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With so-called "strong field ligands" such as cyanide, the five electrons pair up as best they can. Thus ferricyanide ([Fe(CN) 6] 3− has only one unpaired electron. It is low-spin. With so-called "weak field ligands" such as water, the five electrons are unpaired. Thus aquo complex ([Fe(H 2 O) 6] 3+ has only five unpaired electrons. It is ...
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Due to its 4 unpaired electrons in 3d shell, an iron atom has a strong magnetic moment. Ions Fe 2+ have also 4 unpaired electrons in 3d shell and Fe 3+ have 5 unpaired electrons in 3d shell. Therefore, when crystals are formed from iron atoms or ions Fe 2+ and Fe 3+ they can be in ferromagnetic, antiferromagnetic, or ferrimagnetic states.
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Therefore, addition or removal of electron has little effect on complex stability. In this case, there is no restriction on the number of d-electrons and complexes with 12–22 electrons are possible. Small Δ oct makes filling e g * possible (>18 e −) and π-donor ligands can make t 2g antibonding (<18 e −).
Atoms are called "electron-deficient" when they have too few electrons as compared to their respective rules, or "hypervalent" when they have too many electrons. Since these compounds tend to be more reactive than compounds that obey their rule, electron counting is an important tool for identifying the reactivity of molecules.
Iron(II) is a d 6 center, meaning that the metal has six "valence" electrons in the 3d orbital shell. The number and type of ligands bound to iron(II) determine how these electrons arrange themselves. With the so-called "strong field ligands" such as cyanide, the six electrons pair up.
Since the table of standard electrode potentials is defined for a transfer of one mole of electrons, care must be made in determining an electrode potential using two other electrode potentials. Adjustments have to be made for the number of electrons being transfered. For example: (eq1) Fe3+ + 3e- --> Fe(s) is listed as -0.036V