Monday, September 10, 2018

inorganic chemistry - Formation of MnO2 vs [Mn(H2O)6]4+ in aqueous solution


I am looking for reasons why Mn(IV) wouldn't be stable as a hydrate. I know that from standard reduction potentials it exists as a ppt of MnOX2, but what is stopping it from being a hydrated 4+ aqueous cation? Is it that the water ligands would be too polarised and therefore HX+ dissociation would occur very easily? Are there other factors that make it a solid rather than a solvated ion, like lattice enthalpy etc.?




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periodic trends - Comparing radii in lithium, beryllium, magnesium, aluminium and sodium ions

Apparently the of last four, MgX2+ is closest in radius to LiX+. Is this true, and if so, why would a whole larger shell ($\ce{...