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+
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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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.
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