Aqua Ion
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Color of complex ions?
cyano complex ions of transition metals such as Fe 2 + and Cu 2 + are often yellow, while the complex Ofter Aqua green or blue. u can explain the basis for this difference in color. thanks
I can, but to explain adequately takes about five hours, and is based on a large number of molecular orbital theory. Very abbreviated form: The color you see is the white light of any color less absorbed by the material. (We ignore Usually. emission fluorescence, etc.) A material that absorbs high-violet light energy is converted into yellow. A material that absorbs less energy orange or red displayed in blue or green, respectively. (First hypothesis significant uptake in the visible range, which is not always true.) Which means that the cyano complex will absorb more energy of the light that the aquo complex. So far so good. The electrons in the molecules have energies that are quantified in certain energy levels. Electrons may undergo transitions from one level to another, and a way to get hit with a photon of light energy which corresponds exactly to the transition - If a photon has an energy of 350 kJ / mol and a transition is available from 350 kJ / mol, when the molecule absorbs the photon and electron low-energy jumps a higher one. The light energy is to measure the energy difference between the orbitals. This means that the cyano complexes have larger gaps that the complex energy aqueous. In transition metal complexes, the colors are usually due to electrons jumping between the d-orbitals. (Neglects charge transfer absorptions). Complexes octahedral in MC, there are two levels of d-orbitals. When the molecule absorbs a photon, an electron hops from the d orbitals below below above. (Oh, God awful simplified Figgis and Orgel and Tanabe and Sugano turn in their graves, but really do enough to serve our purposes.) In a pool complex, the set of base metal D-orbitals are non-adherence, which means that do not interact strongly with water ligands. The difference is relatively small. In a complex cyano, interact less strongly with the CN-groups, and become very sticky, and have dramatically reduced energy. The gap between the two groups increases as just move the bottom is lower. (Translation of the AM to the crystal field theory: the cyanide ligand field is much stronger than if you increase the division H2O orbital). Tan CN-ligands causes greater energy difference between D-orbital complex water cyano ligands therefore have to absorb high energy photons can cause the transition cyano complexes to absorb the energy of violet light rising lower energy rather than red or orange, if the cyano complexes are yellow instead of blue or green. Want to noted that the ligand is a single variable. The metal oxidation state also play a role. Aqueous metal complex can be red yellow green blue purple and colorless, just choose the right metal. Cyano complexes have different colors of yellow ferricyanide (potassium ferrocyanide instead you mention) is bright red, for example. Fe (II) to Fe (III) changes the color. (Nevermind adding Fe (III) cyano Fe (II) of its complex, resulting in Prussian blue.
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