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MOOREHW15 - Chapter 22 Chemistry of Selected Transition...

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Unformatted text preview: Chapter 22: Chemistry of Selected Transition Elements and Coordination Compounds 60. Answer: violet light (mt-100 nm) Strategy and Explanation: Refer to the color wheel provided in Figure 22.22. Draw a line from the color your eyes detect (assuming you are not color blind) through the center of the wheel to the opposite color (the complimentary color). The complimentary color is the color absorbed by the complex. A yellow complex would absorb violet light (~ 400 nm). 62. Answer: With cyanide ligand, A0 should increase, color changes from purple to yellow-orange; with chloride ligand, AD should decrease, color changes purple to a blue. Strategy and Explanation: Cyanide ion is a strong field ligand, thus no should increase. The color of the solution is expected to change to a yellow-orange shade (assuming approximately 450 nm or blue light is absorbed). Chloride ion is a weak field ligand (weaker than water), thus A0 should decrease. The color of the solution is expected to change to a blue shade (assuming approximately 600 nm or yellow light is absorbed). 63. Answer: (a) red (b) 3.7 x 10-19 J; 220 kamol 102. Strategy and Explanation: (a) The complex absorbs green light. The color complimentary is red. The solution color is expected to be red. (b) First, we follow the method described in the solution to Question 7.20 to determine the energy of one photon, then we find kJ/mol: hc _ 6.626x 10—34 J-sx2.998x108mfs —19 Ephoton = A _9 = 3.7 x 10 J 1x 10 m 540 nmx — l Inn —19 23 3.7 x 10 J 1 k1 6.022x 10 photons =220 kamol X X 1 photon 1000 J 1 mol Answer: See structural formula below; there are two possible geometries: the copper complex is shown in a trigonal hipyramidal geometry while the nickel complex is shown in a square pyramidal geometry Strategy and Explanation: Five-coordinated complexes can adapt two possible geometries, either square pyramidal or trigonal bipyramidal. The geometry a given complex adapts depends on a variety of factors which influence the electronic structure of the complex, such as the types of ligands, the central transition metal oxidation number, the complex ion’s surrounding environment (such as counter ion), and crystal packing. In solution both geometries are often in dynamic equilibrium (fluxional) because the energy difference between the two geometries is very small. In the solid state one often sees a structure that is a mixture of the two ideal geometries (i.e., it is neither square pyramidal nor trigonal bypyramidal but rather somewhere in between). Only in cases where there is a clear energetic preference for one structure over another will one geometry be favored. In this case the copper complex is shown in a trigonal bipyramidal geometry while the nickel complex is shown in a square pyramidal geometry. 3, 3— C] Cl CN NC, | .CN (Cu—Cl nNix Cl I NC, \CN ...
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