Hi would really need help with question 2 only, typed question below: 2. For which of the following pairs would you expect ∆o to be larger and why? a) [Cr(H2O)6]2+ and [Cr(H2O)6]3+ b) [CrF6]3- and [Cr(NH3)6]3+ c) [Fe(CN)6]4- and [Fe(CN)6]3- d) [Ni(H2O)6]2+ and [Ni(en)3]2+ e) [MnF6]4- and [ReF6]4- f) [Ni(en)3]2+ and [Ni(en)3]2+
Hi would really need help with question 2 only, typed question below: 2. For which of the following pairs would you expect ∆o to be larger and why? a) [Cr(H2O)6]2+ and [Cr(H2O)6]3+ b) [CrF6]3- and [Cr(NH3)6]3+ c) [Fe(CN)6]4- and [Fe(CN)6]3- d) [Ni(H2O)6]2+ and [Ni(en)3]2+ e) [MnF6]4- and [ReF6]4- f) [Ni(en)3]2+ and [Ni(en)3]2+
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 66AP
Related questions
Question
100%
Hi would really need help with question 2 only, typed question below:
2. For which of the following pairs would you expect ∆o to be larger and why?
a) [Cr(H2O)6]2+ and [Cr(H2O)6]3+
b) [CrF6]3- and [Cr(NH3)6]3+
c) [Fe(CN)6]4- and [Fe(CN)6]3-
d) [Ni(H2O)6]2+ and [Ni(en)3]2+
e) [MnF6]4- and [ReF6]4-
f) [Ni(en)3]2+ and [Ni(en)3]2+
![1. a)
b)
c)
Tutorial 4
Sketch the representations of the 3d orbitals to show their orientations in space.
Explain why the day orbital is lower in energy than the dx2-y2 orbital in an octahedral complex.
Sketch the possible d-electron configurations for a d6 ion in octahedral crystal field, and give
an example of a complex with this arrangement.
2. For which of the following pairs would you expect to be larger and why?
a) [Cr(H₂O)]²+ and [Cr(H₂O)]³+
[CrF6] and [Cr(NH3)6]³+
c) [Fe(CN)6] and [Fe(CN)6]³-
e) [MnF6] and [ReF6]4
b)
d)
f)
[Ni(H₂O)]²+ and [Ni(en)3]²+
[Ni(en)3]2+ and [Ni(en)3]²+
3. Experimental evidence indicates that the complex K4[Fe(CN)6] has no unpaired electrons, while
[Fe(H₂O)6]Cl2 has four unpaired electrons.
(i) For both complexes give the coordination geometry, the oxidation state and the number of d
electrons.
(ii) Using crystal field energy diagrams, explain the experimental findings.
4. Experimental evidence indicates that the complex [PdCl4] ²- has no unpaired electrons, while
[NiC14]²- has two unpaired electrons.
(i) Describe two possible geometries for a 4-coordinate complex.
(ii) Give the oxidation state and number of d electrons for the two complexes
(iii) Using crystal field energy diagrams, to explain the experimental findings.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcb1fd28-623f-4675-95fd-8852c6893ce5%2F25014f57-a556-442b-8c8e-b4d6e48998e8%2Fm6v0x2_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. a)
b)
c)
Tutorial 4
Sketch the representations of the 3d orbitals to show their orientations in space.
Explain why the day orbital is lower in energy than the dx2-y2 orbital in an octahedral complex.
Sketch the possible d-electron configurations for a d6 ion in octahedral crystal field, and give
an example of a complex with this arrangement.
2. For which of the following pairs would you expect to be larger and why?
a) [Cr(H₂O)]²+ and [Cr(H₂O)]³+
[CrF6] and [Cr(NH3)6]³+
c) [Fe(CN)6] and [Fe(CN)6]³-
e) [MnF6] and [ReF6]4
b)
d)
f)
[Ni(H₂O)]²+ and [Ni(en)3]²+
[Ni(en)3]2+ and [Ni(en)3]²+
3. Experimental evidence indicates that the complex K4[Fe(CN)6] has no unpaired electrons, while
[Fe(H₂O)6]Cl2 has four unpaired electrons.
(i) For both complexes give the coordination geometry, the oxidation state and the number of d
electrons.
(ii) Using crystal field energy diagrams, explain the experimental findings.
4. Experimental evidence indicates that the complex [PdCl4] ²- has no unpaired electrons, while
[NiC14]²- has two unpaired electrons.
(i) Describe two possible geometries for a 4-coordinate complex.
(ii) Give the oxidation state and number of d electrons for the two complexes
(iii) Using crystal field energy diagrams, to explain the experimental findings.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning