The energies of the valence d orbitals on the iron atom in the octahedral \([ \text{Fe(NH}_3\text{)}_6 ]^{2+}\) complex are split according to the electron box level diagram below.(Note: the d orbitals are labeled with just their subscript, to make the labels easier to read.)Complete the diagram by adding the correct number of electrons to each orbital.**Diagram Explanation:**- The diagram is divided into two levels representing different energy states of the d orbitals in an octahedral crystal field.- The vertical axis is labeled as "energy" and represents increasing energy as you move upwards.- The top level has boxes labeled \(d_{z^2}\) and \(d_{x^2-y^2}\), indicating these orbitals have higher energy.- The bottom level has boxes labeled \(d_{xy}\), \(d_{yz}\), and \(d_{xz}\), indicating these orbitals have lower energy.- There is also a section on the right with buttons labeled "1", a down arrow, and an eraser, along with "×" and a curved arrow, suggesting tools for adding, removing, or resetting electrons in the diagram.

The energies of the valence d orbitals on the iron atom in the octahedral (Note: the d orbitals are labeled with just their subscript, to make the labels easier to read.) Complete the diagram by adding the correct number of electrons to each orbital. 1 energy xy yz xz X | S [Fe(NH3)]* complex are split according to the electron box level diagram below. +

The energies of the valence d orbitals on the iron atom in the octahedral (Note: the d orbitals are labeled with just their subscript, to make the labels easier to read.) Complete the diagram by adding the correct number of electrons to each orbital. 1 energy xy yz xz X | S [Fe(NH3)]* complex are split according to the electron box level diagram below. +

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

Write the balanced net ionic equation including heat in the equation. The reaction is exothermic.
Draw the molecular orbital diagram for [Ti(H2O)s]³* with the electrons filled in the orbitals. Clearly label the bonding and anti-bonding orbitals.
Given that the cyanide ion is a high field ligand, determine the electron structure of [Co(CN)6] using an energy diagram of the d orbitals established according to the crystal field theory.
Q5 Explain why [FeF.] is colorless whereas [COFJ is colored but exhibits only a single band in the visible region of the spectrum. C Fe: 4s'3d Co: 4s 3d
Use the thermodynamic data below to compute the average bond enthalpy of the metal-ligand bonds in [Cu(NH3)4]2+(aq). Species ΔfH0kJ/mol S0J/mol/K NH3(aq) -80.29 111.3 Cu2+(aq) 64.77 -99.6 [Cu(NH3)4]2+(aq) -348.5 273.6 Include 3 significant figures
5. Explain why [Fe(OH2)6]2+ is stable in aqueous solution but [Ti(OH2)6]4+ has never been isolated. 6. [Fe(OH₂)6]²+ is more readily oxidised in aqueous solution than [Fe(CN)6]. Briefly explain this observation.
Which of the following can exhibit geometric isomersim? [Zn(NH3)2Cl2] tetrahedral [Pt(NH3)2Cl2] square planar All of these can exhibit geometric isomerism. [Cu(NH3)5Cl]2+ [Cu(NH3)4]2+ square planar
#3
explain why [CoBr4]^-2 is green while [Co(NH3)6]^2+ is orange