Oxidation of S = 3/2 [Co(TACN)_2]^+2 produces a much more stable, almost colorle
ID: 917392 • Letter: O
Question
Oxidation of S = 3/2 [Co(TACN)_2]^+2 produces a much more stable, almost colorless, diamagnetic (S = 0) complex, [Co(TACN)_2]^+3. Bond length changes caused by this oxidation are symmetric and equivalent for the axial and equatorial ligands Why are the bond distance changes identical for all bonds From what you know about the Laporte and spin selection rules why do you think [Co(TACN)_2]^+3, is ~colorless (ie, incredibly weakly colored) What would the excited state look like What do the changes in magnetic properties (S = 3/2 rightarrow S = 0) tell you about the magnitude of TACN's ligand field strength (ie, delta_0) relative to the pairing energy (P) for each of these complexes, [Co(TACN)_2]^+2 and [Co(TACN)_2]^+3 If the Co(111) complex were high-spin, how would its electronic spectrum differ from its Co(11) precursorExplanation / Answer
7a. For a given octahedral complex, the five d atomic orbitals are split into two degenerate sets when constructing a molecular orbital diagram. These are represented by the sets' symmetry labels: t2g (dxz, dyz, dxy) and eg (dz2 and dx2y2). When a molecule possesses a degenerate electronic configuration 1s2 2s2p6 3s2p6d7.
In general, density functional theory finds increasingly broad application in the chemical and material sciences in transition metals there must be degeneracy in either the t2g or eg orbitals. The electronic states of octahedral complexes are classified as either low spin or high spin. The spin of the system is dictated by the chemical environment. This includes the characteristics of the metal center and the types of ligands. the bonding and antibonding pair of electrons are equal in [Co(TACN)]3+ complex.
7b. The Selection Rules governing transitions between electronic energy levels of transition metal complexes are:
The first rule says that allowed transitions must involve the promotion of electrons without a change in their spin. The second rule says that if the molecule has a center of symmetry, transitions within a given set of p or d orbitals (i.e. those which only involve a redistribution of electrons within a given subshell) are forbidden. Charge transfer, either ligand to metal or metal to ligand. These are often extremely intense and are generally found in the UV but they may have a tail into the visible.and d-d transition, these can occur in both the UV and visible region but since they are forbidden transitions have small intensities.
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