1. The molecule listed to the left was originally MX, where the symmetry was On. After reduction of the metal center the coordination environment changed and the ligands along the Z-axis elongated(hint: this means that the extent of overlap of orbitals that interact with the z-axis point charges would be lesser than the On molecule). Draw the crystal field splitting of both the On symmetry molecule as well as elongated z-axis molecule with symmetry labels.

1. The molecule listed to the left was originally MX, where the symmetry was On. After reduction of the metal center the coordination environment changed and the ligands along the Z-axis elongated(hint: this means that the extent of overlap of orbitals that interact with the z-axis point charges would be lesser than the On molecule). Draw the crystal field splitting of both the On symmetry molecule as well as elongated z-axis molecule with symmetry labels.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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1.
The molecule listed to the left was originally MX6 where the symmetry was On.
After reduction of the metal center the coordination environment changed and the
ligands along the Z-axis elongated(hint: this means that the extent of overlap of orbitals
that interact with the z-axis point charges would be lesser than the On molecule). Draw
the crystal field splitting of both the On symmetry molecule as well as elongated z-axis
molecule with symmetry labels.

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The ligand-field-stabilization-energies (LFSE) of three pairs of [ML6]** and [ML6]?" complexes are given in the following table. Calculate the difference in LFSE for each pair of reduced and oxidized complexes, that is, the differences in LFSE between [MLs]*" and [MLs]", assuming [ML6]* complexes are low-spin complexes and [ML6J** complexes are high-spin complexes. Arrange the differences in cm' in order of increase in magnitude. A. (cm') [Co(H2O)s]" 16,750 [Co(H;O).J?" [Mn(H20).] 8,400 15,800 [Mn(H2O)s]** 7,850 [Fe(H2O),J** 14,000 [Fe(H2O)«]?* 9,350 A. 5,500 (Fe"/Fe) <9,580 (Mn"/Mn³")< 25,080 (Co"/Co³") B. 5,560 (Fe²"/Fe")<25,080 (Co²"/Co³")< 25,280 (Mn²"/Mn³") C. -20 (Co²"/Co³") <-3,740 (Fe²"/Fe³") < 25,280 (Mn²"/Mn²") D. 24,260 (Fe"/Fe³") < 25,280 (Mn²"/Mn*")< 33,480 (Co"/Co") E. 9,480 (Mn² /Mn³") < 24,260 (Fe²"/Fe³") < 33,480 (Co²"/Co³")
Coordination compund formula & compound name
True/False: The larger the crystal field splitting of the paramagnetic complex ion, theshorter the wavelength of the ligand absorbed. Blue shift. (Circle One) CFSE (larger, smaller) Wavelength (longer, shorter) Spin (high, low) Color absorbed (Red, Blue, Violet, Yellow)
the spectrochemical series allows us to explain the variety ofcolors observed in transition metal complexes. But in practice, someone attempting to predictthe properties of compounds can occasionally be frustrated by various complicating factors.For instance, the nitrite ligand is presented as having a high field strength, but that is only whenit is the nitrogen of the nitrite that is coordinating to the metal center. Nitrite is also capable ofbinding to the metal center through an oxygen, and when this happens, nitrite is a low fieldstrength ligand. Furthermore, many metals initially precipitate as simple ionic salts before theyhave a chance to form more soluble complex ions. And occasionally, unexpected redoxreactions can lead to complex mixtures. The complex that copper forms with chloride ions is tetrahedral. Write the chemical formula for this complex. Thoroughly describe the energy diagram for the d orbitals.