Preparation and kinetics of hydrolysis of pentaammineperrhenatocobalt(III) ion

Ferromagnetic Exchange Coupling in a Family of MnIII Salen-Type Schiff-Base Out-of-Plane Dimers

“…The magnitude of J Mn–Mn* appears to correlate with the Mn–X bond distances within a very narrow region (2.099(3)–2.270(2) Å), which looks to be related to the effect of the axial ligands rather than the substituent of the saltmen ligands (Figure b). The magnitude of J Mn–Mn* displayed the order H 2 O ≈ ReO 4 – > NO 3 – > N 3 – ≈ NCS – , which differs from the spectrochemical series ranking of ReO 4 – < N 3 – < NO 3 – < H 2 O < NCS – . , This is not surprising because different metal centers were used. The magnetochemical series found for the spin-state mixing in iron­(III) porphyrins displayed the order H 2 O < ReO 4 – < NCS – < N 3 – . , Thus, the J Mn–Mn* vs Mn–X trend with the J Mn–Mn* ∝ Mn–X relationship in our study (Figure b) is more similar to the magnetochemical series than the spectrochemical one, which is the reverse trend to the J Mn–Mn* ∝ (Mn–O1*) −1 relationship.…”

“…The magnitude of J Mn−Mn* appears to correlate with the Mn−X bond distances within a very narrow region (2.099(3)− 2.270(2) Å), which looks to be related to the effect of the axial ligands rather than the substituent of the saltmen ligands (Figure 3b). The magnitude of J Mn−Mn* displayed the order 52,53 This is not surprising because different metal centers were used. The magnetochemical series found for the spin-state mixing in iron(III) porphyrins displayed the order…”

Rhenium(VII) Compounds as Inorganic Precursors for the Synthesis of Organic Reaction Catalysts

“…Rhenium in the +7 oxidation state has ability to create many complex compounds, however, in this paper only one ammonium complex, i.e., hexaamminecobalt(III) perrhenate was discussed. Ammonium complex compounds containing metals like: copper(II), cobalt(II), cobalt(III), zinc(II), nickel(II), cadmium(II) and have been already described in the literature [36,37,38,39,40]. The history of these compounds dates back to 1933, when synthesis methods and selected properties were reported by Wilke-Dorfurt and Gunzert [37].…”

“…Another cobalt complex, namely [Co(NH 3 ) 5 (ReO 4 )](ReO 4 ) 2 , was described by Lenz and Murmann. Their procedure was composed of two stages: in the first, [Co(NH 3 ) 5 H 2 O](ClO 4 ) 3 was dissolved in water and exposed to HReO 4 , resulting in the formation of [Co(NH 3 ) 5 (H 2 O)](ReO 4 ) 3 ·2H 2 O, which in the second stage was dried initially under vacuum for 3 h at 50–60 °C to produce a pink [Co(NH 3 ) 5 (H 2 O)](ReO 4 ) 3 complex, followed by further drying at 95–130 °C for 2–5 h to obtain the violet [Co(NH 3 ) 5 (ReO 4 )](ReO 4 ) 2 [38].…”

Complex ion kinetics. Reaction rates on ion-exchange resins compared to those in water

“…Use of ion-exchange resins has been made in determining the charge of ions,2 the degree of polymerization,3 the number and type of products of a reaction,4 and the rate of reaction5 and in preparative experiments. 6 It has been especially valuable in the reaction product separation of complex ions for analytical7 and preparative 8 purposes. Considerable time is required for many of these separations during which reactions may occur on the complex ions being separated.…”