“…When Ag(II) cations are found in superacidic environments, and in the presence of weakly coordinating anions, they exhibit superb oxidizing properties. This is exemplified by AgF + cations solvated by anhydrous HF acidified with Lewis acids; these species are capable of oxidizing, inter alia, xenon and O 2 while yielding Xe(II) and O + 2 cations, respectively [13]. Since both the first ionization potential of an O 2 molecule and that of a Xe atom exceed 12 eV, Ag(II) cations retain in this electron-deficient environment substantial share (approx.…”
Silver is the heavier congener of copper in the Periodic Table, but the chemistry of these two elements is very different. While Cu(II) is the most common cationic form of copper, Ag(II) is rare and its compounds exhibit a broad range of peculiar physico-chemical properties. These include, but are not limited to: (i) uncommon oxidizing properties, (ii) unprecedented large mixing of metal and ligand valence orbitals, (iii) strong spin-polarization of neighbouring ligands, (iv) record large magnetic superexchange constants, (v) ease of thermal decomposition of its salts with O-, N- or C-ligands, as well as (vi) robust Jahn–Teller effect which is preserved even at high pressure. These intriguing features of the compounds of Ag(II) will be discussed here together with (vii) a possibility of electromerism (electronic tautomerism) for a certain class of Ag(II) salts.
“…When Ag(II) cations are found in superacidic environments, and in the presence of weakly coordinating anions, they exhibit superb oxidizing properties. This is exemplified by AgF + cations solvated by anhydrous HF acidified with Lewis acids; these species are capable of oxidizing, inter alia, xenon and O 2 while yielding Xe(II) and O + 2 cations, respectively [13]. Since both the first ionization potential of an O 2 molecule and that of a Xe atom exceed 12 eV, Ag(II) cations retain in this electron-deficient environment substantial share (approx.…”
Silver is the heavier congener of copper in the Periodic Table, but the chemistry of these two elements is very different. While Cu(II) is the most common cationic form of copper, Ag(II) is rare and its compounds exhibit a broad range of peculiar physico-chemical properties. These include, but are not limited to: (i) uncommon oxidizing properties, (ii) unprecedented large mixing of metal and ligand valence orbitals, (iii) strong spin-polarization of neighbouring ligands, (iv) record large magnetic superexchange constants, (v) ease of thermal decomposition of its salts with O-, N- or C-ligands, as well as (vi) robust Jahn–Teller effect which is preserved even at high pressure. These intriguing features of the compounds of Ag(II) will be discussed here together with (vii) a possibility of electromerism (electronic tautomerism) for a certain class of Ag(II) salts.
“…22 In addition to being vital to understanding the limits of chemical stability, the more stable, high oxidation state fluorides can be used as potent oxidizers. 30,31 Of the "missing" hexafluorides, 2 PdF 6 is probably the most surprising, given that all the other 4d and 5d hexafluorides of Groups 6-8 are known, 7,8 including PtF 6 , 32,33 which was instrumental in the development of xenon chemistry as long ago as 1962. 34,35 There appear to be no experimental reports on PdF.…”
Palladium atoms generated by thermal evaporation and laser ablation were reacted with and trapped in F2/Ar, F2/Ne, and neat F2 matrices. The products were characterized by electronic absorption and infrared spectroscopy, together with relativistic density functional theory calculations as well as coupled cluster calculations. Vibrational modes at 540 and 617 cm(-1) in argon matrices were assigned to molecular PdF and PdF2, and a band at 692 cm(-1) was assigned to molecular PdF4. A band at 624 cm(-1) can be assigned to either PdF3 or PdF6, with the former preferred from experimental considerations. Although calculations might support the latter assignment, our conclusion is that in these detailed experiments there is no convincing evidence for PdF6.
“…Their solution chemistry is quite well known in aqueous solutions, hydrofluoric acid, or anhydrous HF. [1][2][3][4][5] We set out to explore the reactions of fluorides with liquid ammonia, which could yield substances like fluoride ammoniates, amine fluorides and amide-or imide fluorides, [6][7][8][9] or even nitride fluorides and nitrides as the final products of these reactions. [10] With the exception of the nitrides, all these classes of compounds are only scarcely known and could feature interesting properties depending on the metal ion.…”
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