1.1 Porphyrins - Friedrich-Alexander-Universität Erlangen-Nürnberg
1.1 Porphyrins - Friedrich-Alexander-Universität Erlangen-Nürnberg
1.1 Porphyrins - Friedrich-Alexander-Universität Erlangen-Nürnberg
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Discussion and Results 3<br />
Table 24. Determined half-wave potentials E½ for compounds 91 and 92 in comparison to<br />
those obtained for unfunctionalized 53. Values given in V vs. ferrocene E½(Fc/Fc + ) = +0.53 V.<br />
For detailed experimental parameters see paragraph 6.1, p. 138.<br />
Compound E½ Red2 [V] E½ Red1 [V] E½ Ox1 [V] E½ Ox2 [V]<br />
91 -1.02 -0.86 +<strong>1.1</strong>3 +1.35<br />
92 -1.08 -0.79 - a<br />
53 96 -1.23 -0.95 +1.02 +1.25<br />
a only irreversible processes found a<br />
In the cathodic region, both systems show quasi-reversible redox processes whereas in the<br />
anodic region, only for nitro substituted 91 a reversible redox behavior is found. The<br />
irreversible behavior of amino substituted 92 can thereby be due to slowed electron transfer<br />
processes or consecutive chemical reactions leading to detectable cathodic peak potentials<br />
at +0.98 V and +1.08 V of higher peak current ipc and one at +1.37 V of lower ipc while the<br />
corresponding anodic peak potentials at +0.92 V and +0.21 V appear quite separate and only<br />
have very low peak currents. A reliable explanation is not possible based on this data since<br />
several processes might participate in causing that behavior. E.g. a generated porphyrin<br />
radical cation could react with the amino group of another molecule (potentials lie in region<br />
of the first oxidation potential of unfunctionalized 53 96 ) or the amino group could become<br />
oxidized itself and show further reactions. For 91 three reduction processes are detected<br />
whereat the ones of higher potentials show peak currents comparable to the ones observed<br />
for the oxidation processes. For the third process, the half-wave potential can only be<br />
estimated to be around -1.25 V since no clear peaks are observable. The additional reduction<br />
process is thereby due the presence of the reducible nitro group.<br />
Interestingly, for both 91 and 92, the obtained negative half-wave potentials E½ Red are<br />
significantly shifted to higher values compared to 53 (see Table 24) meaning that both<br />
systems are easier to reduce. This effect seems to arise from the higher group<br />
electronegativity of -NH2 and -NO2 (calc. ENG(NH2) = 2.70 and ENG(NO2) = 3.21) compared to<br />
-t-Bu (calc. ENG(NH2) = 2.48). 140 Thus, -NH2 and -NO2 have negative inductive effects easing<br />
electron uptake processes. The same effect is considered to shift the positive half-wave<br />
potentials E½ Ox to higher values for 91 compared to 53 meaning that oxidation is more<br />
difficult to achieve. Thus, the peripheral substituents do indeed influence the electronic<br />
structure of the core system.<br />
- a<br />
121