Iron's oxidation state in oxyhemoglobin
Assigning oxygenated hemoglobin's oxidation state is difficult because oxyhemoglobin (Hb-O 2 ), by experimental measurement, is diamagnetic (no net unpaired electrons), yet the lowest-energy (ground-state) electron configurations in both oxygen and iron are paramagnetic (suggesting at least one unpaired electron in the complex). The lowest-energy form of oxygen, and the lowest energy forms of the relevant oxidation states of iron, are these: Triplet oxygen, the lowest-energy molecular oxygen species, has two unpaired electrons in antibonding π* molecular orbitals. Iron(II) tends to exist in a high-spin 3d6 configuration with four unpaired electrons. Iron(III) (3d5) has an odd number of electrons, and thus must have one or more unpaired electrons, in any energy state. All of these structures are paramagnetic (have unpaired electrons), not diamagnetic. Thus, a non-intuitive (e.g., a higher-energy for at least one species) distribution of electrons in the combination of iron and oxy...
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