2.A first row transition metal ion, M³+, was allowed to react with two sets of monodentate ligands, D andE. The complex [MD6]³+ was found to be highly paramagnetic while the complex [ME6]³ was weaklyparamagnetic. Further studies on [ME]³- revealed the weak paramagnetism of the complex arisesfrom the presence of a single unpaired electron. From these pieces of information, answer thefollowing:3+Hybridization of M³+ in [MD]³+ (No need to write the number of orbitals as superscripts, e.g., sp3):Hybridization of M³+ in [MD6]³- (No need to write the number of orbitals as superscripts, e.g., sp3):Identity of M (No need to write the charge; just write the symbol, e.g. Au):Identity of ligand D: [Choose your answer: water, carbon monoxide, ethylenediamine (en)]Identity of ligand E: [Choose your answer: oxalate, bromide, cyanide]

In a complex ion or molecule, the metal ion provides vacant orbitals and the ligand donates its lone…

A first row transition metal ion, M³+, was allowed to react with two sets of monodentate ligands, D and E. The complex [MD6]³+ was found to be highly paramagnetic while the complex [ME6]³ was weakly paramagnetic. Further studies on [ME6]³- revealed the weak paramagnetism of the complex arises from the presence of a single unpaired electron. From these pieces of information, answer the following: Hybridization of M³+ in [MD]³+ (No need to write the number of orbitals as superscripts, e.g., sp3): Hybridization of M³+ in [MD]³- (No need to write the number of orbitals as superscripts, e.g., sp3): Identity of M (No need to write the charge; just write the symbol, e.g. Au): Identity of ligand D: [Choose your answer: water, carbon monoxide, ethylenediamine (en)] Identity of ligand E: [Choose your answer: oxalate, bromide, cyanide]

A first row transition metal ion, M³+, was allowed to react with two sets of monodentate ligands, D and E. The complex [MD6]³+ was found to be highly paramagnetic while the complex [ME6]³ was weakly paramagnetic. Further studies on [ME6]³- revealed the weak paramagnetism of the complex arises from the presence of a single unpaired electron. From these pieces of information, answer the following: Hybridization of M³+ in [MD]³+ (No need to write the number of orbitals as superscripts, e.g., sp3): Hybridization of M³+ in [MD]³- (No need to write the number of orbitals as superscripts, e.g., sp3): Identity of M (No need to write the charge; just write the symbol, e.g. Au): Identity of ligand D: [Choose your answer: water, carbon monoxide, ethylenediamine (en)] Identity of ligand E: [Choose your answer: oxalate, bromide, cyanide]

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...

See similar textbooks

Similar questions

Take into consideration metal Z(III) ion which is able to form octahedral complexes with elther fluoride or cyanide ions, What can be said about the colors of the complexes formed when one complex ion absorbs at 650 nm while the other at 430 nm?
Hexaamminechromium(III) ion, [Cr(NH³)]³+ is a metal complex containing six ammonia ligands i. ii. Using the Valence Bond Theory, construct the hybridization state of [Cr(NH3)6]³+. Predict the observed colour of the complex ion if the absorbed colour is blue-violet and briefly explain your answer.
Among the complex ions formed by M³* (M is a transition metal in 3d block) are the following: [M(H20).J³*, [M(NH;)6]³*, and [MF6]*. These ions have the following 9 observed colors (listed in arbitrary order): yellow-orange, green, and blue. Match each complex with its color. Explain.
Regarding reactions and mechanisms of coordination compounds, complete and balance the equations below. Unless otherwise stated, the reactions proceed at room temperature in water solution. AgCl + S,0,? [Ni(NH3)6]* +CN→ [Co(H,O)6]** + NH3 + NHẠC1 + SeO2 2- fast [Cr(NH3);H¿O]³+ + OH¯ cold water heat [RHCI(NH3)s]? * + Hg²* +H,O
a) Provide the name of the coordination complex Na[COCI,(NH3),] b) Calculate the orbital multiplicity for a Cr** assuming it is a free ion (Not complex). c) Calculate the spin multiplicity of a metal ion Cr* assuming a high spin crystal field. d) Calculate the quantum number S for metal ion Cr 3* assuming a high spin crystal field splitting.
Complete the structure for the trans-diamminedichloridoplatinum (II) coordination complex. Also, select the overall charge of the complex. C H3N CI NH, Answer Bank Cl₂ NH₁ Pt NO₂ N OH overall charge:
3) A transition metal complex ion with octahedral geometry has a value of 4.4 x 10+*J for the crystal field splitting, A.. What is the wavelength for the absorption maximum, Amar for this complex ion? a) 5.0 x 1015 m c) 524 mm b) 452 nm d) 637 nm
Mn(acac)3 was found to have its ground state to 1st excited state absorption at 500 nm (Δo). The pairing energy for this complex is 28,000 cm-1 . Based on this information, draw the populated ground state d orbital diagram for this complex.
A hypothetical metal M forms the following complexes with the generalized ligands X, Y, and Z: Complex ion Observed color [M(X)6]3+ green [M(Y)6]3+ blue [M(Z)6]3+ yellow Order these ligands according to their ability to split d orbitals. In other words, set up a spectrochemical series, from strongest to weakest ligand field strength. Rank from strongest to weakest ligand field strength. -X -Z -Y
Transition metal complexes are highly likely to be colored because of a) the size of the energy gap within the d orbitals and the number of electrons. In ruby, the red color of ruby is attributed to a small amount of Cr³* substituting into Al2O3 which is made up of shared AIO, octahedra. Provide a hypothesis for the origin of the red color observed in ruby. Red pigments tend to be rare. If you had to design a new material that b) had an approximate bandgap that would absorb green, what ideas do you need to employ to find a new semiconductor that does not contain Cd, Hg or Pb as one of the components (see last lecture for ideas).
An octahedral complex having the formula [M(dien)(NH3)(OH2)F] has a total of 15 isomers. In the sum formula “dien” represents the tridentate diethylenetriamine ligand, which can adopt meridional or facial coordination modes. Draw structures of 8 possible isomers, clearly showing any pairs of enantiomers. The tridentante ligand may be abbreviated as below for simplicity.
Cr(aq) + 3 e Cr(s) Zn²(aq) + 2 e → Zn(s) 2 H₂O() +2 e → H₂(g) + 2 OH(aq) Mn2(aq) + 2 e A(an) + 3 e Mn(s) Al(s) 7. All of the following statements concerning ligand field theory are true EXCEPT A. in low-spin complexes, electrons are concentrated in the day, dys, and dr orbitals. B. in an isolated atom or ion, the five d orbitals have identical energy. C. low-spin complexes contain the maximum number of unpaired electrons. D. the crystal field splitting is larger in low-spin complexes than high-spin complexes. E. the energy difference between d orbitals often corresponds to an energy of visible light. 8. All of the following complexes will be colored (in the visible) EXCEPT A. [Co(en)]2+ B. [Fe(CN)6] C. [Ni(H₂O)]²+ D. [Cd(NH3)4]2+ 9. A positron has a mass number of a(n) a. 0; 1+; proton b. 1; 2+; proton c. 0; 1+; electron d. 1; 2+; electron e. 0; 0; proton -0.76 -0.83 -1.18 -1.66 a. [Cr(CO)6]C13 b. [Cu(OH)4(NH3)2] c. K4[Mn(CN)6] d. [Pt(en)3] (NO3)4 e. [Pt(NH3)2(OH₂)CIJ3PO4 10. In which…