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Manganese(II) chlorate is an unstable chemical compound with the formula Mn(ClO 3) 2. It is unstable even in dilute solution. As a hexahydrate, it is solid below −18°C. Above this it melts, to form an extremely explosive pink liquid. [2]
[4] [2] To produce the anhydrous form, manganese(II) nitrate is reacted with dichlorine hexoxide at 5 °C: [3] Mn(NO 3) 2 + 4 Cl 2 O 6 → NO 2 Mn(ClO 4) 3 + NO 2 ClO 4 + 4 ClO 2 + O 2. The resulting nitryl salt is subsequently heated at 105 °C in a vacuum to produce the anhydrous perchlorate. [3] NO 2 Mn(ClO 4) 3 → Mn(ClO 4) 2 + NO 2 ClO 4
MnCl 3 (OPPh 3) 2, a stable derivative form of MnCl 3. MnCl 3 can be stabilized by complexation to diverse Lewis bases, as has been established over the course of many years of study. [4] Meta stable acetonitrile-solvated Mn(III)Cl 3 can be prepared at room temperature by treating [Mn 12 O 12 (OAc) 16 (H 2 O) 4] with trimethylsilyl chloride. [5]
Anhydrous MnCl 2 adopts a layered cadmium chloride-like structure. The tetrahydrate consists of octahedral cis-Mn(H 2 O) 4 Cl 2 molecules. The trans isomer, which is metastable, is also known. [4] [5] The dihydrate MnCl 2 (H 2 O) 2 is a coordination polymer. Each Mn center is coordinated to four doubly bridging chloride ligands.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
A 2010 study has discovered the presence of natural chlorate deposits around the world, with relatively high concentrations found in arid and hyper-arid regions. [2] The chlorate was also measured in rainfall samples with the amount of chlorate similar to perchlorate. It is suspected that chlorate and perchlorate may share a common natural ...
In Mn(CH 3) 2 (dmpe) 2, Mn(II) is low spin, which contrasts with the high spin character of its precursor, MnBr 2 (dmpe) 2 (dmpe = (CH 3) 2 PCH 2 CH 2 P(CH 3) 2). [38] Polyalkyl and polyaryl derivatives of manganese often exist in higher oxidation states, reflecting the electron-releasing properties of alkyl and aryl ligands. One example is [Mn ...
The chlorite ion adopts a bent molecular geometry, due to the effects of the lone pairs on the chlorine atom, with an O–Cl–O bond angle of 111° and Cl–O bond lengths of 156 pm. [1] Chlorite is the strongest oxidiser of the chlorine oxyanions on the basis of standard half cell potentials.