### Study of Complex Ions Formed by Group 6B Transition Metals**Introduction:**A chemist is studying the complex ions formed by group 6B transition metals. Upon forming a complex ion with CO ligands, denoted as [M(CO)6]2+, the unknown 6B metal ion appears red. The study involves analyzing the d-orbital energy diagrams for complexes with different ligands and comparing their properties.**a. Drawing the d-Orbital Energy Diagram for [M(CO)6]2+:**- **Ligand Context:** CO is assumed to be a strong field ligand.- **Diagram Requirements:** Draw the energy levels of the d-orbitals and include the placement of electrons.**b. Replacement of CO Ligands with Water Ligands:**The scientist replaces the CO ligands of the original complex, [M(CO)6]2+, with water ligands (H2O). In this case:- **Ligand Context:** Assume water is a weak field ligand.- **Diagram Requirements:** Draw the energy levels of the d-orbitals for the new complex, including the placement of electrons.- **Color Expectation:** Describe the expected color change of the ion and explain why.**c. Bond Analysis:**Discuss the similarity and difference between:- The bond holding together the Carbon (C) and Oxygen (O) in CO.- The bond between CO and the metal center in the complex.**d. Spin Comparison of Complexes:**Compare the spin states of the complexes:- Determine whether the complex in (a) has a higher or lower spin than that in (b).- Explain the reasoning behind the comparison based on ligand field strength.**Diagrams and Explanation:**- For part a, you would illustrate how the strong field ligand (CO) causes a large splitting in the d-orbitals, typically leading to a low-spin configuration.- For part b, you would show that the weak field ligand (H2O) causes a smaller splitting of the d-orbitals, which usually results in a high-spin configuration.**Conclusion:**These evaluations help understand how different ligands influence the electronic configuration, color, and spin states of transition metal complexes. The use of CO (a strong field ligand) typically leads to low-spin configurations and distinct colors due to the larger splitting of d-orbitals, whereas water (a weak field ligand) favors

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1.A chemist is studying the complex ions formed by group 6B transition metals. When the unknown 6B metal forms a complex ion with CO ligands, [M(CO)F*, it appears red. a. Draw the d-orbital energy diagram, including electrons, for this metal. Assume CO is a strong field ligand. b. The scientist then replaces the CO ligands of the original complex, [M(CO)6]*, with water ligands. Assume water is a weak field ligand. Draw an energy diagram of the d orbitals, including electrons, for this metal. Describe what color you might now expect the ion to appear and why. c. Name one similarity and one difference between the bond holding together the C and the O of CO and the bond between CO and the metal center? d. Does the complex in la have a higher or lower spin than that in lb? Why?

1.A chemist is studying the complex ions formed by group 6B transition metals. When the unknown 6B metal forms a complex ion with CO ligands, [M(CO)F, it appears red. a. Draw the d-orbital energy diagram, including electrons, for this metal. Assume CO is a strong field ligand. b. The scientist then replaces the CO ligands of the original complex, [M(CO)6], with water ligands. Assume water is a weak field ligand. Draw an energy diagram of the d orbitals, including electrons, for this metal. Describe what color you might now expect the ion to appear and why. c. Name one similarity and one difference between the bond holding together the C and the O of CO and the bond between CO and the metal center? d. Does the complex in la have a higher or lower spin than that in lb? Why?

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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