Predicting color and magnetic properties from a crystal field theory ener...en a certain strong-field ligand forms a tetrahedral complex with Rhto this electron box diagram:energy in kJ/mol-2002+cation, the energies of the valence d orbitals on the rhodium atom are split according-300xyyzXZ-400-5002Z2 2x-y-600Using this diagram, answer the following questions.How many unpaired d electron spins does the rhodium atomhave?Is the complex paramagnetic or diamagnetic?Predict the color of the complex.paramagneticdiamagneticblue or greenred or violetorange or yellowwhite or transparent

In the given question Rh2+ forms a tetrahedral complex with strong field ligand. The energies of the…

Answered: Predicting color and magnetic…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter8: Bonding In Transition Metal Compounds And Coordination Complexes

Section: Chapter Questions

Problem 45P

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a. In the absorption spectrum of the complex ion Cr(NCS)63, there is a band corresponding to the absorption of a photon of light with an energy of 1.75 104 cm-1. Given 1 cm1 = 1.986 1023 J, what is the wavelength of this photon? b. The CrNC bond angle in Cr(NCS)63 is predicted to be 180. What is the hybridization of the N atom in the Ncs- ligand when a Lewis acid-base reaction occurs between Cr3+ and NCs- that would give a 180 CrNC bond angle? Cr(NCS)63 undergoes substitution by ethylenediamine (en) according to the equation Cr(NCS)63+2enCr(NCS)2(en)2++4NCS Does Cr(NCS)2(en)2+ exhibit geometric isomerism? Does Cr(NCS)2(en)2+ exhibit optical isomerism?
Which of the following statement(s) is( are) true? a. The coordination number of a metal ion in an octahedral complex ion is 8. b. All tetrahedral complex ions are low-spin. c. The formula for triaquatrianuninechromiwn(III) sulfate is [Cr(H2O)3(NH3)](SO4)3. d. The electron configuration of Hf2+ is [Xe]4f126s2. e. Hemoglobin contains Fe3+.
Trimethylphosphine, P(CH3)3, can act as a ligand by donating the lone pair of electrons on the phosphorus atom. If trimethylphosphine is added to a solution of nickel(Il) chloride in acetone, a blue compound that has a molecular mass of approximately 270 g and contains 21.5% Ni, 26.0% Cl, and 52.5% P(CH3)3 can be isolated. This blue compound does not have any isomeric forms. What are the geometry and molecular formula of the blue compound?
Is it possible for a complex of a metal in the transition series to have six unpaired electrons? Explain.
Consider the following complex ion, where A and B represent ligands. The complex is known to be diamagnetic. Do A and B produce very similar or very different crystal fields? Explain.
Draw the Crystal field diagrams for [Fe(NO2)6]4- and [FeF6]3-. State whether each complex is high spin or low spin, paramagnetic or diamagnetic, and compare ?oct to P for each complex.
The square-planar complex Pt(en)Cl2 has chloride ligands in a cis configuration. No trans isomer is known. Based on the bond lengths and bond angles of carbon and nitrogen in the ethylenediamine ligand, explain why the trans compound is not possible.
Give the coordination number for each metal ion in the following compounds: (a) [Co(CO3)3]3- (note that CO32- is bidentate in this complex). (b) [Cu(NH3)4]2+. (c) [Co(NH3)4Br2]2(SO4)3. (d) [Pt(NH3)4][PtCl4]. (e) [Cr(en)3](NO3)3. (f) [Pd(NH3)2Br2] (square planar). (g) K3[Cu(Cl)5]. (h) [Zn(NH3)2Cl2]
Define the terms complex ion, ligand, and coordination number. Use an example to illustrate the use of these terms.
Ammonia and potassium iodide solutions are added to an aqueous solution of Cr(NO3)3. A solid is isolated (compound A), and the following data are collected: i. When 0.105 g of compound A was strongly heated in excess 0 2, 0.0203 g CrO3 was formed. ii. In a second experiment it took 32.93 mL of 0.100 M HCI to titrate completely the NH3 present in 0.341 g compound A. iii. Compound A was found to contain 73.53% iodine by mass. iv. The freezing point of water was lowered by 0.64C when 0.601 g compound A was dissolved in 10.00 g H2O (Kf =1.86Ckg/mol). What is the formula of the compound? What is the structure of the complex ion present? (Hints: Cr3+ is expected to be sixcoordinate, with NH3 and possibly I as ligands. The I ions will be the counterions if needed.)
Experiments show that K4[Cr(CN)6] is paramagnetic and has two unpaired electrons. The related complex K4[Cr(SCN)6] is paramagnetic and has four unpaired electrons. Account for the magnetism of each compound using the ligand field model. Predict where the SCN ion occurs in the spectro-chemical series relative to CN.

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