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The higher the oxidation state of the metal, the stronger the ligand field that is created. In the event that there are two metals with the same d electron configuration, the one with the higher oxidation state is more likely to be low spin than the one with the lower oxidation state; for example, Fe 2+ and Co 3+ are both d 6 ; however, the ...
Thus for example neodymium typically forms the +3 oxidation state, despite its configuration [Xe] 4f 4 5d 0 6s 2 that if interpreted naïvely would suggest a more stable +2 oxidation state corresponding to losing only the 6s electrons. Contrariwise, uranium as [Rn] 5f 3 6d 1 7s 2 is not very stable in the +3 oxidation state either, preferring ...
Systematic oxidation state is chosen from close alternatives as a pedagogical description. An example is the oxidation state of phosphorus in H 3 PO 3 (structurally diprotic HPO(OH) 2) taken nominally as +3, while Allen electronegativities of phosphorus and hydrogen suggest +5 by a narrow margin that makes the two alternatives almost equivalent:
An electron may jump from a predominantly ligand orbital to a predominantly metal orbital, giving rise to a ligand-to-metal charge-transfer (LMCT) transition. These can most easily occur when the metal is in a high oxidation state. For example, the colour of chromate, dichromate and permanganate ions is due to LMCT
An example is chromium whose electron configuration is [Ar]4s 1 3d 5 with a d electron count of 5 for a half-filled d subshell, although Madelung's rule predicts [Ar]4s 2 3d 4. Similarly copper is [Ar]4s 1 3d 10 with a full d subshell, and not [Ar]4s 2 3d 9. The configuration of palladium is [Kr]4d 10 with zero 5s electrons.
Element Negative states Positive states Group Notes −5 −4 −3 −2 −1 0 +1 +2 +3 +4 +5 +6 +7 +8 +9 Z; 1 hydrogen: H −1 +1: 1 2 helium: He 0 18
As a result, zinc and cadmium metal are good reducing agents. The elements of group 12 have an oxidation state of +2 in which the ions have the rather stable d 10 electronic configuration, with a full sub-shell. However, mercury can easily be reduced to the +1 oxidation state; usually, as in the ion Hg 2+
In this transformation, iridium changes its formal oxidation state from +1 to +3. The product is formally bound to three anions: one chloride and two hydride ligands. As shown below, the initial metal complex has 16 valence electrons and a coordination number of four whereas the product is a six-coordinate 18 electron complex.