The energies of the valence d orbitals on the cobalt atom in the octahedral [CoF6] 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.energyxyZ22 2x-yyzXZ1し

Step 1: Step 2: Step 3: Step 4:

Answered: The energies of the valence d orbitals…

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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Question five
What is the charge on each of the following complex ions? hexaaquairon(II), [Fe(H2O)6]? tris(carbonato)ferrate(III), [Fe(CO3)3]? diaquatetrachlorovanadate(III), [V(H2O)2Cl4]? Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).
Q4/ geometrical isomerism is found in square planar and octahedral complexes but not found in tetrahedral complexes? Q5/ Which of the following can function as a bidentate ligand? NH₁, CO, CO, OH
The solid anhydrous solid CoCl2 is blue in color. Because it readily absorbs water from the air, it is used as a humidity indicator to monitor if equipment (such as a cell phone) has been exposed to excessive levels of moisture.Predict what product is formed by this reaction, and how many unpaired electrons this complex will have.
Answer the following questions about the transition metals complexes with the chemical formulas [Co(en)3]3+and [CoCl6]3- Would either the low-spin or high-spin configuration result in a paramagnetic complex? One of the complexes is orange while the other is blue. Which cobalt complex is which color? Justify your answer and identify which color the complex will absorb based on its color.
The complex ion CoCl42- has a tetrahedral structure. How many d electrons are on the Co? What is its electronic configuration? Why is the tetrahedral structure stable in this case?
The compound [Fe(H2O)6]SO2 has a pale green color. The compound K4[Fe(CN)6] has a bright yellow color. Which of the following statements are NOT true? Select the correct answer below: A) The compound K4[Fe(CN)6] absorbs higher energy light. B) H2O produces a stronger ligand field than CN−. C) The compound K4[Fe(CN)6] is likely a low-spin complex because it contains strong-field ligands. D) The compound [Fe(H2O)6]SO2 is likely a high-spin complex because it contains weak-field ligands.
2+ When a certain strong-field ligand forms a tetrahedral complex with Zn cation, the energies of the valence d orbitals on the zinc atom are split according to this electron box diagram: energy in kJ/mol -200 -300 -400 -500 -600 xy yz 2 Z 2 2 х -у XZ Using this diagram, answer the following questions. How many unpaired d electron spins does the zinc atom have? Is the complex paramagnetic or diamagnetic? Predict the color of the complex. 0 O paramagnetic O diamagnetic O blue or green O red or violet O orange or yellow O white or transparent.
Which ligand formula and name combination is correct? A NH3, ammonia B C D III E I-, iodino CN-, cyanide SCN, sulfur cyanide Br, bromo
What are the electron configurations for an octahedral d7 complex with 1 weak-field and 2 strong-field ligands?
Experiments can measure not only whether a compound is paramagnetic, but also the number of unpaired electrons. It is found that the octahedral complex ion [Fe(CN),]³- has fewer unpaired electrons than the octahedral complex ion [Fe(OH,),J³*. How many unpaired electrons are pre- sent in each species? Explain. In each case, express the CFSE in terms of A..

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