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.
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.
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...
Related questions
Question
Experimental evidence indicates that the complex [PdCl4]2- has no unpaired electrons, while
[NiCl4]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.
![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%2Fa1ea9fe2-8e18-4ecb-8e37-c75df28d8017%2Fpeiobdt_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.
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