a) Consider the following two cobalt complexes: [Co(H2O)2(OH)4] Complex A [Co(CO)6]3+ Complex B (i) Draw the d-electron configuration for A and B. Label each set of orbitals. (ii) Explain how the d-electron configuration changes when cobalt is replaced by iridium in A and B. (iii) Calculate the CFSE for A and B. Show all calculations and units. (iv) Which of these two complexes (A or B) will interact with a magnet? Motivate your answer.

a) Consider the following two cobalt complexes: [Co(H2O)2(OH)4] Complex A [Co(CO)6]3+ Complex B (i) Draw the d-electron configuration for A and B. Label each set of orbitals. (ii) Explain how the d-electron configuration changes when cobalt is replaced by iridium in A and B. (iii) Calculate the CFSE for A and B. Show all calculations and units. (iv) Which of these two complexes (A or B) will interact with a magnet? Motivate your answer.

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

Depict and explain the Crystal field stabilization theory based on the color the below complexes. (i) [Co(NH3)5(H₂O)3+][CI-]3 red (ii) [Co(NH3)5C12+][CH]2 purple
Sketch the following complexes. If more than one enantiomer exists, sketch just one.(a) mer-Cr(NH3)3(Cl)3 (b) cis-[Fe(H2O)4(CN)2]Cl (c) trans-[Ni(en)2Cl2] (d) fac-Co(NH3)3(CN)3
Determine if each of the following complexes exhibits geometric isomerism. If geometric isomers exist, determine how many there are. (a) octahedral [Fe(o-phen)2Cl2]+.
You have a solution of the following ion: [Fe(H2O)6]3+ a) Is the ion more likely paramagnetic or diamagnetic? Please explain. b) Predict how the crystal field splitting would change (increase or decrease) if all H2O ligands were replaced by NO2- in your solution. c) What is the general color of your original solution and how would the color change in part “b”?
What is the formula for the complex ion made by iron(IIl) with 4 aqua and two thiosulfato (S,0022) ligands? Decide if the complex could be isolated as a chloride salt or a potassium salt and write the chemical formula for the salt.
Write the valence electron configuration for the cobalt ions in the complexes [Co(H2O)6]2+ and draw labelled crystal field splitting diagram (relative to the spherical ion) and calculate the magnetic moment, µ(spin-only) of the cobalt ion in the complexes and as a free metal ion.
Naming complex anions with one type of ligand Name the following complex ions. formula [ca] [v(co)] [MoBr4] name ☐ ☑
Which of the following complexes does not have any optical isomers? Group of answer choices [Ru(phen)2(CN)2] [Co(NH3)Cl5]2- [Mo(NH3)(H2O)(OH)(CN)(CO)Cl]+ [Cu(NH3)(H2O)(OH)Cl], tetrahedral geometry
2. Use crystal field theory to predict the unpaired elections for the following and determine the magnetic moments (spin-only): (a) [Co(H₂O)6]²+ (b) [Cr(H₂O)6]³+ (c) [Fe(CN)6]³- (d) [Fe(CO)s]
Which is correct and which is incorrect from the following sentences? In any case, give a brief explanation. Proposition True False The complex ions [CoF6] 3- and [Co (CN) 6] 3– have the same magnetic properties. 2. The nd orbitals of the central atom of a complex have the same energy. 3. The energy of the d orbitals of the central atom of a complex is higher than the corresponding energy of the free atom or ion. d². d -2 4. In tetrahedral symmetry complexes, the orbitals and are less distant from the dxy dxz² dyz ² substituents than the resulting in a higher energy level. 5. Non-oxidizing acid solutions react with all first-order transition metals.
Cobalt(III) has a coordination number of 6 in all its complexes. Is the carbonate ion amonodentate or bidentate ligand in the [Co(NH3)4(CO3)] + ion?
1. Determine whether the following complexes are low spin or high spin complex (i) (ii) [Co(CN)G]* [CoF6]3- To support you answer, draw the electrons arrangement at t2g and eg sub-orbitals. Explain further why the complexes exhibit different electron arrangements.