. 2024 Aug 6;14(34):24652–24660. doi: 10.1039/d4ra03822c

CH₂Cl₂ determined by cyclic voltammetry (BAr^F₄ = [B{3,5-(CF₃)₂C₆H₃}₄]).^a.

E ⁰ (ΔE_p)^a [mV]
1a³⁰	138 (98)	[1a(Ru)₃]	64 (118)	[1a(Rh)₃]	158 (99)
1b³⁰	206 (116)	[1b(Ru)₃]	116 (140)	[1b(Rh)₃]	190 (86)
1c³¹	275 (160)	[1c(Ru)₃]	204 (122)	[1c(Rh)₃]	283 (86)
1d³⁰	113^b	[1d(Ru)₃]	91 (148)	[1d(Rh)₃]	116 (93)

Potentials vs. the FcH/[FcH]⁺ couple at a glassy carbon working electrode (scan rate 100 mV s⁻¹). Determined on 1 mmol per L samples in anhydrous 0.1 mol per L (nBu₄N)BAr^F₄/CH₂Cl₂ as SE (working electrode: glassy carbon). The difference between oxidation and reduction potential, ΔE_p, is given in brackets.

Determined from square-wave voltammetry due to close peak-to-peak separation, leaving ΔE_p inaccessible.

Redox potentials for the first iron-centred oxidation E01 (vs. FcH/[FcH]+) of 1a–d,30,31[1a–d(Rh)3] and [1a–d(Ru)3], in 0.1 mol per L (nBu4N)BArF4/CH2Cl2 determined by cyclic voltammetry (BArF4 = [B{3,5-(CF3)2C6H3}4]).a.

Redox potentials for the first iron-centred oxidation E⁰₁ (vs. FcH/[FcH]⁺) of 1a–d,^30,31[1a–d(Rh)₃] and [1a–d(Ru)₃], in 0.1 mol per L (ⁿBu₄N)BAr^F₄/CH₂Cl₂ determined by cyclic voltammetry (BAr^F₄ = [B{3,5-(CF₃)₂C₆H₃}₄]).^a.