Abstract
Oxyhemoglobin is diamagnetic (S=0). Assuming that the oxidation state is Fe2+ and the electronic configuration is t 62 , the spin of the six 3d electrons will be paired and we should not expect any paramagnetism from this source. But the ground state of molecular oxygen is known to be a triplet (S= 1). Why, then, does oxyhemoglobin not exhibit paramagnetism attributable to the presence of O2?
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© 1974 Springer-Verlag Berlin Heidelberg
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Weissbluth, M. (1974). Further Aspects. In: Hemoglobin. Molecular Biology Biochemistry and Biophysics, vol 15. Springer, Berlin, Heidelberg. https://doi.org/10.1007/978-3-642-80801-2_9
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DOI: https://doi.org/10.1007/978-3-642-80801-2_9
Publisher Name: Springer, Berlin, Heidelberg
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