.
Selenous acid is the chemical compound with the formula H2SeO3. Structurally, it is more accurately described by O=Se(OH)2. It is the principal oxoacid of selenium; the other being selenic acid.
Selenium compounds are compounds containing the element selenium (Se). Among these compounds, selenium has various oxidation states, the most common ones being −2, +4, and +6. Selenium compounds exist in nature in the form of various minerals, such as clausthalite, guanajuatite, tiemannite, crookesite etc., and can also coexist with sulfide minerals such as pyrite and chalcopyrite. For many mammals, selenium compounds are essential. For example, selenomethionine and selenocysteine are selenium-containing amino acids present in the human body. Selenomethionine participates in the synthesis of selenoproteins. The reduction potential and pKa (5.47) of selenocysteine are lower than those of cysteine, making some proteins have antioxidant activity. Selenium compounds have important applications in semiconductors, glass and ceramic industries, medicine, metallurgy and other fields.
Sodium selenate is the inorganic compound with the formula Na
2SeO
4, not to be confused with sodium selenite. It exists as the anhydrous salt, the heptahydrate, and the decahydrate. These are white, water-soluble solids. The decahydrate is a common ingredient in multivitamins and livestock feed as a source of selenium. The anhydrous salt is used in the production of some glass. Although the selenates are much more toxic, many physical properties of sodium selenate and sodium sulfate are similar.
Tutton's salts are a family of salts with the formula M2M'(SO4)2(H2O)6 (sulfates) or M2M'(SeO4)2(H2O)6 (selenates). These materials are double salts, which means that they contain two different cations, M+ and M'2+ crystallized in the same regular ionic lattice. The univalent cation can be potassium, rubidium, caesium, ammonium (NH4), deuterated ammonium (ND4) or thallium. Sodium or lithium ions are too small. The divalent cation can be magnesium, vanadium, chromium, manganese, iron, cobalt, nickel, copper, zinc or cadmium. In addition to sulfate and selenate, the divalent anion can be chromate (CrO42−), tetrafluoroberyllate (BeF42−), hydrogenphosphate (HPO42−) or monofluorophosphate (PO3F2−). Tutton's salts crystallize in the monoclinic space group P21/a. The robustness is the result of the complementary hydrogen-bonding between the tetrahedral anions and cations as well their interactions with the metal aquo complex [M(H2O)6]2+.
Potassium selenate, K
2SeO
4, is an odorless, white solid that forms as the potassium salt of selenic acid.
Iron(II) selenate (ferrous selenate) is an inorganic compound with the formula FeSeO4. It has anhydrous and several hydrate forms. The pentahydrate has the structure, [Fe(H2O)4]SeO4•H2O, isomorphous to the corresponding iron(II) sulfate. Heptahydrate is also known, in form of unstable green crystalline solid.
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.
The Nickel oxyacid salts are a class of chemical compounds of nickel with an oxyacid. The compounds include a number of minerals and industrially important nickel compounds.
A selenate selenite is a chemical compound or salt that contains selenite and selenate anions (SeO32- and SeO42-). These are mixed anion compounds. Some have third anions.
Praseodymium(III) selenate is an inorganic compound, the salt of praseodymium and selenic acid with the chemical formula Pr2(SeO4)3. It forms green crystals when hydrated.
Thulium(III) selenate is an inorganic compound, with the chemical formula Tm2(SeO4)3. It can be obtained by reacting a thulium(III) oxide and selenic acid solution and crystallizing it. It crystallises with ammonium selenate in an aqueous solution to obtain NH4Tm(SeO4)2·3H2O.
Nickel(II) selenate is a selenate of nickel with the chemical formula NiSeO4.
Erbium(III) selenate is an inorganic compound, with the chemical formula Er2(SeO4)3. It exists as an anhydrate or an octahydrate.
Holmium(III) selenate is an inorganic compound with the chemical formula Ho2(SeO4)3. It exists in the anhydrous form and as an octahydrate. It can be obtained by dissolving holmium(III) oxide in selenic acid solution and evaporating and crystallizing it. It co-crystallizes with other selenates in solution to obtain complex salts such as K3Ho(SeO4)3·nH2O, NH4Ho(SeO4)2·3H2O and CH3NH3Ho(SeO4)2·5H2O.
Cerium(III) selenate is an inorganic compound with the chemical formula Ce2(SeO4)3. It can be obtained by reacting selenic acid and cerium(III) carbonate, and the solvent is evaporated to precipitate crystals. The double salt CsCe(SeO4)2·4H2O can be obtained from mixing cerium(III) selenate and cesium selenate in an aqueous solution, and then evaporating and crystallizing the solution.
Gadolinium(III) selenate is an inorganic compound with the chemical formula Gd2(SeO4)3. It exists as the anhydrate and octahydrate. The octahydrate transforms into the anhydrate when heated to 130 °C.
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