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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+

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
Chemistry
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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
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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.
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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