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Онлайн bitcoin казино рулетка с живым дилером
Онлайн bitcoin казино рулетка с живым дилером
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This is a very narrow viewpoint and leads to lots of mistakes: for example $\ce{[co(h2o)6]^3+}$ is low-spin although $\ce{h2o}$ is fairly low on the spectrochemical series. In truth it depends on (at least) the ligand, the metal, as well as the oxidation state, and there is no magic formula or rule that allows you to combine all three factors. Question 18 20 pts consider two octahedral complexes of co3+: [co (cn). 13- and (co (h2o). ]3+ (20 points) (a). Use the following diagrams to indicate the possible orbital diagrams for [co (cn)6] and [co (h20). ]3+ (assume octahedral geometries for both). The charge on the complex is 3+, so the configuration of the cr ion is 3d3. Placing the electrons in the crystal field splitting diagram for an octahedral complex given in figure 28. 29 according to hund’s rule gives three electrons in the t 2g orbitals. The cfse = 3 × (–0. 4 o) + 0 × (+0. 6 o) = –1. 5 high spin or low spin? Question: how many unpaired electrons do you expect for [co(cn)6]3- ? is this a high-spin or low-spin complex ion? Different ligands are associated with either high or low spin — a "strong field" ligand results in a large ∆o and a low spin configuration, while a "weak field" ligand results in a small ∆o and a high spin configuration. For more details, see the crystal field theory (cft) page. Definition: crystal field stabilization energy. The crystal field stabilization energy is defined as the energy of the electron configuration in the ligand field minus the energy of the electronic configuration in the isotropic field. Cfse = δe = eligand field − eisotropic field. The csfe will depend on multiple factors including:
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Consider the coordination compound, na ]. The lewis acid is. (a) both chromium metal ions are paramagnetic with 3 unpaired electrons. (e) the two complexes absorb their complementary colors. (a) usually produce high spin complexes and small crystal field splittings. (b) usually produce low spin complexes and small crystal field splittings. Different ligands are associated with either high or low spin — a "strong field" ligand results in a large ∆o and a low spin configuration, while a "weak field" ligand results in a small ∆o and a high spin configuration. For more details, see the crystal field theory (cft) page. Do you expect the \([cof_6]^{3-}\) complex ion to be high or low spin? solution. What do we know? the complex has an octahedral shape; f-is a weak-field ligand; the d electron configuration for co is d 6; the splitting energy is small; therefore, the complex is high spin. The charge on the complex is 3+, so the configuration of the cr ion is 3d3. Placing the electrons in the crystal field splitting diagram for an octahedral complex given in figure 28. 29 according to hund’s rule gives three electrons in the t 2g orbitals. The cfse = 3 × (–0. 4 o) + 0 × (+0. 6 o) = –1. 5 high spin or low spin? This is a question that the crystal field theory cannot answer because of its inherent shortcomings. The crystal field theory assumes point-type charges approaching the central metal from the coordinate axes leading to the destabilisation of those $\mathrm d$ orbitals that do not feature a nodal plane in the coordinate axes: $\mathrm{d}_{x^2-y^2}$ and $\mathrm{d}_{z^2}$. Question: how many unpaired electrons do you expect for [co(cn)6]3- ? is this a high-spin or low-spin complex ion?
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