When compared to that of the free thiourea, the vibrational frequency of carbon-sulfur bond in [Cu(tu)3]^+ complex is: a. none of these b. the same C. lower d. higher
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Please solve this fast,please teacher
![When compared to that of the free thiourea,
the vibrational frequency of carbon-sulfur
bond in [Cu(tu)3]^+ complex is:
a. none of these
b. the same
c. lower
d. higher](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc19ad20b-12df-4c1a-a3e4-3bd5b251a181%2F766722cb-a743-4169-8066-75d85eb63ec3%2F3m5sdme_processed.jpeg&w=3840&q=75)
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- The stretching vibration of CO (g) is found at 2138 cm-1. The band is almost always displaced to lower wave number upon coordination of CO to a metal. Explain why this is the case.According to the IR spectroscopy results of [Co(NH3)5ONO]Cl2 and [Co(NH3)5NO2]Cl2 complexes, the symmetrical and asymmetrical NO stretching vibrations found for one of the complexes (I) are 1315 and 1430 cm-1, respectively, for the other complex (II). these values are 1065 and 1430 cm-1, respectively. According to the data, complex (I) is …………… and complex (II) is ………….Explain Jhane Teller distortions for Co(II) octahedral LS and HS complexes?
- The mating energy of the [CoF6]3- ion is 21000 cm−1, and ∆0 is 13000 cm−1. By calculating the KAKE of both the low and high spin states of the complex, determine in which state the compound is more stable.Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all workUse the calculations of CFSE to explain why [Ni(H2O)6]2+ is more reactive than [Co(NH3)6]3+ and [Cr(NH3)6]3+. Assign the number of electronic transitions expected for complexes in the above question. predict the number of peeaks
- Calculate ∆ in kJ/mol if a d1 complex has an absorption maximum at 545 nm.Which statement is true regarding ligand-to-metal charge transfer (LMCT) transitions? Group of answer choices electrons are excited from an orbital on one ligand to an orbital on another ligand electrons are excited from an orbital in the metal center to one on a ligand electrons are excited from a ligand-based orbital to one in the metal center Typical LMCT molar absorptivities are around 10 M-1 cm-1Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (I have a, b, and c, I need help with d, e, and f.) (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work. (b) How many valence d electrons does the metal center have? Justify your answer. (c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers. (d) What electronic transition results from absorption of 864-nm light? (e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy. (f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?
- By using the given 1) electronic absorption spectrum, 2) the Tanabo-Sugano diagram for d3 complex in octahedral ligand field and 3) the absorption/emission spectra, explain the following: a) Ligand field states (to support your explanation show the filling of the orbitals) b) Radiative transitions (to support your explanation refer to fluorescence, phosphorescence and Stokes’ shift)Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work. (b) How many valence d electrons does the metal center have? Justify your answer. (c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers. (d) What electronic transition results from absorption of 864-nm light? (e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy. (f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?Electronic spectra of transition metals complexes are deduced from the term symbols. Please provide 2 other processes that can lead to intense light absorption in transition metal complexes